Inorganic Chemistry Flashcards by Abi Peralta

A species X contains 9 protons, 10 electrons, and 11 neutrons. Predict whether it is
A. A neutral atom
B. an isotope
C. An anion
D. a cation

C. An anion

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The nuclei of tritium would contain ____ neutrons.
A. 1
B. 2
C. 3
D. 4

B. 2

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The total number of electrons at the L shell of an atom is
A. 2
B. 8
C. 18
D. 32

B. 8

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What is the maximum number of electrons in the O orbital?
A. 16
B. 8
C. 32
D. 50

D. 50

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How many electrons can have an / quantum number of 1 and an n quantum number of 2?
A. 5
B. 6
C. 10
D. 14

B. 6

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Which one of the following is an impossible set of quantum number for an electron in an atom?
A. 2,1,-1,-1/2
B. 1,0,0,1/2
C. 5,4,-3,1/2
D. 3,3,3,-1/2

D. 3,3,3,-1/2

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he noble gases are
A. Diatomic
B. monoatomic
C. triatomic
D. monoclinic

B. monoatomic

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Which of the following elements is a halogen?
A. He
B. Na
C. Kr
D. Cl

D. Cl

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Which of the following is an alkali metal?
A. O
B. Ne
C. K
D. Mg

C. K

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Arrange Ca, Be, and Mg according to increasing atomic size.
A. Ca < Mg < Be
B. Ca < Be < Mg
C. Be < Mg < Ca
D. Mg < Be < Ca

C. Be < Mg < Ca

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Arrange Ca, Be, and Mg according to increasing ionization energy.
A. Ca < Mg < Be
B. Ca < Be < Mg
C. Be < Mg < Ca
D. Mg < Be < Ca

A. Ca < Mg < Be

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Arrange Ca, Be, and Mg according to increasing electron affinity.
A. Ca < Mg < Be
B. Ca < Be < Mg
C. Be < Mg < Ca
D. Mg < Be < Ca

A. Ca < Mg < Be

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The oxidation state of Cr in K2CrO4 is
A. +6
B. -6
C. -2
D. +7

A. +6

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The element with the electron configuration 1s22s22p4
is
A. O
B. S
C. Ne
D. N

A. O

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Which bond has the least strength?
A. Covalent bond
B. electrovalent bond
C. van der Waal’s
D. ionic bond

C. van der Waal’s

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An example of ionic compound would be
A. H2O
B. HCl
C. NH3
D. NaCl

D. NaCl

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Which of the following compound would be covalent compound
A. SiO2
B. NaCl
C. LiF
D. KBr

A. SiO2

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NO2 is a molecule with a bent structure, the number of lone pairs in its central atom is
A. one
B. two
C. three
D. four

A. one

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Which of the following molecules have polar bonds and is described to be nonpolar?
A. H2O
B. NH3
C. CO2
D. HCl

C. CO2

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The structure of water can be described as
A. Polar and tetrahedral
B. Polar and linear
C. polar and bent
D. nonpolar and bent

C. polar and bent

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Determine the shape and polarity of a COBr2 molecule.
A. Trigonal palnar, polar
B. Tetrahedral, nonpolar
C. trigonal pyramidal, nonpolar
D. bent, polar

A. Trigonal palnar, polar

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Magnesium has three naturally occurring isotopes with isotopic mass and relative abundance of 23.98 (78.60% ), 24.98 (10.11% ), and 25.98 (11.29% ). Find the true mass of the isotopic mixture.
A. 22
B. 12
C. 24.31
D. 25.1

C. 24.31

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Only two isotopes of copper are present in naturally occurring copper: 62Cu (62.9298 u) and 65CU (64.9278 u). Calculate the percent composition of naturally occurring 62Cu using atomic mass of 63.646u.
A. 69.17%
B. 30.83%
C. 46.65%
D. 53.35%

A. 69.17%

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How many molecules are present in 0.20 gram of hydrogen gas?
A. 1.2 E23
B. 1.2 E22
C. 6 E23
D. 6 E22

D. 6 E22

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How many millimoles are there in 1.76 g of AgNO3? Ag= 107.9; N=14;O=16
A. 25.0
B. 10.4
C. 15.8
D. 30.5

B. 10.4

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What is the weight percent of carbon in carbon monoxide?
A. 30.5%
B. 34.6%
C. 40.3%
D. 42.8%

D. 42.8%

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How many electrons are in 0.01 g of gold?
A. 3 E19
B. 2.4 E21
C. 5 E-5
D. 3.2 E24

B. 2.4 E21

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The percent composition of an unknown element X in CH3X is 32%. Which of the following is element X?
A. H
B. F
C. Cl
D. Li

D. Li

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A protein is known to bind one molecule of oxygen (O2) per molecule of protein. If 12.2 g of protein bind 9.8 mg O2, what is the molecular weight of the protein?
A. 25,700
B. 79,600
C. 38,900
D. 39,800

D. 39,800

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What is the empirical formula for a compound that has the following composition by mass; 30%Si, 8.5%O and 61.2%F?
A. SiOF4
B. Si2OF4
C. Si2OF6
D. Si3OF6

C. Si2OF6

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What is the empirical formula of a compound that contains 7.989 g of carbon and 2.011 g of hydrogen?
A. C2H5
B. C3H
C. C8H2
D. CH3

D. CH3

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A compound is found to contain by mass 22.69% C, 1.41% H and 75.9% Br. What is the molecular formula of the compound if its molecular weight is 422?
A. C7H8Br2
B. C8H6Br4
C. C6H6Br4
D. C8H8Br2

B. C8H6Br4

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A compound containing only carbon, hydrogen, and oxygen was analysed and found to contain 70.6% C, 5.9% H and 23.5% O by mass. The molecular weight of the compound is 136 amu. What is the molecular formula?
A. C8H8O2
B. C8H4O
C. C4H4O
D. C5H6O2

A. C8H8O2

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What is similar about the electronic structure of Be, Mg, and Ca?
A. All the atoms contain a pair of s electrons in their outermost energy level
B. All the atoms contain a pair of p electrons in their outermost energy level
C. All are alkaline earth metals
D. All are in the same second group of the periodic table

A. All the atoms contain a pair of s electrons in their outermost energy level

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He phenomenon in which a steel needle can, with proper care, be made to float on the surface of some water illustrates a property of liquid known as:
A. Compressibility
B. polarizability
C. surface tension
D. triple point

C. surface tension

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Which of the following is different from the group?
A. B
B. Mg
C. As
D. At

B. Mg

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From what mineral is radium obtained?
A. Limestone
B. rutile
C. pitch blende
D. hematite

C. pitch blende

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Which one of the following is most likely to have ionic bonds?
A. HCl
B. Na2O
C. N2O
D. NCl3

B. Na2O

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What is the shape of the molecular structure of NH3?
A. Trigonal planar
B. trigonal pyramidal
C. tetrahedral
D. octahedral

B. trigonal pyramidal

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What is the molecular geometry of antimony pentafluoride?
A. Trigonal bipyramidal
B. octahedral
C. trigonal planar
D. tetrahedral

D. tetrahedral

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When an excess of dry chlorine was passed over 1.12 g heated iron, 3.25 g of a chloride of iron was obtained. What is the empirical formula of the chloride?
A. Fe3Cl
B. Fel2
C. FeCl3
D. Fe2Cl6

C. FeCl3

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Mesitylene, a hydrocarbon that occurs in small amounts in crude oil, has an empirical formula of C3H4. The experimentally determined molecular weight is 121 amu. What is the molecular formula of mesitylene?
A. C9H12
B. C3H4
C. C12H16
D. C6H12

A. C9H12

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The mass of proton or neutron is approximately ______ times that of the electron.
A. 1,736
B. 1,900
C. 1,700
D. 1,836

D. 1,836

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The total number of electrons at the fourth energy level is
A. 2
B. 8
C. 18
D. 32

D. 32

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Which of the following represents is an acceptable set of quantum number?
A. 2,2,-1,-1/2
B. 1,0,0,1/2
C. 5,-4,-3,1/2
D. 3,3,3,-1/2

B. 1,0,0,1/2

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For n=4 what are the possible values of l?
A. 3,2,1
B. 4,3,2,1
C. 3,2,1,0
D. 4,3,2,1,0

C. 3,2,1,0

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For l=2, what are the possible values of ml?
A. 1,0
B. 1,0,-1
C. 2,1,0
D. 2,1,0,-1,-2

D. 2,1,0,-1,-2

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What is the maximum number of electrons that can occupy the subshell 3d?
A. 3
B. 5
C. 6
D. 10

D. 10

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Which of the following Bohr orbits has the lowest energy?
A. n=2
B. n=3
C. n=4
D. n=5

A. n=2

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For n=4, how many values of l are possible?
A. 2
B. 3
C. 4
D. 5

C. 4

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The electronic configuration, 1s22s22p63s23p5, is that of
A. an alkali metal
B. a halogen
C. an inert gas
D. a transition meta

B. a halogen

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Which of the following represents an alkaline earth metal?
A. 1s22s1
B. 1s22s22p63s2
C. 1s22s22p6
D. 1s22s22p63s33p6

B. 1s22s22p63s2

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Protium atom contains no
A. Electron
B. proton
C. neutron
D. positron

C. neutron

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Which of the following is the lightest?
A. Alpha particle
B. beta particle
C. proton
D. hydrogen

B. beta particle

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The electrons in an incomplete outer shell are called
A. shell electron
B. kernel electron
C. chemical electrons
D. valence electron

D. valence electron

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The shape of ‘s’ orbital
A. Pyramidal
B. Tetrahedral
C. spherical
D. dumb-bell shaped

C. spherical

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The chemical family of elements called the noble gases is found in what column of the periodic table?
A. IA
B. IIA
C. VIIA
D. VIIIA

D. VIIIA

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A particular element is located in column IVA of the periodic table. How many dots would be placed around the symbol of this element in its electron dot notation?
A. 1
B. 3
C. 4
D. 8

C. 4

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Atoms of which element have the highest ionization energy?
A. calcium
B. potassium
C. sodium
D. magnesium

D. magnesium

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Transition elements are found in the
A. d & f energy level
B. s energy level
C. d energy level
D. p energy level

C. d energy level

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Which of the following is a metalloid?
A. Ge
B. Al
C. Be
D. Zn

A. Ge

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Which of the following sequences of ionization energies is incorrect?
A. K > Na > Li
B. K > Rb > Cs
C. F > O > C
D. O > S > Se

A. K > Na > Li

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By referring only to the periodic table, arrange the following in order of increasing electronegativity: Ga, P, As, S, O, F.
A. Ga < P < As < S < O < F
B. Ga < As < S < P < O < F
C. Ga < As < P < O < S < F
D. Ga < As < P < S < O < F

D. Ga < As < P < S < O < F

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In which of the following do we find a trigonal- pyramidal geometry?
A. BF3
B. SnCl2
C. PH3
D. TeCl4

C. PH3

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Which identification of shape is incorrect?
A. SbCl5- trigonal bipyramidal
B. SeCl4- seesaw
C. ClF5- square pyramidal
D. ICl3- trigonal pyramidal

D. ICl3- trigonal pyramidal

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Which of following diatomic is most polar?
A. BeO
B. BeS
C. BeSe
D. BeTe

A. BeO

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Which one of the following is a polar molecule? (I) BF3 (II) CF4 (III) NF3 (IV) PCl5
A. II and IV
B. I and III
C. III
D. I

C. III

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The element zinc consist of five isotopes with masses 63.929, 65.926, 66.927, 67.925, and 69.925 amu. The relative abundance of these five isotopes are 48.89, 27.82, 4.110, 18.57, and 0.62 percent respectively. From these data calculate the average atomic mass of zinc.
A. 63.93 amu
B. 66.93 amu
C. 65.389 amu
D. 65.39 amu

D. 65.39 amu

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Calculate the number of molecules in a tablespoon of table sugar, C12H22O11, weighing 10.5 g.
A. 6.0E23
B. 6.29E24
C. 1.85E22
D. 1.13E2

C. 1.85E22

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Calculate the mass in grams of 0.0112 mol of β-sucrose, C6H12O6.
A. 0.0112 g
B. 180 g
C. 1.12 g
D. 2.02 g

D. 2.02 g

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Calculate the number of molecules in 6.2 g of formaldehyde, CH2O.
A. 6.0E23
B. 3.7E24
C. 1.2E23
D. 2.4E23

C. 1.2E23

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One mole of CO2 contains the same number of atoms as in
A. 0.5 mole of S2O3
B. 0.5 mole of PCl3
C. 0.5 mole of H2SO3
D. 0.5 mole of H3BO3

C. 0.5 mole of H2SO3

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60.0 g of a dry-cleaning fluid was analysed and found to contain 10.80 g C, 1.36 g H, and 47.84 g Cl. Determine its empirical formula.
A. C3H3Cl3
B. C2H3Cl3
C. C4H6Cl5
D. CH2Cl2

B. C2H3Cl3

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What is the empirical formula of a compound with the molecular formula C6H12O6?
A. C4H8O4
B. C3H6O3
C. C2H4O2
D. CH2O

D. CH2O

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A compound has the empirical formula CH and a molecular mass of 78. What is the molecular formula of the compound?
A. C2H2
B. C3H3
C. C4H4
D. C6H6

D. C6H6

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Determine the empirical formula of a compound that contains 52.9% aluminium and 47.1% oxygen.
A. AlO
B. Al2O3
C. Al3O2
D. Al4O6

B. Al2O3

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Give the empirical formula of the following compound if a sample contains 40% C, 6.7% H, and 53.3% O by mass.
A. C4HO5
B. CH2O
C. C2H4O2
D. C3H6O3

B. CH2O

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What is the molecular formula of the following compound? Empirical formula CH, molar mass 78 g/mol.
A. CH
B. C2H2
C. C3H3
D. C6H6

D. C6H6

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Give the empirical formula of the following compound if a sample contains 57.8% C, 3.6% H, and 38.6% O by mass.
A. C2HO
B. C4H3O2
C. C8H6O4
D. C12H9O6

B. C4H3O2

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What is the molecular formula of the following compound? Empirical formula C2H3, molar mass 54 g/mol.
A. C2H3
B. C4H6
C. C6H9
D. C8H12

B. C4H6

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Which of the following does not exist as a gaseous diatomic molecule?
A. H2
B. O2
C. S2
D. F2

C. S2

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A bond in which an electron pair is equally shared by two atoms is
A. Ionic
B. Nonpolar covalent
C. polar covalent
D. coordinate covalent

B. Nonpolar covalent

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The bonding in HCl is best characterized as
A. Non polar covalent
B. coordinate covalent
C. ionic
D. polar

D. polar

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In which of the following is the angle between the covalent bonds greatest?
A. CO2
B. CH4
C. NH3
D. H2O

A. CO2

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No two electrons in the same atom can have the same set of quantum numbers is a statement of
A. Hund’s Rule of Multiplicity
B. Heisenberg’s Uncertainty
C. Dalton’s Atomic Theory
D. Pauli’s Exclusion Principle

D. Pauli’s Exclusion Principle

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Isotopes have different
A. Period number
B. group number
C. number of nucleons
D. atomic number

C. number of nucleons

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The azimuthal or secondary quantum number is related to the
A. Direction of turning
B. Shape of electron cloud
C. Orientation in space
D. Distance from the nucleus

B. Shape of electron cloud

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The magnetic quantum number is related to the
A. Direction of turning
B. Shape of the electron cloud
C. Orientation in space
D. Distance from the nucleus

C. Orientation in space

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Which of the following elements has the largest first- ionization energy?
A. Rb
B. Sr
C. Ca
D. K

C. Ca

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Which of the following elements would have the largest second-ionization energy?
A. Sc
B. Sr
C. Ca
D. K

D. K

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Of the following choices, which element is the most metallic?
A. Calcium
B. strontium
C. magnesium
D. barium

D. barium

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Which of the following is an inner f-block metal?
A. Zn
B. Sc
C. Ga
D. U

D. U

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Three sp2 hybrid orbitals lie in the same plane making with each other an angle of
A. 109°28”
B. 60°
C. 90°
D. 120°

D. 120°

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hich of the following is not a type of covalent bond?
A. Polar
B. nonpolar
C. coordinate
D. metallic

D. metallic

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When electrons are shared unequally between atoms or different elements, a _____ covalent bond occurs.
A. Polar
B. nonpolar
C. coordinate
D. molecular

A. Polar

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This covalent bond is most often formed in polyatomic molecules.
A. Polar
B. nonpolar
C. coordinate
D. molecular

C. coordinate

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How many grams of iron oxide, Fe2O3, can be produced from 2.50 g of oxygen reacting with solid iron?
A. 12.5 g
B. 8.32 g
C. 2.50 g
D. 11.2 g

B. 8.32 g

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An iron block weighs 5 Newtons and has a volume of 200 cubic centimeters. What is the density of the block in kg/m3?
A. 800
B. 988
C. 1255
D. 2550

D. 2550

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Hydrogen sulphide is removed from water by contacting the solution with warm air. The operation is
A. Distillation
B. leaching
C. absorption
D. stripping

D. stripping

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Sulphur is undesirable petroleum because
A. It causes engine knocking
B. It poisons the catalyst in the refining process
C. it increases the boiling point of the fuel
D. all that are mentioned

A. It causes engine knocking

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he geometry of the nitrate ion, NO3-, is best described as a
A. Tetrahedron
B. Square pyramid
C. trigonal bipyramid
D. triangular planar structure

D. triangular planar structure

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Very fine precipitates are most easily separated by
A. Distillation
B. filtration
C. centrifugation
D. evaporation

C. centrifugation

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The ion with the largest radius is
A. K+
B. I-
C. Cl-
D. Na+

B. I-

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The colored gas most associated with smog is
A. An oxide of nitrogen
B. On axide of hydrogen
C. an oxide of sulfur
D. a chloride of sulfur

A. An oxide of nitrogen

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A protein is
A. A polysaccharide
B. deoxyribonucleic acid
C. A polymer of amino acids
D. soluble because of the carbonyl groups
E. a polyester

C. A polymer of amino acids

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The bonding in benzene molecule, C6H6, in any of its resonance structures, contains
A. 6 sigma bonds and 6 pi bonds
B. 12 sigma bonds and 6 pi bonds
C. 6 sigma bonds and 12 pi bonds
D. 12 sigma bonds and 3 pi bonds

D. 12 sigma bonds and 3 pi bonds

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When a pot of water boils on the stove, small bubbles form at the bottom of the pan and rise to the surface. What is inside these bubbles?
A. Steam
B. hydrogen gas
C. oxygen gas
D. a vacuum

A. Steam

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Diamond is classified as
A. a covalent crystal
B. an ionic crystal
C. an amorphous solid
D. a metallic crystal

A. a covalent crystal

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A liquid substance that exhibits low intermolecular attractions is expected to have
A. Low viscosity, low boiling point, and low heat of vaporization
B. High viscosity, low boiling point, and low heat of vaporization
C. Low viscosity, high boiling point
D. Low viscosity, low boiling point, and high heat of vaporization

A. Low viscosity, low boiling point, and low heat of vaporization

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How do you classify liquids that vaporized easily?
A. Ideal liquid
B. saturated liquid
C. volatile liquid
D. osmotic liquid

C. volatile liquid

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The resistance of a layer of fluid to flow over the next layer is measured by
A. Viscosity
B. friction factor
C. surface tension
D. density

A. Viscosity

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A substance labelled hygroscopic
A. Reacts with atmospheric oxygen
B. Absorbs water from the atmosphere
C. spontaneously combusts
D. oxidizes easily

B. Absorbs water from the atmosphere

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In the Bronsted system, an acid is defined as
A. An electron pair acceptor
B. A hydroxide ion donor
C. an electron pair donor
D. a proton donor

D. a proton donor

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Elements that readily gain electros tend to have
A. High ionization energy and high electronegativity
B. High ionization energy and low electronegativity
C. low ionization energy and low electronegativity
D. low ionization energy and high electronegativity

A. High ionization energy and high electronegativity

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Which of the following is heavy water?
A. hydrogen dioxide
B. tritium oxide
C. deuterium oxide
D. dihydrogen oxide

C. deuterium oxide

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Which one of the following is a homogeneous mixture
A. Air
B. Iodine crystals
C. nitrogen
D. blue-cheese salad dressing

A. Air

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Which of the following is a pure substance?
A. Air
B. Concrete
C. nitrogen
D. blue-cheese salad dressing

C. nitrogen

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It is a yellowish gas.
A. Cl2
B. N2
C. CO2
D. H2

A. Cl2

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A volumetric analysis of a gaseous mixture is as follows: 12% CO2, 4% O2, 82% N2 and 2% CO. what is the percentage of CO on mass basis?
A. 1%
B. 1.2%
C. 1.5%
D. 1.09%

D. 1.09%

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A solution is prepared by dissolving 22.4 g of MgCl2 in 0.200 L of water. Taking the density of pure water to be 1 g/cc and the density of the resulting solution to be 1.089 g/cc, calculate the mole fraction of MgCl2 in the solution.
A. 0.0189
B. 0.0207
C. 0.0278
D. 0.0307

B. 0.0207

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According to the label, a bottle of vodka has a 40% by volume concentration. This means the vodka contains 40 mL of pure alcohol
A. In each 140 mL of vodka
B. To every 60 mL of vodka
C. to every 100 mL of water
D. mixed with water to make 100 mL vodka

D. mixed with water to make 100 mL vodka

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It is desired to make a 0.1 M solution by adding water to 5 grams of copper sulphate crystals, CuSO4.5H2O. What must be the final volume of the solution?
A. 120 mL
B. 140 mL
C. 180 mL
D. 200 mL

D. 200 mL

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A solution is prepared by dissolving 22.4 g MgCl2 in 0.200 L of water. Taking the density of pure water to be 1 g/cc and the density of the resulting solution to be 1.089 g/cc, calculate the molarity of the resulting solution.
A. 1.00 M
B. 1.10 M
C. 1.15 M
D. 1.25 M

C. 1.15 M

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Calculate the molarity of a solution containing 38% HCl by weight and having a density of 1.19 g/mL solution.
A. 8.7 M
B. 9.4 M
C. 11.7 M
D. 12.4 M

D. 12.4 M

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A solution is prepared by dissolving 22.4 g of MgCl2 in 0.200 L of water. Taking the density of pure water to be 1 g/cc and the density of the resulting solution to be 1.089 g/cc, calculate the molality of the resulting solution.
A. 1.18 m
B. 1.35 m
C. 1.40 m
D. 1.48 m

A. 1.18 m

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Suppose we have an aqueous solution of sulfuric acid whose density is 1.5091 g/cc and which contains 61% H2SO4 by weight. Calculate its molality.
A. 12.50 m
B. 13.2 m
C. 14.8 m
D. 16.0 m

D. 16.0 m

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Calculate the molar concentration of NaBr solution which has a density of 1.167 g/mL and a molality of 2.28.
A. 2.16 M
B. 2.80 M
C. 3.12 M
D. 3.40 M

A. 2.16 M

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What is the normality of a solution of H2SO4 if it has a specific gravity of 1.84 and contains 95.0% H2SO4 by weight?
A. 3.56 N
B. 5.63 N
C. 5.63 N
D. 35.6 N

D. 35.6 N

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What is the normality of a solution made by diluting 50 mL of H2SO4 (sp.gr = 1.080, containing 11.6% H2SO4 by weight) to a liter of solution?
A. 0.24
B. 0.13
C. 0.65
D. 0.98

B. 0.13

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A solution is made by mixing 30.0 mL of 8.00 M HCl, 100 mL of 2.00 M HCl, and enough water to make 200 mL of solution. What is the molarity of HCl in the final solution?
A. 0.455 M
B. 1.00 M
C. 1.20 M
D. 2.20 M

D. 2.20 M

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How much 1.00 M HCl should be mixed with a certain volume of 0.250 M HCl in order to prepare 1.00 L of 0.500 M HCl?
A. 333 mL
B. 667 mL
C. 430 mL
D. 570 mL

A. 333 mL

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What is the concentration of chloride ion in percent in a solution that contains 35 ppm chloride?
A. 3.50 E -6%
B. 3.50 E -5%
C. 3.50 E -5%
D. 3.50 E 2%

B. 3.50 E -5%

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Calculate the molarity of a 5.00 ppm Ca(NO3)2 solution. Ca=40; N=14; O=16
A. 2.56 E -6 M
B. 2.56 E -5 M
C. 3.05 E -5 M
D. 3.05 E -6 M

C. 3.05 E -5 M

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The maximum allowable chloride content according to the National Standard for Drinking Water is 0.2 ppm. What is the equivalent in mg/L?
A. 20
B. 1000
C. 0.2
D. 200

C. 0.2

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A number of electrons has a total charge of 1.1 x 10 -18 C. How many electrons are there?
A. 1
B. 2
C. 4
D. 7

D. 7

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Two charges at +2.0 E -9 C that are 3.0 mm apart repel each other with a force of
A. 4 E -9 N
B. 4 E -3 N
C. 6 E 3 N
D. 3.6 E 7 N

B. 4 E -3 N

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How many calories are developed in 1.0 min in an electric heater which draws 5.0 amperes when connected to a 100-volt line?
A. 4800 cal
B. 5200 cal
C. 6500 cal
D. 7170 cal

D. 7170 cal

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What is the mass of aluminium produced in 1 hr in the electrolysis of molten Al2(SO4)3 if the electrical current is 10 A?
A. 3.36 g
B. 5.04 g
C. 1.00 g
D. 0.167 g

A. 3.36 g

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What current is required to produce two grams of metallic copper from copper sulphate solution in 1.5 hours?
A. 0.87 A
B. 1.12 A
C. 1.52 A
D. 1.85 A

B. 1.12 A

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An aqueous solution of gold (III) nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g Au has been deposited on the cathode. If the atomic weight of Au is 197, determine the duration of the electrolysis.
A. 65.43 mins
B. 23.67 min
C. 58.28 mins
D. 60 minutes

C. 58.28 mins

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A current of electricity was passed through a series of cells containing AgNO3, CuSO4, and H2SO4 solutions for a period of 25 minutes. If the weight of silver deposited was 0.5394 g, what would be the weight of the copper?
A. 0.159 g
B. 1.59 g
C. 15.9 g
D. 159 g

A. 0.159 g

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One faraday of current was passed through the electrolytic cells placed in a series containing solutions of Ag+, Ni+2, and Cr+3 respectively. The amount of Ag (at. Wt. 108), Ni (at. Wt. 59) and Cr (at. Wt. 52) deposited will be:
A. 108 g Ag, 29.5 Ni, 17.5 g Cr
B. 108 g Ag, 108 g Ni, 108 g Cr
C. 108 g Ag, 59 g Ni, 52 g Cr
D. 108 g Ag, 117 g Ni, 166 g Cr

A. 108 g Ag, 29.5 Ni, 17.5 g Cr

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A number of electrons has a total charge of 1.1×10 -18 C. How many electrons are there?
A. 1
B. 2
C. 4
D. 7

D. 7

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Two charges at +2.0 E -9 C that are 3.0 mm apart repel each other with a force of
A. 4 E -9 N
B. 4 E -3 N
C. 6 E 3 N
D. 3.6 E 7 N

B. 4 E -3 N

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A kilogram of molecular hydrogen contains 3.01×10 exp 26 molecules, each consisting of two hydrogen atoms. If all the electrons were removed and placed 1.0 meter away from the protons, what would be the electrical force between them?
A. 8.35 E 26 N
B. 8.35 E 25 N
C. 8.35 E 28 N
D. 8.35 E 23 N

B. 8.35 E 25 N

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A 6 V insulated battery delivers a 5 A current over a period of 20 min. Calculate the heat transfer that must occur to return the battery to its initial temperature.
A. 36 kJ
B. 45 kJ
C. -36 kJ
D. -45 kJ

A. 36 kJ

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What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4)3 for 60.0 minutes using a constant current of 10.0 amperes?
A. 0.187 g
B. 0.373 g
C. 3.25 g
D. 6.47 g

D. 6.47 g

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The number of electrons necessary to produce 1.00 gm of Cu from Cu2+ at the cathode of an electrolytic cell is
A. 1.89×1022
B. 3.04×103
C. 9.47×1021
D. 1.91×1025

A. 1.89×1022

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What is the equivalent molar concentration of 0.273 m KCl? The solution has a density of 1.011 g/mL.
A. 4
B. 0.271
C. 0.421
D. 1.21

B. 0.271

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A 0.5 M solution of H2SO4 is the same as ______ H2SO4.
A. 2 N
B. 1 N
C. 0.5 N
D. 0.1 N

B. 1 N

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Ten milliliters of 10 N H2SO4 is diluted to 80 mL. What is the molarity of the dilute acid solution?
A. 1.6 M
B. 0.8 M
C. 1.25 M
D. 0.625 M

D. 0.625 M

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A 2.5-g sample of groundwater was found to contain 5.4 microgram of Zn2+. What is the concentration of Zn2+ in parts per million?
A. 1.5
B. 2.2
C. 3.0
D. 3.7

B. 2.2

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Calculate the volume of concentrated sulfuric acid (density 1.84 g/mL), containing 98.0% H2SO4 by weight, that would contain 40 g of pure H2SO4.
A. 17.5 mL
B. 19.0 mL
C. 21.9 mL
D. 22.2 mL

D. 22.2 mL

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A solution of HCl has a specific gravity of 1.12 and contains 23.81% HCl by weight. How many grams of HCl are present in each millilitre of the solution?
A. 1.2
B. 12.6
C. 13.2
D. 0.27

D. 0.27

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A solution is made of 25.0 mL of 0.250 M of sulfuric acid and 15.0 mL of 0.500 M hydrochloric acid all diluted to 250 mL. what is the resulting of the hydrated proton?
A. 80.0 M
B. 0.08 M
C. 0.0558 M
D. 0.030M

B. 0.08 M

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How many milliliters of water must be added to 5 mL of 12 M HCl solution to make a 3 M HCl solution?
A. 10 mL
B. 15 mL
C. 20 mL
D. 25 mL

B. 15 mL

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A solution contains 10.6 mg of Na2CO3 per mL. To what volume should 100 mL of the solution be diluted to make it 0.01 N?
A. 1 L
B. 1.5 L
C. 2 L
D. 2.5 L

C. 2 L

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Twenty grams of sulfuric acid crystals is dissolved in water to obtain 500 mL solution. What is the normality of the solution?
A. 0.012 N
B. 0.816 N
C. 0.408 N
D. 0.204

B. 0.816 N

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The molality of a solution of ethyl alcohol in water is 1.54 mol/ kg. How many grams of alcohol are dissolved in 2.5 kg of water?
A. 177
B. 187
C. 192
D. 200

A. 177

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A solution is prepared by dissolving 4.21 g of glucose in 72.3 g of water. What is the molality of the glucose solution?
A. 5.5
B. 0.0234
C. 4.21
D. 0.323

D. 0.323

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A solution is made by dissolving 4.35 g glucose in 25 mL water. Calculate the molality of glucose in the solution.
A. 0.850 m
B. 0.915 m
C. 0.964 m
D. 0.992

C. 0.964 m

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A solution of hydrochloric acid contains 36% HCl by mass. Calculate the molality of HCl in the solution.
A. 10 m
B. 12 m
C. 15 m
D. 18 m

C. 15 m

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What will be the molarity of 56.5 g of silver nitrate in 3.5 liters of solution?
A. 0.946 M
B. 9.46 M
C. 0.0946 M
D. 94.6 M

C. 0.0946 M

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What will be the molarity of the phosphoric acid solution of specific gravity 1.426 and containing 98% by weight of pure phosphoric acid?
A. 1.426 M
B. 2.15 M
C. 14.26 M
D. 3.12 M

C. 14.26 M

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What will be the molarity of 5.6 gm of KMnO4 in 30 mL of the solution?
A. 0.059 M
B. 0.59 M
C. 9 M
D. 1.2 M

D. 1.2 M

What weight in grams of KMnO4 is needed to form a 250 mL solution of 0.10 M?
A. 2.90
B. 3.45
C. 3.95
D. 4.211.09

C. 3.95

The density of a solution that is 20.0% by weight HClO4 is 1.138 g/mL. Calculate the molarity of the HClO4.
A. 0.442
B. 1.99
C. 3.45
D. 2.26

D. 2.26

How many grams of sodium hydroxide is necessary to prepare 250.0 mL of 0.50 M NaOH?
A. 5.0
B. 8.2
C. 6.5
D. 20.0

A. 5.0

Twenty grams of sulfuric acid crystals is dissolved in water to obtain 500 mL solution. What is the molarity of the solution?
A. 0.012 M
B. 0.816 M
C. 0.408 M
D. 0.204 M

C. 0.408 M

Hydrogen peroxide solution of hair bleaching is usually prepared by mixing 5 g of hydrogen peroxide per 100 mL solution. What is the molarity of the solution?
A. 1.0 M
B. 1.95 M
C. 1.5 M
D. 1.8 M

C. 1.5 M

Ten grams of NaCl is added in 90 grams water, what is the mole fraction of NaCl?
A. 0.964
B. 0.054
C. 0.872
D. 0.033

D. 0.033

A solution contains 35% ethyl alcohol (molecular weight of 46 g/mol), 50% water (molecular weight 18 g/mol) and 15% acetic acid (molecular weight of 60 g/mol). Calculate the mole fraction of ethyl alcohol in the mixture.
A. 0.261
B. 0.201
C. 0.310
D. 0.691

B. 0.201

Calculate the mole fraction of H3PO4 in 25% aq H3PO4 solution.
A. 0.105
B. 0.058
C. 0.218
D. 0.719

B. 0.058

What is the mole fraction of ethyl alcohol in an aqueous solution that is 50% ethyl alcohol by mass?
A. 1.09
B. 0.259
C. 0.281
D. 0.719

C. 0.281

A substance with a specific gravity of 0.5 is ______ times as dense as water.
A. One-half
B. 2
C. 5
D. 3

A. One-half

A cube of plastic 1.5 cm on a side has a mass of 1.9 g. What is the density in g/cm3?
A. 1.9
B. 0.56
C. 1.78
D. 3.4

B. 0.56

The density of liquid bromine is 3.12 g/mL. What is the mass of 0.250 L of bromine?
A. 0.780 g
B. 780 g
C. 0.0801 g
D. 80.1 g

B. 780 g

The force between two charges of -3.0 E -9 C that are 50 mm apart is
A. 1.8 E-6 N
B. 3.6 E-15 N
C. 1.6 E-6 N
D. 3.2 E-5 N

D. 3.2 E-5 N

A 100-watt 110-volt incandescent lamp is connected in a series with an electrolytic cell containing cadmium sulphate solution. What weight of cadmium should be deposited by the current flowing for 10 hours?
A. 17.2 g
B. 19.1
C. 21.4
D. 23 g

B. 19.1

How many grams of iron can be plated out at the cathode if a solution of Fe2+ is electrolyzed by a current of 1 ampere for 30 minutes?
A. 0.52
B. 1.04
C. 838
D. 16.6

A. 0.52

A current of 0.75 ampere is passed to a copper (II) sulphate solution for 10 minutes. Calculate the grams of copper deposited.
A. 0.45 g
B. 1.20 g
C. 2.07 g
D. 0.15 g

D. 0.15 g

A chemical engineer wants to make chlorine from molten sodium chloride, if he uses a current of one ampere for 5 minutes, how many grams could be produced?
A. 0.11 g
B. 0.15 g
C. 0.09 g
D. 0.14 g

A. 0.11 g

How many grams of iron (Fe) could be deposited by 8.5 E3 coulombs from a solution of FeCl2?
A. 2.46
B. 0.406
C. 4.48
D. 316.7

A. 2.46

How many coulombs would it take to deposit 1 gram Ag from AgNO3 solution?
A. 800
B. 1000
C. 894
D. 940

C. 894

What current strength in amperes will be required to liberate 10 grams of iodine from KI solution in one hour?
A. 0.021
B. 0.21
C. 2.1
D. 21

C. 2.1

What is the electric current in amperes if 7.25 g Ag is deposited at the cathode in 2.00 hr in the electrolysis of AgNO3 (aq)?
A. 4.32
B. 54
C. 2.56
D. 1.32

How many calories are developed in 1.0 min in an electric heater which draws 5.0 amp when connected to a 110-volt line?
A. 4800 cal
B. 5200 cal
C. 6500 cal
D. 7900 cal

D. 7900 cal

Who determined that energy is radiated only when an electron falls from a higher energy level to a lower energy level?
A. Einstein
B. Rutherford
C. Heisenberg
D. Bohr

D. Bohr

Who determine the charge of an electron by means of oil droplet experiment?
A. Rutherford
B. Heisenberg
C. Millikan
D. de Broglie

C. Millikan

Who showed that electrons can be considered to have both particle character and wave character?
A. Thomson
B. Moseley
C. Heisenberg
D. de Broglie

D. de Broglie

Who determined that no two electrons may have the same set of four quantum numbers?
A. Planck
B. Pauli
C. Hund
D. Rutherford

B. Pauli

The quantity of heat needed to raise the temperature of a substance 1°C is its
A. Heat capacity
B. specific heat
C. enthalpy
D. calorimetry

B. specific heat

The properties of a real gas are most likely to deviate from those properties predicted for an ideal gas when
A. The pressure is low
B. The temperature is high
C. The pressure is high and the temperature is low
D. The pressure is low and the temperature is high

C. The pressure is high and the temperature is low

From the thermal decomposition of a pure solid, we obtained a solid and a gas, each of which is a pure substance. From this information, we can conclude with certainty that
A. The original solid is not an element
B. Both products are elements
C. at least one of the products is an element
D. the solid is a compound and the gas is an elemen

A. The original solid is not an element

Which of the following is not an SI unit?
A. Meter
B. kilogram
C. angstrom
D. pascal

C. angstrom

The critical point for a mixture occurs for which of the following cases?
A. The vapor and the liquid have a single form
B. The vapor phase is stable
C. the liquid has no absorbed gas
D. the liquid is completely vaporized

A. The vapor and the liquid have a single form

Which of the following elements and compounds is unstable in its pure form?
A. Sodium
B. helium
C. carbon dioxide
D. neon

A. Sodium

A substance is oxidized when which of the following occurs?
A. It turns red.
B. It loses electrons.
C. it becomes more negative
D. it gives off heat

B. It loses electrons.

Which of the following affects most of the electrical and thermal properties of materials?
A. The atomic weight expressed in grams per gram-atom
B. The electrons, particularly the outermost ones.
C. The magnitude of the electrical charge of the protons
D. The weight of the atoms

B. The electrons, particularly the outermost ones.

The indicator used to determine the anti-knock characteristics of gasoline is
A. Aniline point
B. octane number
C. cetane number
D. diesel index

B. octane number

It is the reactant which is present in least stoichiometric proportion.
A. Limiting reactant
B. excess reactant
C. catalyst
D. inhibitor

A. Limiting reactant

The element present in complete fertilizers are
A. C, H, O
B. C, H, N
C. Ca, Mg, S
D. N, P, K

D. N, P, K

Because water molecules are associated through hydrogen bonding, water has a high
A. Temperature
B. density
C. boiling point
D. solubility

C. boiling point

The only common liquid in Earth is
A. mercury
B. water
C. petroleum
D. oxygen

B. water

Because oil slick do not dissolve in water, one might expect oil to be composed of ______ molecules.
A. Nonpolar
B. polar
C. subpolar
D. arctic

A. Nonpolar

Which of the following is not true?
A. Solubility of gases in water increases with increasing temperature
B. Solubility of gases in water increases with increasing pressure
C. Solubility of gases in water is important for fish populations
D. Solubility of both oxygen and nitrogen gas increases with pressure

A. Solubility of gases in water increases with increasing temperature

A scientific statement, often mathematical in form, that summarizes experimental data is called a
A. Law
B. theory
C. hypothesis
D. proposition

A. Law

All samples of a pure substance
A. Contain no chemicals
B. Have a variable composition
C. have the same composition
D. are heterogeneous

C. have the same composition

Elements are placed in groups in the periodic table on the basis of
A. Alphabet listing
B. Number of neutrons in the nucleus
C. similar chemical properties
D. order of discovery

C. similar chemical properties

Isotopes have the same
A. Mass number
B. atomic number
C. atomic mass
D. half-life

B. atomic number

Which hydrogen isotope contains one neutron?
A. Protium
B. deuterium
C. tritium
D. none of these

B. deuterium

It is the scattering of light by colloidal particles.
A. Brownian movement
B. Tyndall effect
C. Corioles effect
D. Messner effect

B. Tyndall effect

A type of colloid in which a liquid is dispersed in a liquid, example, milk.
A. Foam
B. emulsion
C. sol
D. aerosol

B. emulsion

A type of colloid in which a liquid/solid is dispersed in a gas example fog, smoke.
A. Aerosol
B. foam
C. emulsion
D. sol

A. Aerosol

A type of colloid in which a gas is dispersed in a liquid, example whipped cream.
A. Aerosol
B. foam
C. emulsion
D. sol

B. foam

It refers to adherence to a surface.
A. Adsorption
B. absorption
C. desorption
D. osmosis

A. Adsorption

Which of the following is an aluminium ore?
A. Sphalerite
B. amalgam
C. galena
D. bauxite

D. bauxite

Which of the following radioisotopes is used in treating cancer?
A. Cobalt-60
B. uranium-233
C. helium-4
D. uranium-238

A. Cobalt-60

A substance that is capable of acting as either an acid or a base.
A. Buffer
B. amphoteric
C. Lewis acid
D. Lewis base

B. amphoteric

A substance (molecule or ion) that can transfer a proton to another substance.
A. Arrhenius acid
B. Arrhenius base
C. Bronsted acid
D. Bronsted base

C. Bronsted acid

The acid found in vinegar is
A. Acetic acid
B. lactic acid
C. formic acid
D. citric acid

A. Acetic acid

The number of equivalents of solute in one Liter of solution is
A. Molarity
B. formality
C. normality
D. molality

C. normality

Two electrons can occupy the same orbital because they have different
A. Principal quantum number
B. Magnetic quantum number
C. angular momentum quantum number
D. spin quantum number

D. spin quantum number

Two isotopes of the same element have
A. the same number of protons, electrons, and neutrons
B. the same number of protons and neutrons but different numbers of electrons
C. the same number of protons and electrons but different numbers of neutrons
D. the same number of electrons and neutrons but different numbers of protons

C. the same number of protons and electrons but different numbers of neutrons

What is the color of nickel chloride?
A. White
B. red
C. yellow
D. green

C. yellow

A physical characteristic of water caused by suspended impurities which makes it cloudy.
A. Turbidity
B. alkalinity
C. pH
D. acidity

A. Turbidity

Which of the following parameter is a chemical characteristics of water?
A. Turbidity
B. color
C. hardness
D. odor

A. Turbidity

A cylindrical oil-storage tank is 60 ft deep and contains an oil of density 55lbm/ft3. Its top is open to the atmosphere. What is the gauge pressure at the bottom of the tank?
A. 140 kPa
B. 152kPa
C. 158kPa
D. 168kPa

C. 158kPa

A pressure gage measures 50kPa vacuum in a system. What is the absolute pressure if the atmospheric pressure is 101 kPa?
A. 151 kPa
B. 51 kPa
C. 85 k Pa
D. 60 kPa

B. 51 kPa

Calculate the gage pressure at a depth of 100 meters in sea water, for which 𝛾 = 10.1 kN/m3.
A. 1010 kPa
B. 1110 kPa
C. 1210 k Pa
D. 1240 kPa

A. 1010 kPa

A Fahrenheit and a centigrade thermometer are both immersed in a fluid and indicates a Fahrenheit reading that is numerically twice that of centigrade reading. What is the temperature of the fluid expressed in as degrees Kelvin?
A. 223
B. 780
C. 433
D. 420

C. 433

At what temperature do the Celsius
scale and Fahrenheit scale readings have the same numerical value?
A. 40°C or 40°F
B. 32°C or 32°F
C. -40°C or -40°F
D. 100°C or 100°F

C. -40°C or -40°F

The volume of the sample of gas is 600 mL at a pressure of 1.65 atm. The pressure of the same gas would exert at a constant temperature, when the volume is changed to 500 mL, would be
A. 2.84 atm
B. 2.74 atm
C. 2.64 atm
D. 2.54 atm

C. 2.64 atm

If a gas with a pressure of 2 atm is raised in temperature from 100 K to 300 K, an the volume remains the same, its pressure
A. is decreased to 1 atm
B. is raised to 3 atm
C. is decreased to 2/3 atm
D. is raised to 6 atm

D. is raised to 6 atm

A bubble of air at 0.010 m3 in volume is formed at the bottom of the lake which is 30 m deep where the temperature is 8°C. the bubble rises to the surface where the water temperature is 26°C and the pressure is atmospheric pressure. The volume of the bubble when it reaches the surface is
A. 0.020 m3
B. 0.036 m3
C. 0.042 m3
D. 0.029 m3

C. 0.042 m3

The density of an unknown element is the gaseous state is 1.6 g/L at 300K and 1 atm. Which of the following could be the element?
A. O2
B. A-
C. He
D. Ne

B. A-

Give one molecule of CO2, what is the volume of the gas ta STP?
A. 1.2 E-24 L
B. 2.65 E-20 L
C. 3.2 E-12 L
D. 3.72 E-23 L

D. 3.72 E-23 L

The relative rate of diffursion of a gas (mol. wt. = 98) as compared to hydrogen will be
A. 1/7
B. 1/5
C. 2/5
D. 1

O2 gas effused to a pinhole in 5 sec. how long will it take an equivalent amount of CO2 to effuse under the same conditions?
A. 4.3 sec
B. 5.9 sec
C. 3.8 sec
D. 0.23 sec

B. 5.9 sec

Under the same conditions of temperature and pressure, which gas will diffuse the slowest rate?
A. helium
B. neon
C. argon
D. radon

D. radon

Find the total pressure exerted by 2 grams of ethane and 3 grams of CO2, in a 5-liter vessel at 50°C.
A. 740 mmHg
B. 30.75 psia
C. 98 kPa
D. 30.715 atm

D. 30.715 atm

A gaseous mixture contains 20 g of N2, 83 g of O2 and 45 g of CO2 in a 5-liter vessel at 50°C.
A. 30.1 g/mol
B. 34.2 g/mol
C. 35.8 g/mol
D. 36.3 g/mol

B. 34.2 g/mol

When evacuated or empty a gas density bulb 29.3125 grams. First, CO2 gas was used to fill the bulb at 40 deg C and 1.0 atm P and it weighs 30.0079g. The bulb was then evavuated and filled with a mixture of CO and CO2 under the same temperature and pressure. With this mixure the bulb weighed 29.9332. Determine the % CO in the mixture.
A. 21
B. 29
C. 32
D. 15

B. 29

The density of a gas of O2 and N2 is 1.1705 g/L at 27°C and 750 mmHg. The % of N2 in the mixture is
A. 70%
B. 68%
C. 30%
D. 32%

A. 70%

Calculate the rms speed of a nitrogen molecule at 25°C.
A. 515 m/s
B. 720 m/s
C. 815 m/s
D. 850 m/s

A. 515 m/s

At 0°C the average velocity of methane molecule in air 600 m/s. What is the total kinetic energy of 1.00 mol of methane molecules moving at this speed?
A. 4.78 E-21 J
B. 2.88 E3 J
C. 5.76 E3J
D. 1.80 E5J

B. 2.88 E3 J

The molecule diameter of CO is 3.19×10-8 cm, at 300K and pressure of 100 mmHg. What is the mean free path of the gas in cm?
A. 6.86×10-8
B. 6.86×10-5
C. 6.86×10-3
D. 6.86×10-4

B. 6.86×10-5

Calculate the gravimetric factor for Fe in Fe2O3.
A. 0.6994
B. 0.5670
C. 0.7850
D. 0.2355

A. 0.6994

Calculate the grams of silver in 1.000 g of AgCl.
A. 0.35 g
B. 0.75 g
C. 0.45 g
D. 0.80 g

B. 0.75 g

Calculate the number of grams of MgCl2 necessary to precipitate 1.000 g of MgNH4PO4.
A. 0.6994 g
B. 0.1540g
C. 0.8905 g
D. 0.3580 g

A. 0.6994 g

Ammonia is burned to for nitric oxide in the following reaction 4NH3 + 5O2 → 4NO + 6H2O. The mass of NO produced if 200 kg of O2 react and reaction proceeds to completion is:
A. 290 kg
B. 150 kg
C. 240 kg
D. 120 kg

B. 150 kg

Suppose a reaction x + 2y +z + 3w → products there are 2 moles of x, and 1 mole for each y, z and w. What is the limiting reactant?
A. x
B. y
C. z
D. w

D. w

Suppose the reaction Ca3(PO4)2 + 3H2OSO4 → 3CaSO4 + 2H3PO4 is carried out starting with 103 g of Ca3(PO4)2 and 75g of H2SO4. How much H2PO4 will be produced Ca=40; P=31; H=1; O=16; S=32 amu
A. 74.9 g
B. 50.0 g
C. 112 g
D. 32.5 g

B. 50.0 g

The gas acetylene is produced according to the following reaction by treating calcium carbide with water:
CaC2 + 2H2O → C2H2 + CaOH2
Calculate the number of hours of service that can be derived from 1.0 lb of carbide in an acetylene lamp burning 2 cu ft. gas per hour at a temperature of 75°F and a pressure of 743 mmHg.
A. 3.11 hr
B. 3.45 hr
C. 2.87 hr
D. 1.86 hr

A. 3.11 hr

Propane is a hydrogen with the formula C3H8 that is used as bottled gas. How many liters of oxygen are needed to bum 1 L of propane gas? Assume all volumes to be measured at the same temperature and pressure.
A. 5 L
B. 6 L
C. 3 L
D. 2 L

A. 5 L

Propane is a hydrogen with the formula C3H8 that is used as bottled ga. How many liters of carbon dioxide are produced by the reaction? Assume all volumes to be measured at the same temperature and pressure.
A. 5 L
B. 6 L
C. 3 L
D. 2 L

C. 3 L

PCl5(g) dissociates into PCl3(g) and Cl2(g) when heated at 250oC and 1 atm. If the density of the gas mixture equilibrium is 4.4 g/L, the fraction of PCl5(g) dissociated is
A. 0.103
B. 0.328
C. 0.725
D. 0.209

A. 0.103

One liter of oxygen is collected at 22°C. The temperature of the room rises to 25°C and then falls to 20°C. Calculate the contraction of the gas in ml as it cools from 25°C to 20°C.
A. 0.17 ml
B. 1.7 ml
C. 17 ml
D. 170 ml

B. 1.7 ml

Two gases occupy two containers, A and B. The gas in A, of volume 0.11 m3, exerts a pressure of 1.38 MPa. The gas in B, of volume 0.16 m3, exerts a pressure of 0.69 MPa. The two containers are united by a tube of negligible volume and the gases are allowed to intermingle. What is the final pressure in the container if the temperature remains constant?
A. 0.78 MPa
B. 0.83 MPa
C. 0.92 MPa
D. 0.97 MPa

D. 0.97 MPa

An ideal gas ahs been placed in a tank at 40°C. The gauge pressure is initially 608 kPa. One-fourth of the gas is released from the tank and thermal equilibrium is established. What will be the gauge pressure if the is 315°C? Take standard atmospheric pressure as 101 kPa.
A. 823 kPa
B. 873 kPa
C. 856 kPa
D. 898 kPa

D. 898 kPa

Estimate the number of molecules left in a volume of the size of a pin head about 1 cubic mm when air is pumped out to give a vacuum of 10-6 mmHg at 25°C.
A. 3.24 E7
B. 5.31 E24
C. 8.02 E23
D. 1.05 E10

A. 3.24 E7

Helium and argon monoatomic gases and their atomic weights are 4 and 40 respectively. Under identical conditions helium will diffuse through a semipermeable membrane
A. 3.16 times as fast as argon
B. 1.58 times as fast as argon
C. 7.32 times as fast as argon
D. 10 times as fast as argon

D. 10 times as fast as argon

A gas mixture contains 50 g of cyanogens, C2N2, and 50 g of CO2.if the total pressure is 2.56 atm, what is the partial pressure of cyanogens?
A. 1.87 atm
B. 1.28 atm
C. 1.39 atm
D. 2.46 atm

A. 1.87 atm

Calculate the root mean square speed of an oxygen molecule at 298 K.
A. 450 m/s
B. 465 m/s
C. 470 m/s
D. 482 m/s

D. 482 m/s

The fermentation of glucose, C6H12O6, preoduces ethyl alcohol,C2H5OH, and carbon dioxide. C6H12O6(aq) → 2C2H5OH(aq) + 2CO2(aq). How many grams of ethanol can be produced from 10 g of glucose?
A. 10.0 g
B. 2.56 g
C. 5.11 g
D. 4.89 g

How many grams of carbon dioxide will be formed when 23 grams of C2H4 reacts with 3 grams of O2?
A. 9.4
B. 6.2
C. 4.1
D. 2.8

D. 2.8

Determine the molar volume in cm3/g mol of n-butane at 460 K and 15 atm assuming ideal gas.
A. 1786
B. 1290
C. 2516
D. 2305

C. 2516

Calculate the pressure at a depth of 100 meters in seawater, for which the specific weight is 10.1 kN/m3.
A. 1212 kPa
B. 1414 kPa
C. 1616 kPa
D. 1010 kPa

D. 1010 kPa

Suppose Isaac Newton weighed 65 kg. calculate the pressure he has exerted on the ground when wearing boots with soles of total area 250 square centimeters.
A. 26 kPa
B. 30 kPa
C. 32 kPa
D. 40 kPa

A. 26 kPa

A solvent storage tank, 19.0 m high contains liquid styrene (sp. gr. 0.929). A pressure gage, which gives kPa reading, s fixed at the base of the tank to be used to determine the level of styrene. Determine the gage pressure when the tank is full of styrene.
A. 173
B. 172000
C. 200.4
D. 17.7

A. 173

How many degrees Celsius is 100 degrees Farenheit?
A. 37.8
B. 2.667
C. 1.334
D. 13.34

A. 37.8

Liquid nitrogen boils at 77 K. What is the boiling point on the Fahrenheit temperature scale?
A. -321°F
B. -141°F
C. -295°F
D. 171°F

A. -321°F

The temperature known as room temperature is nearest to
A. 0 degree Celsius
B. 60 degree Celsius
C. 20 degree Celsius
D. 100 degree Celsius

C. 20 degree Celsius

The volume of a gas is 50ml when the pressure is 1520 mm and the temperature is 0°C. The volume becomes 25 ml when the temperature is raised to 546°C and the pressure is changed. Calculate the final pressure.
A. 9.120 mm
B. 91.20 mm
C. 912.0 mm
D. 9120mm

D. 9120mm

A rubber balloon containing hydrogen has a volume of 3 liters. The temperature is 20°C and the pressure exerted by the hydrogen is 850 mm. The balloon rises to the ceiling where it expands to 3200 ml and the pressure diminishes to 840 mm. Calculate the temperature near the ceiling;
A. 0.36°C
B. 3.6°C
C. 36°C
D. 360°C

D. 360°C

A sealed tank contains oxygen at 27°C and a pressure of 2 atm. If the temperature increases to 100°C, what will be the pressure inside the tank?
A. 2.49 atm
B. 3.44 atm
C. 4.92 atm
D. 5.94 atm

A. 2.49 atm

A volume of 400 cc of air is measured at a pressure of 740 mmHg abs and a temperature of 18 C. What will be the volume at 760 mmHg abs and 0°C?
A. 0.36°C
B. 3.6°C
C. 36°C
D. 360°C

D. 360°C

The volume of a sample of gas is 750 mL at a pressure of 1.60 atm. When the temperature is held constant, the volume of this same sample of gas at 2.0 atm would be
A. 800 mL
B. 700 mL
C. 650 mL
D. 600 mL

A. 800 mL

An ideal gas is in a vessel of volume, V1, at 1 atm. The gas is released and allowed to expand into an evacuated 0.5 L bulb. Once equilibrium has been reached, the temperature remains the same while the pressure is 500 mmHg. Find V1.
A. 0.853 L
B. 0.961 L
C. 1.069 L
D. 1.077 L

Calculate the volume of one gram mole of helium at STP?
A. 5 L
B. 6 L
C. 3 L
D. 2 L

C. 3 L

At STP the density of chlorine is 3.22 kg/cubic meter. What weight of this gas is contained in a flask of 100 cubic centimeter at 24°C and 100 kPa?
A. 0.563 g
B. 0.292 g
C. 0.420 g
D.0.321 g

B. 0.292 g

A 0.7m3 tank contains 4.5 kg of an ideal gas. The gas has a molecular weight of 44 and is at 21°C. What is the pressure of the gas?
A. 289.6 kPa
B.0.292
C. 3.26.7 kPa
D. 357.2 kPa

D. 357.2 kPa

A 287.5 cm3 of vapor at 100°C and 100 kPa has a mass of 0.725 gr. What is the molecular weight of the vapor?
A. 77.94
B. 80.55
C. 326.7 kPa
D. 85.44

A. 77.94

The relative rate of diffusion of a gas (of molecular weight 128) as compared to oxygen.
A. 2 times
B. 1/4 th
C. 1/8 th
D. 1/2

D. 1/2

An unknown gas composed of homonuclear diatomic molecules effuses at a rate that is only 0.355 times that of O2 at the same temperature. What is the identity of the unknown gas?
A. Cl2
B. F2
C. I2
D.Br2

C. I2

At certain temperature the saturation humidity of air-water vapor system is found to be 0.065 kg of water kg of dry air at 101.3 kPa. What is the vapor pressure of water at this temperature?
A. 3.9 kPa
B. 9.6 kPa
C. 6.2 kPa
D. 13.1 kPa

B. 9.6 kPa

At 20°C (approximately room temperature) the average velocity of F2 molecules in air is 902 ml/hr. what is the total kinetic energy of 1 mol of F2 molecules moving at this speed?
A. 5.1 E-21 J
B. 1.54 E 4 J
C. 3.09 E 3 J
D. 1.85 E 5 J

C. 3.09 E 3 J

The molecules of a gas at 10°C would have twice as much average kinetic energy at
A. 20°C
B. 293°C
C. 556°C
D. 859°C

B. 293°C

What volume of 0.125 M H2SO4 is required to completely precipitate all of the barium in 10.00 mL of a 0.150 M barium nitrate solution?
A. 12.0 mL
B. 24.0 mL
C. 6.00 mL
D. 0.206 mL

A. 12.0 mL

What is the mass of the precipitate formed when 12.0 mL of 0.150 M NaCl is added to 25.0 mL of a 0.500 M AgNO3 solution?
A. 258 g
B. 0.258 g
C. 179 g
D. 0.179 g

A sample of vitamin A, C20H30O, contains 4.0E22 atoms of carbon. How many atoms of hydrogen and how many molecules of vitamin A does it contain?
A. 6.0E22 atoms of H, 4.0E22 molecules of vitamin A
B. 4.0E22 atoms of H, 4.0E22 molecules of vitamin A
C. 6E22 atoms of H, 2,0E21 molecules of vitamin A
D. 6.0E22 atoms of H, 8.0E23 molecules of vitamin A

C. 6E22 atoms of H, 2,0E21 molecules of vitamin A

Octane burns according to the following equation: 2C8H8 + 25O2 → 16CO2 + 18H2O. How many grams of CO2 are produced when 5.0 grams of C8H18 are burned?
A. 40.0 g
B. 0.351 g
C. 15.4 g
D. 30.9 g

C. 15.4 g

CO2 exhaled by astronauts is removed from the spaceship atmosphere by reaction with KOH: CO2 + 2KOH → K2CO3 + H2O. How many kg of CO2 can be removed with 1.00kg of KOH?
A. 0.0500 kg
B. 0.786 kg
C. 0.392 kg
D. 1.57 kg

C. 0.392 kg

A byproduct of the reaction that inflates automotive airbags is very reactive sodium, which can ignite in air. Sodium produced during inflation process reacts with another compound added to the airbag contents, KNO3, via the reaction 10Na + 2KNO3 → K3O + 5Na2O + N2. How many grams of KNO3 are required to remove 5.00 g of C8H18 are required to remove 5.00 g of Na?
A. 110 g
B. 2.20 g
C. 4.40 g
D. 1.00 g

C. 4.40 g

For the reaction 3NO2 + H2O → 2HNO3 + NO, how many grams of HNO3 can be form when 1.00 g of NO2 and 2.25 g of H2O are allowed to react?
A. 0.913 g
B. 0.667 g
C. 15.7 g
D. 1.37 g

A. 0.913 g

Consider the equation shown below. If 3 g of oxygen produces 3.4 g of water, how many grams of water would be produced by 6 g of oxygen? 2H2 + O2 → 2H2O.
A. 3.4 g
B. 6.8 g
C. 6.4 g
D. 5.3 g

B. 6.8 g

Calcium hypochlorite, Ca(OCI)2, is used as a bleaching agent. It is produced from sodium hydroxide, calcium hydroxide, and chlorine gas in a solution-phase reaction according to the overall equation
2NaOH + Ca(OH)2 + 2Cl2 → Ca(OCl)2 + 2NaCl + 2 H2O
How many grams od calcium hypochlorite will be produced from 1067 g of Ca(OH)2?
A. 2042 g
B. 1152 g
C. 2059 g
D. 2120 g

C. 2059 g

Sulfuric acid H2SO4, cam be formed from the chemical reaction 2SO + O2 + 2H2O → 2H2SO4. Suppose 400 g of SO2; 175 g O2, and 125 g H2O are mixed and the reaction proceeds until one of the reactants is used up. How many grams of H2SO4 is produced?
A. 612 g
B. 620 g
C. 622 g
D. 630 g

A. 612 g

How much calcium chloride can be made from a starting mixture containing 10 g Ca and 4 g of Cl?
A. 26 g
B. 20.3 g
C. 12.1 g
D. 6.3g

D. 6.3g

The weight of sulfuric acid and of sodium chloride that would be required to prepare 1 liter of hydrochloric acid, density 1.201 g/ml and 40.09% by weight HCl, is __.
A. 595.3 g
B. 646.8 g
C. 6732 g
D. 692.4 g

Some sulfuric acid spilled on a lab bench. It can be neutralized by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid in the following way:
2NaHCO3(s) + H2SO4(aq) → Na2SO4(aq) + 2CO2 + 2H2O(l)
Sodium bicarbonate is added until the fizzing due to the formation of CO2(g) stops. If 35ml of 6.0M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid?
A. 0.42 g
B. 8.8 g
C. 18 g
D. 30.9 g

D. 30.9 g

Energy flows spontaneously from areas of higher temperature to
A. areas of equilibrium
B. areas of lower pressure
C. amounts of lower mass
D. areas of lower temperature

D. areas of lower temperature

Iodine, when heated passes from the solid phase directly to the gaseous phase. This is an example of
A. Charle’s Law
B. sublimation
C. vapor pressure
D. heat of fusion

B. sublimation

The study of chemistry does not include which one of the following?
A. the composition of particle
B. the mechanics of particle motion
C. the structure of particles
D. the properties of particles

B. the mechanics of particle motion

Elements
A. Can be decomposed by chemical means
B. cannot be decomposed by chemical mean
C. contain two or more atoms cemically combined
D. the properties of particles

B. cannot be decomposed by chemical mean

Which of the following is NOT true of solids?
A. true solids have a crystalline structure
B. they take the shape of the container
C. they have a boiling point
D. they have a definite volume

B. they take the shape of the container

Which of the following is NOT true of liquids
A. they gave no definite shape or volume
B. they have a definite shape
C. they have a boiling point
D. their heat of vaporization can be measured

B. they have a definite shape

The composition of a mixture
A. may vary
B. remains constant
C. has a definite ratio throughout
D. is easily calculated

A. may vary

The intrinsic energy in the particles of any pure substance is highest in the
A. solid phase
B. liquid phase
C. gaseous phase
D. gel phase

C. gaseous phase

Which of the following is not a pure substance?
A. water
B. hydrogen
C. milk
D. oxygen

C. milk

A(n)_____ is always composed of the same elements combined in a definite proportion by mass
A. isotope
B. compound
C. ion
D. allotrope

B. compound

Which of the following is true of our understanding of the nature of the atom?
A. It has undergone little, but significant change and is now complete
B. it has undergone change and will likely continue to do so
C. it is just as the ancients originally described it
D. it has undergone such major changes it is retuning to the ancient model

B. it has undergone change and will likely continue to do so

An example of a chemical change is
A. freezing water
B. breaking a glass
C. sublimation of carbon dioxide
D. digestion of food

D. digestion of food

Acetic acid is classified as weak acid because it
A. does not ionize in water
B. does not neutralize bases
C. slightly ionize in water
D. react rapidly with zinc to produce hydrogen

C. slightly ionize in water

According to bronsted lowry theory, an acid is any substance that
A. donates a proton
B. does not neutralize bases
C. donates an electron
D. react rapidly with zinc to produce hydrogen

A. donates a proton

The hydronium ion is a complex ion composed of
A. an electron
B. a neutron
C. a proton
D. a positron

C. a proton

The exact amount of solute dissolve in a given amount of solvent is
A. concentration
B. unsaturated
C. dilution of solution
D. solubility of solute

D. solubility of solute

The chaotic zigzag motion of particle in solution is describe by
A. electrical charge effect
B. tyndall effect
C. brownian movement
D.osmosis

C. brownian movement

The temperature at which the vapor pressure is equal to the prevailing atmospheric pressure is
A. boiling point
B. melting point
C. freezing point
D. critical point

A. boiling point

Cathode rays are composed of
A. positrons
B. protons
C. electrons
D. neutrons

C. electrons

The kind of bond formed between atoms of the same electronegativity will be
A. covalent
B. polar covalent
C. non-polar covalent
D. ionic

C. non-polar covalent

One of the terms does not belong to the set, it is
A. lustrons
B. malieable
C. brittle
D. ductile

C. brittle

One of the following elements do not belong to the group. It is
A. magnesium
B. cesium
C. calcium
D. beryllium

B. cesium

A substance that is being dissolved in a solution is called the
A. electrolyte
B. solvent
C. solute
D. colloid

C. solute

For a chemical equilibrium, a decrease in temperature will
A. Favor the reaction that is exothermic
B. Increase the equilibrium constant of the system
C. have no effect on the system
D. favor the reaction that is endothermic

A. Favor the reaction that is exothermic

For the reaction 2NO(g) + O2(g) ⟷ 2NO2(g), ∆H = −14 kcal, which of the following will cause the formation of more product?
A. Decreased pressure
B. Addition of oxygen
C. increased temperature
D. addition of catalyst

B. Addition of oxygen

For the reaction H2(g) + O2(g) → HI(g) equilibrium constant at 500°C is 62.5 if 5 moles of H2 and 5.0 moles of I2 are placed in 10 liter container at 500°C and allowed to come to equilibrium. Calculate the final concentration of H2.
A. 0.10 mcl/L
B. 0.10 L/mol
C. 0.20 mol/L
D. 0.20l/mol

A. 0.10 mcl/L

For the reaction H2(g) + O2(g) → HI(g) equilibrium constant at 500°C is 62.5. if 5 moles of H2 and 5.0 moles of I2 are placed in a 10 liter container at 500°C and allowed to come to equilibrium. Calculate the final concentration of HI.
A. 0.15 mol/L
B. 0.15 L/mol
C. 0.10 mol/L
D. 0.10L/mol

C. 0.10 mol/L

B. 0.80 mol/L

For the 2NO2 → N2O4(g). At a certain temperature one mole of NO2 is placed in a 10 liter container. After equilibrium is established, there are 0.20 mole of N2O4 present. Calculate the equilibrium constant at this temperature.
A. 55.6 mol/L
B. 5.56 mol/L
C. 5.56 L/mol
D. 55.6 L/mol

C. 5.56 L/mol

Given the formation of HI as an endothermic reaction, to favor the formation of more HI:
A. Increase pressure
B. Increase temperature
C. decrease pressure and temperature
D. add more H

B. Increase temperature

Consider the following reactions at equilibrium: 3H2(g) + N2(g) ⟷ 2NH3(g) + 92 kJ. Which single change in conditions will cause a shift in equilibrium toward an increase in production of NH3?
A. Addition of an inert gas
B. Increase in volume of the system C. removal of hydrogen gas
D. increase in pressure on the system

D. increase in pressure on the system

At equilibrium a 1-liter reactor contains 0.3 mol of A, 0.1 mol of B and 0.6 mol of C, according to the equation: A + B → C. If 0.2 mol of C was added, how many moles of C was left at equilibrium?
A. 0.80
B. 0.45
C. 0.94
D. 0.76

D. 0.76

At equilibrium a 1-liter reactor contains 0.3 mol of A, 0.1 mol of B, and 0.6 mol of C, according to the equation: A + B → C. if 0.4 mol of A was added, how many moles of A was left after equilibrium was reestablished?
A. 0.65
B. 0.05
C. 0.35
D. 0.70

A. 0.65

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature. An analysis of the mixture at equilibrium contained 2.0 mol N2, 3.0 mol H2 and 1.5 mol NH3. How many moles of H2 were present at the beginning of the reaction?
A. 3.0
B. 4.0
C. 4.5
D. 5.3

D. 5.3

At 500 K the equilibrium constant for the reaction 2 NO(g) + CI2(g) = 2 NOCI(g) is Kp= 52.0. An equilibrium mixture of the three gases has partial pressures of 0.095 atm and 0.171 atm for NO and CI2, respectively. What is the partial pressure of NOCI in the mixture
A. 3.53 atm
B. 8.02 E-2atm
C. 0.283 atm
D. 0.845 atm

C. 0.283 atm

At 300°C and 1 atm CO2 is 40% dissociated to CO and O2 according to the equation 2CO2 → 2CO + O2. Its percent dissociation when pressure is increased to 2 atm is
A. 0.350
B. 0.335
C. 0.425
D. 0.375

B. 0.335

Calculate the boiling point of a solution of formed by dissolving 20 g of a nonvolatile non-electrolyte solute (MW=40) in1 kg water.
A. 100.52°C
B. 100.26°C
C. 101.04°C
D. 101.12°C

B. 100.26°C

A mixture of 0.660 grams of camphor and 0.050 gram of an organic solute freezes at 157°C. If the solute contains 10.5% H by w eight, determine the molecular formula of the solute if the freezing point of camphor is 178.4°C and the value of Kf is 38.
A. C10H14
B. C2H6
C. C6H6
D. C8H16

A. C10H14

Glycarin, C3H8O3, is a nonvolatile nonelectrolyte with a density of 1.26 g/mL. at 25°C. Calculate the vapor pressure at 25°C of a solution made by adding 50 mL of glycerin to 500mL of water. The vapor pressure of pure water at 25°C is 23.8 torr.
A. 21.5 torr
B. 23.2 torr
C. 24.0 torr
D. 24.6 torr

B. 23.2 torr

At 25°C the vapor pressure of pure benzene is 0.1252 atm. If we dissolve 6.40 g of an unknown hydrocarbon in 78 g of pure benzene, we observe that the vapor pressure of the benzene in the solution is 0.1192 atm. What is the molar weight of the unknown solid?
A. 120
B. 125
C. 128
D. 132

C. 128

Components A and B form ideal solution. At 350 K, a liquid mixture containing 40% (by mole) A is in equilibrium with a vapor containing 70% (by mole) A. if the vapor pressure of A at 350K is 70 kPa, what is the vapor pressure of B?
A. 25 kPa
B. 20kPa
C. 40 kPa
D. 12 kPa

B. 20kPa

The vapor pressure of pure ethyl alcohol at 30°C is 71.2 torr and that of pure carbon tetrachloride is 121.6 torr. Calculate the pressure above a solution containing 20 g of ethyl alcohol and 60 g of carbon tetrachloride assuming ideal behavior
A. 100 torr
B. 97.8 torr
C. 75.2 torr
D. 95.0 torr

D. 95.0 torr

We dissolve 2.00 g of protein in 1 L water, the osmotic pressure is measured to be 0.021 atm at 25°C what is the approximate molar weight of the protein
A. 20000 g/mol
B. 21000 g/mol
C. 22000 g/mol
D. 23000 g/mol

D. 23000 g/mol

Calculate the osmotic pressure of an aqueous solution of 1 gram of sucrose per 100 mL of solution at 0°C
A. 1.2 atm
B. 0.90 atm
C. 0.655 atm
D. 1.05 atm

The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine its molar mass. The solution contained 3.50 mg of protein dissolved in sufficient water to form 5 mL solution. The osmotic pressure of the solution at 25°C was found to be 1.54 torr. Calculate the molar mass of protein.
A. 8450
B. 9000
C. 9500
D. 9820

A. 8450

At 20°C and one atmosphere, one liter of water will absorb 0.043 g of oxygen or 0.19 g of nitrogen. Atmospheric air is 20.9% oxygen by volume, and the remainder is assumed to be nitrogen. What mass of oxygen will be absorbed by one liter of water exposed to 20°C air at one atmosphere?
A. 0.009 g
B. 0.150 g
C. 0.23g
D. 0.043 g

A. 0.009 g

The reaction CO2 + H2 = CO + H2O was investigated by passing mixtures of CO2 and H2 over a catalyst at 900° at 1 atm pressure. The resulting gas was chilled quickly to room temperature by passage through a capillary and was analyzed, In one experiment the partial pressures were as follows: CO2=0.2142; H2=0.2549; CO=0.2654; H2O=0.2654 atm. Calculate the number of moles of hydrogen present in another equilibrium mixture containing 22.72 moles of CO, 22.72 moles of H2O, and 48.50 moles of CO2
A. 76.45 mole
B. 6.25 mole
C. 9.48 mole
D. 10.1 mole

B. 6.25 mole

From the following heats of reaction:
2C(graphite) + 2H2(g) + O2(g) → 2H3CO(g) ∆H = -217 kJ/mol
2C(graphite) + 2H2(g) + 2O2(g) → 3H2CO2(l) ∆H = -849 kJ/mol
Calculate the heat of the reaction: 2H2CO(g) + O2(g) → 2H2CO2(l)
A. -316 kJ/mol
B. 316 kJ/mol
C. -632 kJ/mol
D. 632 kJ/mol

C. -632 kJ/mol

The difference between heats reaction at constant pressure and constant volume for the reaction 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(l) at 298°K in kJ is
A. -7.43 kJ
B. 3.72 kJ
C. -3.72 kJ
D. 7.43 kJ

A. -7.43 kJ

A 2-L flask is filed with 0.2 mol of HI, it is allowed to reach equilibrium at high temperature. If at equilibrium the flask was found to contain 0.078 M HI, calculate Kp.
A. 4.2E-6
B. 4.2E-5
C. 1.2E-7
D. 0.141

What is the osmotic pressure at 20°C of a 0.0020 M sucrose solution?
A. 0.0486 atm
B. 0.488 atm
C. 4.88 atm
D. 48.8 atm

A. 0.0486 atm

A solvent-water mixture is to be distilled at 95°C. the vapor pressure of the solvent at this temperature is 130mmHg and that of water is 640mmHg. The solvent is immiscible in water and has a molecular weight of 150. The weight of the solvent in kilograms that will be carried over in the distillate with 200kg of water is
A. 358.73
B. 423.57
C. 338.54
D. 524

C. 338.54

4.2 g of a non-ionizing solute was dissolved in 112 g of acetone (Kb=1.71°C/m, Tb=55.95°C). the boiling point of the solution increased to 56.7°C. what is the approximate molecular weight of the solute?
A. 85.8 g/mol
B. 92.7 g/mol
C. 98.1 g/mol
D. 102.7 g/mol

A.85.8 g/mol

A certain amount of solute is added to water to form one molal solution. What is the freezing point of the solution?
A. -1.86°C
B. 1.66°C
C. 0.86°C
D. -0.86°C

A. -1.86°C

Calculate the boiling point at 760mmHg of a solution containing 5.00 grams urea in 75.00grams of water. The molecular weight of urea is 60.06.
A. 95.8°C
B. 100.05°C
C. 100.6°C
D. 101.6°C

C. 100.6°C

The concentration of carbon dioxide in water at 20°C is 1.o E-5 M. The henry’s constant for carbon dioxide dissolution in water is 3.91 E-@ M/stm. What is the partial pressure of CO2 in the air?
A. 2.56 E -5 atm
B. 2.56 E-4 atm
C. 3.75 E-5 atm
D. 3.75 E- 5 atm

The average osmotic pressure of blood is 7.7 atm at 25°C. What concentration of glucose will be isotonic with the blood?
A. 0.25 M
B. 0.31 M
C. 0.36 M
D. 0.42 M

B. 0.31 M

The mass ratio of nitrogen to oxygen in air is
A. 3.77
B. 3.12
C. 4.12
D. 3.29

D. 3.29

The vapor pressure of bromobenzene, C6H8Br, above an ideal-dilute aqueous solution of molality 0.092 mol kg-1 is 23.6 kPa. Calculate the henry’s law constant of bromobenzene.
A. 256 kPa-kg/mol
B. 2.17 kPa-kg/mol
C. 120 kPa-kg/mol
D.1.5 kPa-kg/mol

A. 256 kPa-kg/mol

What is the osmotic pressure in atm produce by a 1.20 M glucose solution at 25°C?
A. 36.0
B. 4.89
C. 27.2
D. 29.3

D. 29.3

The osmotic pressure of a solution containing 0.10 gmol/1000 g water at 25°C is
A. 2.44 atm
B. 4.86 atm
C. 1.22 atm
D. 1.65 atm

A. 2.44 atm

An idea solution is formed from a mixture of the nonvolatile solute urea, CO(NH2)2, and methanol. The vapor pressure of pure methanol at 20°C is 59 mmHg. Calculate the mole fraction of urea that is obtained from mixing 6 g of urea with 32 g of methanol.
A. 0.091
B. 0.10
C. 0.16
D. 0.84

A. 0.091

A 4.266 grams compound is dissolved in 100 grams toluene. What is the molecular weight of the compound if the vapor pressure of the solution 28.209 mmHg. The vapor pressure of toluene at the working temperature is 26.829 mmHg. Assume that the compound is a nonvolatile, non- dissociating solute.
A. 42.5
B. 46.1
C. 56.9
D. 178

D. 178

Calculate the vapor pressure of a solution containing 800 g of table sugar in 100 g water at 25°C vapor pressure of water is 23.6 torr at 25°C.
A. 20.5 torr
B. 21.6 torr
C. 22.1 torr
D. 22.9 torr

D. 22.9 torr

The boiling point of the immiscible liquid system naphthalene – water is 98°C under a pressure of 733 mmHg. The vapor pressure of water at 96°C is 707 mmHg. Calculate the weight % of naphthalene in the distillate.
A. 20.7%
B. 19.5%
C. 18.6%
D. 18.2

A. 20.7%

The vapor pressure of a solution containing 13 grams of a nonvolatile solute in 100 grams of water at 25°C is 27.371 mmHg. Calculate the molecular weight of the solute, assuming that the solution is ideal. The vapor pressure of water at this temperature is 28.065 mmHg.
A. 90.4
B. 92.3
C. 94.1
D. 94.9

B. 92.3

A solution of 1.25 g of a non-electrolyte solute in 20 g of water freezes at 271.94°K. find the molecular weight of the solute.
A. 207.8
B. 179.79
C. 209.6
D. 109.6

D. 109.6

What weight of glycerol would have to be added to 1000 g of water in order to lower its freezing point to -10°C?
A. 579 g
B. 495 g
C. 954 g
D. 594 g

B. 495 g

Calculate the freezing point of a solution containing 4.27 g of sucrose in 50 g water.
A. -0.46°C
B. -0.65°C
C. -0.76°C
D. -0.82°C

A. -0.46°C

Calculate the boiling point of a solution containing 4.27 g of sucrose in 50 g water.
A. 101.71°C
B. 101.12°C
C. 100.87°C
D. 100.13°C

D. 100.13°C

The following data refer to question 1 through 4. Trimellitic acid containing carbon, hydrogen and oxygen has 51.44% C, 2.88% H, and 45.68% O. It can be obtained by oxidation of coal with nitric acid. A 2.416-g sample of this compound was dissolved in 40.0 g of acetone, producing a solution that boils at 56.64°C, Kb for acetone is 1.71°C/molal. Pure acetone has a boiling point of 56.20°C. From the percentage composition, determine the empirical formula, what is the empirical weight of the C, H and O compound in grams per empirical unit?
A. 29
B. 41
C. 70
D. 82

C. 70

The following data refer to question 1 through 4. Trimellitic acid containing carbon, hydrogen and oxygen has 51.44% C, 2.88% H, and 45.68% O. It can be obtained by oxidation of coal with nitric acid. A 2.416-g sample of this compound was dissolved in 40.0 g of acetone, producing a solution that boils at 56.64°C, Kb for acetone is 1.71°C/molal. Pure acetone has a boiling point of 56.20°C. What is the molality of the acetone solution using the change in boiling point?
A. 0.06
B. 0.26
C. 0.42
D. 0.8

B. 0.26

The following data refer to question 1 through 4. Trimellitic acid containing carbon, hydrogen and oxygen has 51.44% C, 2.88% H, and 45.68% O. It can be obtained by oxidation of coal with nitric acid. A 2.416-g sample of this compound was dissolved in 40.0 g of acetone, producing a solution that boils at 56.64°C, Kb for acetone is 1.71°C/molal. Pure acetone has a boiling point of 56.20°C. What is the experimental molecular weight for trimellitic acid?
A. 41
B. 140
C. 200
D. 230

D. 230

The following data refer to question 1 through 4. Trimellitic acid containing carbon, hydrogen and oxygen has 51.44% C, 2.88% H, and 45.68% O. It can be obtained by oxidation of coal with nitric acid. A 2.416-g sample of this compound was dissolved in 40.0 g of acetone, producing a solution that boils at 56.64°C, Kb for acetone is 1.71°C/molal. Pure acetone has a boiling point of 56.20°C. What is the molecular formula for the compound?
A. C2HO
B. C3H2O2
C. C6H4O4
D. C9H6O6

D. C9H6O6

For the reaction: 2A + B ↔ 2C + D, the equilibrium concentrations of A, B, C, and D in mol/L are 2, 1.2, 3.0 and 0.6 respectively. What is the numerical value of Keq?
A. 0.889
B. 1.33
C. 1.12
D. 4.32

C. 1.12

If 1 mole of PCI3 and 1 mole of CI2 are placed in a 5-L container, the following equilibrium is reached PCI3 (g) + CI2 (g) = PCI5 (g) Kc=10 at the temperature maintained. What is the equilibrium molar concentration of PCI3?
A. 0.13
B. 0.11
C. 0.14
D. 0.10

D. 0.10

Consider the reaction: H2(g) + I2(g) → 2HI(g) Keq=25. Determine the number of moles of H2 remaining when 1 mole of both H2 and I2 are equilibrated in a liter box.
A. 1/6 mole
B. 2/7 mole
C. 5/7 mole
D. 5/6 mole

B. 2/7 mole

Given the reaction A + B → 2C; K=50. Determine the final concentration of C when 1 mole of both A and B are added to a 1 liter container containing 0.1 mole of C
A. 0.76 mole
B. 0.88 mole
C. 1.66 mole
D. 1.85 mole

A. 0.76 mole

Given the following reaction:
N2(g) + 3H2(g) = 2NH3(g) ∆H = -30 kJ/mole
How will equilibrium of the following reaction be affected if the temperature is increased?
A. It will be shifted to the right
B. it will be unaffected
C. It will be shifted to the left
D. the equilibrium be shared

A. It will be shifted to the right

For the reaction 2A(g) + B(g) ↔ 3C(g) + D(g). The concentration at equilibrium are 0.30 M of A, 0.60 m of B, 0.20 M of C and 0.50 M of D. Find the equilibrium constant.
A. 0.074
B. 0.047
C. 0.74
D. 0.47

A. 0.074

Methyl alcohol can be prepared commercially by the reaction of hydrogen with carbon monoxide CO + 2H2 CH3OH under equilibrium conditions at 700 K, [H2 ]=0.072M, [CO]=0.020M, and [CH3OH]=0.030M. what is the value of the equilibrium constant?
A. 100
B. 290
C. 180
D. 50

B. 290

The equilibrium constant Kp for the reaction CO + H2O = CO2 + H2 is 10.0 at 690°K. the heat of the reaction ∆H° is = 10,200 cal. Calculate the partial pressure of CO in equilibrium mixture prepared by mixing 0.400 mole of CO and 0.200 mole of H2O in a volume of 5 liters at 500°K.
A. 0.01 atm
B. 1.43 atm
C. 1.65 atm
D. 1.79 atm

C. 1.65 atm

A 1 liter vessel established equilibrium with the following reaction, 2 SO2 + O2 = 2 SO3, has 0.11 mole SO2, 0.05 mole O2 and 0.12 mole SO3. Another 1 liter vessel is used and contains initially 96 g of SO2 how much O2 (in grams) must be added, if at equilibrium, one-half of SO2 will be converted to SO3.
A. 6.04
B. 9.34
C. 13.34
D. 9.60

C. 13.34

Ammonia is formed from a mixture of 3 moles of hydrogen and 1 mole of nitrogen at lower temperatures the yield is higher, but the time required for equilibrium to be reached be too great to be practical except for the addition of catalyst. The pressure is kept as high and the temperature low as practical. Under equilibrium conditions at 400° and 10 atm pressure, 3.85 mole percent of ammonia is obtained. Calculate Kp for the reaction N2 + H2 = 2NH3. The ration of 3 volumes of hydrogen to 1 volume of nitrogen is maintained, regardless of the amount of ammonia formed. Of the 96.15 percent by volume which is not ammonia one-fourth is nitrogen and three- fourths is hydrogen.
A. 0.00139
B. 0.000145
C. 0.000157
D. 0.000164

D. 0.000164

The value of Kc for the reaction C(s) + CO2(g) → 2CO(g) is 1.6. What is the equilibrium concentration of CO if the equilibrium concentration of CO2 is 0.50 M?
A. 0.75M
B. 0.31 M
C. 0.80 M
D. 0.89 M

D. 0.89 M

As the temperature of the reaction is increased, the rate of the reaction increases because the
A. reactant molecules collide less frequently
B. reactant molecules collide less frequently and with greater energy
C. activation energy is lowered
D. reactant molecule collide with greater energy

D. reactant molecule collide with greater energy

In a series of reactions, what is the rate determining step?
A. The main reaction involving the major reactant
B. The slowest reaction
C. The Fastest reaction
D. The reaction with the highest order

B. The slowest reaction

Which three factors affect the rate of a chemical reaction?
A. Temperature, pressure and humidity
B. Temperature, reactant concentration and container volume
C. Temperature, reactant concentration and pressure
D. Temperature, reactant concentration, and catalyst

D. Temperature, reactant concentration, and catalyst

A liquid property which permits an insect such as the water strider to “walk” on water.
A. Surface tension
B. Diffusivity
C. viscosity
D. density

A. Surface tension

The rise of liquids up very narrow tubes is called
A. Surface tension
B. capillarity action
C. viscosity
D. buoyant force

B. capillarity action

Sometimes as we remove heat from a liquid we can temporarily cool it below freezing point without forming a solid. This phenomenon is called
A. Fusion
B. supercooling
C. vaporization
D. sublimation

B. supercooling

In substances that sublime, the intermolecular forces of attraction are
A. Weak the vapor pressure is low
B. Strong and the vapor pressure is low
C. weak and the vapor pressure is high
D. strong and the vapor pressure is high

C. weak and the vapor pressure is high

An element in the lower left corner of the periodic table
A. Is either a metalloid or a nonmetal
B. Is either a metal or metalloid
C. is definitely a metal
D. is definitely a metalloid

C. is definitely a metal

Water, no matter where it is found, consist of hydrogen and oxygen combined in a 1:8 ratio by mass. This is the statement of
A. The law of constant composition
B. The law of conservation of energy
C. the law of multiple proportions
D. the law of conservation of mass

A. The law of constant composition

Which dissolve fastest in coffee?
A. Lump sugar in hot coffee
B. Granular sugar in cold coffee
C. Granular sugar in hot coffee
D. Lump sugar in cold coffee

B. Granular sugar in cold coffee

Who discovered positron?
A. Anderson
B. Pauli
C. Heisenberg
D. Borg

A. Anderson

Which of the following is a qualitative way of expressing concentration?
A. Molarity
B. saturated
C. normality
D. formality

B. saturated

The number of moles of solute per kilogram solvent is
A. Molality
B. molarity
C. normality
D. formality

A. Molality

Properties which depend on the amount of the various substances that make up the solution.
A. Colligative
B. extensive
C. Intensive
D. physical

A. Colligative

A reaction in which the products that are formed react to form the original reactants.
A. Reversible
B. Irreversible
C. redox
D. chemical

A. Reversible

It states that if a stress is applied to a system at equilibrium, the system will shift, if possible in such a way as to reduce the stress.
A. Law of bass action
B. Le Chateller’s principle
C. Rate law
D. Pauli exclusion principle

B. Le Chateller’s principle

In the compound KMnO4, what is the oxidation number of Mn?
A. +6
B. +7
C. +4
D. +3

B. +7

In the reaction Na + Cl2 → NaCl, what is the oxidizing agent?
A. NaCl
B. Cl
C. Na
D. Cl2

D. Cl2

All isotopes of a given element have?
A. All isotopes of a given element have
B. The same number of protons
C. The same number of atomic mass units
D. The same number of neutrons

B. The same number of protons

Group I elements, is also known as
A. Alkaline earth metals
B. halogens
C. alkali metals
D. chalcogen

C. alkali metals

One atomic mass unit is equivalent to _______ of the mass of a mole of carbon
A. 1/2
B. 1/18
C. 1/12
D. 1/8

C. 1/12

The number that expresses the oxidation state of an atom of an element or groups of atoms is called the
A. Indicator
B. valence
C. Displacement factor
D. electrolyte

B. valence

An uneven sharing of electrons between two atoms indicate
A. Bonding
B. coupling
C. electronegativity
D. polarity

D. polarity

Alka-seltzer is an example of
A. Bonding
B. coupling
C. electronegativity
D. polarity

A. Bonding

Brix scale is used for
A. sugar solutions
B. LPG
C. petroleum
D. water

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