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Day 1 > General Inorganic Chemistry and Analytical Chemistry > Flashcards

General Inorganic Chemistry and Analytical Chemistry Flashcards

1
Q

Which of the following is a homogenous mixture?
I. water
II. water and alcohol
III. air

A. I, II and III
B. II and III only
C. I and II only
D. I and III only

A

B. II and III only

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2
Q

NH3 is
A. trigonal planar
B. tetrahedral
C. trigonal pyramid
D. linear

A

C. trigonal pyramid

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3
Q

PH3 is
A. trigonal planar
B. tetrahedral
C. trigonal pyramid
D. linear

A

C. trigonal pyramid

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4
Q

Water is a _____ molecule
A. diatomic
B. triatomic
C. monoatomic
D. tetraatomic

A

B. triatomic

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5
Q

Transition elements are found in the
A. d and f block
B. p block
C. s block
D. d block

A

A. d and f block

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6
Q

An atomic bond resulting from the formation of a molecular orbital by the head-on collision of atomic orbitals.
A. sigma bond
B. ionic bond
C. pi bond
D. covalent bond

A

A. sigma bond

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7
Q

Which does not belong to the group?
A. Cu
B. B
C. Si
D. As

A

A. Cu

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8
Q

The most abundant element in the solar system is
A. hydrogen
B. nitrogen
C. oxygen
D. helium

A

A. hydrogen

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9
Q

P1V1/T1=P2V2/T2 is
A. Charles law
B. Ideal gas law
C. Combined Boyle’s & Charles law
D. Amagat’s law

A

C. Combined Boyle’s & Charles law

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10
Q

H+ is a an _____.
A. proton
B. electron
C. element
D. neutron

A

A. proton

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11
Q

In which of the following is the size of particles increasing?
A. colloids, solution, suspension
B. colloids, suspension, solution
C. solution, suspension, colloids
D. suspension, solution, colloids

A

A. colloids, solution, suspension

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12
Q

Which of the following is the most polar bond?
A. N - O
B. C - C
C. C -H
D. H - F

A

D. H - F

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13
Q

The pair of electrons which do not participate in the bonding is called
A. ione pair of non-bonding electrons
B. ionic bond
C. covalent bond
D. bonding electrons

A

A. ione pair of non-bonding electrons

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14
Q

A chemical reaction which requires heat to produce products.
A. reversible reaction
B. irreversible reaction
C. exothermic reaction
D. endothermic reaction

A

D. endothermic reaction

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15
Q

It is define as the tendency of an atom to attract electrons.
A. ionization energy
B. electronegativity
C. exothermic reaction
D. activation energy

A

B. electronegativity

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16
Q

Dispersion of solid or liquid particles of microscopic size in a gas media such as smoke is
A. a soot
B. a vapor
C. a mist
D. an aerosol

A

D. an aerosol

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17
Q

It is a proton donor.
A. Arrhenius acid
B. Lewis acid
C. Bronsted acid
D. Acetic acid

A

C. Bronsted acid

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18
Q

Which of the following has the greatest affinity to electrons?
A.Na
B. Br
C. Cl
D. K

A

C. Cl

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19
Q

Elements in a given period have the same
A. atomic weight
B. maximum principal quantum number
C. maximum azimuthal quantum number
D. valence electron structure

A

B. maximum principal quantum number

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20
Q

Electron affinity is defined as
A. the change in energy when a gaseous atom in its ground state gains an electron
B. the pull an atom has on the electrons in chemical bond
C. the energy required to remove a valence electron from a neutral gaseous atom in its ground state
D. the energy difference between an electron in its ground and exited states

A

A. the change in energy when a gaseous atom in its ground state gains an electron

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21
Q

A triple bond consist of
A. 3 sigma bonds
B. 1 pi & 2 sigma bonds
C. 1 sigma & 2 pi bonds
D. 3 pi bonds

A

C. 1 sigma & 2 pi bonds

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22
Q

Colligative properties depend on
A. number of solute particles
B. temperature of solution
C. nature of solute
D. nature of solvent

A

A. number of solute particles

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23
Q

It is the Greek word for “salt forming”
A. actinides
B. lanthanides
C. halogen
D. transition

A

C. halogen

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24
Q

Who discovered radium?
A. Marie Curie
B. John Priestly
C. Ernest Rutherford
D. John Dalton

A

A. Marie Curie

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25
Q

Aqua regia is a mixture of
A. hydrochloric & perchloric acid
B. hydrochloric, nitric & perchloric acid
C. nitric & perchloric acid
D. nitric & hydrochloric acid

A

D. nitric & hydrochloric acid

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26
Q

Mayonnaise and milk are examples of
A. emusion
B. suspension
C. colloid
D. mixture

A

A. emusion

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27
Q

Colloidal dispersion has ______ phase while a suspension has ______ phases.
A. 1 and 2
B. 1 and 1
C. 2 and 1
D. 2 and 2

A

A. 1 and 2

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28
Q

Which of the following has no definite stricture?
A. crystalline
B. amorphous
C. amphoteric
D. allotroph

A

B. amorphous

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29
Q

Who discovered positron?
A. Rutherford
B. Chadwick
C. Goldstein
D. Anderson

A

D. Anderson

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30
Q

How many halogens are there in period three?
A. 6
B. 5
C. 4
D. 1

A

D. 1

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31
Q

It is a substance that yields hydronium ions in aqueous solution.
A. Arrhenius acid
B. Lewis acid
C. Bronsted acid
D. Lewis acid

A

C. Bronsted acid

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32
Q

What expressions of concentration are independent of temperature?
A. molality and mole fraction
B. molarity and normality
C. molarity and mole fraction
D. molarity and J molarity

A

A. molality and mole fraction

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33
Q

A yellowish gas.
A. chlorine
B. carbon dioxide
C. nitrogen
D. hydrogen

A

A. chlorine

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34
Q

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

A

C. beta particle

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35
Q

Group 1R elements are also known as
A. alkaline earth metals
B. Halogen
C. alkali metals
D. chalcogen

A

C. alkali metals

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36
Q

Which of the following statement is/are correct?
I. Liquid water is denser than ice.
II. Ice is denser than liquid water.
III. Ice and liquid water have equal densities.
IV. Ice has a more open structure than liquid water due to the allignment of hydrogen molecules.
V. The molecules of liquid water are farther apart than the molecules of ice

A. III and IV only
B. II and IV only
C. I, IV and V only
D. I and IV only

A

C. I, IV and V only

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37
Q

Atomic number is equal to the
A. mass number
B. number of protons
C. number of electrons
D. number of neutrons

A

B. number of protons

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38
Q

One atomic mass unit is equivalent to _____ of the atomic weight of carbon.
A. 12 times
B. 1/12
C. 1/3
D.1/4

A

B. 1/12

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39
Q

The energy needed to remove the most loosely bonded electron of an atom is the
A. ionization energy
B. electron affnity
C. electronegavity
D. kinetic energy

A

A. ionization energy

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40
Q

Who stated that the properties of elements are periodic functions of their atomic weights not atomic number?
A. Ernest Rutherford
B. Henry Moseley
C. Dmitri Mendeleev
D. Neils Bohr

A

C. Dmitri Mendeleev

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41
Q

Calcuim carbonate is also known as
A. chalk
B. feldspar
C. charcoal
D. silica

A

A. chalk

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42
Q

Which of the following has the least strength?
A. covalent bond
B. electrovalent bond
C. van der waals bond
D. ionic bond

A

C. van der waals bond

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43
Q

How many neutrons are there in platinum atom?
A. 78
B. 117
C. 195
D. 273

A

B. 117

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44
Q

Two major types of chemical bonds are observed in chemical bonding: ionic covalent. Which of the following has the bond that is least ionic in character?
A. NaCl
B. H2O
C. CH4
D. H2

A

D. H2

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45
Q

The most abundant element in the solar system is
A. hydrogen
B. Oxygen
C. nitrogen
D. argon

A

A. hydrogen

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46
Q

The number of electrons in an atom of an element is equal to
A. atomic weight
B. atomic number
C. equivalent weight
D. electron affinity

A

B. atomic number

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47
Q

According to Lewis definition, a base is that which
A. gives hydronium ions
B. accepts an electron pair
C. donates an electron
D. is protogenic

A

B. accepts an electron pair

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48
Q

The composition of the nucleus of deuterium is
A. one electron, one proton
B. one protons, one neutron
C. one neutron, one electron
D. two protons, one electron

A

B. one protons, one neutron

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49
Q

Which of the following is the most electronegative?
A. fluorine
B. bromine
C. chlorine
D. iodine

A

A. fluorine

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50
Q

What is the molecular weight of ammonium perchlorate?
A. 116.45 g/mol
B. 97.55 g/mol
C. 122.20 g/mol
D. 86.21 g/mol

A

A. 116.45 g/mol

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51
Q

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

A

D. polarity

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52
Q

All of the following are colligative properties, except
A. solubility
B. vapor pressure lowering
C. freezing point depression
D. boiling point elevation

A

A. solubility

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53
Q

The number that expresses the oxidation state of an atom of an element or group is called the
A. indicator
B. displacement factor
C. valence
D. electrolyte

A

C. valence

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54
Q

A solution used principally to control the pH value of a solution to a point where selective precipitation can be made.
A. acid solution
B. basic solution
C. neutral solution
D. buffer solution

A

D. buffer solution

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55
Q

Hydrogen is common to all
A. acids
B. oxides
C. salts
D. metals

A

A. acids

56
Q

Defines an acid as a compound that dissolves in water to produce hydronium ions.
A. Arrhenius
B. Bronsted-Lowry
C. Lewis
D. Rutherford

A

A. Arrhenius

57
Q

One gram mole of a spacie is weight of the spacie equivalent to its
A. molecular weight
B. atomic number
C. number of nuetrons
D. atomic mass

A

A. molecular weight

58
Q

Along a row in the periodic table of elements have the same
A. energy level
B. configuration
C. electronegativity
D. size

A

A. energy level

59
Q

The electrons of metals are free to move in solids. This explains why
A. metals are unstable
B. metals have high reflectivity
C. metals can be easily molded
D. metals have high conductivity

A

D. metals have high conductivity

60
Q

How many pi bonds are there in a double bond?
A. 0
B. 2
C. 1
D. 3

A

B. 2

61
Q

All isotopes of a given element have
A. equal number of protons and neutrons
B. the same number of atomic mass unit
C. the same number of protons
D. the same number of neurons

A

C. the same number of protons

62
Q

Used to express the ethanol concentration in beverages.
A. % ethanol
B. years
C. proof
D. kara

A

C. proof

63
Q

The universal blood type donor is
A. type A
B. type AB
C. type B
D. type O

A

D. type O

64
Q

Which will dissolve fastest in coffee?
A. lump sugar in hot coffee
B. granular sugar in hot coffee
C. granular sugar in cold coffee
D. lump sugar in cold coffee

A

B. granular sugar in hot coffee

65
Q

As water boils at 1atm, the temperature
A. increases
B. decreases
C. remains constant at 100°C until all is changed to vapor
D. varies

A

C. remains constant at 100°C until all is changed to vapor

66
Q

Saltwater at 1 atm boils at
A. slightly higher than 100°C
B. 100°C
C. less than 100°C
D. 98°C

A

A. slightly higher than 100°C

67
Q

The method of measuring the specific heat of liquids and solid is
A. entropy
B. enthalpy
C. thermometry
D. calorimetry

A

D. calorimetry

68
Q

Which has the greatest rest mass?
A. alpha particle
B. neuron
C. proton
D. electron

A

A. alpha particle

69
Q

Which noble gas is 1% by volume in air
A. argon
B. xenon
C. krypton
D. radon

A

A. argon

70
Q

Which of the following is also known as soda lye or caustic soda which is use in manufacture of soap?
A. sodium chloride
B. sodium hydroxide
C. sodium carbonate
D. ammonia

A

B. sodium hydroxide

71
Q

A complete fertilizer contains
A. N, P and K
B. N, P and C
C. Na, P and K
D. N, P and S

A

A. N, P and K

72
Q

Prussic acid has a formula
A. HNO3
B. HCN
C. C5H5OH
D. H2SO4

A

B. HCN

73
Q

An azeotropic mixture is
A. liquid mixture of two or more substances in which the vapor has the same composition as the liquid
B. a solution of two or more substances that cannot be made
C. a mixture of two or more substances where the boiling point cannot be determined
D. solution of two or more substances present in the same amounts in the liquid phase

A

C. a mixture of two or more substances where the boiling point cannot be determined

74
Q

Which of the following grades has the highest purity?
A. technical grade
B. reagent grade
C. primary standard
D. USP grade

A

C. primary standard

75
Q

The temperature at which a polymer changes from hard and brittle to rubbery and tough is called
A. boiling point
B. glass transition temperature
C. thermosetting temperature
D. melting point

A

C. thermosetting temperature

76
Q

Consider the following reaction
KMnO4 + KCI + H2SO4 → MnSO4 + H2O + Cl2
What is the reducing agent?
A. KMnO4
B. Mn
C. KCI
D. CaCl2

A

A. KMnO4

77
Q

In HAsO3 of the following is covalently bonded?
A. -5
B. -2
C. +6
D. +3

A

D. +3

78
Q

Which of the following is covalently bonded?
A. MgO
B. NaCl
C. KCI
D. CaCl2

A

A. MgO

79
Q

Discovered water by exploding hydrogen and oxygen.
A. Lewis
B. Cavendish
C. Lavoiser
D. Huey

A

B. Cavendish

80
Q

Buffer solution resists changes in acidity. If an acid is added to a buffer solution, the ______ remains the same
A. pH
B. molality
C. concentration
D. mole fraction

A

A. pH

81
Q

Jellies and paints are examples of
A. gen
B. emuision
C. sol
D. aerosol

A

A. gen

82
Q

Which of the following is a heavy ductile metal?
A. Mn
B. Ni
C. Mg
D. Al

A

B. Ni

83
Q

Optical pyrometer is used to
A. determine the voltage at the junction of dissimilar metal
B. measure temperature of solid objects at temperature above 700°C
C. determine the density of an ideal gas
D. measure turbidity of wastewater

A

D. measure turbidity of wastewater

84
Q

Teratogens can cause
A. cancer
B. nervous system breakdown
C. child birth defects
D. skin allergies

A

B. nervous system breakdown

85
Q

Which of the following has the least polar bonding?
A. carbon dioxide
B. oxygen
C. nitrogen dioxide
D. sulfur dioxide

A

B. oxygen

86
Q

The type of intermolecular bond present in water is
A. extended covalent
B. ionic bond
C. polar bond
D. hydrogen bond

A

D. hydrogen bond

87
Q

Which of the following is another allotropic form of graphite?
A. gold
B. silver
C. diamond
D. bronze

A

C. diamond

88
Q

All are isoelectronic, expect
A. Mg2+
B. Na+
C. F
D. Ne

A

C. F

89
Q

Which of the following does not belong to the group?
A. energy
B. force
C. work
D. heat

A

B. force

90
Q

The poorest source of hydrogen is
A. protein, fat and carbohydrate
B. atmosphere
C. fossil fuel
D. water

A

B. atmosphere

91
Q

When atoms collide, they do not lose energy. This is because
A. collision are elastic
B. collisions are adiabatic
C. collisions are elastic
D. Collisions are frictionless

A

C. collisions are elastic

92
Q

Which is not common property to both hydrogen, oxy gen and nitrogen?
A. their densities are lighter than air
B. weak intermolecular forces
C. tasteless, odorless and colorless gas
D. slightly soluble in water

A
93
Q

A hydrocarbon has an empirical formula of CH3. If the molecular weight of the hydrocarbon is 30 g/mol, what is the hydrocarbon?
A. C2H6
B. C2H2
C. C4H10
D. C6H12

A

A. C2H6

94
Q

The state at which the rate of forward reaction is equal to the rate of backward reaction.
A. eutectic acid
B. equilibrium state
C. reversible state
D. ideal state

A

B. equilibrium state

95
Q

It is a substance that yields hydronium ions in aqueous solution.
A. Arrhenius acid
B. Lewis acid
C. Bronsted acid
D. amphoteric

A

A. Arrhenius acid

96
Q

Two bodies are of temperature of 70°F and 200°F respectively. Calculate the difference in temperature in degrees Kelvin.
A. 72.22
B. 65.90
C. 60.25
D. 75.12

A

A. 72.22

97
Q

All these about redox are correct except
A. the total number of the electrons lost by the element reduces is equal to the total number of electrons gained by the element oxidized
B. the reducing agent oxidized
C. reduction is loss in positive valence
D. oxidation is loss of electrons

A

A. the total number of the electrons lost by the element reduces is equal to the total number of electrons

98
Q

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

A

D. green

99
Q

Defines a base as a compound that dissolves in water to produce hydroxide ions
A. another electrons goes from a low energy state to a high one

A

A. another electrons goes from a low energy state to a high one

100
Q

When an electron goes from a high energy state to a low one, what occur?
A. another electron goes from a low energy state to a high one
B. the atom moves faster
C. light is given off
D. this process is not possible

A

C. light is given off

101
Q

Calculate percent oxygen in Fe2(SO4)3.
A. 37%
B. 44%
C. 40%
D. 48%

A

D. 48%

102
Q

A 0.5 M solution of a solute (MW = 57 g/mol) has a density of 2.5 g/mol. Calculate the percent by mass of the solute.
A. 0.75%
B. 2.80%
C. 1.14%
D. 0.42%

A

C. 1.14%

103
Q

A 0.5 M solution of a solute (MW = 57 g/mol) has a density of 2.5 g/mol. Calculate the percent by mole of the solute.
A. 0.18%
B. 0.36%
C. 0.25%
D. o.42%

A

B. 0.36%

104
Q

A 0.5 M solution of a solute (MW = 57 g/mol) has a density of 2.5 g/mol. Calculate the molality of the solution.
A. 0.20
B. 0.30
C. 0.25
D. 0.40

A

A. 0.20

105
Q

A compound has a molecular formula of X4O10. If 1 g of X reacts with oxygen to yield 2.24 g of X4O10, find the element X.
A. S
B. Mg
C. Ca
D. P

A

A. S

106
Q

A 1.038 M sucrose solution has a density of 1.1 g/ml. Calculate the molarity of the solution.
A. 12.4 M
B. 9.7 M
C. 10.87 M
D. 9.0 M

A

A. 12.4 M

107
Q

A 1.038 M sucrose solution has a density of 1.1 g/ml. Calculate the percent by mass sucrose (C12 H22O11).
A. 30.82%
B. 32.27%
C. 31.15%
D. 34.50%

A

B. 32.27%

108
Q

A 1.038 M sucrose solution has a density of 1.1 g/ml. Calculate the percent by mole sucrose (C12 H22O11).
A. 2.45%
B. 2.72%
C. 2.60%
D. 2.84%

A

A. 2.45%

109
Q

A 1.038 M sucrose solution has a density of 1.1 g/ml. Calculate the molality of the solution.
A. 1.39 m
B. 2.15 m
C. 1.89 m
D. 2.30 m

A

A. 1.39 m

110
Q

How many electrons are removed from an atom that changes its oxidation number from -3 to +5?
A. 2
B. 6
C. 8
D. 4

A

C. 8

111
Q

Calculate the molarity of NaOH solution if 5 ml of NaOH is titrated with 25 ml of 0.26 M HCI.
A. 1.0 M
B. 1.5 M
C. 1.3 M
D. 1.7 M

A

C. 1.3 M

112
Q

The pH of an aqueous solution which has an analytical concentration of 1E-7 M of hydronium ion is
A. 6.0
B.6.79
C. 7.0
D. 6.69

A
113
Q

What reacts with AgNO3 to form a silver mirror?
A. aldehydes
B. Acids
C. ketones
D. esters

A

A. aldehydes

114
Q

18.7 g unknown acid is reacted with zinc to produce 800 cc of hydrogen gas at STP. What is the equivalent weight of the acid?
A. 624
B. 173
C. 262
D. 131

A
115
Q

What weight of AgNO3 is required to precipitate the chlorides in a 750 mg solution of 14% BaCl2?
A. 256 mg
B. 80 mg
C. 342 mg
D. 171 mg

A

D. 171 mg

116
Q

Calculate the pH of a solution prepared by mixing 10 ml of 0.1 N NaOH and 25 ml of 0.1 N HAc.
A. 2.46
B. 12.96
C. 4.57
D. 8.72

A

C. 4.57

117
Q

Calculate the pH of a solution prepared by mixing 25 ml of 0.1 N NaOH and 25 ml of 0.1 N HAc.
A. 2.46
B. 12.96
C. 4.57
D. 8.72

A

D. 8.72

118
Q

Calculate the pH of a solution prepared by mixing 30 ml of 0.1 N NaOH and 25 ml of 0.1 N HAc.
A. 2.46
B. 12.96
C. 4.57
D. 8.72

A

B. 12.96

119
Q

hat is the pH of natural water?
A. 5.6 - 6.2
B. 7.0 - 8.3
C. 4.2 - 4.4
D. 2.2 - 2.4

A

A. 5.6 - 6.2

120
Q

Asorbic acid (vitamin C ) contains 40.92 percent C, 4.58 percent H, and O by mass.
A. C3H4O3
B. C3H3O3
C. C3H5O3
D. C6H6O3

A

A. C3H4O3

121
Q

How many grams of water are produced in the combustion of 1 g of glucose, C6H12O6 :
C6H12O6(S) + 6O2 (g) → 6CO2 (g) + 6H2O (I)
A. 0.5
B. 0.6
C. 0.7
D. 0.8

A

B. 0.6

122
Q

One commercial method used to peel potatoes is to soak them in a solution of NaOH for a short time, remove them from the NaOH, and spray off the peel. The concertration of NaOH is normally in the rangeof 3 to 6M. The NaOH is analyzed periodically. In one such analysis, 45.7 ml of 9.5 M H2SO4 is required to neutralize a 20 ml sample of NaOH solution. What is the contration of the NaOH solution?
A. 1.52 M
B. 1.75 M
C. 2.05 M
D. 2.28 M

A

D. 2.28 M

123
Q

A series of measurements are made in order to determine the molar mass of an unknown gas. First, a large flask is evacuated and found to weight 134.567 g. It is then filled with the gas to a pressure of 735 torr at 310°C and reweighed; its mass is now 137.456 g. Finally, the flask filled with water at 31° and found to weigh 1067.9 g. (The density of the water at this temperature is 0.977g/mL). Assuming that the ideal gas equation applies, calculated the molar mass of the unknown gas.
A. 65.2 g/mol
B. 70.8 g/mol
C. 74.2 g/mol
D. 79.7 g/mol

A

D. 79.7 g/mol

123
Q

A gaseous mixture containing 50% mol H2 and 50% mol acetaldehyde is initially contained in a rigid vessel at 1 atm. The formation of ethanol occurs, after a time it was noted that the pressure drop 700 mmHg. Calculate the degree of completion of the reaction.
A. 15.8%
B. 17.2%
C. 7.8%
D. 9.2%

A

C. 7.8%

124
Q

2320 g of tetra-methanol cyclopentane is denoted in the absence of air in a 1000 L closed bomb.
C9H12N4O18 → 4CO2 + 5CO + 5H2O + H2 +2N2
The temperature in the bomb if the pressure rises to 300kPa is
A .425 K
B. 365 K
C. 285 K
D.345 K

A

A .425 K

125
Q

If 1.588 g of nitrogen tetroxide (N2O4) gives a total pressure of 1.0133 bar when partially dissociated in a 500-cm3 glass vessel at 25°C, what is the extent of the reaction?
A. 18.42%
B. 27.81%
C. 38.91%
D. 47.65%

A

B. 27.81%

126
Q

A solid metallic element burns in oxygen to produce an oxide which dissolves in water to give the hydroxide of the metal. The hydroxide obtained from 1 gram of metal neutralizes 111.2 ml of normal hydrochloric acid. The specific heat of the metal is 0.228 cal/g °C. What is the valency of the metal?
A. 1
B. 2
C. 3
D. 4

A

C. 3

127
Q

A solid metallic element burns in oxygen to produce an oxide which dissolves in water to give the hydroxide of the metal. The hydroxide obtained from 1 gram of metal neutralizes 111.2 ml of normal hydrochloric acid. The specific heat of the metal is 0.228 cal/g °C. What is the equivalent weight of the metal?
A. 9.33
B. 8.992
C. 9.002
D. 9.005

A

B. 8.992

128
Q

A 6.30-mg sample of a newly discovered isotope was analyzed and found to contain only 4.75 mg after a period of 27.2 hours. What is the half-life (in hours) of the isotope?
A. 27.2
B. 8.13
C. 92.3
D. 66.7

A

D. 66.7

129
Q

Consider the following reaction at equilibrium: N2O4(g)==2NO2(g). If a 5 L reaction vessel, held at constant temperature, is initially filled with 10 mol pure N2O4(g), and if 3.5 mol NO2(g) are found in the vessel once equilibrium has been established, what is the value of the equilibrium constant, Kc, for this reaction (at the temperature of the experiment)?
A. 0.297 M
B. 1.48M
C. 0.424 M
D. 0.0594 M

A

B. 1.48M

130
Q

The reaction of Br2(g) and Cl2(g) to form BrCl(g) has an equilibrium constant of 15 at a certain temperature. If 10 grams of BrCl is present in a 15-L reaction vessel, initially, what will be the constant of BrCl at equilibrium?
A. 3.8E-3 mol/L
B. 5.77 E-3 mol/L
C. 1.97 E-3 mol/L
D. 9.9 E-4 mol/L

A

D. 9.9 E-4 mol/L

131
Q

Carbom dioxide decomposes at elevated temperature to carbon monoxide and oxygen:
2CO2(g) ↔ 2CO(g) + O2(g)
At 3000 K, 2 mol of CO2 is placed in a 1 L container and allowed to equilibrate. At equilibrium, 0.90 mol CO2 remains. What is the value for Kc at this temperature?
A. 0.82
B. 1.88
C. 2.44
D. 3.12

A

A. 0.82

132
Q

If 1 mol of PCl3 and 1 mol of Cl2 are placed in a 5-L container, the following equilibrium is reached. PCl3(g) + Cl2(g) → PCl5(g) Kc= 10 at the t4emperature maintained. What is the equilibrium molar concentration of PCl3?
A. 0.13
B. 0.11
C. 0.14
D. 0.10

A

B. 0.11

133
Q

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. 1/8 mole
B. 2/7 mole
C. 5/7 mole
D. 5/6 mole

A

B. 2/7 mole

134
Q

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. 0.78 mole
B. 0.88 mole
C. 1.66 mole
D. 1.85 mole

A

C. 1.66 mole

135
Q

For the reaction 2NO2(g) → N2O4(g). At a certain temperature one mole of NO2 is placed in a 1 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

A

B. 5.56 mol/L

136
Q

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

A. 0.074

Day 1 (10 decks)

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