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Chemistry 1110 > Final > Flashcards

Final Flashcards

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1
Q

The metric unit used to measure volume is the

A

liter

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2
Q

How many meters are there in one kilometer?

A

10^3

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3
Q

An extra-strength aspirin contains 0.500 g of aspirin. How many grains is this? (1 grain = 64.8 mg)

A

7.72 Grains

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4
Q

Which measurement represents the largest quantity? A- 4730 ng B- 47.3 mg C- 4.73 × 10-6 kg D- 4.73 × 10-4 g E- 4.73 × 103 μg

A

B 47.3

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5
Q

How many quarts are contained in 450. mL?

A

0.475 quarts

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6
Q

If gasoline sells for 95.4 cents per liter, what is its cost on a per gallon basis? 1 L = 1.06 q

A

$3.60

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7
Q

In scientific notation, the number 185,000,000 is

A

1.85 X 10^8

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8
Q

A 35.0 mL sample of a liquid weighs 27.2 g. What is the density of the liquid?

A

0.777 g/mL

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9
Q

The dosage of quinine when a 145-lb adult takes a 200.-mg tablet is ________ μg drug per kg of body weight.

A

3.04 × 10^3

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10
Q

How many ng are there in 5.2 mg?

A

5.2 X 10^6 ng

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11
Q

What elements are in hydroxyapatite, Ca5(PO4)3OH , a major compound in human bones and teeth? calcium, phosphorous, oxygen, helium A- calcium, phosphorous, oxygen, hydrogen B- carbon, potassium, oxygen, hydrogen C- carbon, phosphorous, oxygen, helium D- carbon, potassium, oxygen, helium E- calcium, phosphorous, oxygen, helium

A

A. calcium, phosphorous, oxygen, hydrogen

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12
Q

Which of the following properties is NOT a characteristic of the Group 1A elements (alkali metals)? Most of them are liquids at room temperature. They are good conductors of heat. They are good conductors of electricity. They are shiny. They react vigorously with water.

A

Most of them are liquids at room temperature.

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13
Q

According to the Atomic Theory,

A

atoms are neither created nor destroyed during a chemical reaction.

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14
Q

Which of the following descriptions of a subatomic particle is correct?

A

A proton has a positive charge and a mass of approximately 1 amu.

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15
Q

The number of neutrons in an atom is equal to

A

the mass number- the atomic number

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16
Q

How many protons are in an isotope of sodium with a mass number of 25?

A

11

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17
Q

The correct symbol for the isotope of potassium with 22 neutrons is

A

41 19 K

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18
Q

The number of dots in the electron dot structure of nitrogen is

A

five

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19
Q

Which of the following is the correct electron-dot structure for carbon?

A

C and one dot on each side

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20
Q

The atomic size of atoms

A

increase going down within a group

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21
Q

Main group elements that are metals usually ________ one or more electrons to form ________, which have a ________ charge.

A

lose; cations; positive

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22
Q

One characteristic of a cation is that

A

it has more protons than electrons.

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23
Q

An element belonging to the halogen family would be expected to have a ________ ionization energy and a ________ electron affinity.

A

Large; Large

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24
Q

All of the following are properties typical of ionic compounds except -have very high melting points and boiling points. - conduct electrical current if dissolved in water. - shatter when crystals are struck. - exist as crystalline solids at room temperature. - form distinct molecules by interaction of specific particles.

A

form distinct molecules by interaction of specific particles.

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25
Q

Which of the following ions does not have the same electron configuration as the noble gas neon? Al3+ O2- Mg2+ S2- F-

A

S2-

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26
Q

An atom with 3 valence electrons will most likely

A

lose three electrons

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27
Q

Which of the following elements is most likely to form an ion with a -2 charge? S Ti K Si Mg

A

S

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28
Q

What is the formula for the ionic compound formed between calcium and sulfur?

A

CaS

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29
Q

What is the name of SnCl2?

A

tin(II) chloride

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30
Q

What is the name of Mg3(PO4)2?

A

magnesium phosphate

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31
Q

A molecule in which the central atom has no lone pairs and forms four single bonds is said to have a ________ shape.

A

Tetrahedral

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32
Q

What is the molecular geometry of PH3?

A

trigonal pyramidal

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33
Q

How many double bonds are there in a molecule of SF2?

A

0

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34
Q

Which of the following molecules has a CCH bond angle of 180°? HCCH H3CCHO H3CCH3 H2CCH2 none of them

A

HCCH

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35
Q

Which element listed is the most electronegative? aluminum iodine chlorine sodium bromine

A

Chlorine

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36
Q

Consider the molecule SiCl4. The electronegativity values for Si and Cl are 1.8 and 3.0, respectively. Based on these values and on consideration of molecular geometry, the Si-Cl bond is ________ and the molecule is ________.

A

polar; non-polar

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37
Q

What is the systematic name of ICl3?

A

iodine trichloride

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38
Q

The formula for phosphorus pentafluoride is ________.

A

PF5

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39
Q

When the reaction shown is correctly balanced, the coefficients are

C6H14 (l) + O2 (g) → CO2 (g) + H2O (g)

A

2, 19, 12, 14

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40
Q

Which of the following is not soluble in water?

iron(II) bromide
iron(III)nitrate
ammonium sulfate
iron(III) hydroxide
potassium sulfide

A

iron(III) Hydroxide

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41
Q

The oxidation number of sulfur in calcium sulfate, CaSO4, is ________.

A

+6

42
Q

In the reaction shown, ________ is the oxidizing agent because it ________.

Ni (s) + CuCl2 (aq) → Cu (s) + NiCl2 (aq)

A

CuCl2; gets reduced

43
Q

The net ionic equation for the reaction between zinc and hydrochloric acid solution is

A

Zn (s) + 2 H+ (aq) → Zn2+ (aq) + H2 (g).

44
Q

The formula weight of copper(II) chloride is ________ g

A

134.45

45
Q

The number of grams in 0.350 mol of Na is ________.

A

8.05

46
Q

In the reaction shown, how many moles of HCl are needed to react with 2.4 moles of Al?

2 Al + 6 HCl → 2 AlCl3 + 3 H2

A

7.2

47
Q

How many grams of fluorine are required to produce 20.0 grams of FeF3 from the reaction shown?

2 Fe + 3F2 → 2 FeF3

A

10.1 g

48
Q

A solution containing 145.0 g AgNO3 is mixed with a CaCl2 solution and 98.4 g of AgCl is recovered. Calculate the % yield of the reaction.

A

80.44%

49
Q

P4 (s) + 10 Cl2 (g) → 4 PCl5 (s) ΔH = -435.2 kcal

Based on the reaction shown, which statement is true?

When 30.97 g P4 (s) react, 435.2 kcal are released.
When 1 mol P4 (s) reacts, 435.2 kcal are released.
When 123.88 g P4 (s) react, 435.2 kcal are consumed.
When 1 mol PCl5 (s) is produced, 435.2 kcal are released.
When 208.22 g PCl5 (s) are produced, 435.2 kcal are consumed.

A

When 1 mol P4 (s) reacts, 435.2 kcal are released.

50
Q

2 Al2O3 (s) → 4 Al (s) + 3 O2 (g) ΔG = +138 kcal

Consider the contribution of entropy to the spontaneity of this reaction. As written, the reaction is ________, and the entropy of the system ________.

A

non-spontaneous; decreases

51
Q

Activation energy can best be described as

A

the difference in energy between reactants and the maximum energy.

52
Q

Part A

In the reaction energy diagrams shown, reaction A is ________, and it occurs ________ reaction B.

A

exergonic;slower than

53
Q

Which statement best describes the way a catalyst works?

It decreases the value of ΔH. It increases the value of Eact. It decreases the value of Eact. It increases the value of ΔG. It increases the value of ΔH

A

It decreases with the value of Eact

54
Q

Which change to this reaction system would cause the equilibrium to shift to the right?

N2 (g) + 3 H2 (g) ↔ 2 NH3 (g) + heat

removal of H2 (g) addition of a catalyst addition of NH3 (g) heating the system lowering the temperature

A

Lowering the temperture

55
Q

Diatomic nitrogen is added to the equilibrium system:

N2 (g) + H2 (g) ↔ 2 NH3(g) + heat

When a new equilibrium is established the concentration of H2 will be ________ the amount at the original equilibrium, and the amount of NH3 will be ________ the amount at the original equilibrium.

greater than; greater than
greater than; less than
less than; greater than
less than; less than
Both changes will be impossible to determine.

A

less than; greater than

56
Q

If we add a catalyst to the following equation, CO + H2O + heat ↔ CO2 + H2, which way will the equilibrium shift?

No effect To the right To the left Not enough information

A

No effect

57
Q

For the following reaction, increasing the pressure will cause the equilibrium to ________.

2 SO2 (g) + O2 (g) ↔ 2 SO3 (g) + heat

shift to the left, towards reactants shift to the right, towards products remain unchanged, but the reaction mixture will get warmer remain unchanged, but the reaction mixture will get cooler Pressure has no effect on equilibrium.

A

shift to the right, towards products

58
Q

A reaction that is spontaneous can be described as

having the same rate in both the forward and reverse directions. increasing in disorder. proceeding in both the forward and reverse directions. releasing heat to the surroundings. proceeding without external influence once it has begun.

A

proceeding without external influence once it has begun.

59
Q

Which of the assumptions of the kinetic-molecular theory best explains the observation that a gas can be compressed?

Gas molecules move at random with no attractive forces between them. In collisions with the walls of the container or with other molecules, energy is conserved. Collisions with the walls of the container or with other molecules are elastic. The velocity of gas molecules is proportional to their Kelvin temperature. The amount of space occupied by a gas is much greater than the space occupied by the actual gas molecules.

A

The amount of space occupied by a gas is much greater than the space occupied by the actual gas molecules.

60
Q

A sealed container with gas at 2.00 atm is heated from 20.0 K to 40.0 K. The new pressure is

2.14 atm. 0.500 atm. 4.00 atm. 1.87 atm. 1.00 atm.

A

4.00 atm

61
Q

If the temperature of a 1.75 liter sample of gas is changed from 30.0°C to 20.0°C at constant pressure, what will be the new volume?

1.69 L 1.81 L 2.63 L 1.17 L 1.57 L

A

1.69 L

62
Q

A 65 mL sample of argon gas has a temperature of 325°C. What will the temperature be in °C when the volume of the gas is decreased to 25 mL at constant pressure?

641°C 1280°C -43°C 125°C 65°C

A

-43 C.

63
Q

According to Avogadro’s Law, the volume of a gas will ________ as the ________ is increased while the ________ are held constant.

increase; pressure; temperature and number of moles increase; temperature; pressure and number of moles increase; number of moles; pressure and temperature decrease; number of moles; pressure and temperature decrease; pressure; temperature and number of moles

A

increase; number of moles; pressure and temperature

64
Q

How many grams of O2 are contained in a 25.0 L sample at 5.20 atm and 28.0°C?

5.26 g 0.164 g 1810 g 168 g 84.2 g

A

168 g

65
Q

In a gas mixture of 35% He and 65% O2 the total pressure is 800 mm Hg. What is the partial pressure of O2?

65 mm Hg 35 mm Hg 100 mm Hg 280 mm Hg 520 mm Hg

A

520 mmHg

66
Q

Which pair of molecules has the strongest dipole-dipole interactions?

NH3 and NH3 CO2 and CO2 NH3 and CH4 CO2 and CH4 CH4 and CH4

A

NH3 and NH3

67
Q

Which intermolecular force is characteristic of compounds with low molar mass, which are liquids at room temperature and have relatively high boiling points?

covalent bonds london forces dipole-dipole forces ionic bonds hydrogen bonds

A

hydrogen bonds

68
Q

A solid compound which has no definite crystalline structure and a poorly defined melting point is referred to as a(an) ________ solid.

amorphous metallic ionic network covalent molecular

A

Amorphous

69
Q

How many grams of NaOH are needed to make 750 mL of a 2.5% (w/v) solution?

20 g 7.5 g 50 g 3.9 g 19 g

A

19 g

70
Q

What is the molarity of a solution prepared by dissolving 0.750 mol CaCl2 in enough water to make 0.500 L of solution?

0.375 M 0.667 M 1.50 M 166.5 M 83.2 M

A

1.50 M

71
Q

How many mL of a 5.00% (w/v) glucose solution are needed to provide 20.0 g of glucose?

4.00 mL 20.0 mL 5.00 mL 200. mL 400. mL

A
  1. mL
72
Q

Calculate the concentration in ppm of a pollutant that has been measured at 450 mg per 150 kg of sample.

3000 ppm 6.0 ppm 3.0 ppm 330 ppm none of the above

A

3.0 ppm

73
Q

What is the final concentration of a solution prepared by adding water to 50.0 mL of 1.5 M NaOH to make 1.00 L of solution?

0.075 M 1.5 M 0.030 M 30 M 7.5 M

A

0.075 M

74
Q

Considering 0.10 M solutions of each substance, which contains the smallest concentration of ions?

K2CO3 FeSO4 Na2SO4 (NH4)3PO4 Ca(NO3)2

A

FeSO4

75
Q

How many grams are in 10.0 mEq of Ca2+?

A
76
Q

What is the osmolarity of a 0.20 M solution of KCl?

0.80 Osmol 0.10 Osmol 0.40 Osmol 0.30 Osmol 0.20 Osmol

A

0.40 Osmol

77
Q

Which has the lowest boiling point?

0.1 M glucose, C6H12O6 0.1 M Na2SO4 0.1 M Al(NO3)3 pure water 0.1 M MgCl2

A

Pure water

78
Q

Which solution is the least concentrated? Each choice refers to the same solute and solvent.

30 g solute in 150 mL solution 2.4 g solute in 2 mL solution 2.4 g solute in 5 mL solution 20 g solute in 50 mL solution 50 g solute in 175 mL solution

A

30 g solute in 150 mL solution

79
Q

A necessary requirement for a Brønsted base is

a lone pair of electrons in its Lewis dot structure. the production of hydronium ion upon reaction with water. the presence of hydroxide in its formula. the presence of a metal ion in its formula. the presence of water as a reaction medium.

A

a lone pair of electrons in its Lewis dot structure.

80
Q

Which net ionic equation correctly represents the neutralization of a solution of barium hydroxide by a solution of nitric acid?

Ba2+ + 2 OH- → Ba(OH)2 Ba2+ + 2 NO3- → Ba(NO3)2 Ba(NO3)2 + H2O → Ba2+ + 2 NO3- H+ + OH- → H2O H+ + NO3- → HNO3

A
81
Q

Hydrogen cyanide, HCN, is a weak acid. Which equation best represents its aqueous chemistry?

HCN (aq) + H2O(l) ↔ H2CN+ (aq) + OH- (aq) H2O (l) ↔ H+ (aq) + OH- (aq) HCN (aq) ↔ H+ (aq) + CN- (aq) HCN (aq) ↔ H- (aq) + CN+ (aq) HCN (aq) + H2O(l) ↔ CN- (aq) + H3O+ (aq)

A
82
Q

Which one of the following is the weakest acid?

HF (Ka = 6.8 x 10-4) HClO (Ka = 3.0 x 10-8) HNO2 (Ka = 4.5 x 10-4) HCN (Ka = 4.9 x 10-10)

A

HCN (Ka = 4.9 x 10-10)

83
Q

If the concentration of OH- in an aqueous solution is 1.4 × 10-7 M, the concentration of H3O+ is ________.

7.1 × 10-8 M 1.3 × 10-8 M 7.1 × 10+6 M 1.0 × 10-7 M 1.4 × 10-7 M

A
84
Q

What is the pH of a solution in which the hydrogen ion concentration is 5.1 × 10-8 M?

8.90 7.29 1.96 × 10-7 5.10 6.71

A

7.29

85
Q

How many mL of 0.100 M NaOH are needed to neutralize 24.0 mL of 0.150 M HCl?

36.0 mL 18.0 mL 24.0 mL 12.0 mL 48.0 mL

A

36.0 mL

86
Q

What is the concentration of an acetic acid solution if a 10.0 mL sample required 26.4 mL of 0.950 M KOH for neutralization?

0.950 M 0.399 M 2.51 M 0.379 M 2.78 M

A

2.51 M

87
Q

Which of the following solutions is a buffer?

a solution of acetic acid and sodium sulfate a solution of hydrochloric acid and sodium sulfate a solution of sulfuric acid and sodium sulfate a solution of hydrochloric acid and sodium acetate a solution of acetic acid and sodium acetate

A

a solution of acetic acid and sodium acetate

88
Q
A
89
Q

The pH of a 250. mL sample of a buffer solution is 9.85. If 1.0 mL of 6 M HCl is added, the pH of the resulting mixture is closest to

10.00 1.65 0.00 7.00 9.70

A

9.70

90
Q

The product from the alpha decay of ![\rm ^{235}{92}U](http://session.masteringchemistry.com/render?expr=%5Crm+%5E%7B235%7D%7B92%7DU) is

![\rm ^{235}{93}Np](http://session.masteringchemistry.com/render?expr=%5Crm+%5E%7B235%7D%7B93%7DNp). ![\rm ^{231}{90}Th](http://session.masteringchemistry.com/render?expr=%5Crm+%5E%7B231%7D%7B90%7DTh). ![\rm ^{236}{92}U](http://session.masteringchemistry.com/render?expr=%5Crm+%5E%7B236%7D%7B92%7DU). ![\rm ^{233}{80}Ra](http://session.masteringchemistry.com/render?expr=%5Crm+%5E%7B233%7D%7B80%7DRa). ![\rm ^{239}{94}Pu](http://session.masteringchemistry.com/render?expr=%5Crm+%5E%7B239%7D%7B94%7DPu).

A

![\rm ^{231}{90}Th](http://session.masteringchemistry.com/render?expr=%5Crm+%5E%7B231%7D%7B90%7DTh)

91
Q

The damaging effects of radiation on the body are a result of

A

the formation of unstable ions or radicals.

92
Q

What is missing in the nuclear reaction shown below?

![\rm ^{10}{5}B + \rm {^{4}{2}}He \; \rightarrow \; \rm ^{13}{7}N + {}](http://session.masteringchemistry.com/render?expr=%5Crm+%5E%7B10%7D%7B5%7DB++%2B+%5Crm+%7B%5E%7B4%7D_%7B2%7D%7DHe+%5C%3B+%5Crightarrow+%5C%3B+%5Crm+%5E%7B13%7D_%7B7%7DN++%2B+%7B%7D)_____

a neutron a beta particle an alpha particle gamma radiation a positron

A

a neutron

93
Q

What is the radiation particle used in the bombardment of nitrogen-14?

![\rm ^{14}{7}N + {}? \; \rightarrow \; ^{14}{6}C + {} ^{1}{1}H](http://session.masteringchemistry.com/render?expr=%5Crm+%5E%7B14%7D%7B7%7DN+%2B+%7B%7D%3F+%5C%3B+%5Crightarrow+%5C%3B+%5E%7B14%7D_%7B6%7DC+%2B+%7B%7D+%5E%7B1%7D_%7B1%7DH)

neutron beta particle alpha particle gamma ray proton

A

neutron

94
Q

The dosage of technetium-99m for myocardial imaging is 280 μCi/kg of body weight. How many mCi should be given to a patient weighing 65 kg? (1 mCi = 1000 μCi)

4.3 mCi 0.0043 mCi 1.8 x 104 mCi 230 mCi 18 mCi

A

18 mCi

95
Q

Iodine-123, which is used for diagnostic imaging in the thyroid, has a half-life of 13 hours. If 50.0 mg of I-123 were prepared at 8:00 A.M. on Monday, how many mg remain at 10:00 A.M. on the following day?

3.13 mg 6.25 mg 50.0 mg 25.0 mg 12.5 mg

A

12.5 mg

96
Q

The half-life of bromine-74 is 25 min. How much of a 4.0 mg sample is still active after 75 min?

4.0 mg 2.0 mg 1.0 mg 0.50 mg 0.25 mg

A

0.50 mg

97
Q

When a positron is emitted from the nucleus of an atom, the nuclear mass

increases by two units. decreases by one unit. decreases by two units. remains the same. increases by one unit.

A

remains the same

98
Q

If absorbed internally, alpha particle emitters are the most damaging because alpha particles

have the greatest energy. have the largest charge. consist of pure energy. have the greatest mass. consist of high energy electrons.

A

have the greatest mass

99
Q

Iodine-131 decays by beta emission to

tellurium-131. iodine-132. iodine-130 bromine-131 xenon-131.

A

xenon-131

100
Q

Which representation of a methane molecule is not correct? (A methane molecule is composed of one carbon atom and four hydrogen atoms.)




none of the above

A
101
Q

Which element is most likely to be “X” in the diatomic molecule shown?

helium hydrogen fluorine oxygen nitrogen

A

oxygen

Chemistry 1110 (1 decks)

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