Chemistry - 2nd Semester Review Packet

Multiple ChoiceIdentify the choice that best completes the statement or answers the question.

____ 1. Which is NOT an assumption of matter made by the kinetic molecular theory of gases?a. Gas particles are small and take up little volume relative to the volume of the space around

them.b. The kinetic energy of particles is determined by their mass and their velocity.c. When particles collide, their total energy is decreased.d. Gas particles are widely dispersed and therefore are not affected significantly by attractive

or repulsive forces.

____ 2. A sample of three mixed gases is at 632.0 mmHg. If the partial pressure of CO2 is 124.3 mmHg and the partial pressure of N2 is 461.9 mmHg, what is the partial pressure of O2?a. 760 mmHg c. 173.8 mmHgb. 45.8 mmHg d. 128 mmHg

____ 3. Which change in state requires that energy be added to the substance?a. freezing c. condensingb. deposition d. vaporizing

____ 4. Which is the state change that occurs when a solid becomes a gas without becoming a liquid first?a. vaporization c. depositionb. sublimation d. freezing

____ 5. Use the following graph for quetions 5-7.

Which is the triple point of this substance?

a. 88° C, 0.95 atm c. 150° C, 1.45 atmb. 110° C, 1.00 atm d. 36° C, 2.1 atm

____ 6. What state of matter will this substance be in at a temperature of 28oC and a pressure of 0.7 atm?

a. solid c. in equilibrium between solid and gasb. liquid d. gas

____ 7. If the temperature of this substance is held constant at 130°C while the pressure is changed from 1.4 atm to 0.8 atm, which is the change in state that will occur?a. vaporization c. depositionb. condensation d. melting

____ 8. The volume of a sample of helium is 4.5 mL at 20.0°C and 203.0 kPa. What will its volume be in the figure?

a. 2.25 mL c. 4.34 mLb. 3.78 mL d. 6.85 mL

____ 9. A balloon is filled with 3.50 L of water at 24.0°C and 2.27 atm. The balloon in the figure is placed outside on a hot day, what is the volume of the balloon (assuming constant pressure)?

a. 2.47 L c. 3.61 Lb. 3.38 L d. 8.19 L

____ 10. Gas is confined in a metal tank in the figure. At 20.20C, the gas exerts a pressure of 8.532 atm. After heating the tank, the pressure of the gas increases to 10.406 atm. What is the temperature of the heated gas?

a. -32.60C c. 84.59Cb. 24.63C d. 92.64C

____ 11. A sample of neon gas occupies a volume of 752 mL at 25°C. What volume will the gas occupy at 50°C if the pressure remains constant?a. 204 mL c. 815 mLb. 408 mL d. 8150 mL

____ 12. A helium-filled balloon has a volume of 50.0 L at 25°C and 1.08 atm. What volume will it have at .855 atm and 10.0°C?a. 15.0 L c. 60.0 Lb. 30.0 L d. 120.0 L

____ 13. What volume does .0685 mol of gas occupy at STP?a. .3707 mol c. 1.53 Lb. .7515 mol d. 3.06 L

____ 14. How many moles of helium gas are contained in a 4.0-L flask at STP?a. 0.045 mol c. 0.17 molb. 0.089 mol d. 89 mol

____ 15. A steel tank with a volume of 9.583 L contains N2 gas under a pressure of 4.972 atm at 31.8 °C. Calculate the number of moles of N2 in the tank.a. 0.002 mol c. 0.525 molb. 0.018 mol d. 1.90 mol

____ 16. When a milkshake is taken in through a straw at a pressure of 0.071 atm, the straw contains 5.0 mL of liquid. How much liquid is consumed at 0.092 atm?a. 0.10 mL c. 6.3 mLb. 3.9 mL d. 7.8 mL

____ 17. A balloon is filled with 3.50 L of water at 24.0°C and 2.27 atm. If the balloon is placed outdoors on a hot day at a temperature of 34.0°C, what is the volume of the balloon at constant pressure?a. 2.47 L c. 3.61 Lb. 3.38 L d. 8.19 L

____ 18. Two liquids that can be mixed together but separate shortly after are:a. immiscible c. miscibleb. insoluble d. soluble

____ 19. A heterogeneous mixture of intermediate sized particles is a:a. colloid c. solvent

b. solute d. suspension

____ 20. A _____ contains the maximum amount of dissolved solute for a given amount of solvent.a. saturated c. suspendedb. supersaturated d. unsaturated

____ 21. Two liquids that are soluble in each other in any proportion are said to be:a. insoluble c. miscibleb. immiscible d. soluble

____ 22. What law states that at a given temperature the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid?a. Boyle’s Law c. Henry’s Lawb. Charles’s Law d. Ideal Gas Law

____ 23. A _____ solution contains more dissolved solute than a saturated solution at the same temperature.a. saturated c. suspendedb. supersaturated d. unsaturated

____ 24. Which of the following statements about a catalyst is true?a. A catalyst can initiate a reaction.b. A catalyst can accelerate a reaction.c. A catalyst can be consumed during a reaction.d. A catalyst can be changed during a reaction.

____ 25. Which of the following factors does NOT affect the rate of the reaction?a. the amount of the reactants c. the size of the container usedb. the physical state of the reactants d. temperature

____ 26. What change can result in a shift in equilibrium during a reaction?a. change in concentration c. change in volume and pressureb. change in temperature d. all of the above

____ 27. In an endothermic reaction, equilibrium shifts _____ when temperature is raised.a. to the left c. to the centerb. to the right d. none

____ 28. Which of the following factors will NOT change the concentration of ammonia (NH3) in the reaction??

a. Decrease in the volume of N2. c. Decrease in pressure.b. Increase in the amount of catalyst. d. Decrease in temperature.

____ 29. According to Le Chatelier’s principle, when the volume is increased, the equilibrium shifts to the right. For which of the following reversible reactions is this true?a.b.c.d.

____ 30. In the reaction heat is evolved. What happens when chlorine (Cl2) is added to the equilibrium mixture at constant volume?a. The temperature of the system increases.

b. The temperature of the system decreases.c. More chlorine is produced.d. The temperature remains unaffected.

____ 31. When acids react with metals, they produce _____ gas.a. hydrogen c. sulfurb. nitrogen d. oxygen

____ 32. A _____ is produced when a base accepts a hydrogen ion from an acid.a. conjugate acid c. acidb. conjugate base d. base

____ 33. What is the pH of blood, given the hydrogen ion concentration is 4.0 x 10-8 M?a. 7.0 c. 7.4b. 7.2 d. 7.6

____ 34. In the Bronsted-Lowry model of acids and bases, an _____ is a hydrogen donor and a _____ is a hydrogen acceptor.a. acid, base c. conjugate acid, conjugate baseb. base, acid d. conjugate base, conjugate acid

____ 35. What is the pH of 0.00045 M of HCl?a. 3.35 c. 9.50b. 4.50 d. 10.65

____ 36. What is the hydrogen ion concentration of an HClO4 solution with the pH of 2.95?a. 0.0295 M c. 2.95 x 10-10 Mb. 0.0011 M d. 8.9 x 10-12 M

____ 37. A solution that contains equal concentrations of hydrogen and hydroxide ions is _____.a. an acid c. neutralb. a base d. ionized

____ 38. At 298 K, the H ion concentration of an aqueous solution is 1.00 10–5 M. What is the pH of the solution?a. –4.04 c. 3.99b. 5.00 d. 3.82

____ 39. Redox reactions involve the _____ of electrons.a. combining c. substitutionb. sharing d. transfer

____ 40. What is the oxidation number of chlorine in NaCl?a. -2 c. 0b. -1 d. +1

____ 41. Oxidation involves the _____ of electrons.a. gain c. displacementb. loss d. bonding

____ 42. The oxidation number of Na(s) is:a. -1 c. +1b. 0 d. +2

____ 43. The electrode where oxidation takes place is called the:

a. anode c. cellb. cathode d. dry cell

____ 44. _____ bonds are formed by the transfer of electrons.a. ionic c. nonpolarb. polar d. metallic

____ 45. In which phase of matter do the particles have the least kinetic energy?a. gases c. solidsb. liquids d. they all have the same

____ 46. How would you describe a solution that has the pH of 8?a. acidic c. neutralb. basic d. buffered

____ 47. How would you describe a solution that has the pOH of 2?a. acidic c. neutralb. basic d. buffered

____ 48. The name given to particles in a solution that do not conduct electricitya. electrolytes c. non-electrolytesb. metals d. non-metals

____ 49. When making kool-aid, which substance is the solute?a. sugar c. containerb. water d. all of the above

____ 50. How many atoms are in the compound Na2SO4?a. 2 c. 5b. 3 d. 7

____ 51. How many grams are in 2.0 moles of sodium hydroxide?a. 20. g c. .050 gb. 80. g d. .040 g

____ 52. Convert 149 grams of sodium phosphate to moles. a. 24400 moles c. 1.26 molesb. 17600 moles d. 0.909 moles

____ 53. What do you call a chemical reaction that releases more energy than it takes in?a. exothermic c. endothermicb. energetic d. exergonic

____ 54. What is the pH of an aqueous solution that is acidic?a. pH < 7 c. pH = 7b. pH > 7 d. pH = 14

____ 55. If the pH of a solution decreases, what happens to the concentration of OH-?a. increases c. stays the sameb. decreases d. all of the above

____ 56. Which of the following is the definition of a Bronsted-Lowry acid?a. oxygen donor c. oxygen acceptorb. hydrogen donor d. hydrogen acceptor

____ 57. What are STP conditions?a. 0 K, 1 atm c. 0 °C, 760 mm Hgb. 0 °C, 760 atm d. 273 K, 1 mm Hg

____ 58. Assume that at STP, 2.84 grams of magnesium react with hydrochloric acid (HCl) to form aqueous magnesium chloride and hydrogen gas. How many L of hydrogen gas are produced?

a. 0.236 L c. 0.256 Lb. 3.08 L d. 2.62 L

____ 59. What pressure, in atmospheres, is exerted by 1.4 moles of oxygen in a 4.87 L container at 21.6°C?

a. 0.14 atm c. 0.51 atmb. 7.0 atm d. 6.4 atm

____ 60. If the system 2 NO2 <--> N2O4 has come to equilibrium and then the pressure is increased, a. [NO2] increases, [N2O4] increases c. [NO2] increases, [N2O4] decreasesb. [NO2] decreases, [N2O4] increases d. [NO2] and [N2O4] remain the same

____ 61. How many grams of potassium phosphate are needed to make 250. mL of a 2.0 M solution?

a. 110 grams c. 110,000 gramsb. 67 grams d. 67,000 grams

____ 62. What is the molality of a solution composed of 197.3 g of sodium nitrate dissolved in 2.0 moles of water?

a. 0.010 m c. 0.86b. 99 m d. 64 m

____ 63. A substance that ionizes completely in an aqueous solution and produces OH- is considered which of the following?a. a weak base c. a strong baseb. a weak acid d. a strong acid

____ 64. Which of the following is a weak organic acid?a. HCl c. HC2H3O2

b. HBr d. H2SO4

____ 65. In the equation NH3 + H2O --> NH4+ + OH-, which species is a Bronsted-Lowry base?

a. NH3 c. NH4+

b. H2O d. OH-

____ 66. An acid-base titration involves which type of reaction?a. combustion c. decompositionb. synthesis d. neutralization

____ 67. What is the molarity of an HCl solution if 40.0 mL is neutralized in a titration by 45.0 mL of 0.200 M NaOH?a. 0.178 M c. 0.356 Mb. 0.225 M d. 0.450 M

____ 68. What is the molarity of Ca(OH)2 solution if 53.4 mL is completely titrated by 10.3 mL of 0.150 M H2SO4?a. 0.0289 M c. 0.0578 Mb. 0.778 M d. 1.56 M

____ 69. How could you increase the solubility of a gas in a liquid? (hint: think about carbonation in pop)

a. decrease pressure c. increase temperatureb. decrease temperature d. none of the above

____ 70. Which phase change is represented by the equation solid + energy --> gas?a. sublimation c. meltingb. deposition d. freezing

____ 71. Which phase change is represented by the equation liquid - energy --> solid?a. melting c. evaporationb. freezing d. condensation

____ 72. Which process involves the gain of electrons?a. oxidation c. titrationb. reduction d. synthesis

____ 73. What is the oxidation number of Na in Na3N?a. +1 c. -1b. +3 d. -3

____ 74. What is the oxidation number of N in LiNO3?a. +1 c. +5b. -1 d. -3

____ 75. What is the oxidation number for solid Iron metal (Fe)?a. +3 c. +1b. +2 d. 0

____ 76. What is the electrode where reduction occurs?a. voltaic c. cathodeb. galvanic d. anode

____ 77. Which metal electrode is located at the anode in the redox reaction between Ag and Zn?a. Ag c. cannot tellb. Zn d. neither Ag nor Zn

____ 78. Which is the short cell notation for the electrochemical cell containing Ba and Au?a. Ba | Ba +2 || Au+3 | Au c. Ba+2 | Ba || Au | Au +3

b. Au | Au +3 || Ba+2 | Ba d. Au+3 | Au || Ba | Ba +2

____ 79. What is the voltage for the electrochemical cell containing Sn and Cs?a. 2.78 V c. 3.06 Vb. -2.78 V d. -3.06 V

____ 80. Is the reaction going to be spontaneous if the reaction is endothermic (ΔH = + ) and the entropy of the reaction is low (ΔS = -)?a. it will always be spontaneous c. it will be spontaneous only at low

temperaturesb. it will be spontaneous only at high

temperaturesd. it will never be spontaneous

____ 81. Which is not a factor affecting the rate of the reaction?a. surface area c. colorb. temperature d. nature of the substance

____ 82. What is the change in enthalpy for the following reaction, given the enthalpies of formations?2 CH3OH + 3 O2 4 H2O (g) + 2 CO2

CH3OH = -201.0 kJ/mol H2O (g) = -241.83 kJ/mol CO2 = -393.509 kJ/mola. -433.339 kJ c. +433.339 kJb. -1352.338 kJ d. +1352.338 kJ

____ 83. Which state of matter has the highest entropy according to the general rule?a. gas c. solidb. liquid d. all of the above

____ 84. What is the name of the acid, HBr?a. bromic acid c. hydrobromic acidb. bromous acid d. hypobromous acid

____ 85. What is the formula for hypochlorous acid?a. HClO c. HClO4

b. HClO2 d. HCl

____ 86. What is the name of the acid, H3PO4?a. hydrophosphoric acid c. phosphorous acidb. phosphoric acid d. perphosphoric acid

____ 87. What type of cell has non-spontaneous redox reactions that convert electrical energy to chemical energy?a. galvanic c. sporadicb. electrolytic d. monastic

____ 88. Which substance is the oxidizing agent in the following reaction?Cl2 + 2 Br - --> 2 Cl - + Br2

a. Cl2 c. Cl -

b. Br - d. Br2

____ 89. Which of the following litmus paper color changes indicates that the solution is basic?a. blue stays blue c. red stays redb. blue turns red d. red turns blue

____ 90. Predict the product(s) of the following reaction: sodium + water ---> a. NaOH + H2 c. NaOHb. NaO + H2 d. Na2O + H2

____ 91. Predict the product(s) of the following reaction: carbon dioxide + water --->a. C(OH)2 c. H2CO3

b. C(OH)2 + H2 d. H2O2+ + CO3

2-

____ 92. For questions 92-95, use the following experimental data:Experiment [N2] [H2] Rate 1 0.020 0.010 .028 2 0.020 0.020 .057 3 0.020 0.040 .114 4 0.040 0.020 .227 5 0.010 0.020 .014

What is the rate equation?

a. R=k[N2]2[H2]2 c. R=k[N2][H2]2

b. R=k[N2]2[H2] d. R=k[N2]2[H2]3

____ 93. What is the overall order of the reaction?a. 2 c. 4b. 3 d. 5

____ 94. What is the k value for the rate reaction?a. 7.0 x 103 c. 5.6 x 10-6

b. 140 d. 1.1 x 10-7

____ 95. What would the rate of reaction be when: [N2] = 0.025 and [H2] = 0.025?a. 4.5 x 108 c. 4.4b. 2.2 x 10-3 d. .11

____ 96. What is the voltage for the electrochemical cell containing Cs and Li?a. 0.13 V c. -5.97 Vb. 5.97 V d. -0.13 V

____ 97. What is the voltage for the electrochemical cell containing Fe II and Sn?a. 0.91 V c. 0.58 Vb. 0.30 V d. 0.63 V

____ 98. What is the voltage for the electrochemical cell containing Cs and Cl2?a. -4.28 V c. 1.56 Vb. -1.56 V d. 4.28 V

Short Answer

99. Calculate the number of moles of ammonia gas (NH3) contained in a 3.0 L vessel at 3.00 x 102 K with a pressure of 1.50 atm.

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100. The specific heat of water is 4.184 J/(g°C). How much heat is absorbed by 15.5 g of water when its temperature is increased from 20.0°C to 50.0°C?

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101. The _______________ of any substance is the amount of heat required to raise the temperature of one gram of that substance by one degree Celsius.

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102. When the change in enthalpy is positive the reaction is _______________. When the change in enthalpy is negative the reaction is _______________.

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103. Write the expression for Keq for the following reaction:

3A (g) + 1B (g) + 1C (g) 7D (g) + 6E (g)

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104. Calculate the hydrogen ion concentration of a solution with a pOH of 4.5, given the ion product constant for water is 1.00 x 10-14

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105. Calculate the pH of a solution of HCl, given the hydrogen ion concentration is 8.87 x 10-9 M.

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106. Calculate the pOH of a solution that has a pH of 2.7 at STP.

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107. Calculate the hydrogen ion concentration of 0.650 M aqueous solution of Sodium hydroxide. The ionization product constant for water is 1.00 x 10-14.

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108. Calculate the hydroxide ion concentration of a solution with a pH of 5.5, given the ion product constant for water is 1.00 x 10-14

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109. Balance the given redox reaction.

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110. Use the oxidation-reduction method to balance the given net ionic redox reaction.

Cu(s) + NO3–(aq) + H+(aq) Cu2+(aq) + NO2(g) + H2O(l)

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111. What can be done to a solution to get a solid to dissolve faster in a liquid?

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Problem

112. Hydrogen chloride and argon form a mixture at room temperature. The partial pressure of hydrogen chloride is 1.2 atm and that of argon is 2.7 atm. What is the total pressure of the mixture of the two gases?

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113. A gas is confined in a cylinder fitted with a movable piston. At 21.0°C, the gas occupies a volume of 6.24 L under a pressure of 2.79 atm. The gas is heated to 99.0°C and compressed to 5.22 atm. What volume does the gas occupy in its final state?

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114. Calculate the temperature of 2.0 moles of a gas occupying a volume of 5.0 L at 2.46 atm.

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115. A 23.0-g sample of water is put into a calorimeter and heated until its temperature increases from 31.0°C to 68.0°C. If the specific heat of water is 4.18 J/(g °C), calculate the heat absorbed by water.

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116. Write the equilibrium constant expression for the following reaction:

5A(g) + 1B(g) + 1C(g) 10D(g) + 6E(g)

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117. Write a chemical equation for the neutralization of sodium hydroxide and hydrochloric acid.

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118. What is the concentration of hydroxide ion [OH–] of an aqueous solution when pH of the solution is 5.5? The ion product constant for water is 1.0 10–14.

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119. Calculate the pH of 0.020 M HCl.

Chemistry - 2nd Semester Review PacketAnswer Section

MULTIPLE CHOICE

1. ANS: C PTS: 1 DIF: Bloom's Level 2NAT: B.2 STA: C2.2c | C2.2f

2. ANS: B PTS: 1 DIF: Bloom's Level 3NAT: UCP.2 | UCP.3 STA: C4.5a | C4.5b

3. ANS: D PTS: 1 DIF: Bloom's Level 2NAT: UCP.3 STA: C5.4c | C5.4d

4. ANS: B PTS: 1 DIF: Bloom's Level 2NAT: UCP.3 | B.2 STA: C5.4c | C5.4d

5. ANS: A PTS: 1 DIF: Bloom's Level 3NAT: UCP.2 | B.2 STA: C5.4B | C5.4A

6. ANS: A PTS: 1 DIF: Bloom's Level 3NAT: B.2 STA: C5.4B | C5.4A

7. ANS: A PTS: 1 DIF: Bloom's Level 4NAT: UCP.3 | B.2 STA: C5.4B | C5.4A

8. ANS: CUse Charles’s law

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.2 | UCP.3 | B.6STA: C4.5c | C4.5b

9. ANS: CUse Charles Law

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.2 | UCP.3 | B.4 | B.6STA: C4.5c | C4.5b

10. ANS: CP1 / T1 = P2 / T2

Convert Celsius to Kelvin

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.2 | UCP.3 | B.4 | B.6STA: C4.5b | C4.5a

11. ANS: C PTS: 1 DIF: Bloom's Level 3NAT: UCP.3 | B.4 | B.6 STA: C4.5c | C4.5b

12. ANS: C PTS: 1 DIF: Bloom's Level 3NAT: UCP.3 | B.6 STA: C4.5a | C4.5c

13. ANS: C PTS: 1 DIF: Bloom's Level 3NAT: UCP.3 | B.6 STA: C4.6a | C4.5b

14. ANS: CAvogadro’s principle states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

FeedbackA Divide 4 by 22.4 to find the number of moles.

B Divide the volume and not the atomic number of helium by 22.4.C Correct!D Divide the volume by 22.4 instead of finding the product of 22.4 and 4.

PTS: 1 DIF: 1 REF: Page 430 | Page 431OBJ: 14.2.3 Relate numbers of particles and volumes by using Avogadro's principle.NAT: UCP.1 | UCP.3 | B.2TOP: Relate numbers of particles and volumes by using Avogadro's principle.KEY: Avogadro's principle - using moles MSC: 3

15. ANS: DAccording to the ideal gas law, PV nRT.

FeedbackA Use the correct numerical value of R. The value of R is not 62.4.B Use the correct numerical value of R. The value of R is not 8.314.C Divide PV by RT to obtain the number of moles of N2.D Correct!

PTS: 1 DIF: 2 REF: Page 436OBJ: 14.3.1 Relate the amount of gas present to its pressure, temperature, and volume by using the ideal gas law. NAT: UCP.1 | UCP.3 | B.4TOP: Relate the amount of gas present to its pressure, temperature, and volume by using the ideal gas law.KEY: Applying the ideal gas law MSC: 3

16. ANS: BUsing Boyle’s law, P1V1 P2V2.

FeedbackA The value of P1 in Boyle's law is 0.072 atm.B Correct!C The product of P1 and V1 in Boyle's law is incorrect.D In Boyle's law, divide P1V1 by 0.092 atm.

PTS: 1 DIF: 1 REF: Page 421OBJ: 14.1.2 Apply the three gas laws to problems involving the pressure, temperature, and volume of a gas.NAT: UCP.1 | UCP.3 | B.4TOP: Apply the three gas laws to problems involving the pressure, temperature, and volume of a gas.KEY: Boyle's law MSC: 3

17. ANS: C

Using Charles’s law, .

FeedbackA First, convert the temperature to Kelvin. Then, use Charles's law.B The value of T2 in Charles's law is 307, and not 297.C Correct!D The pressure is constant, so do not include 2.27 atm in the calculation.

PTS: 1 DIF: 3 REF: Page 423

OBJ: 14.1.2 Apply the three gas laws to problems involving the pressure, temperature, and volume of a gas.NAT: UCP.1 | UCP.3 | B.4TOP: Apply the three gas laws to problems involving the pressure, temperature, and volume of a gas.KEY: Charles's law MSC: 3

18. ANS: A PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 | UCP.3 | B.3 STA: P4.p2A | P4.p2C

19. ANS: A PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 | B.3 STA: C4.7a | C4.7b

20. ANS: A PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 | UCP.3 STA: C4.7a | C4.7b

21. ANS: C PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 | UCP.3 STA: P4.p2A | P4.p2C

22. ANS: C PTS: 1 DIF: Bloom's Level 1NAT: B.3 STA: C3.4g | C4.5b

23. ANS: B PTS: 1 DIF: Bloom's Level 3NAT: UCP.2 | B.3 STA: C4.7a | C4.7b

24. ANS: B PTS: 1 DIF: Bloom's Level 2NAT: B.3 | B.6 STA: C2.3a | C2.3b

25. ANS: C PTS: 1 DIF: Bloom's Level 2NAT: UCP3 | B.3 | B.6 STA: C5.r1a | C5.r1b

26. ANS: D PTS: 1 DIF: Bloom's Level 2NAT: UCP.4 | B.3 STA: C5.3a | C5.3b

27. ANS: B PTS: 1 DIF: Bloom's Level 3NAT: UCP.2 | UCP.4 | B.3 STA: C3.1b | C5.3b

28. ANS: BA catalyst speeds up a reaction, but it does so equally in both directions.

FeedbackA As the volume of nitrogen decreases, the concentration of ammonia decreases.B Correct!C As the pressure of ammonia increases, the concentration of ammonia increases.D As the temperature decreases, the concentration of ammonia increases.

PTS: 1 DIF: 2 REF: Page 572OBJ: 18.2.1 Describe how various factors affect chemical equilibrium.NAT: UCP.4 | B.3 TOP: Describe how various factors affect chemical equilibrium.KEY: Factors affecting chemical equilibrium MSC: 2

29. ANS: DAn increase in the volume implies a decrease in pressure. The number of moles of gaseous reactants (PCl5) is one and the number of moles of products (PCl3 and Cl2) is two. There is a net increase of one mole. On applying Le Chatelier’s principle, the shifting of equilibrium to the right will release the stress of decreased pressure.

FeedbackA The number of moles of the reactants is equal to the number of moles of the product.

Such reactions are not affected by the change in pressure or volume.B The number of moles of the gaseous reactants is three, which is more than the number

of moles of gaseous products (two). According to Le Chatelier's principle, in such reactions, the equilibrium will shift to the left at high pressure or low volume.

C The number of moles of the gaseous reactants is two, which is more than the number of moles of gaseous product (one). According to Le Chatelier's principle, in such reactions, the equilibrium will shift to the left at high pressure or low volume.

D Correct!

PTS: 1 DIF: 2 REF: Page 571OBJ: 18.2.2 Explain how Le Chatelier's principle applies to equilibrium systems.NAT: UCP.2 | UCP.4 | B.3TOP: Explain how Le Chatelier's principle applies to equilibrium systems.KEY: Le Chatelier's principle MSC: 2

30. ANS: BApplying Le Chatelier’s principle, when chlorine is added to the equilibrium mixture, the equilibrium shifts to the left. Thus, more heat is absorbed and the temperature decreases.

FeedbackA Addition of chlorine increases the rate of backward reaction.B Correct!C More chlorine is consumed.D An increase in the rate of backward reaction affects the temperature.

PTS: 1 DIF: 2 REF: Page 571OBJ: 18.2.2 Explain how Le Chatelier's principle applies to equilibrium systems.NAT: UCP.2 | UCP.4 | B.3TOP: Explain how Le Chatelier's principle applies to equilibrium systems.KEY: Le Chatelier's principle MSC: 2

31. ANS: A PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 | B.3 | B.6 STA: C5.r7i | C5.7E

32. ANS: A PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 | B.2 | B.3 STA: C5.r7i | C5.7f

33. ANS: C PTS: 1 DIF: Bloom's Level 3NAT: UCP.3 | B.2 STA: C5.7g | C5.7D

34. ANS: A PTS: 1 DIF: Bloom's Level 2NAT: UCP.2 | B.2 STA: C5.7f | C5.r7i

35. ANS: A PTS: 1 DIF: Bloom's Level 3NAT: UCP.3 STA: C5.7g | C5.7D

36. ANS: B PTS: 1 DIF: Bloom's Level 3NAT: UCP.3 STA: C5.7g | C5.7D

37. ANS: C PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 STA: C5.7B | C5.7D

38. ANS: BpH –log [H ]

FeedbackA The pH of the solution is the negative logarithm of the hydrogen ion concentration.B Correct!C Calculate the pH by taking the negative logarithm of the hydrogen ion concentration.D Use the formula, pH = -log (hydrogen ion concentration), to calculate pH of the

solution.

PTS: 1 DIF: 1 REF: Page 610OBJ: 19.3.3 Calculate the pH and pOH of the aqueous solution.NAT: B.2 | B.3 TOP: Calculate the pH and pOH of the aqueous solution.KEY: pH MSC: 3

39. ANS: D PTS: 1 DIF: Bloom's Level 2NAT: B.1 | B.3 | B.6 STA: C5.6a | C5.2A

40. ANS: B PTS: 1 DIF: Bloom's Level 2NAT: UCP.3 | B.3 STA: C5.6a | C5.2A

41. ANS: B PTS: 1 DIF: Bloom's Level 2NAT: UCP.2 | B.3 STA: C5.6a | C5.6c

42. ANS: B PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 STA: C5.6a | C5.6c

43. ANS: A PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 | B.2 STA: C5.6e | C5.6a

44. ANS: A PTS: 1 DIF: Bloom's Level 1NAT: UCP.2 | B.1 | B.2 | B.3 | B.6 STA: C5.8A | C5.8B

45. ANS: C PTS: 146. ANS: B PTS: 147. ANS: B PTS: 148. ANS: C PTS: 149. ANS: A PTS: 150. ANS: D PTS: 151. ANS: B PTS: 152. ANS: D PTS: 153. ANS: A PTS: 154. ANS: A PTS: 155. ANS: B PTS: 156. ANS: B PTS: 157. ANS: C PTS: 158. ANS: D PTS: 159. ANS: B PTS: 160. ANS: B PTS: 161. ANS: A PTS: 162. ANS: D PTS: 163. ANS: C PTS: 164. ANS: C PTS: 165. ANS: A PTS: 166. ANS: D PTS: 167. ANS: B PTS: 168. ANS: A PTS: 169. ANS: B PTS: 170. ANS: A PTS: 171. ANS: B PTS: 172. ANS: B PTS: 173. ANS: A PTS: 174. ANS: C PTS: 175. ANS: D PTS: 1

76. ANS: C PTS: 177. ANS: B PTS: 178. ANS: A PTS: 179. ANS: A PTS: 180. ANS: D PTS: 181. ANS: C PTS: 182. ANS: B PTS: 183. ANS: A PTS: 184. ANS: C PTS: 185. ANS: A PTS: 186. ANS: B PTS: 187. ANS: B PTS: 188. ANS: A PTS: 189. ANS: D PTS: 190. ANS: A PTS: 191. ANS: C PTS: 192. ANS: B PTS: 193. ANS: B PTS: 194. ANS: A PTS: 195. ANS: D PTS: 196. ANS: A PTS: 197. ANS: B PTS: 198. ANS: D PTS: 1

SHORT ANSWER

99. ANS:.18 mol

Use ideal gas law.PV = nRTn = PV/RT

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3 | B.1STA: C4.6a | C4.5b

100. ANS:1.94 x 103 J

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3STA: C3.1c | C3.1d

101. ANS:specific heat

PTS: 1 DIF: Bloom's Level 2 NAT: UCP.2STA: C3.1c | C3.1d

102. ANS:endothermic, exothermic

PTS: 1 DIF: Bloom's Level 2 NAT: UCP.S | B.3STA: C3.4A | C3.4f

103. ANS:Keq = [D]7[E]6 / [A]3[B]1[C]1

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3 | UCP.4STA: C5.3b | C5.3c

104. ANS:3.16 x 10-10

[H] = Kw / [OH]

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3 | A.1STA: C5.7g | C5.7D

105. ANS:pH = 8.06pH = -log[H]

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3 | A.1STA: C5.7g | C5.7D

106. ANS:pH=11.3

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3STA: C5.7g | C5.7D

107. ANS:[H] = 1.54 x 10-14

[H] = Kw / [OH]

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3STA: C5.7g | C5.7D

108. ANS:3.2 x 10-9

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.3STA: C5.7g | C5.7D

109. ANS:

PTS: 1 DIF: Bloom's Level 3 NAT: UCP.2 | UCP.3 | B.3STA: C5.6a | C5.6b

110. ANS:

Cu(s) + 2NO3–(aq) + 4H+(aq) Cu2+(aq) + 2NO2(g) + 2H2O(l)

PTS: 1 DIF: 2 REF: Page 646OBJ: 20.2.3 Balance net ionic redox equations by the oxidation-number method.NAT: UCP.3 | B.1 | B.2 | B.3TOP: Balance net ionic redox equations by the oxidation-number method.KEY: Oxidation-number method MSC: 2

111. ANS:heat it, stir it, crush the solid

PTS: 1

PROBLEM

112. ANS:3.9 atm

PTS: 1 DIF: 1 REF: Page 391OBJ: 13.1.3 Explain how gas pressure is measured and calculate the partial pressure of a gas.NAT: UCP.3 | B.4TOP: Explain how gas pressure is measured and calculate the partial pressure of a gas.KEY: Dalton's law MSC: 3NOT: The total pressure is the sum of the partial pressures of the two gases.

113. ANS:4.22 L

PTS: 1 DIF: 2 REF: Page 428OBJ: 14.2.2 Apply the combined gas law to problems involving pressure, temperature, and volume of a gas.NAT: UCP.1 | UCP.3 | B.2 | B.4TOP: Apply the combined gas law to problems involving pressure, temperature, and volume of a gas.KEY: The combined gas law MSC: 3NOT: Determine the volume of the gas by using the combined gas law principle. The combined gas law equation is V2 = [V1*P1*(T2+273)]/ [P2*(T1+273)].

114. ANS:75 K–198°C

PTS: 1 DIF: 2 REF: Page 434OBJ: 14.3.1 Relate the amount of gas present to its pressure, temperature, and volume by using the ideal gas law. NAT: UCP.1 | UCP.3 | B.4TOP: Relate the amount of gas present to its pressure, temperature, and volume by using the ideal gas law.KEY: Ideal gas law MSC: 3NOT: According to the ideal gas law equation, PV = nRT.

115. ANS:3.56 103 J

PTS: 1 DIF: 2 REF: Page 497OBJ: 16.2.1 Describe how a calorimeter is used to measure energy absorbed or released.NAT: B.5 | B.6 TOP: Describe how a calorimeter is used to measure energy absorbed or released.KEY: Calorimeter MSC: 3NOT: Absorbed heat = mass of substance * specific heat of substance * (final temperature - initial temperature).

116. ANS:

PTS: 1 DIF: 1 REF: Page 563OBJ: 18.1.2 Write equilibrium expressions for systems that are at equilibrium.NAT: UCP.4 | B.3 TOP: Write equilibrium expressions for systems that are at equilibrium.KEY: Equilibrium expression MSC: 3NOT: Equilibrium expression is the ratio of the concentration of products to the concentration of the reactants.

117. ANS:

NaOH + HCl NaCl + H2O

PTS: 1 DIF: 1 REF: Page 617OBJ: 19.4.1 Write chemical equations for neutralization reactions.NAT: B.3 TOP: Write chemical equations for neutralization reactions.KEY: Neutralization reaction MSC: 2NOT: When an acid reacts with a base, salt and water are produced. This reaction is called neutralization reaction.

118. ANS:3.2 10–9 M

PTS: 1 DIF: 2 REF: Page 613OBJ: 19.3.2 Relate pH and pOH to the ion product constant for water.NAT: B.2 | B.3 TOP: Relate pH and pOH to the ion product constant for water.KEY: Ion product constant for water MSC: 3NOT: Concentration of hydrogen ion = antilog (-pH), concentration of hydroxide ion = ion product constant for water/concentration of hydrogen ion.

119. ANS:1.7

PTS: 1 DIF: 1 REF: Page 614OBJ: 19.3.3 Calculate the pH and pOH of the aqueous solution.NAT: B.2 | B.3 TOP: Calculate the pH and pOH of the aqueous solution.KEY: pH | pOH MSC: 3NOT: For strong monoprotic acid (HCl), the concentration of acid is the concentration of hydrogen ion. pH = -log (concentration of hydrogen ion).