Second Semester Review Chapters 13-14

Chapter 13

51. A gas occupies a volume of 202 mL at a pressure of 505 torr. To what pressure must the gas be subjected in order to change the volume of 65.0 mL. Assume constant temperature.

a. 202 torr

b. 1300 torr

c. 1570 torr

d. 505 torr

e. 2400 torr

52. A balloon has a volume of 1.20L at 24.0 degrees Celsius. The balloon is heated to 48 degrees Celsius. Calculate the new volume of the balloon.

a. 1.20 L

b. 1.30 L

c. 1.70 L

d. 2.10 L

e. 2.40 L

53. A sample of helium gas occupies 2.65 L at 1.20 atm. What pressure would this sample of gas exert in a 1.50 L container at the same temperature?

a. 0.679 atm

b. 3.31 atm

c. 1.20 atm

d. 2.12 atm

54. A gas has a volume of 5.0 L at a certain pressure. How must the pressure be changed to double the volume of the gas at a constant temperature?

a. The pressure must be doubled.

b. The pressure must be halved.

c. The pressure must be quadrupled.

d. There is not enough information to decide.

55. A 6.5 L sample of nitrogen at 25 degrees Celsius and 1.5 atm is allowed to expand to 13.0 L. The temperature remain constant. What is the final pressure?

a. 0.063 atm.

b. 0.12 atm

c. 0.75 atm

d. 3.0 atm

e. 0.38 atm

56. A gas sample is held at constant pressure. The gas occupies 3.62 L of volume when the temperature is 21.6 degrees Celsius. Determine the temperature at which the volume of the gas is 3.45 L.

a. 309 K

b. 281 K

c. 20.6 K

d. 294 K

e. 326 K

57. The lowest possible temperature that can be reached is

a. 0 degrees Celsius.

b. 273 degrees Celsius.

c. 273 K

d. -273 degrees Celsius.

e. -273 K

58. If a temperature and pressure are held constant, the volume and number of moles of a gas are

a. independent of each other.

b. directly proportional.

c. inversely proportional.

d. equal.

59. One mole of CO2 at STP will occupy

a. 1.0 L

b. 22.4 L

c. 44 L

d. 44 g

e. 24.5 L

60. A mole of a gas at STP has a volume of 22.4 L. If the volume increases to 29.1 L and the pressure is changed to 813 torr, calculate the new temperature.

a. 461 K

b. 792 K

c. 379 K

d. 519 K

e. 226 K

61. What volume will 28.0 g of N2 occupy at STP?

a. 5.60 L

b. 11.2 L

c. 22.4 L

d. 44.8 L

62. Which conditions of P and T are most ideal for a gas?

a. high P, high T

b. high P, low T

c. low P, high T

d. low P, low T

63. Use the kinetic molecular theory of gases to predict what would happen to a close sample of a gas whose temperature increased while its volume decreased.

a. Its pressure would decrease.

b. Its pressure would increase.

c. Its pressure would hold constant.

d. The number of moles of the gas would decrease.

Chapter 14

64. Which of the following is most likely to be a solid at room temperature?

a. Na2S

b. HF

c. NH3

d. N2

e. H2O

65. Order the intermolecular forces (dipole-dipole, London Dispersion, Ionic, and Hydrogen Bonding) from weakest to strongest.

a. dipole-dipole, London dispersion, ionic, hydrogen bonding

b. London dispersion, dipole-dipole, London dispersion, ionic

c. hydrogen bonding, dipole-dipole, London dispersion, ionic

d. dipole-dipole, ionic, London dispersion, hydrogen bonding

e. London dispersion, ionic, dipole-dipole, hydrogen bonding

Identify the major attractive force in each of the following molecules.

66. N2

a. dipole-dipole

b. London dispersion

c. Ionic

d. Hydrogen Bonding

67. Na2S

a. dipole-dipole

b. London dispersion

c. Ionic

d. Hydrogen Bonding

68. NH3

a. dipole-dipole

b. London dispersion

c. Ionic

d. Hydrogen Bonding

69. H2S

a. dipole-dipole

b. London dispersion

c. Ionic

d. Hydrogen Bonding

70. At 1 atm of pressure and a temperature of 0 degrees Celsius, which phase(s) of H2O can exist?

a. Ice and water

b. Ice and water vapor

c. Water only

d. Water vapor only.

e. Ice only

71. The normal freezing point of water is

a. 0 degrees Fahrenheit

b. 273 K

c. 32 degrees Celsius

d. 373 degrees Celsius

72. The normal boiling point of water is

a. 0 degrees Fahrenheit

b. 32 degrees Fahrenheit

c. 273 K

d. 373K

73. The bonds between hydrogen and oxygen in a water molecule can be characterized as .

a. Hydrogen Bonds

b. London Forces

c. Intermolecular Forces

d. Intramolecular Forces

74. Calculate the quantity of energy required to change 3.00 mol of liquid water to steam at 100 degrees Celsius. The molar heat of vaporization of water is 40.6 kJ/mol.

a. 40.6 kJ

b. 13.5 kJ

c. 122 kJ

d. 300 kJ

75. Calculate the quantity of energy required to change 26.5g of liquid water to steam at 100 degrees Celsius. The molar heat of vaporization of water is 40.6kJ/mol.

a. 1.08 x 10^3 kJ

b. 59.8 kJ

c. 1.53 kJ

d. 27.6 kJ

76. The specific heat capacity of liquid water is 4.18 kJ/g °C. Calculate the quantity of energy required to heat 1.00 g of water from 26.5°C to 83.7°C.

a. 239 J

b. 57.2 J

c. 13.7 J

d. 350. J

77. The molar heat of fusion of water is 6.02 kJ/mol. Calculate the energy required to melt 3.00 mol of ice.

a. 6.02 kJ/mol

b. 12.0 kJ/mol

c. 18.1 kJ/mol

d. 2.01 kJ/mol

78. Choose the state of water in which the water molecules are farthest apart on average.

a. Steam (vapor)

b. Liquid

c. Ice (solid)

d. All the same.

79. The process of evaporation happens when which of the following occurs?

a. A solid becomes a liquid.

b. A liquid becomes a solid

c. A liquid becomes a gas.

d. A gas becomes a liquid.

e. A solid becomes a gas.

80. As the temperature of a liquid increases, the vapor pressure of the liquid generally…

a. increases

b. decreases

c. stays the same

d. depends on the type of intermolecular forces

81. As the atmospheric pressure around a liquid decreases, the boiling temperature of the liquid…

a. increases

b. decreases

c. stays the same

d. depends on the type of intermolecular forces

82. Which of the following is true for ionic solids dissolved in water?

a. The solution will conduct electricity.

b. The solution will dissolve into neutral molecules.

c. The solution will not conduct electricity.

d. The ions in solution will form a large crystal.

83. Which of the following has the highest melting temperature?

a. H2O

b. CO2

c. S8

d. MgF2

e. P4

84. Name the type of crystalline solid formed by potassium bromide.

a. Molecular Solid

b. Atomic Solid

c. Ionic Solid

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