Chemical Reactions and Quantities, Matter and Energy, … 1406 Practice... · Chemical Reactions and Quantities, Matter and Energy, ... test bank associated with the Chemistry 1406

CHEM 1406 Practice Exam 2:

Chemical Reactions and Quantities, Matter and Energy, and Gases These questions taken from the web resources made available from San Diego Miramar College, a member of the San Diego

Community College District (SDCCD). Modifications have been made for clarity, to correct typos, and better align questions to TCC

curriculum. We thank the faculty of San Diego Miramar College for making this resource available to us. Other sources include the

test bank associated with the Chemistry 1406 Timberlake text.

I. Chemical Reactions and Quantities

Select the best answer to each of the following questions:

1. Predict the missing product in the following unbalanced equation. Mg + N2 → ___

A) MgN

B) Mg3N

C) Mg2N

D) Mg3N2

E) none of the above

2. Which reaction below gives a balanced equation such that the sum of the coefficients equals 10?

A) HCl(aq) + Cr(s) → CrCl3(s) + H2(g)

B) FeCl3(s) + Na2CO3(aq) → Fe2(CO3)3(aq) + NaCl(aq)

C) PbS(aq) + H2O2(aq) → PbSO4(aq) + H2O (l)

D) C4H10(l) + O2(g) → CO2(g) + H2O(l)


3. Which equation below violates the law of conservation of mass?

A) 2CaCO3 → 2CO2 + 2CaCO

B) 4H2 + 2O2 → 4H2O

C) 2HCl + Na2OH → HOH + 2NaCl

D) AgCl + NaNO3 → AgCl + NaNO3

E) all of these

4. Which reaction below gives a balanced equation such that the sum of the coefficients of the reactants

equals 5?

A) C5H10(l) + O2(g) → CO2 (g) + H2O (l)

B) CoCl3(s) + CaCO3 (aq) → Co2(CO3)3(aq) + CaCl2(aq)

C) PbSO4(aq) + H2O(l) → PbS(aq) + H2O2(aq)

D) HBr(aq) + Cr(s) → CrBr3(s) + H2(g)


5. In a combustion reaction, which of the following is not a product?

A) oxygen

B) water

C) carbon dioxide

D) energy

E) all of these are products of a combustion reaction.

6. What is the sum of the coefficients on H2O and H3PO3 in the following equation when balanced?

__PCl3 + __H2O → __H3PO3 + __HCl

A) 2

B) 3

C) 4

D) 6


7. What is the sum of the coefficients on Fe2S3 and HCl in the following equation when balanced?

__FeCl3 + __H2S → __Fe2S3 + __HCl

A) 23

B) 5

C) 6

D) 7


8. What is the sum of all the coefficients after the following equation is balanced?

__CO2 + __H2O → __C6H12O6 + __O2

A) 4

B) 24

C) 18

D) 19


9. Which of the following gives the balanced equation for this reaction?

__K3PO4 + __Ca(NO3)2 → __Ca3(PO4)2 + __KNO3

A) KPO4 + CaNO3 + KNO3

B) K3PO4 + Ca(NO3)2 → Ca3(PO4)2 + 3KNO3

C) 2K3PO4 + Ca(NO3)2 → Ca3(PO4)2 + 6KNO3

D) 2K3PO4 + 3Ca(NO3)2 → Ca3(PO4)2 + 6KNO3

E) K3PO4 + Ca(NO3)2 → Ca3(PO4)2 + KNO3

10. What is the sum of the coefficients when the following equation is balanced?

__ FeCl3 + __ AgNO3 → __ Fe(NO3)3 + __ AgCl

A) 3

B) 4

C) 6

D) 8


11. The following reaction takes place when an electric current is passed through water. It is an

example of a __________ reaction.

2 H2O → 2H2 + O2

A) combination

B) single replacement

C) dehydration

D) decomposition

E) double replacement

12. Which of the following is an oxidation-reduction reaction?

A) CaCl2 + Na2SO4 → CaSO4 + 2NaCl

B) KOH + HNO3 → H2O + KNO3

C) N2 + O2 → 2NO

D) AgNO3 + NaCl → AgCl + NaNO3

E) Al2(SO4)3 + 6KOH → 2 Al(OH)3 + 3K2SO4

13. What is oxidized and what is reduced in the following reaction?

2Al(s) + 3Br2 (g) → 2AlBr3(s)

A) Al is oxidized and Br2 is reduced.

B) AlBr3 is reduced and Br2 is oxidized.

C) Al is reduced and Br2 is oxidized.

D) AlBr3 is reduced and Al is oxidized.

E) AlBr3 is oxidized and Al is reduced.

14. Which of the following describes an oxidation reaction?

A) loss of electrons or loss of oxygen

B) loss of electrons or gain of oxygen

C) loss of electrons or gain of hydrogen

D) gain of electrons or gain of oxygen

E) gain of electrons or loss of H

15. What is the formula weight of beryllium sulfate?

A) 41.0

B) 57.0

C) 105.0

D) 106.8


16. Avogadro's number is the number of

A) particles in 1 mole of a substance.

B) amu in 1 mole of a substance.

C) grams in 1 mole of a substance.

D) moles in 6.02 × 1023

grams of an element.

E) moles in 6.02 × 1023

amu of an element.

17. One mole of helium gas weighs

A) 1.00 g.

B) 2.00 g.

C) 3.00 g.

D) 4.00 g.

E) 8.00 g.

18. What is the molar mass of Mg3(PO4)2, a substance formerly used in medicine as an

antacid?

A) 71.3 g

B) 118.3 g

C) 150.3 g

D) 214.3 g

E) 262.9 g

19. Which amount has the smallest mass?

A) 1.25 mol Na

B) 0.236 mol Mg

C) 0.11 mol Ba

D) 3.75•1022

atoms Se

E) all of the above have the same mass.

20. What is the mass of a thimble of water which contains 4.0•1021

molecules?

A) 1.2 g

B) 1.2•10-8

g

C) 12 g

D) 0.12 g


21. State the mass of oxygen atoms (grams) in one mole of C7H5NO3S (saccharin):

A) 16 g

B) 48 g

C) 183.0 g

D) 32 g


22. The compound MgSO4 is called Epsom salt. What mass is needed to prepare a bath with 5.000 mole of

Epsom salt?

A) 0.04156g

B) 24.06g

C) 120.3g

D) 601.5 g


23. How many molecules of TNT, C7H5N3O6 (Mol. Wt. = 227.0 g/mol ) are in 5.8 moles of TNT?

A) 3.5•1024

B) 21

C) 1.3•103

D) 121


24. Calculate the number of moles of aspirin, C9H8O4, in a 8.0 g tablet.

A) 4.4•10-2

mol

B) 4.6•10-3

mol

C) 4.9 mol

D) 0.022 mol


25. A typical cholesterol deposit in an artery might have a mass of 3.9 mg of cholesterol (C27H46O). How

many molecules of cholesterol are in this mass?

A) 1.01•10-2

B) 1.01•10-5

C) 6.1•1018

D) 6.1•1021


26. Which chemical has a molar mass of 180 g/mol?

A) KI

B) NH3

C) C2Cl6

D) C6H12O6


27. How many grams of N2 will be required to completely react with 9.3 g of H2 in the reaction:

N2 + 3H2 → 2NH3

A) 1.3•102

B) 2.0

C) 43

D) 3.9•102


28. How many moles of Al are needed to react with 2.5 mol of Fe2O3 in the equation:

2Al + Fe2O3 → Al2O3 + 2Fe

A) 135

B) 2.0

C) 5.0

D) 1.25

E) no answer

29. The number of grams of K2O produced from the oxidation of 4.0 grams of K in the reaction:

K(s) + O2 (g) → K2O (g) (Unbalanced)

A) 4.8 g

B) 4.0 g

C) 9.4 g

D) 6.3 g


30. Tungsten W, is produced from tungsten(VI) oxide according to the following unbalanced equation:

__WO3(s) + __H2(g) → __W(s) + __H2O(l).

How many grams of tungsten metal could you produce from 36.0 g of tungsten(VI) oxide?

MWt: WO3= 231.9 g/mol, W = 183.9 g/mol, H2 = 2.0 g/mol, H2O = 18.0 g/mol

A) 183.9 g

B) 45.4 g

C) 28.5 g

D) 1.59 g


31. How many molecules of water, H2O, are present in 75.0 g of H2O?

A) 75.0 molecules

B) 4.17 molecules

C) 7.53 × 1024

molecules

D) 2.51 × 1024

molecules

E) 5.02 × 1024

molecules

For questions #32-34, consider the following equation.

2Mg + O2 → 2MgO

32. The number of moles of oxygen gas needed to react with 4.0 moles of Mg is

A) 1.0 mole

B) 2.0 moles

C) 3.0 moles

D) 4.0 moles

E) 6.0 moles

33. The number of moles of MgO produced when 6.4 g of O2 reacts completely is

A) 0.10 mole

B) 0.20 mole

C) 0.40 mole

D) 0.60 mole

E) 0.80 mole

34. How many grams of O2 will be consumed to make 2.35 mol MgO?

A) 37.6 g B) 150. g C) 0.932 g D) 1.18 g E) 16.0 g

35. How many grams of NO are required to produce 145 g of N2 in the following reaction?

4NH3(g) + 6NO(g) → 5N2 (g) + 6H2O(l)

A) 186 g

B) 155 g

C) 125 g

D) 129 g

E) 145 g

36. The __________ is the minimum energy needed for a chemical reaction to begin.

A) reaction energy

B) activation energy

C) energy of reactants

D) energy of products

E) heat of reaction

Use the labeled diagram below to answer questions 38-40.

37. In the above labeled diagram, which of the following choices best describes the region labeled “A”?

A) heat of reaction B) activation energy C) energy of reactants D) energy of products

38. In the above labeled diagram, which of the following choices best describes the region labeled “B”?


39. In the above labeled diagram, which of the following choices best describes the region labeled “C”?


40. The reaction shown in the above labeled diagram can best be classified as a(n) __________.

A) endothermic reaction

B) exothermic reaction

C) oxidation-reduction reaction

D) catalyzed reaction

E) decomposition reaction

II. Matter and Energy

Select the best answer to each of the following questions. Some useful constants and relationships are listed

below.

Energy Values for Food

Carbohydrates 17 kJ/g or 4.0 cal/g

Protein 17 kJ/g or 4.0 cal/g

Fat 38 kJ/g or 9.1 cal/g

41. Which of the following is a property of a solid?

A) It takes the shape of the container.

B) It fills the volume of the container.

C) The particles move at a rapid rate.

D) The interactions between its particles are very weak.

E) The particles have fixed positions and are very close together.

42. Which of the following is a physical property of both liquids and gases?

A) has its own shape.

B) has a definite volume.

C) has strong interactions between its particles

D) has randomly arranged particles

E) has large spaces between molecule

43. The physical state(s) present when a substance is melting is (are)

A) solid

B) liquid

C) gas

D) solid + liquid

E) liquid + gas

44. The formation of a gas resulting from the escape of high-energy particles from the surface of a liquid is

known as _______.

A) evaporation

B) deposition

C) boiling

D) melting

E) sublimation

Constants for Water

specific heat of water 4.184𝐽

𝑔∙℃ 𝑜𝑟 1.00

𝑐𝑎𝑙

𝑔∙℃

specific heat of ice 2.05𝐽

𝑔∙℃ 𝑜𝑟 0.49

𝑐𝑎𝑙

𝑔∙℃

specific heat of steam 2.00𝐽

𝑔∙℃ 𝑜𝑟 0.48

𝑐𝑎𝑙

𝑔∙℃

heat of fusion 334𝐽

𝑔 𝑜𝑟 80.

𝑐𝑎𝑙

𝑔

heat of vaporization 2260𝐽

𝑔 𝑜𝑟 540

𝑐𝑎𝑙

𝑔

45. When a solid is converted directly to a gas, the change of state is called

A) freezing

B) melting

C) boiling

D) condensation

E) sublimation

46. Air is a(n)

A) compound.

B) heterogeneous mixture.

C) element.

D) homogeneous mixture.

E) None of the above.

47. A vinaigrette salad dressing is best described as a(n)

A) compound

B) heterogeneous mixture

C) suspension

D) homogeneous mixture

E) colloid

48. The primary substances of which all other things are composed are

A) molecules

B) compounds

C) elements

D) electrons

E) protons

49. Which of the following is a physical change?

A) Baking a cake

B) Dry ice subliming

C) Fermenting grapes to produce wine

D) digesting a meal

E) a tomato ripening

50. Which of the following would NOT be a physical change?

A) tearing a piece of aluminum foil

B) boiling water for soup

C) burning gasoline in a lawnmower

D) melting gold to make jewelry

E) All of the above are physical changes.

51. The energy associated with the motion of particles in a substance is called

A) temperature

B) electrical energy

C) heat

D) chemical energy

E) potential energy

52. The phrase "ability to do work" is a definition of

A) specific heat

B) energy

C) calorie

D) heating

E) potential

53. The energy stored in the chemical bonds of a carbohydrate molecule can be classified as _________.

A) specific heat

B) kinetic energy

C) potential energy

D) work

E) a calorie

54. In which of the following would the particles move most rapidly?

A) ice at -20 °C

B) water at 20 °C

C) steam at 110 °C

D) boiling water

E) ice at 0 °C

55. A patient has a temperature of 38.5 °C. What is the temperature in degrees Fahrenheit?

A) 70.5 °F

B) 311 °F

C) 126.9 °F

D) 101.3 °F

E) 11.7 °F

56. On a cold February morning in Green Bay, WI, the temperature is about -7.5˚F. What would that

temperature be in Kelvins?

A) -22 K

B) 266 K

C) 287 K

D) 251 K

E) 344 K

57. How many calories are required to convert 17 g of ice at 0.0 °C to liquid water at 32.0 °C? The heat of

fusion of water is 80. cal/g.

A) 43 000 cal

B) 540 cal

C) 1900 cal

D) 1400 cal

E) 80. cal

58. How many joules are required to raise the temperature of a 35.0 g sample of iron from 25 °C to 35 °C?

Iron has a specific heat of 0.452 J/g °C.

A) 158 J

B) 4.52 J

C) 350 J

D) 15.8 J

E) 170 J

59. The number of joules needed to raise the temperature of 32 g of water from 12 °C to 54 °C is _______.

The specific heat of water is 4.184 J/(g˚C).

A) 1600 J

B) 5600 J

C) 1300 J

D) 180 J

E) 5.6 J

60. How many kilocalories of heat would be equivalent to 387 kJ of heat?

A) 92500 kcal

B) 92.5 kcal

C) 1620 kcal

D) 1.620 kcal

E) 387000 kcal

61. How many calories are required to raise the temperature of a 150. g sample of gold from 25

°C to 175 °C? The specific heat of gold is 0.0308 cal/g °C.

A) 4.62 cal

B) 116 cal

C) 22500 cal

D) 693 cal

E) 130 cal

62. For the heating cooling curve shown, which letter labels the line segment that corresponds being in the

liquid state?

A) a

B) b

C) c

D) d

E) ab

63. The heat of vaporization for water is 540 cal / g and the heat of fusion for water is 80 cal/ g. How much

energy is required to take 5.0 grams of ice at 0°C to 100°C liquid water?

A) 180 cal

B) 500 cal

C) 900 cal

D) 3600 cal


64. A 2.5 g sample of french fries is placed in a calorimeter with 500.0 g of water at an initial temperature of

21 °C. After combustion of the french fries, the water has a temperature of 48 °C. What is the caloric value

(kcal/g) of the french fries?

A) 14 kcal / g

B) 11 kcal / g

C) 0.14 kcal / g

D) 4.2 kcal / g

E) 5.4 kcal / g

65. A serving of fish contains 50 g of protein and 4 g of fat. If protein has a caloric value of 4.0 kcal/g and

fat has 9.1 kcal/g, how many kcal are in the serving?

A) 240 kcal

B) 54.0 kcal

C) 470 kcal

D) 220 kcal

E) 486 kcal

66. A diet has a total caloric intake of 1400 kcal. The diet consists of 50.% carbohydrate, 35% protein, and

15% fat. The number of grams of protein in the diet is approximately…

A) 175 g

B) 300 g

C) 53 g

D) 115 g

E) 123 g

67. The dietary calorie (Cal) is equal to

A) 1000 kcal

B) 1000 cal

C) 100 cal

D) 10 cal

E) 1 cal

68. What is the energy content in kJ for a piece of chocolate cake that contains 34 g of carbohydrate, 10 g of

fat, and 5 g of protein? Round the answers of kJ to the tens place.

A) 820 kJ

B) 2430 kJ

C) 590 kJ

D) 1040 kJ

E) 1150 kJ

69. A 2.3-g sample of butter, a fat, is placed in a calorimeter containing 1900 g of water at an initial

temperature of 17 °C. After the complete combustion of the butter, the water has a temperature of 28 °C.

Assume that the energy absorbed by the calorimeter is negligible. What is the energy value (kJ/g) of butter?

A) 9.1 kJ / g

B) 21 kJ / g

C) 87 kJ / g

D) 38 kJ / g


70. Suppose you go out to dinner, and you order the prime rib (24 g protein, 0 carbohydrate, 10 g fat), a

baked potato with no goodies (2 g protein, 26 g carbohydrate, 0 g fat), a serving of broccoli (5 g protein, 10 g

carbohydrate, 5 g fats), black coffee (0 g protein, 1 g carbohyudrate, 0 g fat), and a piece of carrot cake with

cream cheese icing (5 g protein, 53 g carbohydrate, 30 g fat). How many Calories did you have for dinner?

A) 171 Cal

B) 684 Cal

C) 1344 Cal

D) 909 Cal


III. Gases and the Gas Laws

Select the best answer to each of the following questions.

71. In a gas, the distance between the particles is

A) very close relative to the size of the molecules.

B) close relative to the size of the molecules.

C) fixed relative to the size of the molecules.

D) small relative to the size of the molecules.

E) very large relative to the size of the molecules.

72. Atmospheric pressure is the lowest at which location?

A) Denver, Colorado

B) San Diego, CA

C) Death Valley, CA

D) Manhattan, NY

E) all the same

73. Which law best explains the mechanism of breathing?

A) Avogadro’s Law

B) Gay-Lussac’s Law

C) Boyle’s Law

D) Charles’ Law

E) Natural Law

74. Which postulate from the kinetic molecular theory best explains why gas particles fill their container?

A) A gas consists of small particles that move randomly at high velocities.

B) The attractive forces between particles are often so small that they can be ignored.

C) Volume of gas molecules is negligible compared to the volume of the container.

D) The average kinetic energy of gas molecules is directly proportional to the Kelvin temperature.

E) All of the above.

f) A and B only.

75. Which of the following is NOT part of the kinetic theory of gases?

A) A gas is composed of very small particles.

B) Gas particles move rapidly.

C) There is very little empty space in a gas.

D) Gas particles do not attract or repel one another.

E) Gas particles move faster when the temperature increases.

76. The force caused by the collision of gas particles against the walls of a container is called

A) Pressure

B) Volume

C) Density

D) Quantity of gas

E) Temperature

77. The boiling point of water at sea level is 100 °C. At higher altitudes, the boiling point of water will be

A) lower, because temperatures are lower.

B) higher, because there are fewer water molecules in the air.

C) higher, because the altitude is greater.

D) lower, because the atmospheric pressure is lower.

E) the same, because water always boils at 100 °C.

78. The balloon is put into a chamber whose pressure is less than the atmospheric pressure with temperature

remaining constant. Which letter represents what the balloon will look like after it is put into the chamber?

A) A

B) B

C) C

D) Not enough information

E) The balloon’s size will not change since it still has the same amount of air.

79. A balloon’s temperature is changed from 50 °C to -150 °C at constant pressure. Which letter represents

what the balloon will look like after this temperature change?

A) A

B) B

C) C

D) Not enough information

E) The balloon’s size will not change since it still has the same amount of air.

80. The pressure exerted by a gas on its container is directly proportional to

A) the mass of the individual gas molecules.

B) the number of molecules of gas in the sample.

C) the centigrade temperature of the gas.

D) the Fahrenheit temperature of the gas.

E) the volume of the container.

81. A barometer is a device for measuring __________.

A) atmospheric pressure

B) blood pressure

C) gas pressure in a container

D) gas pressure in the lung

E) vapor pressure

82. If a 1.5 liter flask at 1 atm and 25ºC contains 7.0 mol of carbon dioxide gas, how many moles of nitrogen

will the same size flask contain if the temperature and pressure remain constant?

A) 4.5 mol

B) 1 mole

C) 7.0 mol

D) 14.0 mol

E) Cannot be determined

83. A balloon which contains 0.250 mol of gas and has a volume of 11.2 liters has a pressure of 380. mm

Hg. What will the volume be if the pressure is increased to 1.50 atm [1 atm = 760 mm Hg, R = 0.0821

(L•atm/ mol•K).]

A) 3.73 L

B) 33.6 L

C) 2840 L

D) 5.60 L


84. Determine the volume (L) of 0.350 mol of O2 at STP.

A) 1.46•10-2

L

B) 7.84 L

C) 11.2 L

D) 8.55 L


85. What is the molecular weight of a gas which weighs 6.40 g, at STP and occupies a volume of 4.48 liters.

A) 32.0 g/mol

B) 16 g/mol

C) 1.43 g/mol

D) 0.700 g/mol

E) Cannot be determined

86. A gas sample contains 4.0 g of CH4 and 2.0 g of He. What is the volume of the sample at STP?

A) 17 L

B) 30. L

C) 5.6 L

D) 11 L

E) 130 L

87. An anesthesiologist administers a gas at 20° C to a patient whose body is 37° C. What is the change in

volume (L) of a 1.20 L sample of gas as it goes from room temperature to body temperature?

A) 1.27 L

B) 0.788 L

C) 2.22 L

D) 1.20 L

E) 0.070 L

88. Which combination of changes would produce no change in the pressure of a gas.

Volume Temperature number of moles

A) double no change half

B) half no change double

C) double double no change

D) no change half half

E) no change double no change

89. What unit of temperature must be used in gas law calculations?

A) degrees Fahrenheit

B) degrees Celsius

C) Kelvin

D) either degrees Celsius or degrees Fahrenheit

E) either degrees Celsius or Kelvin

90. The volume of a sample of gas, initially at 25 °C, increases from 158 mL to 450. mL. What is the final

temperature of the sample of gas, if the pressure in the container is kept constant?

A) 8.8 °C

B) 71 °C

C) -168 °C

D) 105 °C

E) 576 °C

91. In Gay-Lussac's Law, the pressure of a gas increases due to an increase in temperature because

A) the molecules strike the walls of the container less often.

B) the molecules strike the walls of the container more often.

C) the molecules get bigger.

D) there is a decrease in the volume of the container.

E) there is an increase in the number of gas particles.

92. What is the pressure in a 10.0 L container of O2 at a T = 87.0°C if the same gas sample only occupied

4.50L at 2.00 atm and 10.0˚C?

A) 0.708 atm

B) 5.65 atm

C) 1.14 atm

D) 7.83 atm


93. A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C.

What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atm and the

temperature is 27 °C?

A) 1100 mL

B) 580 mL

C) 110 mL

D) 100 mL

E) 630 mL

94. A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the

mixture is 330 mmHg and the partial pressure of the oxygen is 1.0 atm, what is the total pressure of the

mixture in torr?

A) 330 torr

B) 1090 torr

C) 430 torr

D) 760 torr

E) 1.4 torr

95. If atmospheric pressure on a certain day is 749 mmHg, what is the partial pressure of nitrogen, given

that nitrogen is about 78.0% of the atmosphere?

A) 760 mmHg

B) 749 mmHg

C) 600 mmHg

D) 584 mmHg

E) 165 mmHg

96. A tank contains a mixture of helium, neon, and argon gases. If the total pressure in the tank is 490

mmHg and the partial pressures of helium and argon are 215 mmHg and 102 mmHg, respectively, what is

the partial pressure of neon?

A) 0.228 mmHg

B) 603 mmHg

C) 377 mmHg

D) 807 mmHg

E) 173 mmHg

97. A 1.20-L container contains 1.10 g of an unknown gas at STP. What is the molecular weight of the

unknown gas?

A) 20.5 g/mole

B) 1.32 g/mole

C) 0.917 g/mole

D) 22.4 g/mole

E) 1.10 g/mole

98. If a gas has a pressure of 12.54 atm and a volume of 22.4 L, what volume must the gas be for the

pressure to change to 2874 mmHg?

A) 0.0977 L

B) 5130 L

C) 6.75 L

D) 74.3 L


99. A container has oxygen gas collected over water at 15.0˚C. If the total pressure in the container is 685

torr, what is the partial pressure of oxygen in the container? (The vapor pressure of water is 12.8 torr at

15.0˚C.)

A) 672 torr

B) 698 torr

C) 700 torr

D) 713 torr

E) 649 torr

100. If a gas has a pressure of 2.54 atm at a temperature of 31.8oC, what must the temperature be changed

to for the pressure to become 395 mmHg?

A) 62.4 °C

B) -210.7 °C

C) 1490 °C

D) 1220 °C

E) -154.8 °C

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Chemical Reactions and Quantities, Matter and Energy, … 1406 Practice... · Chemical Reactions and Quantities, Matter and Energy, ... test bank associated with the Chemistry 1406