Question 1

A block of dry ice (solid CO2, density = 1.56 g/mL)  of dimensions 25.0 cm × 25.0 cm × 25.0 cm is left to sublime (i.e., to pass from the solid phase to the gas phase)  in a closed chamber of dimensions 4.00 m × 5.00 m × 3.00 m.Once the sublimation is complete, what is the partial pressure of carbon dioxide in the chamber at 25°C? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg)

Accepted Answer

A)  172 mmHg
B)  107 mmHg
C)  0.225 mmHg
D)  0.172 mmHg
E)  14.4 mmHgF) B) and D)
G) B) and C)

Question 2

Determine the partial pressure of CO2 in a gas mixture composed of 782.4 grams of CO2 and 2.10 moles of CO.The mixture is at 703.3 K in a 25.8-liter container.

Accepted Answer

A)  4.70 atm
B)  44.5 atm
C)  39.8 atm
D)  22.4 atm
E)  17.8 atmF) B) and C)
G) C) and D)

Question 3

A 0.271-g sample of an unknown vapor occupies 294 mL at 140°C and 847 mmHg.The empirical formula of the compound is CH2.What is the molecular formula of the compound? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  CH2
B)  C2H4
C)  C3H6
D)  C4H8
E)  C6H12F) B) and D)
G) A) and E)

Question 4

A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass.A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at −4.0°C.What is its molecular formula? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  NO
B)  NO2
C)  N3O6
D)  N2O4
E)  N2O5F) A) and D)
G) A) and E)

Question 5

A sample of hydrogen gas exerts a pressure of 466 torr in a container.What is this pressure in atmospheres? (1 atm = 1.01325 ×105 Pa = 760 torr)

Accepted Answer

A)  0.217 atm
B)  0.466 atm
C)  0.613 atm
D)  1.63 atm
E)  4.60 atmF) A) and D)
G) D) and E)

Question 6

What is the final temperature of a gas that expands from a volume of 22.4 L at 278 K to a volume of 38.3 L?

Accepted Answer

A)  163 K
B)  294 K
C)  3.09 K
D)  217 K
E)  475 KF) A) and B)
G) A) and E)

Question 7

What is the density of CO2(g)  at 100.°C and 10.0 atm pressure? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  1.44 g/L
B)  134 g/L
C)  44.0 g/L
D)  53.6 g/L
E)  14.4 g/LF) B) and E)
G) B) and D) E

Question 8

What is the volume occupied by 35.2 g of methane gas (CH4)  at 25°C and 1.0 atm? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  0.0186 L
B)  4.5 L
C)  11.2 L
D)  49.2 L
E)  53.7 LF) B) and C)
G) C) and D) E

Question 9

"The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of __________________ law.

Accepted Answer

A)  Charles's
B)  Boyle's
C)  Amontons's
D)  Avogadro's
E)  Gay-Lussac'sF) All of the above
G) A) and B)

Question 10

"The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure" is a statement of _____________ law.

Accepted Answer

A)  Charles's
B)  Boyle's
C)  Dalton's
D)  Avogadro's
E)  Gay-Lussac'sF) None of the above
G) B) and E) D

Question 11

A flask with a volume of 3.16 L contains 9.33 g of an unknown gas at 32.0°C and 1.00 atm.What is the molar mass of the gas? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  7.76 g/mol
B)  66.1 g/mol
C)  73.9 g/mol
D)  81.4 g/mol
E)  144 g/molF) A) and C)
G) C) and E)

Question 12

If the atmospheric pressure in Denver is 0.8800 atm, what is this pressure expressed in mmHg? (1 atm = 101,325 Pa = 760 torr, 1 torr = 1 mmHg) ?

Accepted Answer

A)  151.5 mmHg
B)  1.16× 10−3 mmHg
C)  863.6 mmHg
D)  8.92 × 104 mmHg
E)  668.8 mmHgF) None of the above
G) A) and B)

Question 13

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L.What volume will it occupy if the pressure is increased to 894 torr at constant temperature?

Accepted Answer

A)  22.3 L
B)  31.2 L
C)  44.9 L
D)  112 L
E)  380 LF) B) and E)
G) A) and E)

Question 14

If 2.3 mol of a gas occupies 50.5 mL, how many moles of the gas will occupy 85.5 mL at the same temperature and pressure?

Accepted Answer

A)  1.4 mol
B)  0.59 mol
C)  3.9 mol
D)  0.26 mol
E)  2.3 molF) A) and E)
G) A) and D)

Question 15

Which figure best represents the concept of pressure? (A sphere represents a gaseous atom.)

Accepted Answer

A)   
B)   
C)   
D)   E) C) and D)
F) A) and C)

Question 16

What is the mass, in grams, of 2.74 L of CO gas measured at 33°C and 945 mmHg? (R = 0.08206 L • atm/mol • K, 1 atm = 760 mmHg)

Accepted Answer

A)  0.263 g
B)  2.46 g
C)  3.80 g
D)  35.2 g
E)  206 gF) C) and D)
G) B) and C)

Question 17

What is the density of SF6(g)  at 27°C and 0.500 atm pressure? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)  3.38 × 10−3 g/L
B)  2.97 g/L
C)  22.4 g/L
D)  32.9 g/L
E)  3.38 kg/LF) None of the above
G) A) and E)

Question 18

Determine the mole fraction of CO in a gas mixture composed of 782.4 grams of CO2 and 2.10 moles of CO.The mixture is at 703.3 K in a 25.8-liter container.

Accepted Answer

A)  0.11
B)  0.89
C)  17.8
D)  0.48
E)  0.52F) None of the above
G) C) and E)

Question 19

The air pressure in a volleyball is 75 psi.What is this pressure in torr? (1 atm = 14.7 psi = 101,325 Pa = 760 torr) ?

Accepted Answer

A)  520 torr
B)  562 torr
C)  3900 torr
D)  7600 torr
E)  75,000 torrF) C) and D)
G) A) and B)

Question 20

A 7.75-L flask contains 0.482 g of hydrogen gas and 4.98 g of oxygen gas at 65°C.What is the partial pressure of oxygen in the flask?

Accepted Answer

A)  0.557 atm
B)  0.043 atm
C)  1.11 atm
D)  33.5 atm
E)  67 atmF) D) and E)
G) A) and B)

Exam 8: Gases

Correct Answer
verified

Determine the partial pressure of CO₂ in a gas mixture composed of 782.4 grams of CO₂ and 2.10 moles of CO.The mixture is at 703.3 K in a 25.8-liter container.

Correct Answer
verified

A 0.271-g sample of an unknown vapor occupies 294 mL at 140°C and 847 mmHg.The empirical formula of the compound is CH₂.What is the molecular formula of the compound? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass.A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at −4.0°C.What is its molecular formula? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

A sample of hydrogen gas exerts a pressure of 466 torr in a container.What is this pressure in atmospheres? (1 atm = 1.01325 ×10⁵ Pa = 760 torr)

Correct Answer
verified

What is the final temperature of a gas that expands from a volume of 22.4 L at 278 K to a volume of 38.3 L?

Correct Answer
verified

What is the density of CO₂(g) at 100.°C and 10.0 atm pressure? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified
E

What is the volume occupied by 35.2 g of methane gas (CH₄) at 25°C and 1.0 atm? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified
E

"The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of __________________ law.

Correct Answer
verified

"The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure" is a statement of _____________ law.

Correct Answer
verified
D

A flask with a volume of 3.16 L contains 9.33 g of an unknown gas at 32.0°C and 1.00 atm.What is the molar mass of the gas? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

If the atmospheric pressure in Denver is 0.8800 atm, what is this pressure expressed in mmHg? (1 atm = 101,325 Pa = 760 torr, 1 torr = 1 mmHg) ?

Correct Answer
verified

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L.What volume will it occupy if the pressure is increased to 894 torr at constant temperature?

Correct Answer
verified

If 2.3 mol of a gas occupies 50.5 mL, how many moles of the gas will occupy 85.5 mL at the same temperature and pressure?

Correct Answer
verified

Which figure best represents the concept of pressure? (A sphere represents a gaseous atom.)

Correct Answer
verified

What is the mass, in grams, of 2.74 L of CO gas measured at 33°C and 945 mmHg? (R = 0.08206 L • atm/mol • K, 1 atm = 760 mmHg)

Correct Answer
verified

What is the density of SF₆(g) at 27°C and 0.500 atm pressure? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Determine the mole fraction of CO in a gas mixture composed of 782.4 grams of CO₂ and 2.10 moles of CO.The mixture is at 703.3 K in a 25.8-liter container.

Correct Answer
verified

The air pressure in a volleyball is 75 psi.What is this pressure in torr? (1 atm = 14.7 psi = 101,325 Pa = 760 torr) ?

Correct Answer
verified

A 7.75-L flask contains 0.482 g of hydrogen gas and 4.98 g of oxygen gas at 65°C.What is the partial pressure of oxygen in the flask?

Correct Answer
verified

Exam 8: Gases

Correct AnswerverifiedShow Answer

Determine the partial pressure of CO2 in a gas mixture composed of 782.4 grams of CO2 and 2.10 moles of CO.The mixture is at 703.3 K in a 25.8-liter container.

Correct AnswerverifiedShow Answer

A 0.271-g sample of an unknown vapor occupies 294 mL at 140°C and 847 mmHg.The empirical formula of the compound is CH2.What is the molecular formula of the compound? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass.A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at −4.0°C.What is its molecular formula? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

A sample of hydrogen gas exerts a pressure of 466 torr in a container.What is this pressure in atmospheres? (1 atm = 1.01325 ×105 Pa = 760 torr)

Correct AnswerverifiedShow Answer

What is the final temperature of a gas that expands from a volume of 22.4 L at 278 K to a volume of 38.3 L?

Correct AnswerverifiedShow Answer

What is the density of CO2(g) at 100.°C and 10.0 atm pressure? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedE

What is the volume occupied by 35.2 g of methane gas (CH4) at 25°C and 1.0 atm? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedE

"The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of __________________ law.

Correct AnswerverifiedShow Answer

"The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure" is a statement of _____________ law.

Correct AnswerverifiedD

A flask with a volume of 3.16 L contains 9.33 g of an unknown gas at 32.0°C and 1.00 atm.What is the molar mass of the gas? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

If the atmospheric pressure in Denver is 0.8800 atm, what is this pressure expressed in mmHg? (1 atm = 101,325 Pa = 760 torr, 1 torr = 1 mmHg) ?

Correct AnswerverifiedShow Answer

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L.What volume will it occupy if the pressure is increased to 894 torr at constant temperature?

Correct AnswerverifiedShow Answer

If 2.3 mol of a gas occupies 50.5 mL, how many moles of the gas will occupy 85.5 mL at the same temperature and pressure?

Correct AnswerverifiedShow Answer

Which figure best represents the concept of pressure? (A sphere represents a gaseous atom.)

Correct AnswerverifiedShow Answer

What is the mass, in grams, of 2.74 L of CO gas measured at 33°C and 945 mmHg? (R = 0.08206 L • atm/mol • K, 1 atm = 760 mmHg)

Correct AnswerverifiedShow Answer

What is the density of SF6(g) at 27°C and 0.500 atm pressure? (R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

Determine the mole fraction of CO in a gas mixture composed of 782.4 grams of CO2 and 2.10 moles of CO.The mixture is at 703.3 K in a 25.8-liter container.

Correct AnswerverifiedShow Answer

The air pressure in a volleyball is 75 psi.What is this pressure in torr? (1 atm = 14.7 psi = 101,325 Pa = 760 torr) ?

Correct AnswerverifiedShow Answer

A 7.75-L flask contains 0.482 g of hydrogen gas and 4.98 g of oxygen gas at 65°C.What is the partial pressure of oxygen in the flask?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Determine the partial pressure of CO₂ in a gas mixture composed of 782.4 grams of CO₂ and 2.10 moles of CO.The mixture is at 703.3 K in a 25.8-liter container.

Correct Answer
verified

A 0.271-g sample of an unknown vapor occupies 294 mL at 140°C and 847 mmHg.The empirical formula of the compound is CH₂.What is the molecular formula of the compound? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Correct Answer
verified

A sample of hydrogen gas exerts a pressure of 466 torr in a container.What is this pressure in atmospheres? (1 atm = 1.01325 ×10⁵ Pa = 760 torr)

Correct Answer
verified

Correct Answer
verified

What is the density of CO₂(g) at 100.°C and 10.0 atm pressure? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified
E

What is the volume occupied by 35.2 g of methane gas (CH₄) at 25°C and 1.0 atm? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified
E

Correct Answer
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Correct Answer
verified
D

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
verified

What is the density of SF₆(g) at 27°C and 0.500 atm pressure? (R = 0.08206 L • atm/K • mol)

Correct Answer
verified

Determine the mole fraction of CO in a gas mixture composed of 782.4 grams of CO₂ and 2.10 moles of CO.The mixture is at 703.3 K in a 25.8-liter container.

Correct Answer
verified

Correct Answer
verified

Correct Answer
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