Question 1

A spacecraft is filled with 0.500 atm of N2 and 0.500 atm of O2. Suppose an object strikes this spacecraft and puts a very small hole in its side. Under these circumstances,

Accepted Answer

A)   O2 is lost from the craft 6.9% faster than N2 is lost.
B)   O2 is lost from the craft 14% faster than N2 is lost.
C)   N2 is lost from the craft 6.9% faster than O2 is lost.
D)   N2 is lost from the craft 14% faster than O2 is lost.
E)   N2 and O2 are lost from the craft at the same rate.F) C) and E)
G) A) and C)

Question 2

A sample of nitrogen gas is confined to a 14.0-L container at 375 torr and 37.0°C. How many moles of nitrogen are in the container? (R = 0.08206 L • atm/K • mol, 1 atm = 760 torr)

Accepted Answer

A)   0.272 mol
B)   2.27 mol
C)   3.69 mol
D)   206 mol
E)   227 molF) B) and C)
G) A) and B)

Question 3

How many grams of carbon dioxide are contained in 550 mL of this gas at STP?

Accepted Answer

A)   0.0245 g
B)   0.0280 g
C)   1080 g
D)   0.560 g
E)   1.1 gF) All of the above
G) C) and D)

Question 4

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 B)
G) B) and E)

Question 5

A sample of gas occupies 24.5 L at a pressure of 1.57 atm. What is the pressure if the volume is increased to 48.3 L at constant temperature?

Accepted Answer

A)   0.796 atm
B)   1.26 atm
C)   3.10 atm
D)   5.38 × 10-4 atm
E)   1.86 × 103 atmF) B) and D)
G) A) and D)

Question 6

________ is the formula to determine the molar mass of a compound using the ideal gas law.

Accepted Answer

The answer of ________ is the formula to determine the...

Question 7

What is the formula which describes the relationship between the pressure, volume, temperature, and moles?

Accepted Answer

A)   
B)   
C)   
D)   
E)   F) All of the above
G) A) and E)

Question 8

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO2 and is heated to 400°C, will it burst?

Accepted Answer

Question 9

A(n) ________ is an instrument used to measure the atmospheric pressure.

Accepted Answer

The answer of A(n) ________ is an instrument used to...

Question 10

A 2.50-L flask contains a mixture of methane (CH4)  and propane (C3H8)  at a pressure of 1.45 atm and 20°C. When this gas mixture is then burned in excess oxygen, 8.60 g of carbon dioxide is formed. (The other product is water.)  What is the mole fraction of methane in the original gas mixture?

Accepted Answer

A)   0.34
B)   1.00
C)   0.66
D)   0.85
E)   0.15F) None of the above
G) C) and E)

Question 11

_______ ________ states that the volume of a fixed amount of gas maintained at constant pressure is directly proportional to the absolute temperature of a gas.

Accepted Answer

The answer of _______ ________ states that the volume of...

Question 12

What mass of KClO3 must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.)  (R = 0.08206 L • atm/K • mol)

Accepted Answer

A)   24.6 g
B)   70.8 g
C)   272 g
D)   408 g
E)   612 gF) C) and E)
G) B) and E)

Question 13

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)

Question 14

A flask containing neon gas is connected to an open-ended mercury manometer. The open end is exposed to the atmosphere, where the prevailing pressure is 745 torr. The mercury level in the open arm is 5.0 cm below that in the arm connected to the flask of neon. What is the neon pressure, in torr?

Accepted Answer

A)   -50. torr
B)   50. torr
C)   695 torr
D)   745 torr
E)   795 torrF) B) and D)
G) A) and C)

Question 15

The catalytic decomposition of hydrogen peroxide yields oxygen gas and water. In an experiment, decomposition of hydrogen peroxide yielded 75.3 mL of gas collected over water at 25°C and 742 torr. What mass of oxygen gas was collected? (Pwater = 24 torr at 25°C, R = 0.08206 L • atm/K • mol)

Accepted Answer

A)   0.00291 g
B)   0.0931 g
C)   0.0962 g
D)   0.0993 g
E)   0.962 gF) A) and B)
G) A) and E)

Question 16

Gases form heterogeneous mixtures or solutions with one another.

Accepted Answer

A) True 
 B)False

Question 17

What are the conditions of STP?

Accepted Answer

A)   0 K and 1 atm
B)   273.15 K and 760 torr
C)   0°C and 760 atm
D)   273.15°C and 760 torr
E)   0°C and 1 torrF) None of the above
G) A) and E)

Question 18

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) B) and E)
G) A) and D)

Question 19

A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?

Accepted Answer

A)   212 torr
B)   289 torr
C)   356 torr
D)   441 torr
E)   359 torrF) A) and C)
G) A) and D)

Question 20

How many molecules of N2 gas are present in a 2.5-L flask at 50°C and 650 mmHg? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg, 1 mole = 6.022 × 1023 molecules)

Accepted Answer

A)   2.1 × 10-23 molecules
B)   4.9 × 1022 molecules
C)   3.1 × 1023 molecules
D)   3.6 × 1025 molecules
E)   0.081 moleculesF) A) and C)
G) B) and D)

Exam 10: Gases

_______ ________ states that the volume of a fixed amount of gas maintained at constant pressure is directly proportional to the absolute temperature of a gas.

Correct AnswerverifiedShow Answer

A(n) ________ is an instrument used to measure the atmospheric pressure.

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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?

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A flask containing neon gas is connected to an open-ended mercury manometer. The open end is exposed to the atmosphere, where the prevailing pressure is 745 torr. The mercury level in the open arm is 5.0 cm below that in the arm connected to the flask of neon. What is the neon pressure, in torr?

Correct AnswerverifiedShow Answer

What mass of KClO3 must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

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

A 2.50-L flask contains a mixture of methane (CH4) and propane (C3H8) at a pressure of 1.45 atm and 20°C. When this gas mixture is then burned in excess oxygen, 8.60 g of carbon dioxide is formed. (The other product is water.) What is the mole fraction of methane in the original gas mixture?

Correct AnswerverifiedShow Answer

A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?

Correct AnswerverifiedShow Answer

A spacecraft is filled with 0.500 atm of N2 and 0.500 atm of O2. Suppose an object strikes this spacecraft and puts a very small hole in its side. Under these circumstances,

Correct AnswerverifiedShow Answer

What are the conditions of STP?

Correct AnswerverifiedShow Answer

A sample of gas occupies 24.5 L at a pressure of 1.57 atm. What is the pressure if the volume is increased to 48.3 L at constant temperature?

Correct AnswerverifiedShow Answer

How many grams of carbon dioxide are contained in 550 mL of this gas at STP?

Correct AnswerverifiedShow Answer

________ is the formula to determine the molar mass of a compound using the ideal gas law.

Correct AnswerverifiedShow Answer

What is the formula which describes the relationship between the pressure, volume, temperature, and moles?

Correct AnswerverifiedShow Answer

The catalytic decomposition of hydrogen peroxide yields oxygen gas and water. In an experiment, decomposition of hydrogen peroxide yielded 75.3 mL of gas collected over water at 25°C and 742 torr. What mass of oxygen gas was collected? (Pwater = 24 torr at 25°C, R = 0.08206 L • atm/K • mol)

Correct AnswerverifiedShow Answer

Gases form heterogeneous mixtures or solutions with one another.

Correct AnswerverifiedShow Answer

A sample of nitrogen gas is confined to a 14.0-L container at 375 torr and 37.0°C. How many moles of nitrogen are in the container? (R = 0.08206 L • atm/K • mol, 1 atm = 760 torr)

Correct AnswerverifiedShow Answer

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

How many molecules of N2 gas are present in a 2.5-L flask at 50°C and 650 mmHg? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg, 1 mole = 6.022 × 1023 molecules)

Correct AnswerverifiedShow Answer

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO2 and is heated to 400°C, will it burst?

Correct AnswerverifiedShow Answer

_ __ states that the volume of a fixed amount of gas maintained at constant pressure is directly proportional to the absolute temperature of a gas.

Correct Answer
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What mass of KClO₃ must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

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

Correct Answer
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A 2.50-L flask contains a mixture of methane (CH₄) and propane (C₃H₈) at a pressure of 1.45 atm and 20°C. When this gas mixture is then burned in excess oxygen, 8.60 g of carbon dioxide is formed. (The other product is water.) What is the mole fraction of methane in the original gas mixture?

Correct Answer
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Correct Answer
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A spacecraft is filled with 0.500 atm of N₂ and 0.500 atm of O₂. Suppose an object strikes this spacecraft and puts a very small hole in its side. Under these circumstances,

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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The catalytic decomposition of hydrogen peroxide yields oxygen gas and water. In an experiment, decomposition of hydrogen peroxide yielded 75.3 mL of gas collected over water at 25°C and 742 torr. What mass of oxygen gas was collected? (P_water = 24 torr at 25°C, R = 0.08206 L • atm/K • mol)

Correct Answer
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Correct Answer
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Correct Answer
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How many molecules of N₂ gas are present in a 2.5-L flask at 50°C and 650 mmHg? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg, 1 mole = 6.022 × 10²³ molecules)

Correct Answer
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An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO₂ and is heated to 400°C, will it burst?

Correct Answer
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