Question 1

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

Question 2

A sample of a gas occupies 1.40 L at 25°C and 760 mmHg.What volume will it occupy at the same temperature and 380 mmHg?

Accepted Answer

A) 2.8 L 
B) 2.10 L 
C) 1.40 L 
D) 1.05 L 
E) 0.700 L 
A) 2.8 L 
B) 2.10 L 
C) 1.40 L 
D) 1.05 L 
E) 0.700 L

Question 3

Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100 cm3 at 95°C and 1000 mmHg (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg).

Accepted Answer

A) 0.19 g/mol 
B) 35.3 g/mol 
C) 70.9 g/mol 
D) 137 g/mol 
E) 384 g/mol 
A) 0.19 g/mol 
B) 35.3 g/mol 
C) 70.9 g/mol 
D) 137 g/mol 
E) 384 g/mol

Question 4

A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr.What is its volume at STP? (R = 0.08206 L • atm/K • mol, 1 atm = 760 torr)

Accepted Answer

A) 25.2 L 
B) 30.6 L 
C) 33.6 L 
D) 37.1 L 
E) 49.2 L 
A) 25.2 L 
B) 30.6 L 
C) 33.6 L 
D) 37.1 L 
E) 49.2 L

Question 5

The pressure of hydrogen sulfide gas in a container is 3.565 ×104 Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)?

Accepted Answer

A) 46.91 torr 
B) 267.4 torr 
C) 351.8 torr 
D) 3612 torr 
E) 2.709 ×104 torr 
A) 46.91 torr 
B) 267.4 torr 
C) 351.8 torr 
D) 3612 torr 
E) 2.709 ×104 torr

Question 6

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

Accepted Answer

A)    
B)    
C)    
D)    
A)    
B)    
C)    
D)

Question 7

What is the initial pressure of a gas having an initial temperature of 905 K, an initial volume of 14.3 L, a final pressure of 0.83 atm, a final temperature of 154 K and a final volume of 2.7 L?

Accepted Answer

A) 26 atm 
B) 0.27 atm 
C) 0.75 atm 
D) 1.3 atm 
E) 0.92 atm 
A) 26 atm 
B) 0.27 atm 
C) 0.75 atm 
D) 1.3 atm 
E) 0.92 atm

Question 8

A gas cylinder containing 1.50 mol compressed methane has a volume of 3.30 L.What pressure does the methane exert on the walls of the cylinder if its temperature is 25°C? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A) 9.00 × 10−2 atm 
B) 0.933 atm 
C) 1.11 atm 
D) 1.70 atm 
E) 11.1 atm 
A) 9.00 × 10−2 atm 
B) 0.933 atm 
C) 1.11 atm 
D) 1.70 atm 
E) 11.1 atm

Question 9

What is the molar mass of an unknown gas if a sample weighing 0.389 g is collected in a flask with a volume of 102 cm3 at 97°C and at a pressure of 728 mmHg? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg).

Accepted Answer

A) 187 g/mol 
B) 121 g/mol 
C) 112 g/mol 
D) 31.6 g/mol 
E) 8.28 × 10−3 g/mol 
A) 187 g/mol 
B) 121 g/mol 
C) 112 g/mol 
D) 31.6 g/mol 
E) 8.28 × 10−3 g/mol

Question 10

A gas evolved during the fermentation of sugar was collected at 22.5°C and 702 mmHg.After purification its volume was found to be 25.0 L.How many moles of gas were collected? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg)

Accepted Answer

A) 0.952 mol 
B) 1.05 mol 
C) 12.5 mol 
D) 22.4 mol 
E) 724 mol 
A) 0.952 mol 
B) 1.05 mol 
C) 12.5 mol 
D) 22.4 mol 
E) 724 mol

Question 11

Determine the mole fraction of CO2 in a gas mixture composed of 10.0 grams of CO2 and 10.0 grams of helium.The mixture is at 75ºC in a 12.0-liter container.

Accepted Answer

A) 0.92 
B) 2.7 
C) 0.23 
D) 0.080 
E) 0.77 
A) 0.92 
B) 2.7 
C) 0.23 
D) 0.080 
E) 0.77

Question 12

A sample of nitrogen gas has a volume of 32.4 L at 20°C.The gas is heated to 220ºC at constant pressure.What is the final volume of the nitrogen gas?

Accepted Answer

A) 2.94 L 
B) 19.3 L 
C) 32.4 L 
D) 54.5 L 
E) 356 L 
A) 2.94 L 
B) 19.3 L 
C) 32.4 L 
D) 54.5 L 
E) 356 L

Question 13

Determine the partial pressure of helium in a gas mixture composed of 10.0 grams of CO2 and 10.0 grams of helium.The mixture is at 75ºC in a 12.0-liter container.

Accepted Answer

A) 5.95 atm 
B) 1.28 atm 
C) 0.541 atm 
D) 0.117 atm 
E) 7.23 atm 
A) 5.95 atm 
B) 1.28 atm 
C) 0.541 atm 
D) 0.117 atm 
E) 7.23 atm

Question 14

Determine the partial pressure of N2 in a gas mixture composed of 1.0 mol of N2 and 1.5 mol of Ar.The mixture is at 0.0ºC in a 10.0-liter container.

Accepted Answer

A) 3.36 atm 
B) 0.00 atm 
C) 5.60 atm 
D) 6.12 atm 
E) 2.24 atm 
A) 3.36 atm 
B) 0.00 atm 
C) 5.60 atm 
D) 6.12 atm 
E) 2.24 atm

Question 15

A sample of nitrogen gas has the temperature drop from 250.°C to 150.°C at constant pressure.What is the final volume if the initial volume is 310.mL?

Accepted Answer

A) 0.186 L 
B) 0.251 L 
C) 0.383 L 
D) 0.410 L 
E) 0.517 L 
A) 0.186 L 
B) 0.251 L 
C) 0.383 L 
D) 0.410 L 
E) 0.517 L

Question 16

A sample of a gas has an initial pressure of 0.987 atm and a volume of 12.8 L.What is the final pressure if the volume is increased to 25.6 L?

Accepted Answer

A) 2.03 atm 
B) 1.97 atm 
C) 0.494 atm 
D) 0.003 atm 
E) 323.4 atm 
A) 2.03 atm 
B) 1.97 atm 
C) 0.494 atm 
D) 0.003 atm 
E) 323.4 atm

Question 17

Gases are sold in large cylinders for laboratory use.What pressure is exerted by 2.500 kg of oxygen gas (O2) stored at 22°C in a 40.0-L cylinder? (R = 0.08206 L • atm/K • mol)

Accepted Answer

A) 3.55 atm 
B) 1.51 ×103 atm 
C) 47.3 atm 
D) 7.56 × 104 atm 
E) 10.2 atm 
A) 3.55 atm 
B) 1.51 ×103 atm 
C) 47.3 atm 
D) 7.56 × 104 atm 
E) 10.2 atm

Question 18

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 molecules 
A) 2.1 × 10−23 molecules 
B) 4.9 × 1022 molecules 
C) 3.1 × 1023 molecules 
D) 3.6 × 1025 molecules 
E) 0.081 molecules

Question 19

If 25.5 L of oxygen are cooled from 150°C to 50°C at constant pressure, what is the new volume of oxygen?

Accepted Answer

A) 0.0514 L 
B) 19.5 L 
C) 33.4 L 
D) 0.03 L 
E) 3.5 L 
A) 0.0514 L 
B) 19.5 L 
C) 33.4 L 
D) 0.03 L 
E) 3.5 L

Question 20

The pressure of sulfur dioxide in a container is 159 kPa.What is this pressure in atmospheres? (1 atm = 101,325 Pa = 760 torr)?

Accepted Answer

A) 0.209 atm 
B) 0.637 atm 
C) 1.57 atm 
D) 21.2 atm 
E) 1.59×104 atm 
A) 0.209 atm 
B) 0.637 atm 
C) 1.57 atm 
D) 21.2 atm 
E) 1.59×104 atm

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?

A sample of a gas occupies 1.40 L at 25°C and 760 mmHg.What volume will it occupy at the same temperature and 380 mmHg?

Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100 cm³ at 95°C and 1000 mmHg (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg).

A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr.What is its volume at STP? (R = 0.08206 L • atm/K • mol, 1 atm = 760 torr)

The pressure of hydrogen sulfide gas in a container is 3.565 ×10⁴ Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)?

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

What is the initial pressure of a gas having an initial temperature of 905 K, an initial volume of 14.3 L, a final pressure of 0.83 atm, a final temperature of 154 K and a final volume of 2.7 L?

A gas cylinder containing 1.50 mol compressed methane has a volume of 3.30 L.What pressure does the methane exert on the walls of the cylinder if its temperature is 25°C? (R = 0.08206 L • atm/K • mol)

What is the molar mass of an unknown gas if a sample weighing 0.389 g is collected in a flask with a volume of 102 cm³ at 97°C and at a pressure of 728 mmHg? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg).

A gas evolved during the fermentation of sugar was collected at 22.5°C and 702 mmHg.After purification its volume was found to be 25.0 L.How many moles of gas were collected? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg)

Determine the mole fraction of CO₂ in a gas mixture composed of 10.0 grams of CO₂ and 10.0 grams of helium.The mixture is at 75ºC in a 12.0-liter container.

A sample of nitrogen gas has a volume of 32.4 L at 20°C.The gas is heated to 220ºC at constant pressure.What is the final volume of the nitrogen gas?

Determine the partial pressure of helium in a gas mixture composed of 10.0 grams of CO₂ and 10.0 grams of helium.The mixture is at 75ºC in a 12.0-liter container.

Determine the partial pressure of N₂ in a gas mixture composed of 1.0 mol of N₂ and 1.5 mol of Ar.The mixture is at 0.0ºC in a 10.0-liter container.

A sample of nitrogen gas has the temperature drop from 250.°C to 150.°C at constant pressure.What is the final volume if the initial volume is 310.mL?

A sample of a gas has an initial pressure of 0.987 atm and a volume of 12.8 L.What is the final pressure if the volume is increased to 25.6 L?

Gases are sold in large cylinders for laboratory use.What pressure is exerted by 2.500 kg of oxygen gas (O₂) stored at 22°C in a 40.0-L cylinder? (R = 0.08206 L • atm/K • mol)

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)

If 25.5 L of oxygen are cooled from 150^°C to 50^°C at constant pressure, what is the new volume of oxygen?

The pressure of sulfur dioxide in a container is 159 kPa.What is this pressure in atmospheres? (1 atm = 101,325 Pa = 760 torr)?

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Exam 8: Gases

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?

A sample of a gas occupies 1.40 L at 25°C and 760 mmHg.What volume will it occupy at the same temperature and 380 mmHg?

Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100 cm3 at 95°C and 1000 mmHg (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg).

A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr.What is its volume at STP? (R = 0.08206 L • atm/K • mol, 1 atm = 760 torr)

The pressure of hydrogen sulfide gas in a container is 3.565 ×104 Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)?

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

What is the initial pressure of a gas having an initial temperature of 905 K, an initial volume of 14.3 L, a final pressure of 0.83 atm, a final temperature of 154 K and a final volume of 2.7 L?

A gas cylinder containing 1.50 mol compressed methane has a volume of 3.30 L.What pressure does the methane exert on the walls of the cylinder if its temperature is 25°C? (R = 0.08206 L • atm/K • mol)

What is the molar mass of an unknown gas if a sample weighing 0.389 g is collected in a flask with a volume of 102 cm3 at 97°C and at a pressure of 728 mmHg? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg).

A gas evolved during the fermentation of sugar was collected at 22.5°C and 702 mmHg.After purification its volume was found to be 25.0 L.How many moles of gas were collected? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg)

Determine the mole fraction of CO2 in a gas mixture composed of 10.0 grams of CO2 and 10.0 grams of helium.The mixture is at 75ºC in a 12.0-liter container.

A sample of nitrogen gas has a volume of 32.4 L at 20°C.The gas is heated to 220ºC at constant pressure.What is the final volume of the nitrogen gas?

Determine the partial pressure of helium in a gas mixture composed of 10.0 grams of CO2 and 10.0 grams of helium.The mixture is at 75ºC in a 12.0-liter container.

Determine the partial pressure of N2 in a gas mixture composed of 1.0 mol of N2 and 1.5 mol of Ar.The mixture is at 0.0ºC in a 10.0-liter container.

A sample of nitrogen gas has the temperature drop from 250.°C to 150.°C at constant pressure.What is the final volume if the initial volume is 310.mL?

A sample of a gas has an initial pressure of 0.987 atm and a volume of 12.8 L.What is the final pressure if the volume is increased to 25.6 L?

Gases are sold in large cylinders for laboratory use.What pressure is exerted by 2.500 kg of oxygen gas (O2) stored at 22°C in a 40.0-L cylinder? (R = 0.08206 L • atm/K • mol)

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)

If 25.5 L of oxygen are cooled from 150°C to 50°C at constant pressure, what is the new volume of oxygen?

The pressure of sulfur dioxide in a container is 159 kPa.What is this pressure in atmospheres? (1 atm = 101,325 Pa = 760 torr)?

Atoms and Elements

Electrons and the Periodic Table

Compounds and Chemical Bonds

How Chemists Use Numbers

The Mole and Chemical Formulas

Molecular Shape

Solids, Liquids, and Phase Changes

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Using Balanced Chemical Equations

Acids and Bases

Equilibrium

Organic Chemistry

Biochemistry

Nuclear Chemistry

Electrochemistry

Filters

Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100 cm³ at 95°C and 1000 mmHg (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg).

The pressure of hydrogen sulfide gas in a container is 3.565 ×10⁴ Pa.What is this pressure in torr? (1 atm = 101,325 Pa = 760 torr)?

What is the molar mass of an unknown gas if a sample weighing 0.389 g is collected in a flask with a volume of 102 cm³ at 97°C and at a pressure of 728 mmHg? (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg).

Determine the mole fraction of CO₂ in a gas mixture composed of 10.0 grams of CO₂ and 10.0 grams of helium.The mixture is at 75ºC in a 12.0-liter container.

Determine the partial pressure of helium in a gas mixture composed of 10.0 grams of CO₂ and 10.0 grams of helium.The mixture is at 75ºC in a 12.0-liter container.

Determine the partial pressure of N₂ in a gas mixture composed of 1.0 mol of N₂ and 1.5 mol of Ar.The mixture is at 0.0ºC in a 10.0-liter container.

Gases are sold in large cylinders for laboratory use.What pressure is exerted by 2.500 kg of oxygen gas (O₂) stored at 22°C in a 40.0-L cylinder? (R = 0.08206 L • atm/K • mol)

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)

If 25.5 L of oxygen are cooled from 150^°C to 50^°C at constant pressure, what is the new volume of oxygen?