Question 1

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

Question 2

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

Question 3

"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's 
A) Charles's 
B) Boyle's 
C) Dalton's 
D) Avogadro's 
E) Gay-Lussac's D

Question 4

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) 0.52 
A) 0.11 
B) 0.89 
C) 17.8 
D) 0.48 
E) 0.52

Question 5

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) C6H12 
A) CH2 
B) C2H4 
C) C3H6 
D) C4H8 
E) C6H12

Question 6

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

Question 7

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

Accepted Answer

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

Question 8

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/L 
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/L

Question 9

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

Question 10

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

Question 11

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

Question 12

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) N2O5 
A) NO 
B) NO2 
C) N3O6 
D) N2O4 
E) N2O5

Question 13

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

Question 14

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

Question 15

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

Question 16

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

Question 17

"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's 
A) Charles's 
B) Boyle's 
C) Amontons's 
D) Avogadro's 
E) Gay-Lussac's

Question 18

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

Question 19

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 mmHg 
A) 151.5 mmHg 
B) 1.16× 10−3 mmHg 
C) 863.6 mmHg 
D) 8.92 × 104 mmHg 
E) 668.8 mmHg

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

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)

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

"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.

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.

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)

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)

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

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

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.

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)?

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?

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)

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)

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)

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?

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

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?

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)?

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?

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

Physical Properties of Solutions

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Using Balanced Chemical Equations

Acids and Bases

Equilibrium

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Exam 8: Gases

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)

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

"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.

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.

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)

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)

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

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

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.

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)?

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?

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)

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)

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)

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?

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

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?

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)?

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?

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

Physical Properties of Solutions

Chemical Reactions and Chemical Equations

Using Balanced Chemical Equations

Acids and Bases

Equilibrium

Organic Chemistry

Biochemistry

Nuclear Chemistry

Electrochemistry

Filters

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)

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

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.

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)

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

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.

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)