Question 1

Of the following, __________ is a valid statement of Charles' law.

Accepted Answer

A)    = constant 
B)    = constant 
C) PV = constant 
D) V = constant × n 
E) V = constant × P 
A)    = constant 
B)    = constant 
C) PV = constant 
D) V = constant × n 
E) V = constant × P

Question 2

A sample of H2 gas (2.0 L)at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25°C into a 7.0 L flask. The total pressure in the flask is __________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25°C.

Accepted Answer

A) 0.56 
B) 2.8 
C) 1.0 
D) 1.6 
E) 24 
A) 0.56 
B) 2.8 
C) 1.0 
D) 1.6 
E) 24

Question 3

The reaction of 50 mL of Cl2 gas with 50 mL of CH4 gas via the equation: Cl2 (g)+ CH4 (g)→ HCl (g)+ CH3Cl (g)
Will produce a total of __________ mL of products if pressure and temperature are kept constant.

Accepted Answer

A) 100 
B) 50 
C) 200 
D) 150 
E) 250 
A) 100 
B) 50 
C) 200 
D) 150 
E) 250

Question 4

The molecular weight of a gas that has a density of 7.10 g/L at 25.0°C and 1.00 atm pressure is __________ g/mol.

Accepted Answer

A) 174 
B) 14.6 
C) 28.0 
D) 5.75 × 10-3 
E) 6.85 × 10-2 
A) 174 
B) 14.6 
C) 28.0 
D) 5.75 × 10-3 
E) 6.85 × 10-2

Question 5

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L)the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.

Accepted Answer

A) 10.9 
B) 13.2 
C) 2.07 
D) 7.56 
E) 48.4 
A) 10.9 
B) 13.2 
C) 2.07 
D) 7.56 
E) 48.4

Question 6

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle's law to calculate the pressure (torr)when the volume is reduced to 7.88 L at a constant temperature of 25.0°C.

Accepted Answer

A) 846 
B) 0.118 
C) 5.26 × 104 
D) 526 
E) 1.11 
A) 846 
B) 0.118 
C) 5.26 × 104 
D) 526 
E) 1.11

Question 7

When gases are treated as real, via use of the van der Waals equation, the actual volume occupied by gas molecules __________ the pressure exerted and the attractive forces between gas molecules __________ the pressure exerted, as compared to an ideal gas.

Accepted Answer

A) decreases, increases 
B) increases, increases 
C) increases, decreases 
D) does not affect, decreases 
E) does not affect, increases 
A) decreases, increases 
B) increases, increases 
C) increases, decreases 
D) does not affect, decreases 
E) does not affect, increases

Question 8

A sample of a gas (1.50 mol)is contained in a 15.0 L cylinder. The temperature is increased from 100°C to 150°C. The ratio of final pressure to initial pressure   is __________.

Accepted Answer

A) 1.50 
B) 0.667 
C) 0.882 
D) 1.13 
E) 1.00 
A) 1.50 
B) 0.667 
C) 0.882 
D) 1.13 
E) 1.00

Question 9

The molecular weight of a gas is __________ g/mol if 6.7 g of the gas occupies 6.3 L at STP.

Accepted Answer

A) 24 
B) 3.6 × 103 
C) 27 
D) 3.0 × 102 
E) 1.8 × 10-2 
A) 24 
B) 3.6 × 103 
C) 27 
D) 3.0 × 102 
E) 1.8 × 10-2

Question 10

A gas in a 325 mL container has a pressure of 695 torr at 19°C. There are __________ mol of gas in the flask.

Accepted Answer

A) 1.24 × 10-2 
B) 1.48 × 10-2 
C) 9.42 
D) 12.4 
E) 80.6 
A) 1.24 × 10-2 
B) 1.48 × 10-2 
C) 9.42 
D) 12.4 
E) 80.6

Question 11

The pressure exerted by a column of liquid is equal to the product of the height of the column times the gravitational constant times the density of the liquid, P = ghd. How high a column of methanol (d = 0.79 g/mL)would be supported by a pressure that supports a 713 mm column of mercury (d = 13.6 g/mL)?

Accepted Answer

A) 713 mm 
B) 41 mm 
C) 1.2 × 104 mm 
D) 9.7 × 103 mm 
E) 17 mm 
A) 713 mm 
B) 41 mm 
C) 1.2 × 104 mm 
D) 9.7 × 103 mm 
E) 17 mm

Question 12

At a temperature of __________°C, 0.444 mol of CO gas occupies 11.8 L at 912 torr.

Accepted Answer

A) 379 
B) 73.0 
C) 14.0 
D) 32.0 
E) 116 
A) 379 
B) 73.0 
C) 14.0 
D) 32.0 
E) 116

Question 13

An ideal gas differs from a real gas in that the molecules of an ideal gas __________.

Accepted Answer

A) have no attraction for one another 
B) have appreciable molecular volumes 
C) have a molecular weight of zero 
D) have no kinetic energy 
E) have an average molecular mass 
A) have no attraction for one another 
B) have appreciable molecular volumes 
C) have a molecular weight of zero 
D) have no kinetic energy 
E) have an average molecular mass

Question 14

A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol of He and 0.56 mol of Ne. The partial pressure of Ne is __________ atm.

Accepted Answer

A) 1.7 
B) 1.5 
C) 0.60 
D) 0.35 
E) 1.0 
A) 1.7 
B) 1.5 
C) 0.60 
D) 0.35 
E) 1.0

Question 15

A sample of O2 gas (2.0 mmol)effused through a pinhole in 5.0 s. It will take __________ s for the same amount of CO2 to effuse under the same conditions.

Accepted Answer

A) 4.3 
B) 0.23 
C) 3.6 
D) 5.9 
E) 6.9 
A) 4.3 
B) 0.23 
C) 3.6 
D) 5.9 
E) 6.9

Question 16

A pressure of 1.25 atm is the same as a pressure of __________ of mm Hg.

Accepted Answer

A) 193 
B) 760. 
C) 950. 
D) 29.9 
E) 33.0 
A) 193 
B) 760. 
C) 950. 
D) 29.9 
E) 33.0

Question 17

Since air is a mixture, it does not have a "molar mass." However, for calculation purposes, it is possible to speak of its "effective molar mass." (An effective molar mass is a weighted average of the molar masses of a mixture's components.)If air at STP has a density of 1.285 g/L, its effective molar mass is __________ g/mol.

Accepted Answer

A) 26.94 
B) 31.49 
C) 30.00 
D) 34.42 
E) 28.80 
A) 26.94 
B) 31.49 
C) 30.00 
D) 34.42 
E) 28.80

Question 18

Of the following gases, __________ will have the greatest rate of effusion at a given temperature.

Accepted Answer

A) NH3 
B) CH4 
C) Ar 
D) HBr 
E) HCl 
A) NH3 
B) CH4 
C) Ar 
D) HBr 
E) HCl

Question 19

The temperature and pressure specified by STP are __________ °C and __________ atm.

Accepted Answer

The answer of The temperature and pressure specified by STP...

Question 20

The molecular weight of a gas is __________ g/mol if 3.5 g of the gas occupies 2.1 L at STP.

Accepted Answer

A) 41 
B) 5.5 × 103 
C) 37 
D) 4.6 × 102 
E) 2.7 × 10-2 
A) 41 
B) 5.5 × 103 
C) 37 
D) 4.6 × 102 
E) 2.7 × 10-2

Exam 10: Gases

Of the following, __________ is a valid statement of Charles' law.

A sample of H2 gas (2.0 L)at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25°C into a 7.0 L flask. The total pressure in the flask is __________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25°C.

The reaction of 50 mL of Cl2 gas with 50 mL of CH4 gas via the equation: Cl2 (g)+ CH4 (g)→ HCl (g)+ CH3Cl (g) Will produce a total of __________ mL of products if pressure and temperature are kept constant.

The molecular weight of a gas that has a density of 7.10 g/L at 25.0°C and 1.00 atm pressure is __________ g/mol.

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L)the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle's law to calculate the pressure (torr)when the volume is reduced to 7.88 L at a constant temperature of 25.0°C.

When gases are treated as real, via use of the van der Waals equation, the actual volume occupied by gas molecules __________ the pressure exerted and the attractive forces between gas molecules __________ the pressure exerted, as compared to an ideal gas.

A sample of a gas (1.50 mol)is contained in a 15.0 L cylinder. The temperature is increased from 100°C to 150°C. The ratio of final pressure to initial pressure is __________.

The molecular weight of a gas is __________ g/mol if 6.7 g of the gas occupies 6.3 L at STP.

A gas in a 325 mL container has a pressure of 695 torr at 19°C. There are __________ mol of gas in the flask.

At a temperature of __________°C, 0.444 mol of CO gas occupies 11.8 L at 912 torr.

An ideal gas differs from a real gas in that the molecules of an ideal gas __________.

A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol of He and 0.56 mol of Ne. The partial pressure of Ne is __________ atm.

A sample of O2 gas (2.0 mmol)effused through a pinhole in 5.0 s. It will take __________ s for the same amount of CO2 to effuse under the same conditions.

A pressure of 1.25 atm is the same as a pressure of __________ of mm Hg.

Of the following gases, __________ will have the greatest rate of effusion at a given temperature.

The temperature and pressure specified by STP are __________ °C and __________ atm.

The molecular weight of a gas is __________ g/mol if 3.5 g of the gas occupies 2.1 L at STP.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

A sample of H₂ gas (2.0 L)at 3.5 atm was combined with 1.5 L of N₂ gas at 2.6 atm pressure at a constant temperature of 25°C into a 7.0 L flask. The total pressure in the flask is __________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25°C.

The reaction of 50 mL of Cl₂ gas with 50 mL of CH₄ gas via the equation: Cl₂ (g)+ CH₄ (g)→ HCl (g)+ CH₃Cl (g) Will produce a total of __________ mL of products if pressure and temperature are kept constant.

When gases are treated as real, via use of the van der Waals equation, the actual volume occupied by gas molecules the pressure exerted and the attractive forces between gas molecules the pressure exerted, as compared to an ideal gas.

A sample of O₂ gas (2.0 mmol)effused through a pinhole in 5.0 s. It will take __________ s for the same amount of CO₂ to effuse under the same conditions.

The temperature and pressure specified by STP are °C and atm.