Question 1

A 40.2 L constant-volume cylinder containing 2.21 mol He is heated until the pressure reaches 4.20 atm. What is the final temperature?

Accepted Answer

A)  258 K 
B)  658 K 
C)  931 K 
D)  804 K 
E)  1074 K 
A)  258 K 
B)  658 K 
C)  931 K 
D)  804 K 
E)  1074 K

Question 2

How many liters of H2 are needed to make 327 L of NH3 by the reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g),
If the gases are at the same temperature and pressure?

Accepted Answer

A)  654 L 
B)  491 L 
C)  218 L 
D)  38.5 L 
E)  327 L 
A)  654 L 
B)  491 L 
C)  218 L 
D)  38.5 L 
E)  327 L

Question 3

Chloroform became popular as an anesthetic after Queen Victoria delivered her eighth child while anesthetized by chloroform in 1853. What is the molar mass of chloroform if 4.85 grams is 0.918 liters at 35°C and 850 torr?

Accepted Answer

A)  149 g/mol 
B)  119 g/mol 
C)  123 g/mol 
D)  134 g/mol 
E)  110 g/mol 
A)  149 g/mol 
B)  119 g/mol 
C)  123 g/mol 
D)  134 g/mol 
E)  110 g/mol

Question 4

The statement, "For a fixed mass of gas at constant temperature, gas volume is inversely proportional to gas pressure." is known as:

Accepted Answer

A)  Avogadro's Law 
B)  Boyle's Law 
C)  Charles' Law 
D)  Graham's Law 
E)  Kelvin's Law 
A)  Avogadro's Law 
B)  Boyle's Law 
C)  Charles' Law 
D)  Graham's Law 
E)  Kelvin's Law

Question 5

What volume of oxygen gas, at 533°C and 750 torr, could be produced by the decomposition of 38.1 g of potassium chlorate? The other product is potassium chloride.

Accepted Answer

A)  35.9 L 
B)  31.3 L 
C)  30.4 L 
D)  20.7 L 
E)  10.4 L 
A)  35.9 L 
B)  31.3 L 
C)  30.4 L 
D)  20.7 L 
E)  10.4 L

Question 6

A gaseous mixture consists of 50.0% O2, 25.0% N2, and 25.0% Cl2, by mass. At standard temperature and pressure, the partial pressure of:

Accepted Answer

A)  Cl2(g) is greater than 0.25 atm 
B)  O2(g) is equal to 380 torr 
C)  Cl2(g) is less than 0.25 atm 
D)  N2(g) is equal to 0.20 atm 
E)  O2(g) is equal to 1.6 atm 
A)  Cl2(g) is greater than 0.25 atm 
B)  O2(g) is equal to 380 torr 
C)  Cl2(g) is less than 0.25 atm 
D)  N2(g) is equal to 0.20 atm 
E)  O2(g) is equal to 1.6 atm

Question 7

In the reaction CH4 + 2 O2 → CO2 + 2 H2O, how many liters of O2 react with 5.0 liters of CH4? All gas volumes are measured at the same temperature and pressure but not at STP.

Accepted Answer

A)  0.22 L 
B)  10 L 
C)  5.0 L 
D)  2.5 L 
E)  20 L 
A)  0.22 L 
B)  10 L 
C)  5.0 L 
D)  2.5 L 
E)  20 L

Question 8

A sample of oxygen gas is collected over water at 23°C at a barometric pressure of 751 mmHg (the vapor pressure of water at 23°C = 21 mmHg). The partial pressure of oxygen gas in the sample collected is ________.

Accepted Answer

A)  0.96 atm 
B)  21 mmHg 
C)  751 mmHg 
D)  1.02 atm 
E)  44 mmHg 
A)  0.96 atm 
B)  21 mmHg 
C)  751 mmHg 
D)  1.02 atm 
E)  44 mmHg

Question 9

How many liters of gas is 23.4 grams of nitrogen at 750 mmHg and 28.0°C?

Accepted Answer

A)  586 L 
B)  20.9 L 
C)  0.771 L 
D)  20.4 L 
E)  1.94 L 
A)  586 L 
B)  20.9 L 
C)  0.771 L 
D)  20.4 L 
E)  1.94 L

Question 10

Convert to the equivalent pressure in atmospheres, 421 kPa.

Accepted Answer

A)  4.27 × 105 atm 
B)  320 atm 
C)  0.554 atm 
D)  0.00415 atm 
E)  4.15 atm 
A)  4.27 × 105 atm 
B)  320 atm 
C)  0.554 atm 
D)  0.00415 atm 
E)  4.15 atm

Question 11

A 1.37 L vessel contains He at a temperature of 24.5°C and a pressure of 205 mmHg. A 721 mL vessel contains Ne at a temperature of 36.2°C and a pressure of 0.185 atm. Both of these gases are placed in a 2.00 L vessel at 302 K. What is the final pressure (in atm) in the 2.00 L vessel?

Accepted Answer

A)  0.250 atm 
B)  0.187 atm 
C)  0.0657 atm 
D)  0.455 atm 
E)  0.390 atm 
A)  0.250 atm 
B)  0.187 atm 
C)  0.0657 atm 
D)  0.455 atm 
E)  0.390 atm

Question 12

Calculate the height of a column of liquid glycerol (d = 1.26 g/cm3), in meters, required to exert the same pressure as 4.91 m of water.

Accepted Answer

A)  4.91 m 
B)  3.90 m 
C)  6.19 m 
D)  3.65 m 
E)  5.16 m 
A)  4.91 m 
B)  3.90 m 
C)  6.19 m 
D)  3.65 m 
E)  5.16 m

Question 13

2.24 L NH3(g) at 2.0 atm and 0°C:

Accepted Answer

A)  contains 0.050 mole NH3 
B)  weighs 1.70 g 
C)  contains 6.02 × 1022 molecules of NH3 
D)  contains 3.6 × 1023 H atoms 
E)  contains 3.6 × 1023 N atoms 
A)  contains 0.050 mole NH3 
B)  weighs 1.70 g 
C)  contains 6.02 × 1022 molecules of NH3 
D)  contains 3.6 × 1023 H atoms 
E)  contains 3.6 × 1023 N atoms

Question 14

If 4.800 × 10-5 mol of uranium-238 will effuse through a hole in 125 seconds, how many mol of uranium-235 will effuse through the same hole in the same amount of time?

Accepted Answer

A)  4.74 × 10-5 mol 
B)  4.77 × 10-5 mol 
C)  4.80 × 10-5 mol 
D)  4.86 × 10-5 mol 
E)  4.83 × 10-5 mol 
A)  4.74 × 10-5 mol 
B)  4.77 × 10-5 mol 
C)  4.80 × 10-5 mol 
D)  4.86 × 10-5 mol 
E)  4.83 × 10-5 mol

Question 15

According to the kinetic-molecular theory of gases:

Accepted Answer

A)  gaseous particles are in constant, nonlinear motion 
B)  at constant temperature, all particles have equal translational kinetic energy 
C)  the faster a given particle is moving, the greater its translational kinetic energy 
D)  at constant temperature, average kinetic energy is a function of gas volume 
E)  all interparticle collisions are completely inelastic 
A)  gaseous particles are in constant, nonlinear motion 
B)  at constant temperature, all particles have equal translational kinetic energy 
C)  the faster a given particle is moving, the greater its translational kinetic energy 
D)  at constant temperature, average kinetic energy is a function of gas volume 
E)  all interparticle collisions are completely inelastic

Question 16

Calculate the height in meters of a column of liquid glycerol (density = 1.26 g/cm3) required to exert the same pressure as 760 mmHg (d = 13.60 g/cm3).

Accepted Answer

A)  8.20 m 
B)  8.20 × 103 m 
C)  70.4 m 
D)  0.704 m 
E)  44.4 m 
A)  8.20 m 
B)  8.20 × 103 m 
C)  70.4 m 
D)  0.704 m 
E)  44.4 m

Question 17

A gaseous hydrocarbon weighing 0.290 g occupies a volume of 125 mL at 25°C and 760 mmHg. What is the molar mass of this compound?

Accepted Answer

A)  113 g/mol 
B)  4.76 × 103 g/mol 
C)  43.1 g/mol 
D)  10.5 g/mol 
E)  56.7 g/mol 
A)  113 g/mol 
B)  4.76 × 103 g/mol 
C)  43.1 g/mol 
D)  10.5 g/mol 
E)  56.7 g/mol

Question 18

Convert to the equivalent pressure in atmospheres, 1250 mmHg.

Accepted Answer

A)  9.50 × 105 atm 
B)  490 atm 
C)  1.64 atm 
D)  0.608 atm 
E)  1.22 atm 
A)  9.50 × 105 atm 
B)  490 atm 
C)  1.64 atm 
D)  0.608 atm 
E)  1.22 atm

Question 19

Convert 8.50 kg/cm2 to the equivalent pressure in atmospheres.

Accepted Answer

A)  8.78 atm 
B)  1.12 atm 
C)  9.53 atm 
D)  8.23 atm 
E)  7.47 atm 
A)  8.78 atm 
B)  1.12 atm 
C)  9.53 atm 
D)  8.23 atm 
E)  7.47 atm

Question 20

Of the following values, the most likely to be observed for the volume of 1.00 mole of He(g) at 0°C and 1000 atm is:

Accepted Answer

A)  17.4 mL 
B)  46 mL 
C)  22.4 mL 
D)  11.2 mL 
E)  22.4 L 
A)  17.4 mL 
B)  46 mL 
C)  22.4 mL 
D)  11.2 mL 
E)  22.4 L

Exam 6: Gases

A 40.2 L constant-volume cylinder containing 2.21 mol He is heated until the pressure reaches 4.20 atm. What is the final temperature?

How many liters of H2 are needed to make 327 L of NH3 by the reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g), If the gases are at the same temperature and pressure?

Chloroform became popular as an anesthetic after Queen Victoria delivered her eighth child while anesthetized by chloroform in 1853. What is the molar mass of chloroform if 4.85 grams is 0.918 liters at 35°C and 850 torr?

The statement, "For a fixed mass of gas at constant temperature, gas volume is inversely proportional to gas pressure." is known as:

What volume of oxygen gas, at 533°C and 750 torr, could be produced by the decomposition of 38.1 g of potassium chlorate? The other product is potassium chloride.

A gaseous mixture consists of 50.0% O2, 25.0% N2, and 25.0% Cl2, by mass. At standard temperature and pressure, the partial pressure of:

In the reaction CH4 + 2 O2 → CO2 + 2 H2O, how many liters of O2 react with 5.0 liters of CH4? All gas volumes are measured at the same temperature and pressure but not at STP.

A sample of oxygen gas is collected over water at 23°C at a barometric pressure of 751 mmHg (the vapor pressure of water at 23°C = 21 mmHg). The partial pressure of oxygen gas in the sample collected is ________.

How many liters of gas is 23.4 grams of nitrogen at 750 mmHg and 28.0°C?

Convert to the equivalent pressure in atmospheres, 421 kPa.

A 1.37 L vessel contains He at a temperature of 24.5°C and a pressure of 205 mmHg. A 721 mL vessel contains Ne at a temperature of 36.2°C and a pressure of 0.185 atm. Both of these gases are placed in a 2.00 L vessel at 302 K. What is the final pressure (in atm) in the 2.00 L vessel?

Calculate the height of a column of liquid glycerol (d = 1.26 g/cm3), in meters, required to exert the same pressure as 4.91 m of water.

2.24 L NH3(g) at 2.0 atm and 0°C:

If 4.800 × 10-5 mol of uranium-238 will effuse through a hole in 125 seconds, how many mol of uranium-235 will effuse through the same hole in the same amount of time?

According to the kinetic-molecular theory of gases:

Calculate the height in meters of a column of liquid glycerol (density = 1.26 g/cm3) required to exert the same pressure as 760 mmHg (d = 13.60 g/cm3).

A gaseous hydrocarbon weighing 0.290 g occupies a volume of 125 mL at 25°C and 760 mmHg. What is the molar mass of this compound?

Convert to the equivalent pressure in atmospheres, 1250 mmHg.

Convert 8.50 kg/cm2 to the equivalent pressure in atmospheres.

Of the following values, the most likely to be observed for the volume of 1.00 mole of He(g) at 0°C and 1000 atm is:

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

How many liters of H₂ are needed to make 327 L of NH₃ by the reaction: N₂ (g) + 3 H₂ (g) → 2 NH₃ (g), If the gases are at the same temperature and pressure?

A gaseous mixture consists of 50.0% O₂, 25.0% N₂, and 25.0% Cl₂, by mass. At standard temperature and pressure, the partial pressure of:

In the reaction CH₄ + 2 O₂ → CO₂ + 2 H₂O, how many liters of O₂ react with 5.0 liters of CH₄? All gas volumes are measured at the same temperature and pressure but not at STP.

2.24 L NH₃(g) at 2.0 atm and 0°C:

If 4.800 × 10^-5 mol of uranium-238 will effuse through a hole in 125 seconds, how many mol of uranium-235 will effuse through the same hole in the same amount of time?

Convert 8.50 kg/cm² to the equivalent pressure in atmospheres.