Question 1

The volume of HCl gas required to react with excess Ca to produce 11.4 L of hydrogen gas at 1.62 atm and 62.0°C is __________ L.

Accepted Answer

The answer of The volume of HCl gas required to...

Question 2

A gas is considered "ideal" if one mole of it in a one-liter container exerts a pressure of exactly 1 atm at room temperature.

Accepted Answer

A) True 
 B)False

Question 3

In ideal gas equation calculations, expressing pressure in Pascals (Pa), necessitates the use of the gas constant, R, equal to __________.

Accepted Answer

A) 0.08206 atm L mol-1K-1 
B) 8.314 J mol-1K-1 
C) 62.36 L torr mol-1K-1 
D) 1.987 cal mol-1K-1 
E) none of the above 
A) 0.08206 atm L mol-1K-1 
B) 8.314 J mol-1K-1 
C) 62.36 L torr mol-1K-1 
D) 1.987 cal mol-1K-1 
E) none of the above

Question 4

At 333 K, which of the pairs of gases below would have the most nearly identical rates of effusion?

Accepted Answer

A) N2O and NO2 
B) CO and N2 
C) N2 and O2 
D) CO and CO2 
E) NO2 and N2O4 
A) N2O and NO2 
B) CO and N2 
C) N2 and O2 
D) CO and CO2 
E) NO2 and N2O4

Question 5

The density of air at STP is 1.285 g/L. Which of the following cannot be used to fill a balloon that will float in air at STP?

Accepted Answer

A) CH4 
B) NO 
C) Ne 
D) N H3 
E) HF 
A) CH4 
B) NO 
C) Ne 
D) N H3 
E) HF

Question 6

A 1.44-g sample of an unknown pure gas occupies a volume of 0.335 L at a pressure of 1.00 atm and a temperature of 100.0°C. The unknown gas is __________.

Accepted Answer

A) argon 
B) helium 
C) krypton 
D) neon 
E) xenon 
A) argon 
B) helium 
C) krypton 
D) neon 
E) xenon

Question 7

A sample of a gas originally at 25°C and 1.00 atm pressure in a 2.5 L container is subject to a pressure of 0.85 atm and a temperature of 15°C. The final volume of the gas is __________ L.

Accepted Answer

A) 3.0 
B) 2.8 
C) 2.6 
D) 2.1 
E) 0.38 
A) 3.0 
B) 2.8 
C) 2.6 
D) 2.1 
E) 0.38

Question 8

The volume of 0.25 mol of a gas at 72.7 kPa and 15°C is __________ m3.

Accepted Answer

A) 8.1 × 10-5 
B) 1.2 × 10-4 
C) 4.3 × 10-4 
D) 8.2 × 10-3 
E) 2.2 × 10-1 
A) 8.1 × 10-5 
B) 1.2 × 10-4 
C) 4.3 × 10-4 
D) 8.2 × 10-3 
E) 2.2 × 10-1

Question 9

The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42 °C is __________ mm Hg.

Accepted Answer

A) 263 
B) 134 
C) 395 
D) 116 
E) 0.347 
A) 263 
B) 134 
C) 395 
D) 116 
E) 0.347

Question 10

The reaction of 100 mL of Cl2 gas with 100 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 11

The density of N2O at 1.53 atm and 45.2°C is __________ g/L.

Accepted Answer

A) 18.2 
B) 1.76 
C) 0.388 
D) 9.99 
E) 2.58 
A) 18.2 
B) 1.76 
C) 0.388 
D) 9.99 
E) 2.58

Question 12

A sample of H2 gas (12.28 g)occupies 100.0 L at 400.0 K and 2.00 atm. A sample weighing 9.49 g occupies __________ L at 353 K and 2.00 atm.

Accepted Answer

A) 109 
B) 68.2 
C) 54.7 
D) 147 
E) 77.3 
A) 109 
B) 68.2 
C) 54.7 
D) 147 
E) 77.3

Question 13

The volume of hydrogen gas at 38.0°C and 763 torr that can be produced by the reaction of 4.33 g of zinc with excess sulfuric acid is __________ L.

Accepted Answer

A) 1.68 
B) 2.71 × 10-4 
C) 3.69 × 104 
D) 2.84 
E) 0.592 
A) 1.68 
B) 2.71 × 10-4 
C) 3.69 × 104 
D) 2.84 
E) 0.592

Question 14

The density of nitric oxide (NO)gas at 1.21 atm and 46.2°C is __________ g/L.

Accepted Answer

A) 0.0462 
B) 0.722 
C) 1.39 
D) 0.319 
E) 9.6 
A) 0.0462 
B) 0.722 
C) 1.39 
D) 0.319 
E) 9.6

Question 15

Which of the following is not part of the kinetic-molecular theory?

Accepted Answer

A) Atoms are neither created nor destroyed by ordinary chemical reactions. 
B) Attractive and repulsive forces between gas molecules are negligible. 
C) Gases consist of molecules in continuous, random motion. 
D) Collisions between gas molecules do not result in the loss of energy. 
E) The volume occupied by all of the gas molecules in a container is negligible compared to the volume of the container. 
A) Atoms are neither created nor destroyed by ordinary chemical reactions. 
B) Attractive and repulsive forces between gas molecules are negligible. 
C) Gases consist of molecules in continuous, random motion. 
D) Collisions between gas molecules do not result in the loss of energy. 
E) The volume occupied by all of the gas molecules in a container is negligible compared to the volume of the container.

Question 16

The density of chlorine gas at 1.21 atm and 34.9°C is __________ g/L.

Accepted Answer

A) 0.0479 
B) 0.295 
C) 0.423 
D) 1.70 
E) 3.39 
A) 0.0479 
B) 0.295 
C) 0.423 
D) 1.70 
E) 3.39

Question 17

SO2 (5.00 g)and CO2 (5.00 g)were placed in a 750.0 mL container at 50.0°C. The partial pressure of CO2 in the container was __________ atm.

Accepted Answer

A) 6.78 
B) 2.76 
C) 1.60 
D) 0.192 
E) 4.02 
A) 6.78 
B) 2.76 
C) 1.60 
D) 0.192 
E) 4.02

Question 18

The Mond process produces pure nickel metal via the thermal decomposition of nickel tetracarbonyl: Ni(CO)4 (l)→ Ni (s)+ 4CO (g).
What volume (L)of CO is formed from the complete decomposition of 444 g of Ni(CO)4 at 752 torr and 22.0°C?

Accepted Answer

A) 0.356 
B) 63.7 
C) 255 
D) 20.2 
E) 11.0 
A) 0.356 
B) 63.7 
C) 255 
D) 20.2 
E) 11.0

Question 19

Sodium bicarbonate is reacted with concentrated hydrochloric acid at 25.0°C and 1.50 atm. The reaction of 7.75 kg of bicarbonate with excess hydrochloric acid under these conditions will produce __________ L of CO2.

Accepted Answer

A) 1.82 x 103 
B) 2.85 x 104 
C) 1.82 x 104 
D) 1.50 x 103 
E) 8.70 x 102 
A) 1.82 x 103 
B) 2.85 x 104 
C) 1.82 x 104 
D) 1.50 x 103 
E) 8.70 x 102

Question 20

SO2 (5.00 g)and CO2 (5.00 g)are placed in a 750.0 mL container at 50.0°C. The partial pressure of SO2 in the container was __________ atm.

Accepted Answer

A) 2.76 
B) 4.02 
C) 6.78 
D) 0.192 
E) 1.60 
A) 2.76 
B) 4.02 
C) 6.78 
D) 0.192 
E) 1.60

Exam 10: Gases

The volume of HCl gas required to react with excess Ca to produce 11.4 L of hydrogen gas at 1.62 atm and 62.0°C is __________ L.

A gas is considered "ideal" if one mole of it in a one-liter container exerts a pressure of exactly 1 atm at room temperature.

In ideal gas equation calculations, expressing pressure in Pascals (Pa), necessitates the use of the gas constant, R, equal to __________.

At 333 K, which of the pairs of gases below would have the most nearly identical rates of effusion?

The density of air at STP is 1.285 g/L. Which of the following cannot be used to fill a balloon that will float in air at STP?

A 1.44-g sample of an unknown pure gas occupies a volume of 0.335 L at a pressure of 1.00 atm and a temperature of 100.0°C. The unknown gas is __________.

A sample of a gas originally at 25°C and 1.00 atm pressure in a 2.5 L container is subject to a pressure of 0.85 atm and a temperature of 15°C. The final volume of the gas is __________ L.

The volume of 0.25 mol of a gas at 72.7 kPa and 15°C is __________ m3.

The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42 °C is __________ mm Hg.

The reaction of 100 mL of Cl2 gas with 100 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 density of N2O at 1.53 atm and 45.2°C is __________ g/L.

A sample of H2 gas (12.28 g)occupies 100.0 L at 400.0 K and 2.00 atm. A sample weighing 9.49 g occupies __________ L at 353 K and 2.00 atm.

The volume of hydrogen gas at 38.0°C and 763 torr that can be produced by the reaction of 4.33 g of zinc with excess sulfuric acid is __________ L.

The density of nitric oxide (NO)gas at 1.21 atm and 46.2°C is __________ g/L.

Which of the following is not part of the kinetic-molecular theory?

The density of chlorine gas at 1.21 atm and 34.9°C is __________ g/L.

SO2 (5.00 g)and CO2 (5.00 g)were placed in a 750.0 mL container at 50.0°C. The partial pressure of CO2 in the container was __________ atm.

The Mond process produces pure nickel metal via the thermal decomposition of nickel tetracarbonyl: Ni(CO)4 (l)→ Ni (s)+ 4CO (g). What volume (L)of CO is formed from the complete decomposition of 444 g of Ni(CO)4 at 752 torr and 22.0°C?

Sodium bicarbonate is reacted with concentrated hydrochloric acid at 25.0°C and 1.50 atm. The reaction of 7.75 kg of bicarbonate with excess hydrochloric acid under these conditions will produce __________ L of CO2.

SO2 (5.00 g)and CO2 (5.00 g)are placed in a 750.0 mL container at 50.0°C. The partial pressure of SO2 in the container was __________ atm.

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

The volume of 0.25 mol of a gas at 72.7 kPa and 15°C is __________ m³.

The reaction of 100 mL of Cl₂ gas with 100 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 density of N₂O at 1.53 atm and 45.2°C is __________ g/L.

A sample of H₂ gas (12.28 g)occupies 100.0 L at 400.0 K and 2.00 atm. A sample weighing 9.49 g occupies __________ L at 353 K and 2.00 atm.

SO₂ (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0°C. The partial pressure of CO₂ in the container was __________ atm.

The Mond process produces pure nickel metal via the thermal decomposition of nickel tetracarbonyl: Ni(CO)₄ (l)→ Ni (s)+ 4CO (g). What volume (L)of CO is formed from the complete decomposition of 444 g of Ni(CO)₄ at 752 torr and 22.0°C?

Sodium bicarbonate is reacted with concentrated hydrochloric acid at 25.0°C and 1.50 atm. The reaction of 7.75 kg of bicarbonate with excess hydrochloric acid under these conditions will produce __________ L of CO₂.

SO₂ (5.00 g)and CO₂ (5.00 g)are placed in a 750.0 mL container at 50.0°C. The partial pressure of SO₂ in the container was __________ atm.