Question 1

Given the equation   
Determine the number of liters of O2 consumed at STP when 270.0 grams of C2H6 is burned.

Accepted Answer

Question 2

The density of ammonia gas in a 4.32 L container at 837 torr and 45.0 °C is g/L.

Accepted Answer

A)  3.86 
B)  0.194 
C)  0.717 
D)  4.22 × 10- 2 
E)  0.432 
A)  3.86 
B)  0.194 
C)  0.717 
D)  4.22 × 10- 2 
E)  0.432

Question 3

What volume (L) of NH3 gas at STP is produced by the complete reaction of 7.5 g of H2O according to the following reaction?

Accepted Answer

A)  3.1 
B)  19 
C)  28 
D)  9.3 
E)  0.32 
A)  3.1 
B)  19 
C)  28 
D)  9.3 
E)  0.32

Question 4

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

Accepted Answer

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

Question 5

A sample of oxygen gas (O2) was found to effuse at a rate equal to three times that of an unknown gas. The molecular weight of the unknown gas is g/mol.

Accepted Answer

A)  4 
B)  10.7 
C)  96 
D)  288 
E)  55 
A)  4 
B)  10.7 
C)  96 
D)  288 
E)  55

Question 6

Zinc reacts with aqueous sulfuric acid to form hydrogen gas:
 
In an experiment, 225 mL of wet H2 is collected over water at 27 °C and a barometric pressure of 748 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27 °C is
26)74 torr.

Accepted Answer

A)  567 
B)  4.79 × 106  
C)  4.31 × 105  
D)  0.567 
E)  431 
A)  567 
B)  4.79 × 106  
C)  4.31 × 105  
D)  0.567 
E)  431

Question 7

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

Question 8

Arrange the following gases in order of increasing average molecular speed at 25 °C.

Accepted Answer

A)  CO2 2 2 2 2 2 
C)  CO2 2 2 2 2 2 
E)  He 2 2 2 
A)  CO2 2 2 2 2 2 
C)  CO2 2 2 2 2 2 
E)  He 2 2 2

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 mmHg.

Accepted Answer

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

Question 10

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

Question 11

The density of chlorine (Cl2) gas at 25 °C and 60. kPa is g/L)

Accepted Answer

A)  20 
B)  4.9 
C)  0.86 
D)  0.58 
E)  1.7 
A)  20 
B)  4.9 
C)  0.86 
D)  0.58 
E)  1.7

Question 12

A gas vessel is attached to an open- end manometer filled with a nonvolatile liquid of density 0.993 g/mL as shown below.
 
The difference in heights of the liquid in the two sides of the manometer is 32.3 cm when the atmospheric pressure is 765 mmHg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is atm.

Accepted Answer

A)  0.976 
B)  1.08 
C)  1.04 
D)  1.01 
E)  0.993 
A)  0.976 
B)  1.08 
C)  1.04 
D)  1.01 
E)  0.993

Question 13

A closed- end manometer was attached to a vessel containing argon. The difference in the mercury levels in the two arms of the manometer was 12.2 cm. Atmospheric pressure was 783 mmHg. The pressure of the argon in the container was mmHg.

Accepted Answer

A)  661 
B)  122 
C)  882 
D)  771 
E)  795 
A)  661 
B)  122 
C)  882 
D)  771 
E)  795

Question 14

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

Question 15

Calcium hydride (CaH2) reacts with water to form hydrogen gas:
 
How many grams of CaH2 are needed to generate 48.0 L of H2 gas at a pressure of 0.888 atm and a temperature of 32 °C?

Accepted Answer

A)  50.7 
B)  71.7 
C)  143 
D)  35.8 
E)  0.851 
A)  50.7 
B)  71.7 
C)  143 
D)  35.8 
E)  0.851

Question 16

The rms speed of methane molecules at 45.0 °C is m/sec.

Accepted Answer

The answer of The rms speed of methane molecules at...

Question 17

The volume of 0.65 mol of an ideal gas at 365 torr and 97 °C is _ L.

Accepted Answer

A)  0.054 
B)  9.5 
C)  41 
D)  11 
E)  2.4 × 10- 2 
A)  0.054 
B)  9.5 
C)  41 
D)  11 
E)  2.4 × 10- 2

Question 18

The kinetic- molecular theory predicts that pressure rises as the temperature of a gas increases because _ .

Accepted Answer

A)  the gas molecules collide less frequently with the wall 
B)  the gas molecules collide more frequently with the wall 
C)  the average kinetic energy of the gas molecules decreases 
D)  the gas molecules collide more energetically with the wall 
E)  both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall 
A)  the gas molecules collide less frequently with the wall 
B)  the gas molecules collide more frequently with the wall 
C)  the average kinetic energy of the gas molecules decreases 
D)  the gas molecules collide more energetically with the wall 
E)  both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall

Question 19

Which one of the following gases would deviate the least from ideal gas behavior?

Accepted Answer

A)  CH3Cl 
B)  F2  
C)  Ne 
D)  CO2  
E)  Kr 
A)  CH3Cl 
B)  F2  
C)  Ne 
D)  CO2  
E)  Kr

Question 20

The reaction of 50 mL of Cl2 gas with 50 mL of CH4 gas via the equation:
Cl2 (g) + C2H4 (g) -C2H4Cl2 (g)
Will produce a total of mL of products if pressure and temperature are kept constant.

Accepted Answer

A)  125 
B)  150 
C)  50 
D)  25 
E)  100 
A)  125 
B)  150 
C)  50 
D)  25 
E)  100

Exam 10: Gases

Given the equation Determine the number of liters of O2 consumed at STP when 270.0 grams of C2H6 is burned.

The density of ammonia gas in a 4.32 L container at 837 torr and 45.0 °C is g/L.

What volume (L) of NH3 gas at STP is produced by the complete reaction of 7.5 g of H2O according to the following reaction?

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

A sample of oxygen gas (O2) was found to effuse at a rate equal to three times that of an unknown gas. The molecular weight of the unknown gas is g/mol.

Zinc reacts with aqueous sulfuric acid to form hydrogen gas: In an experiment, 225 mL of wet H2 is collected over water at 27 °C and a barometric pressure of 748 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27 °C is 26)74 torr.

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

Arrange the following gases in order of increasing average molecular speed at 25 °C.

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 mmHg.

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 _.

The density of chlorine (Cl2) gas at 25 °C and 60. kPa is g/L)

A closed- end manometer was attached to a vessel containing argon. The difference in the mercury levels in the two arms of the manometer was 12.2 cm. Atmospheric pressure was 783 mmHg. The pressure of the argon in the container was mmHg.

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.

Calcium hydride (CaH2) reacts with water to form hydrogen gas: How many grams of CaH2 are needed to generate 48.0 L of H2 gas at a pressure of 0.888 atm and a temperature of 32 °C?

The rms speed of methane molecules at 45.0 °C is m/sec.

The volume of 0.65 mol of an ideal gas at 365 torr and 97 °C is _ L.

The kinetic- molecular theory predicts that pressure rises as the temperature of a gas increases because _ .

Which one of the following gases would deviate the least from ideal gas behavior?

The reaction of 50 mL of Cl2 gas with 50 mL of CH4 gas via the equation: Cl2 (g) + C2H4 (g) -C2H4Cl2 (g) Will produce a total of mL of products if pressure and temperature are kept constant.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

Filters

Given the equation Determine the number of liters of O₂consumed at STP when 270.0 grams of C₂H₆is burned.

What volume (L) of NH₃gas at STP is produced by the complete reaction of 7.5 g of H₂O according to the following reaction?

A sample of oxygen gas (O₂) was found to effuse at a rate equal to three times that of an unknown gas. The molecular weight of the unknown gas is g/mol.

Zinc reacts with aqueous sulfuric acid to form hydrogen gas: In an experiment, 225 mL of wet H₂is collected over water at 27 °C and a barometric pressure of 748 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27 °C is 26)74 torr.

The density of chlorine (Cl₂) gas at 25 °C and 60. kPa is g/L)

Calcium hydride (CaH₂) reacts with water to form hydrogen gas: How many grams of CaH₂are needed to generate 48.0 L of H₂gas at a pressure of 0.888 atm and a temperature of 32 °C?

The reaction of 50 mL of Cl₂gas with 50 mL of CH₄gas via the equation: Cl₂(g) + C₂H₄(g) -C₂H₄Cl₂(g) Will produce a total of mL of products if pressure and temperature are kept constant.