Question 1

A "gas" is a substance in which the molecules are separated on the average by distances that are large compared with the sizes of the molecules.

Accepted Answer

A) True 
 B)False

Question 2

Which gas has molecules with the greatest average molecular speed at 25$\circ$C

Accepted Answer

A)  CH4 
B)  Kr 
C)  N2 
D)  CO2 
E)  Ar 
A)  CH4 
B)  Kr 
C)  N2 
D)  CO2 
E)  Ar

Question 3

How many liters of oxygen gas at 153$\circ$C and 0.820 atm can be produced by the decomposition of 22.4 g of solid KClO3 (The other decomposition product is solid potassium chloride.)

Accepted Answer

A)  0.085 L 
B)  3.0 L 
C)  4.20 L 
D)  7.79 L 
E)  11.7 L 
A)  0.085 L 
B)  3.0 L 
C)  4.20 L 
D)  7.79 L 
E)  11.7 L

Question 4

10.0 g of gaseous ammonia and 6.50 g of oxygen gas are introduced into a previously evacuated 5.50 L vessel. If the ammonia and oxygen then react to yield NO gas and water vapor, what is the final density of the gas mixture inside the vessel at 23ºC

Accepted Answer

A)  1.32 g/L 
B)  1.68 g/L 
C)  2.20 g/L 
D)  3.00 g/L 
E)  16.5 g/L 
A)  1.32 g/L 
B)  1.68 g/L 
C)  2.20 g/L 
D)  3.00 g/L 
E)  16.5 g/L

Question 5

5.00 g of hydrogen gas and 50.0 g of oxygen gas are introduced into an otherwise empty 9.00 L steel cylinder, and the hydrogen is ignited by an electric spark. If the reaction product is gaseous water and the temperature of the cylinder is maintained at 35ºC, what is the final gas pressure inside the cylinder

Accepted Answer

A)  0.92 atm 
B)  2.58 atm 
C)  6.96 atm 
D)  7.86 atm 
E)  18.3 atm 
A)  0.92 atm 
B)  2.58 atm 
C)  6.96 atm 
D)  7.86 atm 
E)  18.3 atm

Question 6

A particular coal sample contains 2.32% S. When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume (L) of SO2(g), measured at 25$\circ$C and 749 mmHg, is produced by burning 2.0 * 106 lb of this coal
 (1 lb = 454 g)

Accepted Answer

Question 7

The magnitude of the van der Waals "a" constant reflects the strength of the attractions between molecules of a given type of gas.

Accepted Answer

A) True 
 B)False

Question 8

On a spring morning (20.$\circ$C) you fill your tires to a pressure of 2.25 atmospheres. As you ride along, the tire heats up to 45$\circ$C from the friction on the road. What is the pressure in your tires now in units of atmospheres

Accepted Answer

A)  2.14 atmospheres 
B)  2.34 atmospheres 
C)  2.64 atmospheres 
D)  2.94 atmospheres 
E)  None of the above 
A)  2.14 atmospheres 
B)  2.34 atmospheres 
C)  2.64 atmospheres 
D)  2.94 atmospheres 
E)  None of the above

Question 9

A sample of oxygen gas has a volume of 545 mL at 35$\circ$C. The gas is heated to 151ºC at constant pressure in a container that can contract or expand. What is the final volume of the oxygen gas

Accepted Answer

A)  750. mL 
B)  396 mL 
C)  417 mL 
D)  267 mL 
E)  126 mL 
A)  750. mL 
B)  396 mL 
C)  417 mL 
D)  267 mL 
E)  126 mL

Question 10

Which of these gases will have the greatest density at the same specified temperature and pressure

Accepted Answer

A)  H2 
B)  CClF3 
C)  CO2 
D)  C2H6 
E)  CF4 
A)  H2 
B)  CClF3 
C)  CO2 
D)  C2H6 
E)  CF4

Question 11

A 250 mL flask contains 3.4 g of neon gas at 45$\circ$C. Calculate the pressure of the neon gas inside the flask.

Accepted Answer

A)  0.050 atm 
B)  0.46 atm 
C)  18 atm 
D)  38 atm 
E)  3.5 x 102 atm 
A)  0.050 atm 
B)  0.46 atm 
C)  18 atm 
D)  38 atm 
E)  3.5 x 102 atm

Question 12

Baking powder is made up of sodium hydrogen carbonate and calcium hydrogen phosphate. When baking powder is wet, these components react to produce carbon dioxide. The equation for this reaction is given below.NaHCO3(aq) + CaHPO4(aq) $\rarr$NaCaPO4(aq) + CO2(g) + H2O(l) Assuming all of the carbon dioxide was released as a gas, how many liters of CO2(g) would be formed at room temperature from 4.00 g of NaHCO3 and excess CaHPO4

Accepted Answer

A)  Approximately 1.16 liters 
B)  Approximately 1.36 liters 
C)  Approximately 1.56 liters 
D)  Approximately 1.76 liters 
E)  None of the above 
A)  Approximately 1.16 liters 
B)  Approximately 1.36 liters 
C)  Approximately 1.56 liters 
D)  Approximately 1.76 liters 
E)  None of the above

Question 13

A 792 mg sample of a gas containing only sulfur and oxygen occupies a volume of 372 mL at 54$\circ$C and 678 mmHg. Identify the gas in the sample. (R = 0.08206 L*atm/K*mol)

Accepted Answer

A)  SO 
B)  SO2 
C)  SO3 
D)  S2O 
E)  S2O2 
A)  SO 
B)  SO2 
C)  SO3 
D)  S2O 
E)  S2O2

Question 14

Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100. cm3 at 95$\circ$C, and 1,000. mmHg.

Accepted Answer

A)  0.19 g/mol 
B)  35.3 g/mol 
C)  70.9 g/mol 
D)  137 g/mol 
E)  384 g/mol 
A)  0.19 g/mol 
B)  35.3 g/mol 
C)  70.9 g/mol 
D)  137 g/mol 
E)  384 g/mol

Question 15

If the pressure of a gas sample is quadrupled and the absolute temperature is doubled, by what factor does the volume of the sample change

Accepted Answer

A)  8 
B)  2 
C)  1/2 
D)  1/4 
E)  1/8 
A)  8 
B)  2 
C)  1/2 
D)  1/4 
E)  1/8

Question 16

Calculate the volume occupied by 25.2 g of CO2 at 0.84 atm and 25$\circ$C. R = 0.08206 L.atm/K.mol.

Accepted Answer

A)  0.060 L 
B)  1.34 L 
C)  16.7 L 
D)  24.2 L 
E)  734 L 
A)  0.060 L 
B)  1.34 L 
C)  16.7 L 
D)  24.2 L 
E)  734 L

Question 17

How many grams of N2O, nitrous oxide, are contained in 500. mL of the gas at STP

Accepted Answer

A)  0.782 g 
B)  0.882 g 
C)  0.982 g 
D)  1.082 g 
E)  None of the above 
A)  0.782 g 
B)  0.882 g 
C)  0.982 g 
D)  1.082 g 
E)  None of the above

Question 18

Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O2) when stored at 22$\circ$C in a 40.0 L cylinder

Accepted Answer

A)  3.6 atm 
B)  10. atm 
C)  47 atm 
D)  1,500 atm 
E)  7.6 * 104 atm 
A)  3.6 atm 
B)  10. atm 
C)  47 atm 
D)  1,500 atm 
E)  7.6 * 104 atm

Question 19

Which of the following describes Dalton's Law

Accepted Answer

A)  The pressure of a gas is proportional to its volume. 
B)  The total pressure of a gas mixture is the sum of the partial pressures of each gas in the mixture. 
C)  The temperature of a gas is proportional to its volume. 
D)  Only one variable can be changed from an initial state to a final state for a gas. 
A)  The pressure of a gas is proportional to its volume. 
B)  The total pressure of a gas mixture is the sum of the partial pressures of each gas in the mixture. 
C)  The temperature of a gas is proportional to its volume. 
D)  Only one variable can be changed from an initial state to a final state for a gas.

Question 20

Today is a beautiful day for a picnic in the mountains, so we seal our peanut butter sandwich in a plastic sandwich bag at the base of the mountain. The approximate volume of the sandwich bag not occupied by the sandwich is 200. mL. The pressure at the base of the mountain is 1.0 atm. If the pressure at the top of the mountain is 0.80 atm, what is the final volume (mL) of gas in our sandwich bag

Accepted Answer

A)  250 mL 
B)  260 mL 
C)  270 mL 
D)  280 mL 
E)  None of the above 
A)  250 mL 
B)  260 mL 
C)  270 mL 
D)  280 mL 
E)  None of the above

Exam 5: Gases

A "gas" is a substance in which the molecules are separated on the average by distances that are large compared with the sizes of the molecules.

Which gas has molecules with the greatest average molecular speed at 25 ∘\circ∘ C

How many liters of oxygen gas at 153 ∘\circ∘ C and 0.820 atm can be produced by the decomposition of 22.4 g of solid KClO3 (The other decomposition product is solid potassium chloride.)

10.0 g of gaseous ammonia and 6.50 g of oxygen gas are introduced into a previously evacuated 5.50 L vessel. If the ammonia and oxygen then react to yield NO gas and water vapor, what is the final density of the gas mixture inside the vessel at 23ºC

A particular coal sample contains 2.32% S. When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume (L) of SO2(g), measured at 25 ∘\circ∘ C and 749 mmHg, is produced by burning 2.0 * 106 lb of this coal (1 lb = 454 g)

The magnitude of the van der Waals "a" constant reflects the strength of the attractions between molecules of a given type of gas.

On a spring morning (20. ∘\circ∘ C) you fill your tires to a pressure of 2.25 atmospheres. As you ride along, the tire heats up to 45 ∘\circ∘ C from the friction on the road. What is the pressure in your tires now in units of atmospheres

A sample of oxygen gas has a volume of 545 mL at 35 ∘\circ∘ C. The gas is heated to 151ºC at constant pressure in a container that can contract or expand. What is the final volume of the oxygen gas

Which of these gases will have the greatest density at the same specified temperature and pressure

A 250 mL flask contains 3.4 g of neon gas at 45 ∘\circ∘ C. Calculate the pressure of the neon gas inside the flask.

A 792 mg sample of a gas containing only sulfur and oxygen occupies a volume of 372 mL at 54 ∘\circ∘ C and 678 mmHg. Identify the gas in the sample. (R = 0.08206 L*atm/K*mol)

Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100. cm3 at 95 ∘\circ∘ C, and 1,000. mmHg.

If the pressure of a gas sample is quadrupled and the absolute temperature is doubled, by what factor does the volume of the sample change

Calculate the volume occupied by 25.2 g of CO2 at 0.84 atm and 25 ∘\circ∘ C. R = 0.08206 L.atm/K.mol.

How many grams of N2O, nitrous oxide, are contained in 500. mL of the gas at STP

Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O2) when stored at 22 ∘\circ∘ C in a 40.0 L cylinder

Which of the following describes Dalton's Law

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Which gas has molecules with the greatest average molecular speed at 25^$\circ$C

How many liters of oxygen gas at 153^$\circ$C and 0.820 atm can be produced by the decomposition of 22.4 g of solid KClO₃ (The other decomposition product is solid potassium chloride.)

A particular coal sample contains 2.32% S. When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume (L) of SO₂(g), measured at 25^$\circ$C and 749 mmHg, is produced by burning 2.0 * 10⁶ lb of this coal (1 lb = 454 g)

On a spring morning (20.^$\circ$C) you fill your tires to a pressure of 2.25 atmospheres. As you ride along, the tire heats up to 45^$\circ$C from the friction on the road. What is the pressure in your tires now in units of atmospheres

A sample of oxygen gas has a volume of 545 mL at 35^$\circ$C. The gas is heated to 151ºC at constant pressure in a container that can contract or expand. What is the final volume of the oxygen gas

A 250 mL flask contains 3.4 g of neon gas at 45^$\circ$C. Calculate the pressure of the neon gas inside the flask.

A 792 mg sample of a gas containing only sulfur and oxygen occupies a volume of 372 mL at 54^$\circ$C and 678 mmHg. Identify the gas in the sample. (R = 0.08206 Latm/Kmol)

Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100. cm³ at 95^$\circ$C, and 1,000. mmHg.

Calculate the volume occupied by 25.2 g of CO₂ at 0.84 atm and 25^$\circ$C. R = 0.08206 L.atm/K.mol.

How many grams of N₂O, nitrous oxide, are contained in 500. mL of the gas at STP

Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O₂) when stored at 22^$\circ$C in a 40.0 L cylinder