Question 1

As the temperature of a gas increases, the density of the gas will

Accepted Answer

A) increase. 
B) decrease. 
C) remain constant. 
A) increase. 
B) decrease. 
C) remain constant.

Question 2

According to the kinetic theory of gases, particles of a gas

Accepted Answer

A) are very large. 
B) are very far apart. 
C) lose their valence electrons. 
D) move slowly. 
E) decrease kinetic energy as temperature increases. 
A) are very large. 
B) are very far apart. 
C) lose their valence electrons. 
D) move slowly. 
E) decrease kinetic energy as temperature increases.

Question 3

According to the kinetic theory of gases, a gas can be compressed much more than a liquid or solid because

Accepted Answer

A) a gas is composed of very small particles. 
B) the particles of a gas are very far apart. 
C) gas particles move rapidly. 
D) gas particles do not attract or repel one another. 
E) gas particles move faster when the temperature increases. 
A) a gas is composed of very small particles. 
B) the particles of a gas are very far apart. 
C) gas particles move rapidly. 
D) gas particles do not attract or repel one another. 
E) gas particles move faster when the temperature increases.

Question 4

According to Boyle's, when volume increases, pressure decreases.

Accepted Answer

A) True 
 B)False

Question 5

Oxygen makes up about ________ percent of the atmosphere.

Accepted Answer

The answer of Oxygen makes up about ________ percent of...

Question 6

At 570. mm Hg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C, if the moles are constant?

Accepted Answer

A) 1560 mmHg 
B) 210. mmHg 
C) 700. mmHg 
D) 690. mmHg 
E) 470. mmHg 
A) 1560 mmHg 
B) 210. mmHg 
C) 700. mmHg 
D) 690. mmHg 
E) 470. mmHg

Question 7

The air we breathe is about 21% oxygen.

Accepted Answer

A) True 
 B)False

Question 8

The pressure exerted by the particles of vapor above a liquid is called the ________.

Accepted Answer

A) vapor pressure 
B) barometric pressure 
C) standard pressure 
D) molar pressure 
E) atmospheric pressure 
A) vapor pressure 
B) barometric pressure 
C) standard pressure 
D) molar pressure 
E) atmospheric pressure

Question 9

A sample of argon gas at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0.00 °C. What is the new pressure?

Accepted Answer

A) 105 atm 
B) 45.5 atm 
C) 54.9 atm 
D) 23.8 atm 
E) 42.7 atm 
A) 105 atm 
B) 45.5 atm 
C) 54.9 atm 
D) 23.8 atm 
E) 42.7 atm

Question 10

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr, if the moles are constant?

Accepted Answer

A) 530 mL 
B) 450 mL 
C) 970 mL 
D) 240 mL 
E) 400 mL 
A) 530 mL 
B) 450 mL 
C) 970 mL 
D) 240 mL 
E) 400 mL

Question 11

The atmospheric pressure in Denver, CO is 633 mmHg. What is this pressure in atm?

Accepted Answer

A) 1.20 atm 
B) 633 atm 
C) 0.833 atm 
D) 1.00 atm 
E) 127 atm 
A) 1.20 atm 
B) 633 atm 
C) 0.833 atm 
D) 1.00 atm 
E) 127 atm

Question 12

Ideal Gas Law calculations require the pressure to be in units of atm.

Accepted Answer

A) True 
 B)False

Question 13

The relationship P1V1 = P2V2 is called ________.

Accepted Answer

A) Boyle's Law 
B) Charles's Law 
C) Gay-Lussac's Law 
D) The Combined Gas Law 
E) Avogadro's Law 
A) Boyle's Law 
B) Charles's Law 
C) Gay-Lussac's Law 
D) The Combined Gas Law 
E) Avogadro's Law

Question 14

A tank contains a mixture of helium, neon, and argon gases. If the total pressure in the tank is 490. mmHg and the partial pressures of helium and argon are 215 mmHg and 102 mmHg, respectively, what is the partial pressure of neon?

Accepted Answer

A) 0.228 mmHg 
B) 603 mmHg 
C) 377 mmHg 
D) 807 mmHg 
E) 173 mmHg 
A) 0.228 mmHg 
B) 603 mmHg 
C) 377 mmHg 
D) 807 mmHg 
E) 173 mmHg

Question 15

How many moles of neon occupy a volume of 14.3 L at STP?

Accepted Answer

A) 36.7 moles 
B) 32.0 moles 
C) 6.45 moles 
D) 0.638 moles 
E) 1.57 moles 
A) 36.7 moles 
B) 32.0 moles 
C) 6.45 moles 
D) 0.638 moles 
E) 1.57 moles

Question 16

In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules

Accepted Answer

A) move rapidly in random directions. 
B) are attracted to each other by strong forces. 
C) are close together in their container. 
D) move with a kinetic energy equal to their centigrade temperature. 
E) occasionally come to rest. 
A) move rapidly in random directions. 
B) are attracted to each other by strong forces. 
C) are close together in their container. 
D) move with a kinetic energy equal to their centigrade temperature. 
E) occasionally come to rest.

As the temperature of a gas increases, the density of the gas will

According to the kinetic theory of gases, particles of a gas

According to the kinetic theory of gases, a gas can be compressed much more than a liquid or solid because

According to Boyle's, when volume increases, pressure decreases.

Oxygen makes up about ________ percent of the atmosphere.

At 570. mm Hg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C, if the moles are constant?

The air we breathe is about 21% oxygen.

The pressure exerted by the particles of vapor above a liquid is called the ________.

A sample of argon gas at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0.00 °C. What is the new pressure?

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr, if the moles are constant?

The atmospheric pressure in Denver, CO is 633 mmHg. What is this pressure in atm?

Ideal Gas Law calculations require the pressure to be in units of atm.

The relationship P₁V₁ = P₂V₂ is called ________.

A tank contains a mixture of helium, neon, and argon gases. If the total pressure in the tank is 490. mmHg and the partial pressures of helium and argon are 215 mmHg and 102 mmHg, respectively, what is the partial pressure of neon?

How many moles of neon occupy a volume of 14.3 L at STP?

In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules

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Exam 8: Gases

As the temperature of a gas increases, the density of the gas will

According to the kinetic theory of gases, particles of a gas

According to the kinetic theory of gases, a gas can be compressed much more than a liquid or solid because

According to Boyle's, when volume increases, pressure decreases.

Oxygen makes up about ________ percent of the atmosphere.

At 570. mm Hg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C, if the moles are constant?

The air we breathe is about 21% oxygen.

The pressure exerted by the particles of vapor above a liquid is called the ________.

A sample of argon gas at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0.00 °C. What is the new pressure?

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr, if the moles are constant?

The atmospheric pressure in Denver, CO is 633 mmHg. What is this pressure in atm?

Ideal Gas Law calculations require the pressure to be in units of atm.

The relationship P1V1 = P2V2 is called ________.

A tank contains a mixture of helium, neon, and argon gases. If the total pressure in the tank is 490. mmHg and the partial pressures of helium and argon are 215 mmHg and 102 mmHg, respectively, what is the partial pressure of neon?

How many moles of neon occupy a volume of 14.3 L at STP?

In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules

Chemistry in Our Lives

Chemistry and Measurements

Energy and Matter

Atoms

Nuclear Chemistry

Ionic and Molecular Compounds

Chemical Reactions and Quantities

Solutions

Reaction Rates and Chemical Equilibrium

Acids and Bases

Introduction to Organic Chemistry: Hydrocarbons

Alcohols, Phenols, Thiols, and Ethers

Aldehydes, Ketones, and Chiral Molecules

Carbohydrates

Carboxylic Acids and Esters

Lipids

Amines and Amides

Amino Acids and Proteins

Enzymes and Vitamins

Nucleic Acids and Protein Synthesis

Metabolic Pathways for Carbohydrates

Metabolism and Energy Production

Metabolic Pathways for Lipids and Amino Acids

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The relationship P₁V₁ = P₂V₂ is called ________.