Exam 5: Gases and the Kinetic-Molecular Theory

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State Amontons's Law and illustrate it with a graph, using standard x-y coordinate axes. Be sure to label the axes unambiguously with the correct gas variables.

(Essay)

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Question 81

Small quantities of hydrogen can be prepared by the addition of hydrochloric acid to zinc. A sample of 195 mL of hydrogen was collected over water at 25 $\degree$ C and 753 torr. What mass of hydrogen was collected? (P_water = 24 torr at 25 $\degree$ C)

(Multiple Choice)

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Question 82

A flask containing argon gas is connected to an closed-ended mercury manometer. The closed end is under vacuum. If the mercury level in the closed arm is 230. mm above that in the arm connected to the flask, what is the argon pressure, in torr?

(Multiple Choice)

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Question 83

The rate of diffusion of a gas is inversely proportional to its molar mass.

(True/False)

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Question 84

A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remained constant. If the initial volume is 400 mL, what is the final volume?

(Multiple Choice)

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Question 85

State Avogadro's Law.

(Short Answer)

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Question 86

A gas consists of 85.7 % carbon and 14.3% hydrogen, by weight. A sample of this gas weighing 0.673 g occupies 729 mL at a pressure of 720.0 mmHg and a temperature of 77 $\degree$ C. Calculate its empirical and molecular formulas.

(Multiple Choice)

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Question 87

The ideal gas law tends to become inaccurate when

(Multiple Choice)

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Question 88

According to the postulates of kinetic-molecular theory, the molecules of all gases at a given temperature have the same average kinetic energy.

(True/False)

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Question 89

"The rate of effusion of a gas is inversely proportional to the square root of its molar mass" is a statement of ______________________ Law.

(Multiple Choice)

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Question 90

For a gas obeying Charles's Law, a plot of V versus 1/T will give a straight line passing through the origin.

(True/False)

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Question 91

A compound composed of carbon, hydrogen, and chlorine effuses through a pinhole 0.411 times as fast as neon. Select the correct molecular formula for the compound.

(Multiple Choice)

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Question 92

. If the partial pressure of argon is 200. torr, what is the pressure of methane, in torr?

(Multiple Choice)

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Question 93

"The total pressure in a mixture of unreacting gases is equal to the sum of the partial pressures of the individual gases" is a statement of __________________ Law.

(Multiple Choice)

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Question 94

The ozone layer is important because

(Multiple Choice)

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Question 95

Select the gas with the highest average kinetic energy per mole at 298 K.

(Multiple Choice)

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Question 96

Use the van der Waals equation for real gases to calculate the pressure exerted by 1.00 mole of ammonia at 27 $\degree$ C in a 750-mL container. (a = 4.17 L²*atm/mol², b = 0.0371 L/mol)

(Multiple Choice)

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Question 97

Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its pressure, other factors remaining constant?

(Multiple Choice)

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Question 98

A flask with a volume of 3.16 L contains 9.33 grams of an unknown gas at 32.0 $\degree$ C and 1.00 atm. What is the molar mass of the gas?

(Multiple Choice)

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Question 99

A carbon dioxide sample weighing 44.0 g occupies 32.68 L at 65 $\degree$ C and 645 torr. What is its volume at STP?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 103

Exam 5: Gases and the Kinetic-Molecular Theory

State Amontons's Law and illustrate it with a graph, using standard x-y coordinate axes. Be sure to label the axes unambiguously with the correct gas variables.

Small quantities of hydrogen can be prepared by the addition of hydrochloric acid to zinc. A sample of 195 mL of hydrogen was collected over water at 25 °\degree° C and 753 torr. What mass of hydrogen was collected? (Pwater = 24 torr at 25 °\degree° C)

A flask containing argon gas is connected to an closed-ended mercury manometer. The closed end is under vacuum. If the mercury level in the closed arm is 230. mm above that in the arm connected to the flask, what is the argon pressure, in torr?

The rate of diffusion of a gas is inversely proportional to its molar mass.

A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remained constant. If the initial volume is 400 mL, what is the final volume?

State Avogadro's Law.

A gas consists of 85.7 % carbon and 14.3% hydrogen, by weight. A sample of this gas weighing 0.673 g occupies 729 mL at a pressure of 720.0 mmHg and a temperature of 77 °\degree° C. Calculate its empirical and molecular formulas.

The ideal gas law tends to become inaccurate when

According to the postulates of kinetic-molecular theory, the molecules of all gases at a given temperature have the same average kinetic energy.

"The rate of effusion of a gas is inversely proportional to the square root of its molar mass" is a statement of ______________________ Law.

For a gas obeying Charles's Law, a plot of V versus 1/T will give a straight line passing through the origin.

A compound composed of carbon, hydrogen, and chlorine effuses through a pinhole 0.411 times as fast as neon. Select the correct molecular formula for the compound.

. If the partial pressure of argon is 200. torr, what is the pressure of methane, in torr?

"The total pressure in a mixture of unreacting gases is equal to the sum of the partial pressures of the individual gases" is a statement of __________________ Law.

The ozone layer is important because

Select the gas with the highest average kinetic energy per mole at 298 K.

Use the van der Waals equation for real gases to calculate the pressure exerted by 1.00 mole of ammonia at 27 °\degree° C in a 750-mL container. (a = 4.17 L2*atm/mol2, b = 0.0371 L/mol)

Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its pressure, other factors remaining constant?

A flask with a volume of 3.16 L contains 9.33 grams of an unknown gas at 32.0 °\degree° C and 1.00 atm. What is the molar mass of the gas?

A carbon dioxide sample weighing 44.0 g occupies 32.68 L at 65 °\degree° C and 645 torr. What is its volume at STP?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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Small quantities of hydrogen can be prepared by the addition of hydrochloric acid to zinc. A sample of 195 mL of hydrogen was collected over water at 25 $\degree$ C and 753 torr. What mass of hydrogen was collected? (P_water = 24 torr at 25 $\degree$ C)

A gas consists of 85.7 % carbon and 14.3% hydrogen, by weight. A sample of this gas weighing 0.673 g occupies 729 mL at a pressure of 720.0 mmHg and a temperature of 77 $\degree$ C. Calculate its empirical and molecular formulas.

Use the van der Waals equation for real gases to calculate the pressure exerted by 1.00 mole of ammonia at 27 $\degree$ C in a 750-mL container. (a = 4.17 L²*atm/mol², b = 0.0371 L/mol)

A flask with a volume of 3.16 L contains 9.33 grams of an unknown gas at 32.0 $\degree$ C and 1.00 atm. What is the molar mass of the gas?

A carbon dioxide sample weighing 44.0 g occupies 32.68 L at 65 $\degree$ C and 645 torr. What is its volume at STP?