Exam 5: Gases and the Kinetic-Molecular Theory

A weather balloon was initially at a pressure of 0.950 atm, and its volume was 35.0 L. The pressure decreased to 0.750 atm, without loss of gas or change in temperature. What was the change in the volume?

(Multiple Choice)

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Question 41

A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?

(Multiple Choice)

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Question 42

Aluminum metal shavings (10.0 g) are placed in 100. mL of 6.00 M hydrochloric acid. What is the maximum volume of hydrogen, measured at STP, which can be produced? 2Al(s) + 6HCl(aq)  2AlCl₃(aq) + 3H₂(g)

(Short Answer)

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Question 43

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

(Short Answer)

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Question 44

For an ideal gas, a plot of PV/nRT versus P gives a straight line with a positive slope.

(True/False)

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Question 45

What is the pressure in a 7.50-L flask if 0.15 mol of carbon dioxide is added to 0.33 mol of oxygen? The temperature of the mixture is 48.0°C.

(Multiple Choice)

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Question 46

A 500-mL sample of argon at 800 torr has its absolute temperature quadrupled. If the volume remains unchanged what is the new pressure?

(Multiple Choice)

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Question 47

A flask containing neon gas is connected to an open-ended mercury manometer. The open end is exposed to the atmosphere, where the prevailing pressure is 745 torr. The mercury level in the open arm is 50. mm below that in the arm connected to the flask of neon. What is the neon pressure, in torr?

(Multiple Choice)

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Question 48

State Avogadro's Law.

(Essay)

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Question 49

A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100 torr, what is the new pressure?

(Multiple Choice)

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Question 50

The most probable speed of an oxygen molecule in the gas phase at room temperature is 450 m/s. The root-mean-square speed (u_rms) is therefore

(Multiple Choice)

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Question 51

A sample of ammonia gas at 65.5°C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is -15.8°C and its pressure is 524 torr?

(Multiple Choice)

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Question 52

What are the conditions of STP?

(Multiple Choice)

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Question 53

A flask containing argon gas is connected to a 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 54

According to the kinetic theory of gases, in a collision between two molecules the kinetic energy of one molecule will decrease by the same amount that the kinetic energy of the other one increases.

(True/False)

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Question 55

Nitrogen will behave most like an ideal gas

(Multiple Choice)

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Question 56

A 20.0-L container holds 15.3 mol of Cl₂ gas at 227°C. a. Calculate the pressure in atmospheres, assuming ideal behavior. b. Calculate the pressure in atmospheres, assuming van der Waals behavior. The van der Waals constants for Cl₂ are a = 6.49 atmL²/mol² and b = 0.0562 L/mol.

(Essay)

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Question 57

If 0.750 L of argon at 1.50 atm and 177°C and 0.235 L of sulfur dioxide at 95.0 kPa and 63.0°C are added to a 1.00-L flask and the flask's temperature is adjusted to 25.0°C, what is the resulting pressure in the flask?

(Multiple Choice)

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Question 58

At very high pressures (~ 1000 atm), the measured pressure exerted by real gases is greater than that predicted by the ideal gas equation. This is mainly because

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Question 59

Starting from the Ideal Gas Equation, derive an equation corresponding to Charles's Law, stating all important assumptions or conditions.

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Question 60

Showing 41 - 60 of 115

Exam 5: Gases and the Kinetic-Molecular Theory

A weather balloon was initially at a pressure of 0.950 atm, and its volume was 35.0 L. The pressure decreased to 0.750 atm, without loss of gas or change in temperature. What was the change in the volume?

A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?

Aluminum metal shavings (10.0 g) are placed in 100. mL of 6.00 M hydrochloric acid. What is the maximum volume of hydrogen, measured at STP, which can be produced? 2Al(s) + 6HCl(aq)  2AlCl3(aq) + 3H2(g)

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

For an ideal gas, a plot of PV/nRT versus P gives a straight line with a positive slope.

What is the pressure in a 7.50-L flask if 0.15 mol of carbon dioxide is added to 0.33 mol of oxygen? The temperature of the mixture is 48.0°C.

A 500-mL sample of argon at 800 torr has its absolute temperature quadrupled. If the volume remains unchanged what is the new pressure?

A flask containing neon gas is connected to an open-ended mercury manometer. The open end is exposed to the atmosphere, where the prevailing pressure is 745 torr. The mercury level in the open arm is 50. mm below that in the arm connected to the flask of neon. What is the neon pressure, in torr?

State Avogadro's Law.

A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100 torr, what is the new pressure?

The most probable speed of an oxygen molecule in the gas phase at room temperature is 450 m/s. The root-mean-square speed (urms) is therefore

A sample of ammonia gas at 65.5°C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is -15.8°C and its pressure is 524 torr?

What are the conditions of STP?

A flask containing argon gas is connected to a 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?

According to the kinetic theory of gases, in a collision between two molecules the kinetic energy of one molecule will decrease by the same amount that the kinetic energy of the other one increases.

Nitrogen will behave most like an ideal gas

A 20.0-L container holds 15.3 mol of Cl2 gas at 227°C. a. Calculate the pressure in atmospheres, assuming ideal behavior. b. Calculate the pressure in atmospheres, assuming van der Waals behavior. The van der Waals constants for Cl2 are a = 6.49 atmL2/mol2 and b = 0.0562 L/mol.

If 0.750 L of argon at 1.50 atm and 177°C and 0.235 L of sulfur dioxide at 95.0 kPa and 63.0°C are added to a 1.00-L flask and the flask's temperature is adjusted to 25.0°C, what is the resulting pressure in the flask?

At very high pressures (~ 1000 atm), the measured pressure exerted by real gases is greater than that predicted by the ideal gas equation. This is mainly because

Starting from the Ideal Gas Equation, derive an equation corresponding to Charles's Law, stating all important assumptions or conditions.

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The 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: Bonding, Structure, and Reactivity

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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Aluminum metal shavings (10.0 g) are placed in 100. mL of 6.00 M hydrochloric acid. What is the maximum volume of hydrogen, measured at STP, which can be produced? 2Al(s) + 6HCl(aq)  2AlCl₃(aq) + 3H₂(g)

The most probable speed of an oxygen molecule in the gas phase at room temperature is 450 m/s. The root-mean-square speed (u_rms) is therefore

A 20.0-L container holds 15.3 mol of Cl₂ gas at 227°C. a. Calculate the pressure in atmospheres, assuming ideal behavior. b. Calculate the pressure in atmospheres, assuming van der Waals behavior. The van der Waals constants for Cl₂ are a = 6.49 atmL²/mol² and b = 0.0562 L/mol.