Question 1

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.

Accepted Answer

A)   0.252 atm
B)   0.592 atm
C)   1.69 atm
D)   3.96 atm
E)   4.80 atmF) A) and D)
G) A) and E)

Question 2

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) F1F1F1S1F1F1F10 2AlCl3(aq) + 3H2(g)

Accepted Answer

Question 3

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

Accepted Answer

A) True 
 B)False

Question 4

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

Accepted Answer

Ideal Gas Equation is PV = nRT. Charles'...

Question 5

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?

Accepted Answer

A)   212 torr
B)   289 torr
C)   356 torr
D)   441 torr
E)   359 torrF) A) and B)
G) A) and C)

Question 6

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?

Accepted Answer

A)   increased by 44.3 L
B)   increased by 9.3 L
C)   increased by 7.4 L
D)   decreased by 27.6 L
E)   decreased by 7.4 LF) B) and D)
G) D) and E)

Question 7

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?

Accepted Answer

A)   -50. torr
B)   50. torr
C)   695 torr
D)   795 torr
E)   none of the aboveF) C) and E)
G) All of the above

Question 8

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?

Accepted Answer

A)   0.0851 atm
B)   0.244 atm
C)   0.946 atm
D)   1.74 atm
E)   1.86 atmF) A) and B)
G) B) and E)

Question 9

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

Accepted Answer

A)   200 torr
B)   400 torr
C)   800 torr
D)   2400 torr
E)   3200 torrF) B) and C)
G) B) and E)

Question 10

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 atmF1F1F1S1F1F1F10L2/mol2 and b = 0.0562 L/mol.

Accepted Answer

a. 31.4 at...

Question 11

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

Accepted Answer

A)   such high pressures cannot be accurately measured.
B)   real gases will condense to form liquids at 1000 atm pressure.
C)   gas phase collisions prevent molecules from colliding with the walls of the container.
D)   of attractive intermolecular forces between gas molecules.
E)   the volume occupied by the gas molecules themselves becomes significant.F) All of the above
G) A) and B)

Question 12

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?

Accepted Answer

A)   10 torr
B)   50 torr
C)   100 torr
D)   200 torr
E)   1000 torrF) D) and E)
G) A) and E)

Question 13

What are the conditions of STP?

Accepted Answer

A)   0 K and l atm
B)   273.15 K and 760 torr
C)   0°C and 760 atm
D)   273.15°C and 760 torr
E)   none of the aboveF) B) and C)
G) A) and E)

Question 14

State Avogadro's Law.

Accepted Answer

Equal volumes of gas...

Question 15

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.

Accepted Answer

A) True 
 B)False

Question 16

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?

Accepted Answer

A)   -230.
B)   230.
C)   530.
D)   790.
E)   none of the aboveF) B) and D)
G) D) and E)

Question 17

Nitrogen will behave most like an ideal gas

Accepted Answer

A)   at high temperature and high pressure.
B)   at high temperature and low pressure.
C)   at low temperature and high pressure.
D)   at low temperature and low pressure.
E)   at intermediate (moderate)  temperature and pressure.F) A) and B)
G) A) and E)

Question 18

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?

Accepted Answer

The answer of Which of the lines on the figure...

Question 19

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?

Accepted Answer

A)   3.69 L
B)   11.6 L
C)   20.2 L
D)   63.5 L
E)   not possible, since the volume would have to be negativeF) None of the above
G) B) and E)

Question 20

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

Accepted Answer

A)   equal to 450 m/s.
B)   slightly less than 450 m/s.
C)   much less than 450 m/s.
D)   slightly greater than 450 m/s.
E)   much greater than 450 m/s.F) A) and B)
G) A) and C)

Exam 5: Gases and the Kinetic-Molecular Theory

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.

Correct AnswerverifiedShow Answer

What are the conditions of STP?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Nitrogen will behave most like an ideal gas

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedIdeal Gas Equation is PV = nRT. Charles'...View AnswerShow Answer

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.

Correct Answerverifieda. 31.4 at...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

State Avogadro's Law.

Correct AnswerverifiedEqual volumes of gas...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

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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)

Correct Answer
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Ideal Gas Equation is PV = nRT. Charles'...
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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.

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a. 31.4 at...
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Equal volumes of gas...
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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

Correct Answer
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