Question 1

For which of the following changes is it not clear whether the volume of a particular sample of an ideal gas will increase or decrease?

Accepted Answer

The volume change is uncertain in A because both increasing temperature and increasing pressure have opposite effects on volume according to the ideal gas law (PV=nRT), making the net effect unclear without specific values.

Question 2

Charles's Law states that the volume of a gas held at constant pressure is directly proportional to the absolute temperature.Which of the following is a consequence of Charles's Law?

Accepted Answer

Charles's Law states that the volume of a gas is directly proportional to its absolute temperature at constant pressure. Therefore, if the air inside a sealed balloon is heated, the volume of the air will increase, causing the balloon to expand and rise.

Question 3

Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 3.50 L sample were cooled from 90.0^oC to 30.0^oC.

Accepted Answer

According to Charles's Law, at constant pressure, the volume of a gas is directly proportional to its absolute temperature. Therefore, V1/T1 = V2/T2, where V1 is the initial volume, T1 is the initial temperature, V2 is the final volume (what we want to find), and T2 is the final temperature. We can rearrange this equation to solve for V2: V2 = V1(T2/T1). Plugging in the values, we get V2 = 3.50 L * (303 K/363 K) = 2.92 L. Therefore, the answer is D.

Question 4

A sample of gas initially occupies 3.35 L at a pressure of 0.950 atm at 13.0^oC.What will the volume be if the temperature is changed to 22.5^oC, and the pressure is changed to 1.05 atm?

Accepted Answer

The answer of A sample of gas initially occupies 3.35...

Question 5

If the initial pressure of a 3.00 L gas sample is 2.50 atm, what will the pressure be if the volume is changed to 4.00 L at constant temperature?

Accepted Answer

According to Boyle's Law, at constant temperature, the pressure and volume of a gas are inversely proportional. That means P1V1 = P2V2. Plugging in the given values, we get:

P1V1 = P2V2
(2.50 atm)(3.00 L) = P2(4.00 L)
P2 = (2.50 atm)(3.00 L)/(4.00 L) = 1.88 atm

Therefore, the pressure will be 1.88 atm when the volume is changed to 4.00 L. Choice D is the correct answer.

Question 6

A sample of gas initially occupies 5.50 L at a pressure of 0.750 atm at 13.0^oC.What will the pressure be if the temperature is changed to 22.5^oC, and the volume is changed to 1.50 L?

Accepted Answer

We can use the combined gas law to solve for the final pressure:

(P1 x V1)/T1 = (P2 x V2)/T2

Where:
P1 = 0.750 atm (initial pressure)
V1 = 5.50 L (initial volume)
T1 = 13.0°C + 273 = 286 K (initial temperature converted to Kelvin)
P2 = ? (final pressure, what we're solving for)
V2 = 1.50 L (final volume)
T2 = 22.5°C + 273 = 296 K (final temperature converted to Kelvin)

Plugging in the values:

(0.750 atm x 5.50 L)/286 K = (P2 x 1.50 L)/296 K

Solving for P2:

P2 = (0.750 atm x 5.50 L x 296 K)/(286 K x 1.50 L)
P2 = 2.84 atm

Therefore, the answer is D) 2.84 atm.

Question 7

Given a fixed amount of gas in a rigid container (no change in volume), what temperature will the gas have to be changed to if the pressure is initially 1.50 atm at 42.0^oC, and the desired final pressure is 3.00 atm?

Accepted Answer

The answer of Given a fixed amount of gas in...

Question 8

Given a fixed amount of gas in a rigid container (no change in volume), what pressure will the gas exert if the pressure is initially 2.50 atm at 22.0^oC, and the temperature is changed to 66.0^oC?

Accepted Answer

Using the ideal gas law, pressure is directly proportional to temperature when volume is constant. Convert temperatures to Kelvin (22°C = 295K, 66°C = 339K) and use P1/T1 = P2/T2 to find the new pressure: (2.50 atm / 295K) = (P2 / 339K), solving gives P2 = 2.87 atm.

Question 9

Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 2.00 L sample were cooled from 60.0^oC to 30.0^oC.

Accepted Answer

The answer of Given a fixed amount of gas held...

Question 10

Given a fixed amount of gas in a rigid container (no change in volume), what temperature will the gas have to be changed to if the pressure is initially 3.50 atm at 22.0^oC, and the desired final pressure is 1.75 atm?

Accepted Answer

According to Gay-Lussac's law, the pressure of a gas is directly proportional to its temperature, assuming the volume remains constant. Therefore, to decrease the pressure from 3.50 atm to 1.75 atm, the temperature must be decreased. The correct answer is A, -126°C.

Question 11

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 1.75 L sample at 23.0^oC were to have a final volume of 3.50 L.

Accepted Answer

The answer of Given a fixed amount of gas held...

Question 12

Given a fixed amount of gas in a rigid container (no change in volume), what pressure will the gas exert if the pressure is initially 1.50 atm at 22.0^oC, and the temperature is changed to 11.0^oC?

Accepted Answer

According to the Ideal Gas Law, PV=nRT, the pressure (P) and temperature (T) are directly proportional when the volume (V) and amount of gas (n) are constant. Therefore, we can use the following equation to solve for the final pressure (P2):
P1/T1 = P2/T2
where P1 and T1 are the initial pressure and temperature, and T2 is the final temperature. 
Plugging in the values: 
(1.50 atm)/(295 K) = P2/(284 K)
Solving for P2: 
P2 = (1.50 atm)(284 K)/(295 K) = 1.44 atm
Therefore, the answer is D) 1.44 atm.

Question 13

If the volume of a sample of gas is held constant, while the temperature is decreased, the pressure will

Accepted Answer

The answer of If the volume of a sample of...

Question 14

If the temperature of a gas at a constant pressure is increased, the volume will

Accepted Answer

According to Charles's Law, at a constant pressure, the volume of a gas is directly proportional to its absolute temperature. This means that as the temperature increases, the volume will also increase because the gas molecules will collide more frequently with the sides of the container, exerting more pressure and causing the gas to expand to fill the available space. Therefore, choice D is the correct answer.

Question 15

The pressure-volume relationship expressed by Boyle's law can be explained by the kinetic molecular theory as follows:

Accepted Answer

The answer of The pressure-volume relationship expressed by Boyle's law...

Question 16

Which of the following statements is incorrect? (Assume that pressure and amount of gas are constant.)

Accepted Answer

Charles's law states that the volume of a gas is directly proportional to its temperature in kelvins, assuming pressure and amount of gas are constant. This means if the temperature doubles, the volume doubles (B is correct), and if the volume is halved, the temperature in kelvins is halved (C is correct, assuming the temperature is measured in kelvins). Statement A correctly summarizes Charles's law. Statement E is a general principle of gas behavior when cooled. Statement D is incorrect because it confuses Charles's law (which relates volume and temperature) with the effect on pressure, and it does not apply under the assumption of constant pressure.

Question 17

A given mass of gas in a rigid container is heated from 100^oC to 500^oC.Which of the following best describes what will happen to the pressure of the gas?

Accepted Answer

According to Gay-Lussac's Law, for a given mass of gas at constant volume, the pressure is directly proportional to its absolute temperature (in Kelvin). The temperature increases from 373K to 773K, which is not a factor of five, so the pressure increases by a factor less than five.

Question 18

A gas in a closed container with constant volume is heated from room temperature to 100 $\degree$C.According to the kinetic molecular theory, the

Accepted Answer

According to the kinetic molecular theory, as the temperature of a gas increases, the average velocity of the molecules also increases. However, the other answer choices are not supported by the theory.

Question 19

A sample of gas initially occupies 4.25 L at a pressure of 0.850 atm at 23.0^oC.What will the volume be if the temperature is changed to 11.5^oC, and the pressure is changed to 1.50 atm?

Accepted Answer

Using the combined gas law, (P1 * V1) / T1 = (P2 * V2) / T2, where temperatures are in Kelvin, the final volume V2 can be calculated. Converting temperatures to Kelvin: T1 = 296.15 K and T2 = 284.65 K. Solving for V2 gives approximately 2.31 L.

Question 20

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 3.50 L sample at 23.0^oC were to have a final volume of 1.50 L.

Accepted Answer

The correct answer is C.The ideal gas law states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature. If the pressure and number of moles of gas are held constant, then the volume of the gas is inversely proportional to the temperature. Therefore, if the volume of the gas is decreased by a factor of 2, then the temperature must be increased by a factor of 2. This means that the temperature must be increased from 23.0^oC to 46.0^oC. However, the question asks for the temperature to which the gas would have to be changed, which means that the temperature must be decreased by 46.0^oC. Therefore, the correct answer is (-146^o)C.

Quiz 9: The Gaseous State

For which of the following changes is it not clear whether the volume of a particular sample of an ideal gas will increase or decrease?

Charles's Law states that the volume of a gas held at constant pressure is directly proportional to the absolute temperature.Which of the following is a consequence of Charles's Law?

Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 3.50 L sample were cooled from 90.0^oC to 30.0^oC.

A sample of gas initially occupies 3.35 L at a pressure of 0.950 atm at 13.0^oC.What will the volume be if the temperature is changed to 22.5^oC, and the pressure is changed to 1.05 atm?

If the initial pressure of a 3.00 L gas sample is 2.50 atm, what will the pressure be if the volume is changed to 4.00 L at constant temperature?

A sample of gas initially occupies 5.50 L at a pressure of 0.750 atm at 13.0^oC.What will the pressure be if the temperature is changed to 22.5^oC, and the volume is changed to 1.50 L?

Given a fixed amount of gas in a rigid container (no change in volume) , what temperature will the gas have to be changed to if the pressure is initially 1.50 atm at 42.0^oC, and the desired final pressure is 3.00 atm?

Given a fixed amount of gas in a rigid container (no change in volume) , what pressure will the gas exert if the pressure is initially 2.50 atm at 22.0^oC, and the temperature is changed to 66.0^oC?

Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 2.00 L sample were cooled from 60.0^oC to 30.0^oC.

Given a fixed amount of gas in a rigid container (no change in volume) , what temperature will the gas have to be changed to if the pressure is initially 3.50 atm at 22.0^oC, and the desired final pressure is 1.75 atm?

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 1.75 L sample at 23.0^oC were to have a final volume of 3.50 L.

Given a fixed amount of gas in a rigid container (no change in volume) , what pressure will the gas exert if the pressure is initially 1.50 atm at 22.0^oC, and the temperature is changed to 11.0^oC?

If the volume of a sample of gas is held constant, while the temperature is decreased, the pressure will

If the temperature of a gas at a constant pressure is increased, the volume will

The pressure-volume relationship expressed by Boyle's law can be explained by the kinetic molecular theory as follows:

Which of the following statements is incorrect? (Assume that pressure and amount of gas are constant.)

A given mass of gas in a rigid container is heated from 100^oC to 500^oC.Which of the following best describes what will happen to the pressure of the gas?

A gas in a closed container with constant volume is heated from room temperature to 100 $\degree$ C.According to the kinetic molecular theory, the

A sample of gas initially occupies 4.25 L at a pressure of 0.850 atm at 23.0^oC.What will the volume be if the temperature is changed to 11.5^oC, and the pressure is changed to 1.50 atm?

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 3.50 L sample at 23.0^oC were to have a final volume of 1.50 L.

Quiz 9: The Gaseous State

For which of the following changes is it not clear whether the volume of a particular sample of an ideal gas will increase or decrease?

Charles's Law states that the volume of a gas held at constant pressure is directly proportional to the absolute temperature.Which of the following is a consequence of Charles's Law?

Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 3.50 L sample were cooled from 90.0oC to 30.0oC.

A sample of gas initially occupies 3.35 L at a pressure of 0.950 atm at 13.0oC.What will the volume be if the temperature is changed to 22.5oC, and the pressure is changed to 1.05 atm?

If the initial pressure of a 3.00 L gas sample is 2.50 atm, what will the pressure be if the volume is changed to 4.00 L at constant temperature?

A sample of gas initially occupies 5.50 L at a pressure of 0.750 atm at 13.0oC.What will the pressure be if the temperature is changed to 22.5oC, and the volume is changed to 1.50 L?

Given a fixed amount of gas in a rigid container (no change in volume) , what temperature will the gas have to be changed to if the pressure is initially 1.50 atm at 42.0oC, and the desired final pressure is 3.00 atm?

Given a fixed amount of gas in a rigid container (no change in volume) , what pressure will the gas exert if the pressure is initially 2.50 atm at 22.0oC, and the temperature is changed to 66.0oC?

Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 2.00 L sample were cooled from 60.0oC to 30.0oC.

Given a fixed amount of gas in a rigid container (no change in volume) , what temperature will the gas have to be changed to if the pressure is initially 3.50 atm at 22.0oC, and the desired final pressure is 1.75 atm?

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 1.75 L sample at 23.0oC were to have a final volume of 3.50 L.

Given a fixed amount of gas in a rigid container (no change in volume) , what pressure will the gas exert if the pressure is initially 1.50 atm at 22.0oC, and the temperature is changed to 11.0oC?

If the volume of a sample of gas is held constant, while the temperature is decreased, the pressure will

If the temperature of a gas at a constant pressure is increased, the volume will

The pressure-volume relationship expressed by Boyle's law can be explained by the kinetic molecular theory as follows:

Which of the following statements is incorrect? (Assume that pressure and amount of gas are constant.)

A given mass of gas in a rigid container is heated from 100oC to 500oC.Which of the following best describes what will happen to the pressure of the gas?

A gas in a closed container with constant volume is heated from room temperature to 100 °\degree° C.According to the kinetic molecular theory, the

A sample of gas initially occupies 4.25 L at a pressure of 0.850 atm at 23.0oC.What will the volume be if the temperature is changed to 11.5oC, and the pressure is changed to 1.50 atm?

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 3.50 L sample at 23.0oC were to have a final volume of 1.50 L.

Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 3.50 L sample were cooled from 90.0^oC to 30.0^oC.

A sample of gas initially occupies 3.35 L at a pressure of 0.950 atm at 13.0^oC.What will the volume be if the temperature is changed to 22.5^oC, and the pressure is changed to 1.05 atm?

A sample of gas initially occupies 5.50 L at a pressure of 0.750 atm at 13.0^oC.What will the pressure be if the temperature is changed to 22.5^oC, and the volume is changed to 1.50 L?

Given a fixed amount of gas in a rigid container (no change in volume) , what temperature will the gas have to be changed to if the pressure is initially 1.50 atm at 42.0^oC, and the desired final pressure is 3.00 atm?

Given a fixed amount of gas in a rigid container (no change in volume) , what pressure will the gas exert if the pressure is initially 2.50 atm at 22.0^oC, and the temperature is changed to 66.0^oC?

Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 2.00 L sample were cooled from 60.0^oC to 30.0^oC.

Given a fixed amount of gas in a rigid container (no change in volume) , what temperature will the gas have to be changed to if the pressure is initially 3.50 atm at 22.0^oC, and the desired final pressure is 1.75 atm?

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 1.75 L sample at 23.0^oC were to have a final volume of 3.50 L.

Given a fixed amount of gas in a rigid container (no change in volume) , what pressure will the gas exert if the pressure is initially 1.50 atm at 22.0^oC, and the temperature is changed to 11.0^oC?

A given mass of gas in a rigid container is heated from 100^oC to 500^oC.Which of the following best describes what will happen to the pressure of the gas?

A gas in a closed container with constant volume is heated from room temperature to 100 $\degree$ C.According to the kinetic molecular theory, the

A sample of gas initially occupies 4.25 L at a pressure of 0.850 atm at 23.0^oC.What will the volume be if the temperature is changed to 11.5^oC, and the pressure is changed to 1.50 atm?

Given a fixed amount of gas held at constant pressure, calculate the temperature to which the gas would have to be changed if a 3.50 L sample at 23.0^oC were to have a final volume of 1.50 L.