Q: A 2.00 L container holds 0.080 mol of oxygen gas at 300 K. What is the pressure inside the container? (Use $$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

$$P = \dfrac{nRT}{V} = \dfrac{0.080 \times 0.0821 \times 300}{2.00} = 0.984\ \mathrm{atm}$$

Q: A mixture contains 2.0 mol of nitrogen and 3.0 mol of oxygen in a 10.0 L container at 400 K. What is the total pressure of the mixture? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

$$P = \dfrac{nRT}{V} = \dfrac{5.0 \times 0.0821 \times 400}{10.0} = 16.42\ \mathrm{atm}$$

Q: According to Dalton’s Law of Partial Pressures, which equation correctly expresses the total pressure of a gas mixture?

$$P_{\text{total}} = P_1$ + P_2$ + P_3$ + \ldots$$

Q: A sample of helium gas occupies 5.00 L at 1.00 atm and 273 K. How many moles of helium are present? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

$$n = \dfrac{PV}{RT} = \dfrac{1.00 \times 5.00}{0.0821 \times 273} = 0.224\ \mathrm{mol}$$

Q: A scuba tank contains a mixture of gases at a total pressure of 200 atm. If the partial pressure of oxygen is 40 atm and nitrogen is 150 atm, what is the partial pressure of other gases present?

$$P_{\text{other}} = 200 - 40 - 150 = 10\ \mathrm{atm}$$

Q: A weather balloon is filled with 10.0 mol of hydrogen at 1.00 atm and 273 K. What is the volume of the balloon? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

$$V = \dfrac{nRT}{P} = \dfrac{10.0 \times 0.0821 \times 273}{1.00} = 224\ \mathrm{L}$$

Question 1

Which of the following is NOT an assumption of the ideal gas law?

Accepted Answer

Gas particles lose energy during collisions with each other.

Question 2

A 2.00 L container holds 0.080 mol of oxygen gas at 300 K. What is the pressure inside the container? (Use $$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

Accepted Answer

$$P = \dfrac{nRT}{V} = \dfrac{0.080 	imes 0.0821 	imes 300}{2.00} = 0.984\ \mathrm{atm}$$

Question 3

Which of the following best describes absolute zero?

Accepted Answer

The temperature at which all molecular motion ceases.

Question 4

A mixture contains 2.0 mol of nitrogen and 3.0 mol of oxygen in a 10.0 L container at 400 K. What is the total pressure of the mixture? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

Accepted Answer

$$P = \dfrac{nRT}{V} = \dfrac{5.0 	imes 0.0821 	imes 400}{10.0} = 16.42\ \mathrm{atm}$$

Question 5

According to Dalton’s Law of Partial Pressures, which equation correctly expresses the total pressure of a gas mixture?

Accepted Answer

$$P_{	ext{total}} = P_1$ + P_2$ + P_3$ + \ldots$$

Question 6

Which value is closest to the ideal gas constant $$R in $$units of $$\mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$}$$?

Accepted Answer

$$0.0821$$

Question 7

A sample of helium gas occupies 5.00 L at 1.00 atm and 273 K. How many moles of helium are present? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

Accepted Answer

$$n = \dfrac{PV}{RT} = \dfrac{1.00 	imes 5.00}{0.0821 	imes 273} = 0.224\ \mathrm{mol}$$

Question 8

Which scenario would cause a real gas to deviate most from ideal behavior?

Accepted Answer

At high pressure and low temperature.

Question 9

A scuba tank contains a mixture of gases at a total pressure of 200 atm. If the partial pressure of oxygen is 40 atm and nitrogen is 150 atm, what is the partial pressure of other gases present?

Accepted Answer

$$P_{	ext{other}} = 200 - 40 - 150 = 10\ \mathrm{atm}$$

Question 10

If the temperature of a fixed amount of gas in a rigid container is doubled (in Kelvin), what happens to the pressure?

Accepted Answer

The pressure doubles.

Question 11

A weather balloon is filled with 10.0 mol of hydrogen at 1.00 atm and 273 K. What is the volume of the balloon? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$})$$

Accepted Answer

$$V = \dfrac{nRT}{P} = \dfrac{10.0 	imes 0.0821 	imes 273}{1.00} = 224\ \mathrm{L}$$

Question 12

Which of the following best explains why the ideal gas law does not accurately predict the behavior of real gases at very high pressures?

Accepted Answer

The volume of gas particles is no longer negligible compared to the container.

Question 13

A 3.00 L flask contains a mixture of argon and neon at 2.00 atm and 350 K. If the partial pressure of argon is 1.20 atm, what is the partial pressure of neon?

Accepted Answer

$$P_{	ext{Ne}} = 2.00 - 1.20 = 0.80\ \mathrm{atm}$$

Question 14

Which of the following is a correct rearrangement of the ideal gas law to solve for temperature?

Accepted Answer

$$T = \dfrac{PV}{nR}$$

Question 15

A gas sample at 1.00 atm and 273 K occupies 22.4 L. If the pressure is increased to 2.00 atm at constant temperature, what is the new volume?

Accepted Answer

$$V_2$$ = \dfrac{$$P_1$$ $$V_1$$}{$$P_2$$} = \dfrac{1.00 	imes 22.4}{2.00} = 11.2\ \mathrm{L}$$

Question 16

Which of the following statements about absolute zero is correct?

Accepted Answer

It is the lowest possible temperature, $$0\ \mathrm{K}$$, where the kinetic energy of particles is minimal.

Question 17

A hospital stores oxygen gas in a 50.0 L tank at 25.0°C and 150 atm. How many moles of oxygen are present? ($$R = 0.0821\ \mathrm{L\cdot atm\cdot $$mol^{-1}$$\cdot K$$^{-1}$$}$$; $$T = 25.0^\circ\mathrm{C} = 298\ \mathrm{K})$$

Accepted Answer

$$n = \dfrac{PV}{RT} = \dfrac{150 	imes 50.0}{0.0821 	imes 298} = 307\ \mathrm{mol}$$

Ideal Gas Law, Dalton’s Law of Partial Pressures, and Absolute Zero

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