Q: A 2.50 L sample of hydrogen gas has a pressure of 0.750 atm. What will its volume be if the pressure is increased to 1.50 atm at constant temperature?

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{0.750 \text{ atm} \times 2.50 \text{ L}}{1.50 \text{ atm}} = 1.25 \text{ L}$$

Q: A 0.684 L sample of helium gas, initially at 0°C, is heated at constant pressure. If the final volume of the gas is 0.986 L, what is its final temperature in °C?

$$T_2$$ = \frac{$$V_2$$ $$T_1$$}{$$V_1$$} = \frac{0.986 \text{ L} \times 273 \text{ K}}{0.684 \text{ L}} = 393 \text{ K} \rightarrow $$120^{\circ}$$\text{C}$$

Q: Calculate the new volume of a 0.896 mol sample of hydrogen gas that originally occupies 908 mL at 717 torr and 20°C, after its temperature and pressure are changed to 20°C and 1.07 atm, respectively.

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{0.943 \text{ atm} \times 0.908 \text{ L}}{1.07 \text{ atm}} = 0.801 \text{ L}$$

Q: A sample of gas occupies 3.50 L at 0.750 atm. If the pressure is increased to 1.50 atm at constant temperature, what is the final volume?

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{0.750 \text{ atm} \times 3.50 \text{ L}}{1.50 \text{ atm}} = 1.75 \text{ L}$$

Q: If 0.896 mol of hydrogen gas occupies 908 mL at 717 torr and 20°C, what is the pressure in atm?

$$P = \frac{717 \text{ torr}}{760 \text{ torr/atm}} = 0.943 \text{ atm}$$

Q: A sample of gas at 1.00 atm pressure has a volume of 5.00 L. If the pressure is changed to 0.330 atm at constant temperature, what is the new volume?

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{1.00 \text{ atm} \times 5.00 \text{ L}}{0.330 \text{ atm}} = 15.2 \text{ L}$$

Q: Which equation is used to convert pressure from torr to atm?

$$P_{\text{atm}} = \frac{P_{\text{torr}}}{760}$$

Question 1

A 2.50 L sample of hydrogen gas has a pressure of 0.750 atm. What will its volume be if the pressure is increased to 1.50 atm at constant temperature?

Accepted Answer

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{0.750 	ext{ atm} 	imes 2.50 	ext{ L}}{1.50 	ext{ atm}} = 1.25 	ext{ L}$$

Question 2

A 0.684 L sample of helium gas, initially at 0°C, is heated at constant pressure. If the final volume of the gas is 0.986 L, what is its final temperature in °C?

Accepted Answer

$$T_2$$ = \frac{$$V_2$$ $$T_1$$}{$$V_1$$} = \frac{0.986 	ext{ L} 	imes 273 	ext{ K}}{0.684 	ext{ L}} = 393 	ext{ K} ightarrow $$120^{\circ}$$	ext{C}$$

Question 3

Calculate the new volume of a 0.896 mol sample of hydrogen gas that originally occupies 908 mL at 717 torr and 20°C, after its temperature and pressure are changed to 20°C and 1.07 atm, respectively.

Accepted Answer

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{0.943 	ext{ atm} 	imes 0.908 	ext{ L}}{1.07 	ext{ atm}} = 0.801 	ext{ L}$$

Question 4

Which of the following correctly describes Boyle's Law?

Accepted Answer

$$P_1$$ $$V_1$$ = $$P_2$$ $$V_2$$; pressure and volume are inversely proportional at constant temperature.

Question 5

A sample of gas occupies 3.50 L at 0.750 atm. If the pressure is increased to 1.50 atm at constant temperature, what is the final volume?

Accepted Answer

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{0.750 	ext{ atm} 	imes 3.50 	ext{ L}}{1.50 	ext{ atm}} = 1.75 	ext{ L}$$

Question 6

Which of the following is a correct statement of Charles's Law?

Accepted Answer

$$\frac{V_1$}{T_1$} = \frac{V_2$}{T_2$}$$; volume and temperature are directly proportional at constant pressure.

Question 7

If 0.896 mol of hydrogen gas occupies 908 mL at 717 torr and 20°C, what is the pressure in atm?

Accepted Answer

$$P = \frac{717 	ext{ torr}}{760 	ext{ torr/atm}} = 0.943 	ext{ atm}$$

Question 8

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

Accepted Answer

Gas particles have significant volume.

Question 9

A sample of gas at 1.00 atm pressure has a volume of 5.00 L. If the pressure is changed to 0.330 atm at constant temperature, what is the new volume?

Accepted Answer

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{1.00 	ext{ atm} 	imes 5.00 	ext{ L}}{0.330 	ext{ atm}} = 15.2 	ext{ L}$$

Question 10

Which equation is used to convert pressure from torr to atm?

Accepted Answer

$$P_{	ext{atm}} = \frac{P_{	ext{torr}}}{760}$$

Question 11

A gas sample is heated at constant pressure from 273 K to 546 K. If its initial volume is 1.00 L, what is its final volume?

Accepted Answer

$$V_2$$ = \frac{$$V_1$$ $$T_2$$}{$$T_1$$} = \frac{1.00 	ext{ L} 	imes 546 	ext{ K}}{273 	ext{ K}} = 2.00 	ext{ L}$$

Question 12

Which of the following is the correct combined gas law equation?

Accepted Answer

$$\frac{P_1$ V_1$}{T_1$} = \frac{P_2$ V_2$}{T_2$}$$

Question 13

A 1.00 mol sample of an ideal gas at 273 K and 1.00 atm occupies what volume?

Accepted Answer

$$V = \frac{nRT}{P} = \frac{1.00 	ext{ mol} 	imes 0.0821 	ext{ L atm mol}^{-1} 	ext{ K}^{-1} 	imes 273 	ext{ K}}{1.00 	ext{ atm}} = 22.4 	ext{ L}$$

Question 14

Which of the following is a direct consequence of the kinetic molecular theory of gases?

Accepted Answer

Gas pressure results from collisions of particles with the walls of the container.

Question 15

A gas sample at 1.00 atm and 273 K has a volume of 22.4 L. If the temperature is doubled and the pressure is halved, what is the new volume?

Accepted Answer

$$V_2$$ = $$V_1$$ 	imes \frac{$$T_2$$}{$$T_1$$} 	imes \frac{$$P_1$$}{$$P_2$$} = 22.4 	ext{ L} 	imes \frac{546}{273} 	imes \frac{1.00}{0.50} = 89.6 	ext{ L}$$

Question 16

Which of the following is the correct value for the universal gas constant R in units of L atm mol⁻¹ K⁻¹?

Accepted Answer

$$R = 0.0821 	ext{ L atm mol}^{-1} 	ext{ K}^{-1}$$

Gas Laws: Boyle's, Charles', and Combined Gas Law – Study Notes

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