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 908 \text{ mL}}{1.07 \text{ atm}} = 801 \text{ mL}$$

Q: A sample of gas occupies 3.50 L at a pressure of 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: A 0.684 L sample of helium gas is heated at constant pressure from 0°C to a final volume of 0.986 L. What is the final temperature in Kelvin?

$$T_2$$ = \frac{$$V_2$$ $$T_1$$}{$$V_1$$} = \frac{0.986 \text{ L} \times 273 \text{ K}}{0.684 \text{ L}} = 393 \text{ K}$$

Q: A gas sample has a volume of 2.00 L at 273 K. What will its volume be at 546 K, assuming constant pressure?

$$V_2$$ = \frac{$$V_1$$ $$T_2$$}{$$T_1$$} = \frac{2.00 \text{ L} \times 546 \text{ K}}{273 \text{ K}} = 4.00 \text{ L}$$

Q: Which of the following is a correct conversion from torr to atm?

$$1 \text{ atm} = 760 \text{ torr}$$

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 908 	ext{ mL}}{1.07 	ext{ atm}} = 801 	ext{ mL}$$

Question 4

Which of the following statements about Boyle's Law is correct?

Accepted Answer

At constant temperature, the pressure and volume of a gas are inversely proportional: $$P_1$$ $$V_1$$ = $$P_2$$ $$V_2$$

Question 5

A sample of gas occupies 3.50 L at a pressure of 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 NOT an assumption of the kinetic molecular theory of gases?

Accepted Answer

Gas particles have significant attractive or repulsive forces between them.

Question 7

A 0.684 L sample of helium gas is heated at constant pressure from 0°C to a final volume of 0.986 L. What is the final temperature in Kelvin?

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}$$

Question 8

If the pressure of a gas is decreased from 1.00 atm to 0.500 atm at constant temperature, what happens to the volume?

Accepted Answer

The volume doubles.

Question 9

Which equation correctly represents Charles's Law?

Accepted Answer

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

Question 10

A gas sample has a volume of 2.00 L at 273 K. What will its volume be at 546 K, assuming constant pressure?

Accepted Answer

$$V_2$$ = \frac{$$V_1$$ $$T_2$$}{$$T_1$$} = \frac{2.00 	ext{ L} 	imes 546 	ext{ K}}{273 	ext{ K}} = 4.00 	ext{ L}$$

Question 11

Which of the following is a correct conversion from torr to atm?

Accepted Answer

$$1 	ext{ atm} = 760 	ext{ torr}$$

Question 12

A gas sample 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 13

Which of the following is a correct statement about the relationship between pressure and volume for a gas at constant temperature?

Accepted Answer

Pressure and volume are inversely proportional.

Question 14

A sample of gas at 1.00 atm and 273 K occupies 22.4 L. What is the number of moles of gas present?

Accepted Answer

$$n = \frac{PV}{RT} = \frac{1.00 	ext{ atm} 	imes 22.4 	ext{ L}}{0.0821 	ext{ L atm mol}^{-1} 	ext{ K}^{-1} 	imes 273 	ext{ K}} = 1.00 	ext{ mol}$$

Question 15

Which of the following is the correct value for the universal gas constant $$R in $$units of $$	ext{L atm mol}^{-1} 	ext{ K}^{-1}$$?

Accepted Answer

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

Question 16

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

Accepted Answer

At constant pressure, the volume of a gas is directly proportional to its temperature in Kelvin.

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

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