Q: A scuba tank contains 8.00 L of air at 200 atm. If the air is released at 1.00 atm and temperature remains constant, what volume will the air occupy?

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{200 \times 8.00}{1.00} = 1600\ \text{L}$$

Q: A sample of gas occupies 5.0 L at 2.0 atm. What will its volume be at 1.0 atm (constant T)?

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{2.0 \times 5.0}{1.0} = 10.0\ \text{L}$$

Q: A 2.0 mol sample of gas at 300 K exerts a pressure of 4.82 atm. What is its volume? ($$R = 0.0821)$$

$$V = \frac{nRT}{P} = \frac{2.0 \times 0.0821 \times 300}{4.82} = 10.2\ \text{L}$$

Q: Standard Temperature and Pressure (STP) correspond to:

$$0^\circ \text{C}$$ \text{and}~1~\text{atm}$

Q: A compressed gas cylinder contains 5.0 L of gas at 400 K. What will the volume be at 200 K if pressure and moles remain constant?

$$V_2$$ = $$V_1$$ \frac{$$T_2$$}{$$T_1$$} = 5.0 \times \frac{200}{400} = 2.5\ \text{L}$$

Q: In a mixture with gases at 200, 400, and 600 kPa, total pressure is:

$$200 + 400 + 600 = 1200\ \text{kPa}$$

Q: If 5.0 L of gas at 1.0 atm expands to 15.0 L, the new pressure is:

$$P_2$$ = \frac{$$P_1$$ $$V_1$$}{$$V_2$$} = \frac{1.0 \times 5.0}{15.0} = 0.33\ \text{atm}$$

Question 1

A medical oxygen tank contains 15.0 L of O$$_2$$ gas at 1.20 atm and 298 K. If the gas is released into a room at 1.00 atm and 310 K, what will be the final volume of the oxygen? (Assume ideal gas behavior.)

Accepted Answer

$$V_2$$ = \frac{$$P_1$$ $$V_1$$ $$T_2$$}{$$P_2$$ $$T_1$$} = \frac{1.20 	imes 15.0 	imes 310}{1.00 	imes 298} = 18.7\ 	ext{L}$$

Question 2

Which statement best explains why a balloon expands when heated?

Accepted Answer

The kinetic energy of gas particles increases, causing them to collide with the walls more forcefully.

Question 3

A scuba tank contains 8.00 L of air at 200 atm. If the air is released at 1.00 atm and temperature remains constant, what volume will the air occupy?

Accepted Answer

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{200 	imes 8.00}{1.00} = 1600\ 	ext{L}$$

Question 4

Which law states that pressure and volume are inversely related at constant temperature?

Accepted Answer

Boyle's Law

Question 5

A sample of gas occupies 5.0 L at 2.0 atm. What will its volume be at 1.0 atm (constant T)?

Accepted Answer

$$V_2$$ = \frac{$$P_1$$ $$V_1$$}{$$P_2$$} = \frac{2.0 	imes 5.0}{1.0} = 10.0\ 	ext{L}$$

Question 6

Which equation expresses the Ideal Gas Law?

Accepted Answer

$$PV = nRT$$

Question 7

At STP, the volume of one mole of gas is roughly:

Accepted Answer

$$22.4\ 	ext{L}$$

Question 8

Which law states that total pressure equals the sum of individual gas pressures?

Accepted Answer

Dalton's Law

Question 9

A 2.0 mol sample of gas at 300 K exerts a pressure of 4.82 atm. What is its volume? ($$R = 0.0821)$$

Accepted Answer

$$V = \frac{nRT}{P} = \frac{2.0 	imes 0.0821 	imes 300}{4.82} = 10.2\ 	ext{L}$$

Question 10

When temperature increases at constant pressure, gas volume:

Accepted Answer

Increases

Question 11

Standard Temperature and Pressure (STP) correspond to:

Accepted Answer

$$0^\circ 	ext{C}$$ 	ext{and}~1~	ext{atm}$

Question 12

According to Avogadro's Law, equal volumes of gases at the same temperature and pressure contain:

Accepted Answer

Equal numbers of molecules

Question 13

A compressed gas cylinder contains 5.0 L of gas at 400 K. What will the volume be at 200 K if pressure and moles remain constant?

Accepted Answer

$$V_2$$ = $$V_1$$ \frac{$$T_2$$}{$$T_1$$} = 5.0 	imes \frac{200}{400} = 2.5\ 	ext{L}$$

Question 14

In the equation $$PV = nRT$$, the variable $$n$$ represents:

Accepted Answer

Moles

Question 15

A key postulate of the Kinetic Molecular Theory is that gas particles:

Accepted Answer

Have negligible volume and elastic collisions

Question 16

If temperature ($$T) $$doubles at constant pressure, volume will:

Accepted Answer

Double

Question 17

In a mixture with gases at 200, 400, and 600 kPa, total pressure is:

Accepted Answer

$$200 + 400 + 600 = 1200\ 	ext{kPa}$$

Question 18

Which variable must be constant for Boyle's Law to apply?

Accepted Answer

Temperature

Question 19

If 5.0 L of gas at 1.0 atm expands to 15.0 L, the new pressure is:

Accepted Answer

$$P_2$$ = \frac{$$P_1$$ $$V_1$$}{$$V_2$$} = \frac{1.0 	imes 5.0}{15.0} = 0.33\ 	ext{atm}$$

Gas Laws and Stoichiometry: Study Notes for General Chemistry

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