Q: A patient with COPD is given oxygen from a tank at 3800 mmHg in a 12 L container. If the oxygen is released until the pressure drops to 570 mmHg (with temperature and amount of gas constant), what is the final volume of the oxygen gas? Use Boyle’s law.

$$V_2 = 12$$\ \mathrm{L} \times \frac{3800\ \mathrm{mmHg}}{570\ \mathrm{mmHg}} = 80\ \mathrm{L}$$

Q: A tank of nitrous oxide (N$$_2O) $$has a pressure of 48 psi. What is this pressure in atmospheres? (1 atm = 14.7 psi)

$$48\ \mathrm{psi} \times \frac{1\ \mathrm{atm}}{14.7\ \mathrm{psi}} = 3.3\ \mathrm{atm}$$

Q: A weather balloon is filled with 15.0 L of helium at 25°C and 685 mmHg. What is the pressure in mmHg when the balloon rises to where the temperature is -35°C and the volume is 34.0 L? (Assume the amount of gas does not change.)

$$P_2 = 685$$\ \mathrm{mmHg} \times \frac{15.0\ \mathrm{L}}{34.0\ \mathrm{L}} \times \frac{238\ \mathrm{K}}{298\ \mathrm{K}} = 241\ \mathrm{mmHg}$$

Q: A sample of helium gas has a volume of 5.40 L at 15°C. What is the final volume at 42°C, if pressure and amount of gas do not change? (Use Charles’s law.)

$$V_2 = 5.40$$\ \mathrm{L} \times \frac{315\ \mathrm{K}}{288\ \mathrm{K}} = 5.91\ \mathrm{L}$$

Q: A hospital oxygen tank has a pressure of 120 atm at 25°C. If a fire raises the temperature to 402°C, what is the new pressure? Will the tank rupture if its limit is 180 atm? (Use Gay-Lussac’s law.)

$$P_2 = 120$$\ \mathrm{atm} \times \frac{675\ \mathrm{K}}{298\ \mathrm{K}} = 270\ \mathrm{atm}$$; Yes, it will rupture.

Q: A 25.0-mL bubble is released from a diver’s tank at 4.00 atm and 11°C. What is the volume of the bubble at the surface (1.00 atm, 18°C)? (Use the combined gas law.)

$$V_2 = 25.0$$\ \mathrm{mL} \times \frac{4.00\ \mathrm{atm}}{1.00\ \mathrm{atm}} \times \frac{291\ \mathrm{K}}{284\ \mathrm{K}} = 102\ \mathrm{mL}$$

Q: A weather balloon with a volume of 44 L contains 2.0 moles of helium. If 3.0 moles are added (total 5.0 moles), what is the final volume? (Pressure and temperature constant.)

$$V_2 = 44$$\ \mathrm{L} \times \frac{5.0}{2.0} = 110\ \mathrm{L}$$

Q: What is the volume, in liters, of 64.0 g of O$$_2$$ gas at STP?

$$64.0\ \mathrm{g}\ O_2$ \times \frac{1\ \mathrm{mol}}{32.00\ \mathrm{g}} \times \frac{22.4\ \mathrm{L}}{1\ \mathrm{mol}} = 44.8\ \mathrm{L}$$

Q: A mountain climber inhales air at −8°C. If the final volume in the lungs is 569 mL at 37°C, what was the initial volume inhaled? (Pressure and amount of gas constant.)

$$V_1 = 569$$\ \mathrm{mL} \times \frac{265\ \mathrm{K}}{310\ \mathrm{K}} = 486\ \mathrm{mL}$$

Question 1

A patient with COPD is given oxygen from a tank at 3800 mmHg in a 12 L container. If the oxygen is released until the pressure drops to 570 mmHg (with temperature and amount of gas constant), what is the final volume of the oxygen gas? Use Boyle’s law.

Accepted Answer

$$V_2 = 12$$\ \mathrm{L} 	imes \frac{3800\ \mathrm{mmHg}}{570\ \mathrm{mmHg}} = 80\ \mathrm{L}$$

Question 2

Which property of a gas is directly related to the kinetic energy of its particles?

Accepted Answer

Temperature

Question 3

A tank of nitrous oxide (N$$_2O) $$has a pressure of 48 psi. What is this pressure in atmospheres? (1 atm = 14.7 psi)

Accepted Answer

$$48\ \mathrm{psi} 	imes \frac{1\ \mathrm{atm}}{14.7\ \mathrm{psi}} = 3.3\ \mathrm{atm}$$

Question 4

A weather balloon is filled with 15.0 L of helium at 25°C and 685 mmHg. What is the pressure in mmHg when the balloon rises to where the temperature is -35°C and the volume is 34.0 L? (Assume the amount of gas does not change.)

Accepted Answer

$$P_2 = 685$$\ \mathrm{mmHg} 	imes \frac{15.0\ \mathrm{L}}{34.0\ \mathrm{L}} 	imes \frac{238\ \mathrm{K}}{298\ \mathrm{K}} = 241\ \mathrm{mmHg}$$

Question 5

A sample of helium gas has a volume of 5.40 L at 15°C. What is the final volume at 42°C, if pressure and amount of gas do not change? (Use Charles’s law.)

Accepted Answer

$$V_2 = 5.40$$\ \mathrm{L} 	imes \frac{315\ \mathrm{K}}{288\ \mathrm{K}} = 5.91\ \mathrm{L}$$

Question 6

A hospital oxygen tank has a pressure of 120 atm at 25°C. If a fire raises the temperature to 402°C, what is the new pressure? Will the tank rupture if its limit is 180 atm? (Use Gay-Lussac’s law.)

Accepted Answer

$$P_2 = 120$$\ \mathrm{atm} 	imes \frac{675\ \mathrm{K}}{298\ \mathrm{K}} = 270\ \mathrm{atm}$$; Yes, it will rupture.

Question 7

A 25.0-mL bubble is released from a diver’s tank at 4.00 atm and 11°C. What is the volume of the bubble at the surface (1.00 atm, 18°C)? (Use the combined gas law.)

Accepted Answer

$$V_2 = 25.0$$\ \mathrm{mL} 	imes \frac{4.00\ \mathrm{atm}}{1.00\ \mathrm{atm}} 	imes \frac{291\ \mathrm{K}}{284\ \mathrm{K}} = 102\ \mathrm{mL}$$

Question 8

A weather balloon with a volume of 44 L contains 2.0 moles of helium. If 3.0 moles are added (total 5.0 moles), what is the final volume? (Pressure and temperature constant.)

Accepted Answer

$$V_2 = 44$$\ \mathrm{L} 	imes \frac{5.0}{2.0} = 110\ \mathrm{L}$$

Question 9

What is the volume, in liters, of 64.0 g of O$$_2$$ gas at STP?

Accepted Answer

$$64.0\ \mathrm{g}\ O_2$ 	imes \frac{1\ \mathrm{mol}}{32.00\ \mathrm{g}} 	imes \frac{22.4\ \mathrm{L}}{1\ \mathrm{mol}} = 44.8\ \mathrm{L}$$

Question 10

A heliox mixture for a COPD patient has a total pressure of 7.00 atm. If the partial pressure of O$$_2 is 1140 $$mmHg, what is the partial pressure of He in atm?

Accepted Answer

$$P_{He} = 7.00\ \mathrm{atm} - 1.50\ \mathrm{atm} = 5.50\ \mathrm{atm}$$

Question 11

Which law explains why the volume of a gas increases when the number of moles increases, if pressure and temperature are constant?

Accepted Answer

Avogadro’s law

Question 12

A mountain climber inhales air at −8°C. If the final volume in the lungs is 569 mL at 37°C, what was the initial volume inhaled? (Pressure and amount of gas constant.)

Accepted Answer

$$V_1 = 569$$\ \mathrm{mL} 	imes \frac{265\ \mathrm{K}}{310\ \mathrm{K}} = 486\ \mathrm{mL}$$

Question 13

Which of the following best describes the force of gas particles hitting the walls of a container?

Accepted Answer

Pressure

Question 14

A sample contains 8.00 g of O$$_2$$ gas in a 5.00 L balloon. If 4.00 g more O$$_2 is $$added (at constant T and P), what is the new volume?

Accepted Answer

$$V_2 = 5.00$$\ \mathrm{L} 	imes \frac{12.00\ \mathrm{g}}{8.00\ \mathrm{g}} = 7.50\ \mathrm{L}$$

Question 15

Which of the following is NOT a factor that affects the volume of a gas, assuming the amount of gas is constant?

Accepted Answer

Color of the gas

Properties and Laws of Gases: GOB Chemistry Study Notes

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