1. A scuba diver 40 ft below the ocean surface inhales 80.0 mL of compressed air
ID: 549787 • Letter: 1
Question
1. A scuba diver 40 ft below the ocean surface inhales 80.0 mL of compressed air from a scuba tank at a pressure of 2.50 atm and a temperature of 7 C.
What is the pressure of the air, in atm, in the lungs when the gas expands to 180.0 mL at a body temperature of 37 C, and the amount of gas remains constant?
Express the pressure in atmospheres to three significant figures.
2. In 1783, Jacques Charles launched his first balloon filled with hydrogen gas, which he chose because it was lighter than air. The balloon, which had a volume of 31 000 L at STP, reached an altitude of 1000 m, where the pressure was 640 mmHgand the temperature was -5 C.
What was the volume, in liters, of the balloon at these conditions?
Express your answer using two significant figures.
3.In a gas mixture, the partial pressures are nitrogen 450 torr , oxygen 120 torr , and helium 240 torr
What is the total pressure (torr) exerted by the gas mixture?
4.In a gas mixture, the partial pressures are argon 445 mmHg , neon 55 mmHg , and nitrogen 125 mmHg . What is the total pressure (atm) exerted by the gas mixture?
Explanation / Answer
Q1
V1 = 80 mL
P1 = 2.5 atm
T1 = 7°C = 7+273 = 280 K
P2 =
V2 = 180
T2 = 37 °C = 37+273 = 310
Apply ideal gas law ratios
P1V1/T1 = P2V2/T2
2.5*80/280 = P2*180/310
P2 = 2.5*80/280 /(180/310) = 1.230 atm
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