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Unformatted text preview: compressed air in a scuba tank at a pressure of 3.00 atm and a temperature of 8 o C. What is the pressure of air in the lungs if the gas expands to 200.0 ml at a body temperature of 37 o C? P 1 = 3.00 atm P 2 = ? V1 = 50.0 ml V 2 = 200.0 ml T 1 = 8 C + 273 = 281 K T 2 = 37 C +273 =310 K P 1 V 1 = P 2 V 2 T 1 T 2 P 1 V 1 x T 2 = P 2 T 1 V 2 (3.00 atm x 50.0 ml) x 310 K = 0.827 atm 281 K 200.0 ml 2pts 5. A gas mixture containing oxygen, nitrogen and helium exerts a total pressure of 800 torr. If the partial pressure are oxygen 425 torr and helium 80 torr, what is the particle pressure (torr) of nitrogen in the mixture? P total = P O2 + P N2 + P He 800 torr = 425 torr + P N2 + 80 torr 800 – (425+80) = P N2 800 505 = P N2 295 torr = P N2 (Note: In addition and subtraction look at number of places after decimal point to report final answer; Also, in this problem make sure all pressures are in the same units)...
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 Spring '08
 Hanover
 pH, 40 feet, 283 K, 310 K, 383 K, 715 ml

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