One mole of oxygen gas is at a pressure of 5.30 atm and a temperature of 31.0°C.

Question

One mole of oxygen gas is at a pressure of 5.30 atm and a temperature of 31.0°C. (a) If the gas is heated at constant volumeuntil the pressure triples, what is the final temperature?
°C
(b) If the gas is heated so that both the pressure and volume aredoubled, what is the final temperature?
°C (a) If the gas is heated at constant volumeuntil the pressure triples, what is the final temperature?
°C
(b) If the gas is heated so that both the pressure and volume aredoubled, what is the final temperature?
°C

Explanation / Answer

PV = nRT

from which we get the combined gas law (since n and R remainconstant):

PV/T = P'V'/T' P' = 3P   (pressure triples) V' = V (volume is held constant) Thus: PV/T = (3P)V/T' T' = (3P)VT/PV T' = 3T T' = 3(273+31) = 912 K = 638.84oC
b) PV/T = P'V'/T' P' = 3P   (pressure triples) V' = 3V (volume triples) PV/T = (3P)(3V)/T' T' = 9PVT/PV T' = 9T T' = 9(301) = 2736 K = 2463oC
P' = 3P   (pressure triples) V' = 3V (volume triples) PV/T = (3P)(3V)/T' T' = 9PVT/PV T' = 9T T' = 9(301) = 2736 K = 2463oC

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