A 325 ml sample of gas is initially at a pressure of 721 torr and a temperature of 32°c. if this gas is compressed to a volume of 286 ml and the pressure increases to 901 torr, what will be the new temperature of the gas (reported to three significant figures in °c) ?

Question

Chemistry

Broderick Franklin

12 May, 09:03

A 325 ml sample of gas is initially at a pressure of 721 torr and a temperature of 32°c. if this gas is compressed to a volume of 286 ml and the pressure increases to 901 torr, what will be the new temperature of the gas (reported to three significant figures in °c) ?

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Ryker Stephens · Answer 1

You can solve this question by using the ideal gas PV=nRT formula. Be careful though because the temperature used in the equation is kelvin, not celcius. The formula to determine the temperature would be: T = PV/nR

The calculation would be:

T1/T2 = (P1V1/nR) / (P2V2/nR)

32+273.15/T2 = (325*721) / (286*901)

305.15/T2 = 0.90934

T2 = 305.15 / 0.90934 = 335.57 K = 62.4C