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Bugsy23
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Homework Statement
A sample of 8.02*10^-1 moles of nitrogen gas ([tex]\gamma[/tex]=1.4) occupies a volume of 2*10^-2m^3 at pressure 1*10^5pa and temperature 300K. The gas is adiabatically compressed to half its original volume. What is the change in entropy of the gas?
Homework Equations
S2-S1=CvIn(P2/P1)+CpIn(V2/V1)
PV=nRT
The Attempt at a Solution
I have already worked out the values for Cv and Cp and the change in volume of the gas, but I don't know how to find the change in pressure. Since nitrogen behaves as an ideal gas, it should be possible to find it using PV=nRT, but that also requires knowing the change in temperature. Is there a different way of working out the change in pressure?