A sample of 1.60 mol H2 (Cv = 20.5 J K-1 mol-1) at 21°C and 1.50 atm undergoes a reversible adiabatic compression until the final pressure is 4.50 atm. Calculate the final volume of the gas sample and the work associated with this process. Assume that the gas behaves ideally.
The Attempt at a Solution
pv=nRT → (1.5 atm)(V0=(1.6 mol)(0.08206 atm mol K)(294 K)
V0=25.734016 L (tried this initially as I was given Cv, but that was wrong)
P1V1=P2V2→(1.5 atm)(25.734016 L)=(4.5 atm)(V) →8.57800533 L (which was wrong)
ΔE=-(4.5)(17.1501067)= -77.202 J (nope)
ΔE=(1.6 mol)(20.5 K mol)(294 K)= 9643.2 J (Nope)
I'm not really sure where I went wrong with this, any input would be really helpful