
#1
Feb912, 08:44 PM

P: 4

1. The problem statement, all variables and given/known data
When one mole of an ideal gas is compressed adiabatically to onehalf of its original volume, the temperature of the gas increases from 273 to 433K. Assuming that Cv is independent of temperature, calculate the value of Cv for this gas. 2. Relevant equations Cv = dU/dT dU = dq + dw dq = 0 for adiabatic processes, thus dU=dw PV = nRT 3. The attempt at a solution Cv = pdV / dT Cv = (nRT/V)(dV/dT) I'm stuck here. Assuming I'm correct thus far, do I use the initial or final values for T and V (i.e. do I use 273K or 433K?) 



#2
Feb912, 10:26 PM

P: 2

I think we might be in the same class...
I've been trying to verify my solution, but no luck so far. This is what I got: Cv = (dU/dT) dU = dq + dw, but dq = 0, so dU = dw and Cv = dU/dT w = nRTln(V2/V1), but V2 = 1/2V1, so w = nRTln(1/2), and dw = nR*ln(1/2)*dT Substitute the last equation for dw in Cv=dw/dT and you get Cv = (nR*ln(1/2)*dT)/dT which simplifies to Cv = nR*ln(1/2). That's what I got, but I'm not confident that it's correct. 



#3
Feb912, 10:48 PM

P: 4

Elber 10am MWF?




#4
Feb912, 10:56 PM

P: 2

How to calculate Cv
Yeah.




#5
Feb912, 11:11 PM

P: 4

T1/T2 = (V2/V1)^γ1 then you also find the value of P1 and P2 from P1V1^γ= P2V2^γ The put the values in adiabatic process equation ∂W = (P1V1P2V2)/γ1 Then use your formulae 



#6
Feb1012, 12:53 AM

P: 4

Thanks guys. This is pretty crucial assistance.




#7
Feb1012, 03:37 AM

P: 69

CpCv = R (gas constant) (Cp/Cv) = γ Eliminate Cp from these two equations to get Cv. 


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