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Jake4
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Homework Statement
Two somewhat related problems:
1. Using the expression for change in entropy of an ideal gas per mole:
ΔS=CV+R ln(V)
Calculate the change in entropy, change in Helmholtz Free Energy and change in Gibbs Free Energy when 1 mole of an ideal gas is compressed from 1 atm to 20 atm at 20°Cand
2. An ideal gas has a molar specific heat given by CV=A+BT where A and B are constants.
Using a thermodynamic identity find an expression for the change in entropy as it goes from V1, T1 to V2 , T2.
Homework Equations
dS= CVdT/T
The Attempt at a Solution
My main issues with these problems (I may be totally missing something) is that CV is given in both, yet they imply a change in Volume. By definition, CV is the heat capacity at constant Volume. Is this something I should simply overlook to carry out the calculations?
Thank you so much for the help :)