Recent content by wwildlifee

I also thought that the entropy of the initial state S1 (and final state) might be needed. However, I thought that there is a way to express ΔA and ΔG only in terms of the variables which are given in the problems. So I tried, but it is an impossible work (at this point)! Thanks for your kind...

So, is it enough to express ΔG as ΔH - Δ(TS) ? I assume the processes are all reversible. And I think it is okay to use Cv and Cp here. 1) ΔU = Cv (T2 - T1), ΔH = Cp (T2 - T1), ΔS = 0 (because dq = 0) 2) ΔU = Cv (T2 - T1), ΔH = Cp (T2 - T1), ΔS = Cp ln(T2/T1) - R ln(P2/P1) (from dH = TdS + Vdp)...

The definition of G is G = H - TS, so ΔG is ΔG = ΔH - Δ(TS) = ΔH - TΔS - SΔT I'm not sure that I understand your question correctly, but U, H, S, A and G are state functions, so if I know the initial and final state, I think the details of the process do not matter.:rolleyes:

This course is the classical thermodynamics. So all I've got are dU = Tds - pdV dH = Tds + Vdp dA = d(U-TS) = dU - TdS - SdT = -pdV - SdT dG = d(H-TS) = dH - TdS - SdT = Vdp - SdT Maxwell relations, and the Gibbs-Helmholtz equation. I I tried to solve case 1 by separating the adiabatic process...

I can get the changes in S for the processes above, so if I already know S1, S2 = delta_S + S1 respectively. Is it a hint for calculating the delta_A and delta_G for processes in which temperature changes?

Thanks[emoji2] However this is not what I do not know. What I want to know is how to handle the integration of (-SdT) in dA or dG for the processes above(adiabatic, isobaric, isochoric).

Homework Statement Calculate changes in A and G of one mole of an ideal gas that undergoes the following processes respectively. 1. adiabatic expansion from (T1, P1) to (T2, P2) 2. isobaric expansion from (P, V1, T1) to (P, V2, T2) (if it is not isothermal) 3. isochoric expansion from (V, P1...