## Thermodynamics problem 4.58

Volume: $\Delta S = nR\ln \frac{V_{2}}{V_{1}}$
Temperature: $\Delta S = nC\ln \frac{T_{2}}{T_{1}}$

asannajust_1J
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### Thermodynamics problem 4.58

(a) Verify that there is no difference in the state function S for a process in which 1.00 mol of nitrogen molecules in a cylinder of volume 3.00 L at 302 K undergoes the following three steps: (i) cooling at constant volume until T 5 75.6 K; (ii) heating at constant pressure until T 5 302 K; (iii) compressing at constant temperature until V 5 3.00 L. Calculate DU and DS for this entire cycle. (b) What are the values of q and w for the entire cycle? (c) What are DSsurr and DStotal for the cycle? If any values are nonzero, explain how this can be so, despite entropy being a state function. (d) Is the process spontaneous, nonspontaneous, or at equilibrium.

I calculated s for each part and the sum is equal to zero. For part c, I am assuming Ssurr is not also equal to zero however since each step would have a different effect on the surroundings. Not sure if this is the correct assumption or reasoning.

Tanmay Singhal 1H
Posts: 143
Joined: Sat Jul 20, 2019 12:16 am

### Re: Thermodynamics problem 4.58

i think you can assume that. im not entirely sure though

SnehinRajkumar1L
Posts: 101
Joined: Thu Jul 11, 2019 12:15 am

### Re: Thermodynamics problem 4.58

Yes, you can assume that. The volume and pressure return to the initial state.