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### 9.35 Explained

Posted: Thu Feb 08, 2018 11:58 pm
I'm super confused about how the answer is figured out in this question.

Container A is filled with 1.0 mol of the atoms of an ideal monatomic gas. Container B has 1.0 mol of atoms bound together as diatomic molecules that are not vibrationally active. Container C has 1.0 mol of atoms bound together as diatomic molecules that are vibrationally active. The containers all start at Ti and the temperature increases to Tf. Rank the containers in order of increasing change in entropy. Explain your reasoning.

Thanks!

(Claire Woolson Dis 1K)

### Re: 9.35 Explained

Posted: Fri Feb 09, 2018 12:17 am
Ideal gas = highest entropy
Vibrationally active (generating heat and disorder by moving) = second highest entropy
Not vibrationally active = least entropy

### Re: 9.35 Explained

Posted: Fri Feb 09, 2018 8:25 am
This problem is also on the solutions manual error sheet, where there is an explanation. The actual answer is that the change in entropy of B is less than that of C. However, The change in entropy of C is equal to the change in entropy of A. (B<C=A)