## 9.85 (a)

$\Delta S = \frac{q_{rev}}{T}$

Andy Liao 1B
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Joined: Thu Jul 13, 2017 3:00 am

### 9.85 (a)

9.85 Potassium nitrate dissolves readily in water, and its enthalpy of solution is +34.9 kJ.mol-1. (a) Does the enthalpy of solution favor the dissolving process? (b) Is the entropy change of the system likely to be positive or negative when the salt dissolves? (c) Is the entropy change of the system primarily a result of changes in positional disorder or thermal disorder? (d) Is the entropy change of the surroundings primarily a result of changes in positional disorder or thermal disorder? (e) What is the driving force for the dissolution of KNO3?

I understand every part but part (a). The answer is that the change in enthalpy does not favor the dissolution process. Can someone please explain to me why this is true?

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