Chemical Thermodynamics Question 234
Question: What is the free energy change for the conversion of 1 mole of water into steam at $ 373.2K $ . The heat of vaporization $ ( \Delta ,H_{v} ) $ of water of $ 373.2K $ is $ 9.1kcalmo{{l}^{-1}} $ . The entropy change is 25.5 cal/mol deg.
Options:
A) $ -401.6cal/mol $
B) $ -416.6cal/mol $
C) $ 516.5cal/mol $
D) $ -516.5cal/mol $
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Answer:
Correct Answer: B
Solution:
- $ \Delta G=\Delta H-T\Delta S $
$ \therefore \Delta G=9100-373.2\times 25.5=-416.6calmo{{l}^{-1}} $
BETA
