A) \[-100\]
B) \[+100\]
C) \[+342\]
D) \[-342\]
Correct Answer: A
Solution :
\[\Delta H=+35.3kJ/mol\] \[\Delta S=\frac{\Delta H}{T}=\frac{+35.3}{35.3}=0.1kJ/mol/K\] \[\Delta S=0.1\times {{10}^{3}}=1000J/mol/K\] Entropy change in the transition of vapour to liquid is negative, \[\Delta S=-100\].You need to login to perform this action.
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