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Entropy changes for the process H(2)O(...

Entropy changes for the process
`H_(2)O(l) rarr H_(2)O(g)`
at normal pressure and 274 K are given below `Delta G_(system) = - 22.13, Delta S_("surroundings") = + 22.05`
Then process is non spontaneous because

A

`Delta G_("system")` is -ve

B

`Delta G_("surrounding")` is +ve

C

`Delta S_("universe")` is -ve

D

`Delta G_(system) ne Delta S_("surrounding")`

Text Solution

Verified by Experts

The correct Answer is:
C
For a process to be spontaneous `Delta S_("universe")` must be positive. Here,
`Delta S_("universe") = - 22.13 + 22.05 = - 0.08 kJ`
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