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Enthalpy and entropy changes of reaction...

Enthalpy and entropy changes of reaction are `40.63 kJ mol^(-1)` and `108.8 J K^(-1) mol^(-1)`, respectively. Predict the feasibility of the reaction at `27^(@)C`.

Text Solution

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`DeltaH = 40.63 kJ mol^(-1) = 40630 J K^(-1) mol^(-1)`
`DeltaS = 108.0 J K^(-1) mol^(-1)`
`T = 27^(@)C = 27 + 273 = 300 K`
Now `DeltaG = DeltaH -TDeltaS`
` = 40630 J mol^(-1)(300K)xx(108.8J K^(-1) mol^(-1))`
`DeltaG = 7990 J mol^(-1)`
Since `DeltaG` is positive, the reaction is not feasible in the forward direction.
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