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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`.

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Here, we are given `: Delta H =40.63 kJ mol^(-1) = 40630 J mol^(-1) , Delta S = 108 J K^(-1) mol^(-1)`
`T = 27^(@) C = 27 +273 =300K`
`:. Delta G =Delta H = T Delta S = 40630 J mol^(-1) - 300 K xx 108.8 JK^(-1) mol^(-1) = 7990 J mol^(-1)`
Since `Delta G` comes out to be positive ( i.e., ` Delta G gt 0)` , the reaction is not feasible in the forward direction.
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