For a certain reaction the change in enthalpy and change in entropy are `40.63 kJ mol^(-1)` and `100 JK^(-1)` .What is the value of `Delta G` at `27^(@)C` and indicate whether the reaction is possible or not ?

Explanation

We know that : `Delta G = Delta H - T Delta S`
Given `T=27+273=300 K, Delta H=40.63xx10^(3)J mol^(-1), =40630 J mol^(-1), Delta S = 100 JK^(-1)`
`Delta G = 40630-300xx100=40630-30000 =+10630 J`
Positive value of `Delta G` indicates that the reaction is not possible.