Gibbs-Helmoholtz equation relates the free energy change to the enthalpy and entropy changes of the process as
`(DeltaG)_(PT) = DeltaH - T DeltaS`
The magnitude of `DeltaH` does not change much with the change in temperature but the enrgy factor `T DeltaS` changes appreciably. Thus, spontaneity of a process depends very much on temperature.
The enthalpy change for a certain reaction at `300K` is `-15.0 kcal mol^(-1)`. The entropy change under these conditions is `-7.2 cal K^(-) mol^(-1)`. The free enegry change for the reaction and its spontaneous//nonspontaneous character will be

Options

A. `-12.84 kcal mol^(-1)`, spontaneous
B. `-12.16 kcal mol^(-1)`, spontaneous
C. `12.84 kcal mol^(-1)`, non spontaneous
D. `12.0 kcal mol^(-1)`, spontaneous

Explanation

`DeltaG = DeltaH - T DeltaS`
`= - 15.0 kcal mol^(-1) -300 xx (-7.2 cal K^(-1) mol^(-1))`
`=- 12.84 kcal mol^(-1)`