Gibbs Helmholtz equation relates the enthalpy, entropy and free energy change of the process at constant pressure and temperature as
`DeltaG=DeltaH-TDeltaS " (at constant P, T)"`
In General the magnitude of `DeltaH` does not change much with the change in temperature but the terms `TDeltaS` changes appreciably. Hence in some process spontaneity is very much dependent on temperature and such processes are generally known as entropy driven process.
For the reaction at 298 K, `A_(2)B_(4)rarr2AB_(2)`
`DeltaH=2" kJ"` and `DeltaS` = 20 J/K at constant P and T, the reaction will be

Options

A. spontaneous and entropy driven
B. spontaneous and enthalpy driven
C. non-spontaneous
D. at equilibrium

Answer

A

Explanation

`(DeltaG)_(PT)=2000-(20xx298)`
`=-3960 " J"//"mol"`