The correct relationship between free energy change in a reaction and the corresponding equilibrium constant, `K_(c)` is

Options

A. `DeltaS - RT` in `K_(c)`
B. `-DeltaG= RT` ln `K_(c)`
C. `DeltaG^(@)= RT` ln in `K_(C)`
D. `-DeltaG^(@) =RT` ln `K_(c)`

Answer

D

Explanation

The standard free energy change `(DeltaG^(@))` is related to equilibrium constant K as
`DeltaG^(@) = -RT ln K, DeltaG^(@) = -2.303 RT log K`