If the `E_(cell)^(@)` for a given reaction has a positive value, then which of the following gives the correct relationship for the values of `DeltaG^(@)` and `K_(eq)` :-

Options

A. `Delta G^(@) gt 0 , K_(eq) gt 1`
B. `Delta G^(@) lt 0 , K_(eq) gt 1`
C. `Delta G^(@) lt 0 , K_(eq) lt 1`
D. `Delta G^(@) gt 0 , K_(eq) lt 1`

Answer

D

Explanation

`Delta G^(@) = - n FE^(@)`
`E^(@) lt 0 , Delta G^(@) =- RT` ln `K_(eq)` .
`Delta G^(@) gt 0 ` and `K_(eq) lt 1`