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. `DeltaG^(@) gt0,K_(eq) lt 1`
B. `DeltaG^(@) gt0,K_(eq)gt1`
C. `DeltaG^(@)lt0,K_(eq)gt1`
D. `DeltaG^(@)lt0,K_(eq)lt1`

Answer

A

Explanation

`DeltaG^(@)=-nFE_(cell)^(@)` . . . (i)
and `DeltaG^(@)=-RT" ln "K_(eq)` . . . (ii)
From (i), if `E_(cell)^(@)` is negative, `DeltaG^(@)` will be positive, i.e., `DeltaG^(@)gt0`
From (ii), `DeltaG^(@)` can be positive only if `K_(eq)lt1`.