If `E_(cell)^(ɵ)` for a given reaction is negative, which gives the correct relationships for the values of `DeltaG^(ɵ)` and `K_(eq)`?

Options

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

Answer

A

Explanation

`DeltaG^(@)=-nFE^(@)`
`E^(@)` is negative
So `DeltaG^(@)=+ve`
`DeltaG^(@)=-2.303RT" log "K`
`thereforeK_(eq) lt1`