If the `E_("cell")^(@)` for a given reaction has a negative value, which of the following gives the correct relationships for the values of `Delta G^(@) and K_(eq)` ?

Options

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

Answer

C

Explanation

`E_("cell")^(@) = -ve`
`Delta G^(@) = -nF " "E_("cell")^(@)`
`Delta G^(@) =+ve rArr Delta G gt 0`
`Delta G^(@) = -2.303 " RT log "K_(eq)`
`therefore K_(eq) lt 1`