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) ?

If the E_("cell")^(@) for a given reaction has a negative value, which

1.	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) ?
Answer» `DELTA G^(@) lt 0, K_(EQ) gt 1` `Delta G^(@) lt 0, K_(eq) lt 1` `Delta G^(@) gt 0, K_(eq) lt 1` `Delta G^(@) gt 0, K_(eq) gt 1` Solution :`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`