If the E°cell for a given reaction has a negative value, which of the following gives the correct relationships for the values of and Keq? Option 1) Option 2) Option 3) Option 4)

Gibbs energy of the reaction -

$\Delta_{r}G=-nFE_{cell}$

- wherein

$\Delta _{r}G =$ gibbs energy of the reaction

$E_{cell}=$ emf of the cell

nF = amount of charge passed

$\Delta G^{\circ}=-nFE^{\circ}_{cell}$

If $E^{\circ}_{cell}=-ve$ then $\Delta G^{\circ}=+ve$

i.e. $\Delta G^{\circ}>0$

$\Delta G^{\circ}=-nRT$ log Keq

For $\Delta G^{\circ}=+ve$ , log Keq = -Ve

i.e. Keg < 1

Option 1)

this is the correct option

Option 2)

this is the incorrect option

Option 3)

this is the incorrect option

Option 4)

this is the incorrect option

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