Answer
The one with a positive $E^{\circ}{cell}$ value proceeds towards the formation of more products at equilibrium.
Work Step by Step
The one with a positive $E^{\circ}{cell}$ value proceeds towards the formation of more products at equilibrium.
We have a relation connecting $ \Delta G^{\circ}$ and $E^{\circ}{cell}$.
$ \Delta G^{\circ}= -n FE^{\circ}{cell}$
Where
$ \Delta G^{\circ} = standard\ free\ energy\ change$
n = number of electrons involved in cell reaction.
F = Faraday’s constant
$E^{\circ}{cell}= Standard cell EMF $
So if we substitute a negative $E^{\circ}{cell}$ value in the above equation, $ \Delta G^{\circ}$ becomes positive which means the reaction is non-spontaneous.
On the other hand, if we substitute a positive $E^{\circ}{cell}$ value in the above equation, $ \Delta G^{\circ}$ becomes negative which means the reaction is spontaneous and products will form.
