Answer
Please see the work below.
Work Step by Step
We can predict the spontaneity of a reaction from the sign of $ \Delta G^{\circ}$.
If $ \Delta G^{\circ}$ is negative, the reaction is spontaneous and if positive, it is non-spontaneous.
There is a relation connecting $ \Delta G^{\circ}$ and $ E^{\circ}{cell}$.
$ \Delta G^{\circ} = -nF E^{\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
If $ E^{\circ}{cell}$ value is negative, $ \Delta G^{\circ}$ becomes positive which means the reaction is non spontaneous.
On the other hand if $ E^{\circ}{cell}$ is positive, $ \Delta G^{\circ}$ becomes positive which means the reaction is spontaneous.
