What does a positive standard cell potential indicate about a redox reaction?

In the context of an electrochemical reaction, a positive standard cell potential ($E^{\circ }$) indicates that the redox reaction is expected to occur spontaneously under standard conditions.1

When the calculated $E^{\circ }$ for a net reaction is positive, it signifies that the process has a thermodynamic tendency to proceed from reactants to products. This value is directly related to the standard Gibbs free energy change ($\Delta G^{\circ }$) of the reaction, where $\Delta G^{\circ }=-nF{E}^{\circ }$. Because a spontaneous process requires a negative change in Gibbs free energy, a positive $E^{\circ }$ value ensures that $\Delta G^{\circ }$ is negative, confirming the reaction's spontaneity.12

Conversely, if the standard cell potential were negative, the reaction would not be spontaneous in the forward direction as written, though it could proceed spontaneously in the reverse direction.1