The electrical potential energy (voltage) of this cell is 0.53 V. When describing an electrochemical cell like this one, the reaction is often described as only going forward: Zn(s)+Ni2+(aq)⟶Ni(s)+Zn2+(aq) However, many oxidation–reduction processes are reversible. For example, recharging a battery reverses the direction of a reaction and puts electrical energy back into the system. In fact, you can rewrite the previous equation as an equilibrium and show energy as a product from the forward reaction: Zn(s)+Ni2+(aq)↽−−⇀Ni(s)+Zn2+(aq)+energy Write an equilibrium expression for this reaction.