Which equation relates cell potential to concentrations in electrochemical cells?

The Nernst equation is a critical relationship in electrochemistry that connects the cell potential (voltage) of an electrochemical cell to the concentrations of the reactants and products involved in the reaction. It is crucial for understanding how variations in concentration affect the driving force of electrochemical reactions.

Specifically, the Nernst equation allows us to calculate the cell potential under non-standard conditions by incorporating the standard cell potential along with the effects of the concentrations of ions participating in the redox reaction. The equation typically takes the form of:

[ E = E^\circ - \frac{RT}{nF} \ln Q ]

where ( E ) is the cell potential under non-standard conditions, ( E^\circ ) is the standard cell potential, ( R ) is the universal gas constant, ( T ) is the temperature in Kelvin, ( n ) is the number of moles of electrons exchanged, ( F ) is Faraday's constant, and ( Q ) is the reaction quotient representing the ratio of the concentrations of the products to the reactants.

This relationship is significant because it highlights how changes in the concentrations of reactants or products can influence the overall cell potential, allowing chemists to predict