At 298 K a cell reaction has a standard cell potential of +0.17 V. The equilibrium constant for the reaction is 5.5 × 10⁵. What is the value of n for the reaction?

The Nernst Equation relates the cell potential of an electrochemical reaction to the concentrations of the reactants and products. It is expressed as E = E° - (RT/nF)ln(Q), where E is the cell potential, E° 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 transferred, F is Faraday's constant, and Q is the reaction quotient.

The standard cell potential (E°) is the voltage measured under standard conditions (1 M concentration, 1 atm pressure, and 25°C) for a galvanic cell. It indicates the tendency of a chemical reaction to occur spontaneously; a positive E° suggests a spontaneous reaction, while a negative E° indicates non-spontaneity.

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction. It is related to the standard cell potential through the equation ΔG° = -nFE°, where ΔG° is the change in Gibbs free energy. A larger K value indicates a greater tendency for the reaction to favor products at equilibrium.