The lead storage battery uses the reaction: (b) Calculate ∆G for this reaction on a cold winter's day (10 °F) in a battery that has run down to the point where the sulfuric acid concentration is only 0.100 M.

Gibbs Free Energy (∆G) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. It is crucial for determining the spontaneity of a reaction; a negative ∆G indicates a spontaneous process, while a positive ∆G suggests non-spontaneity. The relationship between ∆G, enthalpy (∆H), and entropy (∆S) is given by the equation ∆G = ∆H - T∆S.

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 standard cell potential, R is the 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. This equation is essential for calculating the cell potential under non-standard conditions, such as varying concentrations.

The concentration of reactants and products affects the position of equilibrium in a chemical reaction, as described by Le Chatelier's Principle. When the concentration of a reactant is decreased, the equilibrium shifts to favor the formation of more reactants, while an increase in product concentration shifts it towards products. In the context of the lead storage battery, the low concentration of sulfuric acid (0.100 M) will influence the Gibbs Free Energy and the overall cell potential, impacting the battery's performance.