Gibbs Free Energy

To calculate the standard Gibbs free energy change (ΔG°) for the reaction, we use the relation between Gibbs free energy and the standard electrode potential (E°) given by the equation:

ΔG° = -nFE°

Where:

• n = number of moles of electrons exchanged in the balanced equation.
• F = Faraday's constant = 96485 C/mol.
• E° = standard electrode potential = 1.1 V.

For the given reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), the number of moles of electrons exchanged (n) is 2, due to the transfer from Zn⁰ to Zn²⁺ and Cu²⁺ to Cu⁰. Substituting the known values:

ΔG° = -2 × 96485 × 1.1

ΔG° = -212267 J/mol

Finally, to match the options format, we convert this into kJ/mol:

ΔG° = -212.27 J/mol

Thus, the standard Gibbs free energy change for the reaction is approximately -212.27 J/mol, which matches the provided correct answer choice.