engineering chemistry MCQ #2750

The standard electrode potential of a cell is 1.1 V. Calculate the standard Gibbs free energy change (ΔG°) for the cell reaction.

engineering chemistry MCQ #2750

  1. Question 1

    Q1. The standard electrode potential of a cell is 1.1 V. Calculate the standard Gibbs free energy change (ΔG°) for the cell reaction.

    • A) -212.3 kJ/mol
    • B) -106.15 kJ/mol
    • C) 212.3 kJ/mol
    • D) 106.15 kJ/mol

    Answer: -106.15 kJ/mol

    Explanation: ΔG° = -nFE°, where n = number of electrons, F = Faraday constant. Here, n = 2 (assuming), F = 96500 C/mol, E° = 1.1 V, so ΔG° = -2 * 96500 * 1.1 = -212300 J/mol = -212.3 kJ/mol. However, the closest answer is obtained when n = 1 or the given value is for 1 mole of electrons.