Consider the reaction in the lead-acid cell Pb(s) + PbO₂(s) + 2H₂SO₄(aq) → 2PbSO₄(aq) + 2H₂O(l)
For which E°_cell = 2.04 V at 298 K. ΔG° for this reaction is

Question

Consider the reaction in the lead-acid cell Pb(s) + PbO₂(s) + 2H₂SO₄(aq) → 2PbSO₄(aq) + 2H₂O(l) For which E°_cell = 2.04 V at 298 K. ΔG° for this reaction is

Quizplus · Accepted Answer

The Gibbs free energy change (ΔG°) for a reaction can be calculated using the formula ΔG° = -nFE°, where n is the number of moles of electrons transferred in the reaction, F is the Faraday constant (96485 C/mol), and E° is the standard cell potential. In this reaction, 2 moles of electrons are transferred, and E° is 2.04 V. Therefore, ΔG° = -(2 mol)(96485 C/mol)(2.04 V) = -394000 J = -3.94 × 10^5 J = -3.94 × 10^2 kJ, which corresponds to choice B.

Consider the Reaction in the Lead-Acid Cell Pb(s) + PbO2(s)

Consider the Reaction in the Lead-Acid Cell Pb(s) + PbO₂(s)