Refer to the tabulated values of ∆Gf° in Appendix IIB to calculate E°cell for a fuel cell that employs the reaction between methane gas (CH4) and oxygen to form carbon dioxide and gaseous water.

Verified step by step guidance

1. Identify the balanced chemical equation for the reaction: CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(g).
2. Use the standard Gibbs free energy of formation (∆G_f°) values from Appendix IIB for each species involved in the reaction: CH_4(g), O_2(g), CO_2(g), and H_2O(g).
3. Calculate the standard Gibbs free energy change (∆G°) for the reaction using the formula: ∆G° = Σ(∆G_f° of products) - Σ(∆G_f° of reactants).
4. Use the relationship between Gibbs free energy change and cell potential: ∆G° = -nFE°_cell, where n is the number of moles of electrons transferred and F is the Faraday constant.
5. Solve for the standard cell potential (E°_cell) using the equation: E°_cell = -∆G° / (nF).