Fuel Cells — MCQ Practice

Which of the following statements is INCORRECT regarding a hydrogen-oxygen fuel cell?

For a hydrogen-oxygen fuel cell, if the standard Gibbs free energy change ($Delta G^circ$) for the overall reaction is $-474.4,\text{kJ/mol}$ and the standard enthalpy change ($Delta H^circ$) is $-571.6,\text{kJ/mol}$ at $298,\text{K}$, what is the theoretical maximum efficiency of the fuel cell?

In an alkaline fuel cell, the electrolyte used is a solution of:

Which of the following is a major environmental advantage of hydrogen-oxygen fuel cells over internal combustion engines?

Consider a fuel cell operating at standard conditions. If the standard cell potential ($E^circ_{cell}$) is $1.23,\text{V}$ for the reaction $2H_2(g) + O_2(g) \rightarrow 2H_2O(l)$, calculate the standard Gibbs free energy change ($Delta G^circ$) for this reaction. (Given: Faraday's constant, $F = 96485,\text{C/mol}$)

Which of the following statements best describes the primary function of the electrolyte in a fuel cell?