Consider the hydrogen-oxygen fuel cell where: H₂(g)+ O₂(g) H₂O(l)$\Delta$G° = -237.18 kJ/mol H₂ Which of the following statements is true?

Question

Quizplus · Accepted Answer

A) At standard conditions, the maximum work that the fuel cell could do on the surroundings is equal to the Gibbs free energy change of the reaction, which is -237.18 kJ/mol. Therefore, statement A is true.
B) In reality, the fuel cell cannot convert all the energy released by the reaction into useful work, and some energy is lost as waste heat. Hence, statement B is true.
C) The reversible pathway provides the maximum work possible, and in reality, a fuel cell cannot operate perfectly reversibly. Therefore, some energy is lost as waste heat in the fuel cell. Therefore, statement C is true.
D) As all three statements (A, B and C) are true, answer D is correct. 
E) All three statements are true, so answer E is not correct.

Consider the Hydrogen-Oxygen Fuel Cell Where: H2(g)+ O2(g) H2O(l) Δ\DeltaΔ

Consider the Hydrogen-Oxygen Fuel Cell Where: H₂(g)+ O₂(g) H₂O(l) $\Delta$