Q 1(c) [10 Marks] A hydrogen fuel cells operates with the following reactions: H2 2 e + 2 H+ (at the anode), AG = 0 kJ/mol 12 O2 + 2 e + 2 H+ H20 (at the cathode), AG = -232.7 kJ/mol where AH is 285 kJ/mol. For fuel cells, the electrical work represents the Gibbs free energy and the maximum possible energy conversion efficiency, Nmax, is given by: JAG nmax = AH Given that the Gibbs free energy equals the electrical work (under constant temperature and pressure), and the electrical work equals the product of the charge and voltage, therefore: W = AG = -nFE Where F is Faraday's constant, n is the number of moles of electrons produced per mole of H2 (in this case 2) and E is the cell voltage. Use this information to calculate: (i) the maximum possible energy conversion efficiency and CS404 - Interfacial and Supramolecular Chemistry Resit Examinations 2018/2019 Page 2 of 7 (ii) the voltage that can be achieved for this fuel cell