9. Consider the acid mole hydrogen fuel cell: H+ (aq) + e¯ → H₂ (g) 02(g) +2H+( Pt H2(g) (PH₂) HCl(aq) (0.1 molal)|02 (g) (Po₂) Pt *(aq) + 2e − → H₂O (1) Ered = 0V Ered = 1.2288 V a. What is the overall reaction AND the standard cell potential? 10 points b. While the pressure of H₂ used in an actual proton exchange membrane (PEM) based fuel cell can be up to 400 kPa or greater, the ambient partial pressure of O2 is typically ~20 kPa. Calculate the actual maximum voltage from the fuel cell assuming T = 298 K, PH₂ = 400 kPa, and, Po₂ = 20 kPa. Assume the HCL solution is ideal. 15 points c. Consider the enthalpy of formation of liquid water at 298 K: AH (H₂O(1)) = -285.8 kJ mol-1. Use Ece to determine AG of water, AND then calculate AS for the fuel cell reaction. 15 points d. Calculate the change in voltage if the temperature of the cell, given the parameters in part (b), is increased from 298 K to 308 K. 15 points e. Explicitly write out the reaction quotient used in calculating the cell voltage with the Nernst Equation. If the product formed in the reaction goes into the acid solution, explain whether (and how) changing the concentration of HCl(aq) could change the voltage of the cell. 10 points f. What is the voltage of the cell when it reaches equilibrium? 5 points