A hydrogen fuel cell, in which oxygen gas was used as oxidant, was operated at the room temperature and pressure for 1.5 hours. At the end of this process, 0.065 moles of oxygen was determined to be consumed. Assuming both fuel and oxidant gases as ideal gases, a) Write the half reactions occurring at this fuel cell. b) What is the maximum theoretical voltage that can be produced in this fuel cell? Is it possible to obtain this voltage for a non-ideal system? Write 3 reasons explaining your answer. c) Calculate the volume of consumed fuel in liters during the period of 1.5 hours. d) What is the electric charge (in coulombs) passing through the fuel cell at the end of the period of 1.5 hours? e) Calculate the current (in ampere) at the end of the same period. ADDITIONAL INFORMATION: R= 0.0821 atm.L/mol.K, The charge of 1 mole of electrons is 96500 Coulombs