i need question (c) answered, please

Q4: 13 marks A membrane electrolysis chlor-alkali plant operating continuously (at constant current and voltage) at room temperature and pressure (RTP) produces 65 tonne day of NaOH (40 g mol-") as a primary product. The balanced total reaction equation for the process is provided below. The average operating cell voltage for the plant is 3.1 V. NaCl + H2O + NaOH + 12 Cl2 + 12 H2 (a) How much (1) chlorine (71 g mol") and (ii) hydrogen (2.0 g mol-') in tonne day does the plant produce? [3 marks] (b) What is the daily electrical energy consumption of the electrolysers (in MWh day-')? [4 marks] (c) The standard enthalpy of reaction for this process is +223 kJ mol-1 (NaOH). What is the thermodynamic efficiency of this plant? [3 marks] (d) How much energy in MWh day-') could the plant save if it used an oxygen-depolarised cathode electrolyser instead, which has an operating cell voltage of 2.1 V? [3 marks] + Add to Additional information: RTP conditions: Pressure = 1 atm (101325 Pa). Temperature = 25 C = 298 K. Volume of 1 mole of ideal gas at RTP = 24.0L mol-1 P(O2) in air = 0.21 atm Gas constant R = 8.314 J molt K-1 Faraday constant F = 96 485 C mol-1 1 kWh = 3.6x1063 Atomic masses (g mol-"): H 1.00 Li 6.94 16.00 ci 35.5 Fe 55.85 Zn 65.38 Ag 107.87