Structured questions1 The half-equations and standard electrode potential at 25 °C for two half-cells are given below:Hg2Cl2(s) + 2e– → 2Hg(s) + 2Cl–(aq) E° = +0.24VFe3+(aq) + e– → Fe2+(aq) E° = +0.77V(a) Write a cell diagram for the electrochemical cell constructed using the above two half-cells.(b) Write the overall equation for the electrochemical cell.(c) Calculate the above cell e.m.f. of the electrochemical cell at standardised conditions.(d) Chlorine gas is bubbled into the Fe3+(aq)/Fe2+(aq) half-cell and the e.m.f. of the cell is observed. Explain how the electrode potential of the cell will change.(e) Calculate the electrode potential of the cell if the ratio of _ Fe2+Fe3+ _ is 1.00 × 10–3 while the concentration of Cl– remains unchanged.(f) What is the effect of adding lead(II) nitrate solution to the Hg2Cl2(s)/Cl–(aq) half–cell?Essay Question1 (a) The overall chemical change taking place during the industrial electrolytic manufacture of aluminium metal is represented by the following equation:2Al2O3 + 3C → 4Al + 3CO2(i) Explain all the chemical changes that take place in the process that results in the overall equation in the electrolytic process.(ii) Using the electrode potential values, explain why aluminium metal cannot be produced from the electrolysis of aluminium salt solutions using graphite electrodes.(b) Explain what is anodisation. An aluminium object with a surface area of 100 cm2 is to be anodised. Calculate the quantity of coulombs of electricity to increase its oxide layer by 1.00 × 10–4 cm in thickness. [Density of Al2O3 is 4.00 g cm–3]