(a)(i) Define oxidation in terms of electron transfer. (ii) Write balanced equations for the half reactions for the following changes in acidic solution: Mn...

(a)(i) Define oxidation in terms of electron transfer.

(ii) Write balanced equations for the half reactions for the following changes in acidic solution: Mn0\(^-_4\) + Fe\(^{2+}\) —> Mn\(^{2+}\) + Fe\(^{3+}\)

(b)(i) Distinguish between an electrolytic celI and an electrochemical cell.

(ii) Sketch a cell for the electrolysis of molten magnesium chloride. Lable the anode and the cathode and indicate the direction of electron flow. Give the electrode reactions.

(iii) Give one reason why a platinum anode is not suitable for the eloctrolysis in (b)(i) above.

(c) Calculate the mass of lead that would be deposited from a solution of lead (II) trioxonitrate by the same quantity of electrically depositing 1.35g of copper. (Cu = 63.5, Pb = 207)