(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)
(a)(i) Oxidation in terms of electron transfer
Oxidation is the process in which an atom, ion or molecule loses electron(s).
Example:
\[Fe^{2+} \rightarrow Fe^{3+} + e^-\]
(a)(ii) Balanced half-reactions in acidic solution
