15. Consider the following redox reaction. Please note a table of standard reduction potentials is available at the end of this exam booklet. a) (2 marks) Balance the reaction in

acidic solution, showing which half-reaction is taking place at the cathode and the anode in the overall reaction as written. b) (2 marks) Show using a calculation whether the reaction as written will be spontaneous or non-spontaneous at standard conditions and at 298 K. c) (1 mark) What is the value of n in the Nernst equation for this redox reaction? d) (2 marks) What is the concentration of Pb2+ (in M) below which the redox reaction (as written) will become spontaneous, provided that all other aqueous species are maintained in their standard states? e) (1 mark) Balance this redox reaction in a basic solution. I O_{3}^{-}(a q)+H^{+}(a q)+P b O_{2(s)} \rightarrow I_{2(s)}+P b^{2+}(a q)+H_{2} O_{(t)}