Use the standard electrode potentials given in the following table to answer the questions below: Half-Reaction E V Lit + Li |-3,04 e- Mg2+ + 2e- Mg -2,37 Zn2+ + 2e- = Zn |-0,76 Fe3+ + 3e- 2 Fe -0,4 Pb2+ + 2e- Pb -0,13 2H* + 2e- = H2(g) 0,00 Cu2+ + 2e- 2 Cu +0,34 Ag* + Ag +0,80 e- Au3+ + 3e- = Au +1,50 (a) Which of the metals on the list can reduce Mg2*(aq) to Mg(s)? Explain your answer. (3) (b) Which of the metals on the list is most readily reduced? Explain your answer. (3) (c) Provide a balanced chemical equation using the half-reaction method for the reaction of Ag*(aq) with Zn(s). Show all the steps and determine if the reaction be spontaneous (product-favoured). (8) (d) Predict the chemical reactions that will occur at the two electrodes in the electrolysis of an aqueous sodium hydroxide solution. What is the minimum voltage needed for this reaction to take place? (8)