A galvanic cell was formed using Alphavium and Betanium:

Reduction Potentials:

Av³⁺(aq) + 3e^- Av(s) E^o = -0.43 V

Bn⁴⁺(aq) + 4e^- Bn(s) E^o = +0.11 V

a.1, Which metal is more susceptible to corrosion by oxygen? Explain. a.2, Write a net ionic equation for this reaction.

b, Write the cell notation for this cell.

c, Which metal is the oxidizing agent? Explain how you know.

d, Which metal acts as the cathode?

e, Which substance(s) would be considered an electrolyte?

f, If the salt in the salt bridge is NH4NO3, describe the direction of ion movement in the salt bridge.

g, Does this cell contain an inert electrode? Explain.

h, Calculate the E^o_cell. Show all work.

i, Is this cells reaction spontaneous or non-spontaneous? Explain.

j, Which element is the stronger reducing agent: Av or Bn? Explain how you know.

k, The reduction potentials shown above were measured relative to the standard hydrogen electrode. What would Betaniums reduction potential be if it were measured relative to copper/copper(II) standard electrode? l, Suggest three (3) ways to prevent corrosion of a sample of Alphavium. Explain why each strategy would work.