A student measured the potential of a galvanic cell made with 1.00 M CuSO4 in one cell and 1.00 M AgNO3 in the other. There is a Cu electrode in the CuSO4 and an Ag electrode in the AgNO3. The potential (E) measured for the cell is 0.458 V and the Cu electrode is negative.

a.) At which electrode is oxidation occurring?

b.) Write the equation for the oxidation half-reaction.

c.) Write the equation for the reduction half-reaction.

d.) If the potential of the silverIsilver ion electrode (E AgIAg+) is taken to be 0.000 V, what is the value of the potential for the oxidation reaction?

e.) If E AgIAg+ equals 0.800 V (as in standard tables of reduction potentials), what is the value of E CuICus+ ?

f.) Write the net ionic equation for the spontaneous reaction that occurs in the cell.

g.) If 6.0 M NH3 is added to the solution of CuSO4 until all of the Cu2+ ion is essentially converted to Cu(NH3)4^2+ ion, the voltage of the cell (E) goes up to 0.883 V and the Cu electrode is still negative. Find the residual concentration of Cu2+ ion in the cell.