A voltaic cell is constructed using Hg/Hg+2 for one half-cell and Cr/Cr+3 for the other half-cell. The half-cells are at standard conditions and contain equal-mass electrodes and the same volume of solutions. Reference: Cr+3(aq) + 3 e- ---> Cr(s) E0 = -0.74 V; Hg+2(aq) + 2 e- ---> Hg(l) E0 = +0.80 V

(a) Write the balanced net ionic equation for the spontaneous reaction produced in the cell.

(b) Calculate the value of E0 for the spontaneous reaction.

(c) What is the value of the standard free-energy change, delta G0, for the spontaneous reaction? Use appropriate units with your answer.

(d) If the cell operates until [Cr+3] is 1.09 M in the Cr/Cr+3 half-cell, what is [Hg+2] in the Hg/Hg+2 half-cell?

(e) In another voltaic cell with the same half-cells, [Hg+2] is 1.00 M and [Cr+3] is 0.050 M. How should Ecell for this cell compare to the value in (b)? Justify your answer