In aqueous acidic solution, permanganate ion, MnO4 can be reduced to the pale-pink manganese (ID) ion, Mn?. Under standard conditions, the reduction potential of a MnO | Mn half-cell is E = 1.50 V. Assuming the half-cell is combined with X+ 1X2+ half-cell in a galvanic cell, with [H30'] = [Mn? ] = [MnO4] = [X2+] = 1 M. a. Write down the equations for the reactions at the anode and the cathode. b. What is the overall cell reaction? c. Calculate the standard cell potential difference, E. d. Suppose the XO X2 MnO, O Mn2+ cell is operated at pH 2.00 with [Mn] = 0.001M. [MnO:] = 0.12 M, and [X27 = 0.015 M. Calculate the cell voltage, E at 25°C