Consider the following electrochemical cell: Cu(s) | Cu(NO3)2(aq) || Fe(NO3)2(aq), Fe(NO3)3(aq) | Pt(s)
a. Write reduction half-reactions for each electrode, leaving out spectator ions. Calculate the cell potential if all reactants are in their standard states. Given the sign of this potential, tell from which electrode electrons will flow from the cell into an external circuit if the actual electrode potentials are close to their E° values. (In other words, which electrode must be the anode and which the cathode for the reaction to be spontaneous?) Write the net reaction for this galvanic cell.
b. Calculate the actual potential of the above cell (at 25 °C) if [Cu(NO3)2] = 0.0010 M, [Fe(NO3)2] = 0.010 M, and [Fe(NO3)3] = 1.0 × 10-5 M.
c. If this cell delivers a constant current of 180 mA for 45 min, what mass of Cu(s) will be produced or consumed (and which is it)? Assuming the cell potential stays at the value you calculated in part b throughout this period, what power is generated and how much energy is dissipated?