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Two half cells in a galvanic cell consist of one iron electroide in a solution of iron sulphate and a silver electrode in a silver nitrate solution

a) Assume that the cell is operating as a galvanic cell. State the oxidation half reaction, the reduction half reaction and the overall cell reaction. Describe what willhappen to the mass of the cathode and the mass of the anode while the cell is operating.

b) repeat part a assuming that the cell is anelectrolytic cell

  • chemisry -

    Fe^+2 + 2e ==> Fe Eo = ??
    Ag^+1 + e ==> Ag Eo = ??

    Look up Eo values for each, reverse the one with the larger negative value and add the two half cells. You should obtain a + voltage.
    a) oxidation occurs at the anode and reduction at the cathode; multiply the Ag reaction by 2 and add the two half cells (one oxidation and one reduction) to obtain the cell reaction.
    b)If you get through a you should be able to do b on your own.

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