Question

PLEASEHELP i am having a major difficulty finding the answer to this question

Give the balanced equation with states for both the cathode and the anode reactions of the electrochemical cell shown. Be sure to include electrons in your equations.

Pt(s) l F-(aq) l F2(g) ll Cl-(aq), AuCl4-(aq) l Au(s)

Answer 1

2F^-(aq) ==> F2(g) + 2e
AuCl4^-(aq) + 3e ==> Au(s) + 4Cl^-(aq)

The half reactions I have written are the reaction at the electrodes for the cell as drawn; however, I must point out that this cell, as drawn, will not occur spontaneously. To occur spontaneously, you place the Au/AuCl4^- on the left side and the F^-/F2 on the right and reverse both half equations I've written to obtain a cell potential of +2.87-0.82 = +??volt.

Answer 2

thank you :]