Considering a galvanic cell consisting of the following two redoxcouples: Ag + +

Question

Considering a galvanic cell consisting of the following two redoxcouples:
Ag+ +e->>>>>>Ag         E0 = + 0.80 V
Bi3+ + 3e>>>>>Bi          E0 = + 0.20 V

a) Write the reduction half reaction?
b) Write the oxidation half reaction?
c) Write the equation for the cell reaction?
d)Write the standard cell potential, E0cell,for the cell?

Explanation / Answer

Ag+ +e->>>>>>Ag         E0 = + 0.80 V Bi3+ + 3e>>>>>Bi          E0 = + 0.20 V Hmm. This seems to be giving both reactions in Reduction form. Itwould be helpful to know the starting Elements. both of the above are Reduction. Now, if it was Ag ---> Ag+ +e-, then that would be oxidation, same if it was Bi ---> Bi{3+}+ 3e-. But, they are currently both written as reductions, so Idon't know which is being reduced or which is being oxidized bylooking at just that. Or maybe I'm just wrong? Example of the difference I'm trying to relay: Assume Ag+ is being reduced and Bi is being oxidized. You'reequation would be. Ag{+} + Bi ---> Ag + Bi{3+} But if Ag is being oxidized and Bi{3+} reduced, then it is: Ag + Bi{3+} ---> Ag{+} + Bi Get what I'm trying to say?

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