Using the following data, determine the standard cell potential E^o cell for the

Question

Using the following data, determine the standard cell potential E^o cell for the electrochemical cell constructed using the following reaction, where zinc is the anode and lead is the cathode.

Zn(s) + Pb2+(aq) -> Zn2+(aq) + Pb(s)

Half-reaction: Standard Reduction Potential:

Zn2+(aq) + 2e- -> Zn(s)= -0.763

Pb2+(aq) + 2e- -> Pb(s)= -0.126

a. -0.889 V

b. +0.889 V

c. +0.637 V

d. +1.274 V

e. -0.637 V

Which is the best answer? And what equation exactly do you use to solve this problem thanks for the help!

Explanation / Answer

Zn(s) + Pb2+(aq) -> Zn2+(aq) + Pb(s)

Half-reaction: Standard Reduction Potential:

Zn2+(aq) + 2e- -> Zn(s)= -0.763

Pb2+(aq) + 2e- -> Pb(s)= -0.126

Eo = -0.126 - (-0.763)

= +0.637 V

( note ; Eo > 0 , so this reaction should occur)

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