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20. Electrochemistry
Standard Reduction Potentials
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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)Pb(s) + Br2(l) → Pb2+(aq) + 2 Br-(aq)Given the standard reduction potentials:Pb2+(aq) + 2 e- → Pb(s) E° = -0.13 VBr2(l) + 2 e- → 2 Br-(aq) E° = +1.07 VWhat is the standard cell potential (E°cell) for the reaction?
A
1.20 V
B
0.80 V
C
0.94 V
D
1.00 V
Verified step by step guidance1
Identify the half-reactions involved in the overall reaction. The given half-reactions are: Pb2+(aq) + 2 e- → Pb(s) with E° = -0.13 V and Br2(l) + 2 e- → 2 Br-(aq) with E° = +1.07 V.
Determine which half-reaction is the oxidation and which is the reduction. In the overall reaction, Pb(s) is oxidized to Pb2+(aq), and Br2(l) is reduced to 2 Br-(aq).
Write the oxidation half-reaction: Pb(s) → Pb2+(aq) + 2 e-. The standard potential for this oxidation reaction is the negative of the reduction potential: E° = +0.13 V.
Write the reduction half-reaction: Br2(l) + 2 e- → 2 Br-(aq). The standard potential for this reduction reaction is given as E° = +1.07 V.
Calculate the standard cell potential (E°cell) by adding the standard potentials of the oxidation and reduction half-reactions: E°cell = E°(oxidation) + E°(reduction) = +0.13 V + 1.07 V.
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