Two electrochemical cells are assembled in which the following reactions occur: V^2+ + VO^2+ + 2H^+ - 2V^3+ + H2O; E°_Cell = 0.616 V and V^3+ + Ag^+ + H2O - VO^2+ + Ag(s) + 2H^+; E°_Cell = 0.439 V.

Question

Two electrochemical cells are assembled in which the following reactions occur: V^2+ + VO^2+ + 2H^+ -> 2V^3+ + H2O; E°_Cell = 0.616 V and V^3+ + Ag^+ + H2O -> VO^2+ + Ag(s) + 2H^+; E°_Cell = 0.439 V. If E°_Ag+\|Ag = 0.799 V, what is E°_V3+\|V2+ ?

Prashant Kotian · Accepted Answer

Correct answer: A. Adding the two given cell reactions yields: V^2+ + Ag^+ -> V^3+ + Ag. The total cell potential E°_total = 0.616 + 0.439 = 1.055 V. This also equals E°_Ag+\|Ag - E°_V3+\|V2+. So, 1.055 = 0.799 - E°_V3+\|V2+, which gives E°_V3+\|V2+ = 0.799 - 1.055 = -0.256 V. Therefore, correct answer is A.

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