Two electrochemical cells are assembled in which the following reactions occur:V2+ + VO2+ + 2H+ → 2V

Question

Two electrochemical cells are assembled in which the following reactions occur:

V²⁺ + VO²⁺ + 2H⁺ → 2V³⁺ + H₂O; E°_Cell = 0.616 V

V³⁺ + Ag⁺ + H₂O → VO²⁺ + Ag(s) + 2H⁺; E°_Cell = 0.439 V

If $E_{Ag^{+}|Ag}^{o}$= 0.799 V, what is$E_{V^{3 +}|V^{2 +}}^{o}$?

Accepted Answer

$E_{V^{2 +}|V^{3 +}}^{o} = 1 	imes 0.616 + 1 	imes 0.439 - 1 	imes 0.799 = 0.256	ext{ V}$$	herefore E_{V^{3 +}|V^{2 +}}^{o} = - 0.256	ext{ V}$

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