6. A voltaic cell based on the reaction between aqueous Br2 and vanadium(III) ions has E^∘cell =

First, we need to identify the half-reactions. The overall reaction is a redox reaction, which m

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6. A voltaic cell based on the reaction between aqueous \( \mathrm{Br}_{2} \) and vanadium(III) ions has \( E^{\circ}{ }_{\text {cell }}=1.39 \mathrm{~V} \) : \[ \mathrm{Br}_{2}(\mathrm{aq})+2 \mathrm{~V}^{3+}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 2 \mathrm{VO}^{2+}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{Br}^{-}(\mathrm{aq}) \] What is \( E^{\text {vanadium, }} \), the standard electrode potential for the reduction of \( \mathrm{VO}^{2+} \) to \( \mathrm{V}^{3+} \) ?

          6. A voltaic cell based on the reaction between aqueous \( \mathrm{Br}_{2} \) and vanadium(III) ions has \( E^{\circ}{ }_{\text {cell }}=1.39 \mathrm{~V} \) :
\[
\mathrm{Br}_{2}(\mathrm{aq})+2 \mathrm{~V}^{3+}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 2 \mathrm{VO}^{2+}(\mathrm{aq})+4 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{Br}^{-}(\mathrm{aq})
\]

What is \( E^{\text {vanadium, }} \), the standard electrode potential for the reduction of \( \mathrm{VO}^{2+} \) to \( \mathrm{V}^{3+} \) ?

6. A voltaic cell based on the reaction between aqueous Br2 and vanadium(III) ions has E^∘cell =1.39 V :

Br2(aq)+2 V^3+(aq)+2 H2O(l) → 2 VO^2+(aq)+4 H^+(aq)+2 Br^-(aq)

What is E^vanadium,, the standard electrode potential for the reduction of VO^2+ to V^3+ ?

Added by Joseph S.

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