The standard reduction potentials at 295K for the following half cells are given below: NO _ 3 ^ - + 4 H ^ + + 3 e ^ - → NO(g) + 2 H _ 2 O E ^ o = 0 . 97V V ^ 2 + (aq) + 2 e ^ - → V(s) E ^ o = - 1 . 19V Fe ^ 3 + (aq) +

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For feasibility, check , E ^ o cell = E _ cathode ( reduction ) ^ o - E _ anode ( oxidation ) ^ o > 0 The E ^ o values when metal acts as anode and NO _ 3 ^ - reaction is cathodic reaction. For Vanadium metal, E _ cell ^ o = 0 . 97 + 1 . 19 = 2 . 16V For Iron metal, E _ cell ^ o = 0 . 97 + 0 . 04 = 1 . 01V For silver metal, E _ cell ^ o = 0 . 97 - 0 . 80 = 0 . 17V For Gold metal, E _ cell ^ o = 0 . 97 - 1 . 140 = - 0 . 17V For electrodes having oxidation potential greater than - 0 . 97V , E ^ o cell > 0 ∴ Ag, Fe and V can be oxidised

${{NO}_{3}}^{-} + 4{H}^{+} + 3{e}^{-} \to NO\left(g\right) + 2{H}_{2}O$	${E}^{o} = 0 . 97V$
${V}^{2 +}\left(aq\right) + 2{e}^{-} \to V\left(s\right)$	${E}^{o} = - 1 . 19V$
${Fe}^{3 +}\left(aq\right) + 3{e}^{-} \to Fe\left(s\right)$	${E}^{o} = - 0 . 04V$
${Ag}^{+}\left(aq\right) + {e}^{-} \to Ag\left(s\right)$	${E}^{o} = 0 . 80V$
${Au}^{3 +}\left(aq\right) + 3{e}^{-} \to Au\left(s\right)$	${E}^{o} = 1 . 40V$

The standard reduction potentials at 295K for the following half...

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