For the reduction of NO⊖3 ion in an aqueous solution, E⊖ is +0.96 V, the values of E⊖ for some metal ions are given below: (i)V2+(aq)+2e−→V; E⊖=−1.19V(ii)Fe3+(aq)+3e−→Fe; E⊖=−0.04V(iii)Au3+(aq)+3e−→Au; E⊖=+1.40V(iv)Hg2+(aq)+2e−→Hg; E⊖=+0.86VThe pair(s) of metals that is/are oxidized by NO⊖3 in aqueous solution is/are (IIT-JEE, 2010)

For the reduction of NO⊖3 ion in an aqueous solution, E⊖ is +0.96

1.	For the reduction of NO⊖3 ion in an aqueous solution, E⊖ is +0.96 V, the values of E⊖ for some metal ions are given below: (i)V2+(aq)+2e−→V; E⊖=−1.19V(ii)Fe3+(aq)+3e−→Fe; E⊖=−0.04V(iii)Au3+(aq)+3e−→Au; E⊖=+1.40V(iv)Hg2+(aq)+2e−→Hg; E⊖=+0.86VThe pair(s) of metals that is/are oxidized by NO⊖3 in aqueous solution is/are (IIT-JEE, 2010)
Answer» For the reduction of $N O_{3}^{⊖}$ ion in an aqueous solution, $E^{⊖}$ is +0.96 V, the values of $E^{⊖}$ for some metal ions are given below: $(i) V^{2 +} (a q) + 2 e^{-} \to V; E^{⊖} = - 1.19 V$ $(i i) F e^{3 +} (a q) + 3 e^{-} \to F e; E^{⊖} = - 0.04 V$ $(i i i) A u^{3 +} (a q) + 3 e^{-} \to A u; E^{⊖} = + 1.40 V$ $(i v) H g^{2 +} (a q) + 2 e^{-} \to H g; E^{⊖} = + 0.86 V$ The pair(s) of metals that is/are oxidized by $N O_{3}^{⊖}$ in aqueous solution is/are (IIT-JEE, 2010)