For the reduction of NO3− ion is an aqueous solution, E° is +0.96V. Values of E° for some metal ions are given below:V(aq.)2++2e−⟶V; E∘=−1.19VFe(aq.)3++3e−⟶Fe; E∘=−0.04VAu(aq.)3++3e−⟶Au; E∘=+1.40VHg(aq.)2++2e−⟶Hg; E∘=+0.86VThe pair(s) of metals that is (are) oxidized by NO3− in aqueous solution is (are):

V and Hg , Hg and Fe , Fe and V

For the reduction of NO3− ion is an aqueous solution, E° is +0.96V. Values of E° for some metal ions are given below:V(aq.)2++2e−⟶V; E∘=−1.19VFe(aq.)3++3e−⟶Fe; E∘=−0.04VAu(aq.)3++3e−⟶Au; E∘=+1.40VHg(aq.)2++2e−⟶Hg; E∘=+0.86VThe pair(s) of metals that is (are) oxidized by NO3− in aqueous solution is (are):

NO 3 - ion in an aqueous solution E 0 is +0.96V. It can oxidize only those metals that have standard reduction potentials E 0 less than NO 3 - . Metals: V, Fe and Hg can be oxidized by NO 3 - . Options A, B, and D are correct.

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For the reduction of ${NO}_{3}^{-}$ ion is an aqueous solution, E° is +0.96V. Values of E° for some metal ions are given below:
$\begin{array}{ll} V_{(aq .)}^{2 +} + 2 e^{-} ⟶ V; E^{\circ} = - 1 .19 V \\ {Fe}_{(aq .)}^{3 +} + 3 e^{-} ⟶ Fe; E^{\circ} = - 0 .04 V \\ {Au}_{(aq .)}^{3 +} + 3 e^{-} ⟶ Au; E^{\circ} = + 1 .40 V \\ {Hg}_{(aq .)}^{2 +} + 2 e^{-} ⟶ Hg; E^{\circ} = + 0 .86 V \end{array}$
The pair(s) of metals that is (are) oxidized by ${NO}_{3}^{-}$ in aqueous solution is (are):

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V and Hg

Hg and Fe

Fe and Au

Fe and V

answer is A, B, D.

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Detailed Solution

${NO}_{3}^{-}$ ion in an aqueous solution E₀ is +0.96V. It can oxidize only those metals that have standard reduction potentials E₀
less than ${NO}_{3}^{-}$ . Metals: V, Fe and Hg can be oxidized by ${NO}_{3}^{-}$ .

Options A, B, and D are correct.

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