The standard reduction potentials at 298 ~K for the following half cells are given below: NO₃⁻+4 H⁺+3 e⁻ → NO(g)+2 H₂ O E^(θ)=0.97 ~V V²⁺(aq)+2 e⁻ → V E^(θ)=-1.19 ~V Fe³⁺(aq)+3 e⁻ → Fe E^(θ)=-0.04 ~V Ag⁺(aq)+e⁻ → Ag(s) E^(θ)=0.80 ~V Au³⁺(aq)+3 e⁻ → Au(s) E^(θ)=1.40 ~V The number of metal(s) which will be oxidized by NO₃⁻ in aqueous solution is _ _ _ _ _.

JEE Main 2023 Redox Reactions and Electrochemistry Question with Answer (6 Apr Evening shift, Q11)

JEE Main 20236 Apr, Evening shiftChemistryHardRedox Reactions and Electrochemistry138× since 2002

The standard reduction potentials at

298 \mathrm{~K}

for the following half cells are given below:

\mathrm{NO}_{3}^{-}+4 \mathrm{H}^{+}+3 \mathrm{e}^{-} \rightarrow \mathrm{NO}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O} \quad \mathrm{E}^{\theta}=0.97 \mathrm{~V}

\mathrm{V}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{V} \quad\quad\quad \mathrm{E}^{\theta}=-1.19 \mathrm{~V}

\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe} \quad\quad\quad \mathrm{E}^{\theta}=-0.04 \mathrm{~V}

\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(\mathrm{s}) \quad\quad\quad \mathrm{E}^{\theta}=0.80 \mathrm{~V}

\mathrm{Au}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Au}(\mathrm{s}) \quad\quad\quad \mathrm{E}^{\theta}=1.40 \mathrm{~V}

The number of metal(s) which will be oxidized by

\mathrm{NO}_{3}^{-}

in aqueous solution is __________.

Your answerType your answer. Integers and decimals are accepted.