The standard reduction potentials at 298 ~K for the following half cells are given below: Cr₂ O₇²⁻+14 H⁺+6 e⁻ → 2 Cr³⁺+7 H₂ O, E^(°)=1.33 ~V ll Fe³⁺(aq)+3 e⁻ → Fe E^(°)=-0.04 ~V Ni²⁺(aq)+2 e⁻ → Ni E^(°)=-0.25 ~V Ag⁺(aq)+e⁻ → Ag E^(°)=0.80 ~V Au³⁺(aq)+3 e⁻ → Au E^(°)=1.40 ~V Consider the given electrochemical reactions, The number of metal(s) which will be oxidized be Cr₂ O₇²⁻, in aqueous solution is _ _ _ _ _.

JEE Main 2024 Redox Reactions and Electrochemistry Question with Answer (9 Apr Morning shift, Q10)

JEE Main 20249 Apr, Morning shiftChemistryHardRedox Reactions and Electrochemistry138× since 2002

The standard reduction potentials at

298 \mathrm{~K}

for the following half cells are given below :

\mathrm{Cr}_2 \mathrm{O}_7^{2-}+14 \mathrm{H}^{+}+6 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cr}^{3+}+7 \mathrm{H}_2 \mathrm{O}, \quad \mathrm{E}^{\circ}=1.33 \mathrm{~V}

\begin{array}{ll} \mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe} & \mathrm{E}^{\circ}=-0.04 \mathrm{~V} \\ \mathrm{Ni}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Ni} & \mathrm{E}^{\circ}=-0.25 \mathrm{~V} \\ \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Ag} & \mathrm{E}^{\circ}=0.80 \mathrm{~V} \\ \mathrm{Au}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Au} & \mathrm{E}^{\circ}=1.40 \mathrm{~V} \end{array}

Consider the given electrochemical reactions, The number of metal(s) which will be oxidized be

\mathrm{Cr}_2 \mathrm{O}_7^{2-}

, in aqueous solution is _________.

Your answerType your answer. Integers and decimals are accepted.