(A) The reduction potential order is $E^\circ_{Z/Z^-} > E^\circ_{Y/Y^-} > E^\circ_{X/X^-}$.Species with higher reduction potential act as stronger oxi

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$Y^-$ oxidizes $X$ but does not oxidize $Z^-$

(A) The reduction potential order is $E^\circ_{Z/Z^-} > E^\circ_{Y/Y^-} > E^\circ_{X/X^-}$.Species with higher reduction potential act as stronger oxidizing agents.Therefore,$Z$ is the strongest oxidizing agent and $X$ is the weakest.$Y^-$ can oxidize species with a lower reduction potential than itself.Since $E^\circ_{Y/Y^-} > E^\circ_{X/X^-}$,$Y^-$ can oxidize $X$ to $X^+$.Since $E^\circ_{Y/Y^-} Thus,$Y^-$ oxidizes $X$ but does not oxidize $Z^-$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Easy

At $25^\circ C$,$1 \, atm$ of gas $X$ is bubbled through a solution containing $1 \, M$ $Y^-$ and $1 \, M$ $Z^-$. If the reduction potential order is $Z > Y > X$,then:

A
$Y^-$ oxidizes $X$ but does not oxidize $Z^-$
B
$Y^-$ oxidizes $Z^-$ but does not oxidize $X$
C
$Y^-$ oxidizes both $X$ and $Z^-$
D
$Y^-$ reduces both $X$ and $Z^-$

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Electrochemistry

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Electrode potential and ECell

Given the electrode potentials:
$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.771 \ V$
$I_2 + 2e^- \to 2I^{-}; E^o = 0.536 \ V$
The $E^o_{\text{cell}}$ for the cell reaction $2Fe^{3+} + 2I^{-} \to 2Fe^{2+} + I_2$ is:

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For the decomposition of $Al_2O_3$ at $500^{\circ}C$,the free energy change is $\frac{2}{3} Al_2O_3 \to \frac{4}{3} Al + O_2$,$\Delta G = +966 \ kJ \ mol^{-1}$. The potential difference required for the electrolytic reduction of $Al_2O_3$ at $500^{\circ}C$ is ........... $V$.

Medium

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When does a cell reaction occur spontaneously?

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For the given cell reaction $Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} \rightarrow Fe^{3+}_{(aq)} + Ag_{(s)}$,the standard cell potential is:
Given:
$Ag^{+} + e^{-} \rightarrow Ag \quad E^0 = x \ V$
$Fe^{2+} + 2e^{-} \rightarrow Fe \quad E^0 = y \ V$
$Fe^{3+} + 3e^{-} \rightarrow Fe \quad E^0 = z \ V$

DifficultJEE MAIN 2025

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Given,for $Sn^{4+} / Sn^{2+}$,standard reduction potential is $0.15 \ V$ and for $Au^{3+} / Au$,standard reduction potential is $1.5 \ V$. For the reaction,$3 Sn^{2+} + 2 Au^{3+} \longrightarrow 3 Sn^{4+} + 2 Au$,the value of $E_{\text{cell}}^{\circ}$ is:

MediumMHT CET 2010

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At $25^\circ C$,$1 \, atm$ of gas $X$ is bubbled through a solution containing $1 \, M$ $Y^-$ and $1 \, M$ $Z^-$. If the reduction potential order is $Z > Y > X$,then:

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Given the electrode potentials:$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.771 \ V$$I_2 + 2e^- \to 2I^{-}; E^o = 0.536 \ V$The $E^o_{\text{cell}}$ for the cell reaction $2Fe^{3+} + 2I^{-} \to 2Fe^{2+} + I_2$ is:

For the decomposition of $Al_2O_3$ at $500^{\circ}C$,the free energy change is $\frac{2}{3} Al_2O_3 \to \frac{4}{3} Al + O_2$,$\Delta G = +966 \ kJ \ mol^{-1}$. The potential difference required for the electrolytic reduction of $Al_2O_3$ at $500^{\circ}C$ is ........... $V$.

When does a cell reaction occur spontaneously?

For the given cell reaction $Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} \rightarrow Fe^{3+}_{(aq)} + Ag_{(s)}$,the standard cell potential is:Given:$Ag^{+} + e^{-} \rightarrow Ag \quad E^0 = x \ V$$Fe^{2+} + 2e^{-} \rightarrow Fe \quad E^0 = y \ V$$Fe^{3+} + 3e^{-} \rightarrow Fe \quad E^0 = z \ V$

Given,for $Sn^{4+} / Sn^{2+}$,standard reduction potential is $0.15 \ V$ and for $Au^{3+} / Au$,standard reduction potential is $1.5 \ V$. For the reaction,$3 Sn^{2+} + 2 Au^{3+} \longrightarrow 3 Sn^{4+} + 2 Au$,the value of $E_{\text{cell}}^{\circ}$ is:

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Given the electrode potentials:
$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.771 \ V$
$I_2 + 2e^- \to 2I^{-}; E^o = 0.536 \ V$
The $E^o_{\text{cell}}$ for the cell reaction $2Fe^{3+} + 2I^{-} \to 2Fe^{2+} + I_2$ is:

For the given cell reaction $Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} \rightarrow Fe^{3+}_{(aq)} + Ag_{(s)}$,the standard cell potential is:
Given:
$Ag^{+} + e^{-} \rightarrow Ag \quad E^0 = x \ V$
$Fe^{2+} + 2e^{-} \rightarrow Fe \quad E^0 = y \ V$
$Fe^{3+} + 3e^{-} \rightarrow Fe \quad E^0 = z \ V$