(C) The deposition of metals during electrolysis occurs in the order of their reduction potentials,starting from the highest reduction potential to th

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(C) The deposition of metals during electrolysis occurs in the order of their reduction potentials,starting from the highest reduction potential to the lowest reduction potential.Given standard reduction potentials: $E_A^\circ = -1.2 \ V$,$E_B^\circ = 0.6 \ V$,$E_C^\circ = 0.85 \ V$,and $E_D^\circ = -0.76 \ V$.Arranging these in decreasing order: $0.85 \ V (C) > 0.6 \ V (B) > -0.76 \ V (D) > -1.2 \ V (A)$.Thus,the sequence of deposition is $C, B, D, A$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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The standard electrode potentials $\left( E_{M^{+}/M}^\circ \right)$ of four metals $A, B, C$ and $D$ are $-1.2 \ V, 0.6 \ V, 0.85 \ V$ and $-0.76 \ V$,respectively. The sequence of deposition of metals on applying potential is

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A
$A, C, B, D$
B
$B, D, C, A$
C
$C, B, D, A$
D
$D, A, B, C$

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Electrode potential and ECell

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Given $E^{0}_{Fe^{3+}|Fe} = -0.036 \, V$ and $E^{0}_{Fe^{2+}|Fe} = -0.439 \, V$,the standard electrode potential for the reaction $Fe^{3+}_{(aq)} + e^{-} \rightarrow Fe^{2+}_{(aq)}$ is ........... $V$.

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Consider the following ${E^0}$ values:
${E^0}_{Fe^{3+}/Fe^{2+}} = + 0.77 \ V$
${E^0}_{Sn^{2+}/Sn} = - 0.14 \ V$
Under standard conditions,the potential for the reaction $Sn_{(s)} + 2Fe^{3+}_{(aq)} \to 2Fe^{2+}_{(aq)} + Sn^{2+}_{(aq)}$ is ............ $V$.

MediumAIEEE 2004

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Discuss the method to determine the cell potential of any cell when a standard hydrogen electrode is considered as the anode,with a suitable example.

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Addition of powdered lead and iron to a solution which is $1.0 \, M$ in both $Pb^{2+}$ and $Fe^{2+}$ would result in [$E^{\circ}_{Fe^{2+}/Fe} = -0.44 \, V$ and $E^{\circ}_{Pb^{2+}/Pb} = -0.13 \, V$]

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The standard reduction potentials of $Cu^{2+}$,$Zn^{2+}$,$Sn^{2+}$ and $Ag^{+}$ are $0.34 \ V$,$-0.76 \ V$,$-0.14 \ V$ and $0.80 \ V$ respectively. Which of the following solutions can be stored in the given vessel without any reaction occurring (under standard conditions)?

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The standard electrode potentials $\left( E_{M^{+}/M}^\circ \right)$ of four metals $A, B, C$ and $D$ are $-1.2 \ V, 0.6 \ V, 0.85 \ V$ and $-0.76 \ V$,respectively. The sequence of deposition of metals on applying potential is

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Given $E^{0}_{Fe^{3+}|Fe} = -0.036 \, V$ and $E^{0}_{Fe^{2+}|Fe} = -0.439 \, V$,the standard electrode potential for the reaction $Fe^{3+}_{(aq)} + e^{-} \rightarrow Fe^{2+}_{(aq)}$ is ........... $V$.

Consider the following ${E^0}$ values:${E^0}_{Fe^{3+}/Fe^{2+}} = + 0.77 \ V$${E^0}_{Sn^{2+}/Sn} = - 0.14 \ V$Under standard conditions,the potential for the reaction $Sn_{(s)} + 2Fe^{3+}_{(aq)} \to 2Fe^{2+}_{(aq)} + Sn^{2+}_{(aq)}$ is ............ $V$.

Discuss the method to determine the cell potential of any cell when a standard hydrogen electrode is considered as the anode,with a suitable example.

Addition of powdered lead and iron to a solution which is $1.0 \, M$ in both $Pb^{2+}$ and $Fe^{2+}$ would result in [$E^{\circ}_{Fe^{2+}/Fe} = -0.44 \, V$ and $E^{\circ}_{Pb^{2+}/Pb} = -0.13 \, V$]

The standard reduction potentials of $Cu^{2+}$,$Zn^{2+}$,$Sn^{2+}$ and $Ag^{+}$ are $0.34 \ V$,$-0.76 \ V$,$-0.14 \ V$ and $0.80 \ V$ respectively. Which of the following solutions can be stored in the given vessel without any reaction occurring (under standard conditions)?

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Consider the following ${E^0}$ values:
${E^0}_{Fe^{3+}/Fe^{2+}} = + 0.77 \ V$
${E^0}_{Sn^{2+}/Sn} = - 0.14 \ V$
Under standard conditions,the potential for the reaction $Sn_{(s)} + 2Fe^{3+}_{(aq)} \to 2Fe^{2+}_{(aq)} + Sn^{2+}_{(aq)}$ is ............ $V$.