(C) The standard reduction potential of $Mg^{2+}/Mg$ is $-2.37\,V$ and that of $Zn^{2+}/Zn$ is $-0.762\,V$.$A$ metal with a more negative reduction po

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(C) The standard reduction potential of $Mg^{2+}/Mg$ is $-2.37\,V$ and that of $Zn^{2+}/Zn$ is $-0.762\,V$.$A$ metal with a more negative reduction potential is a stronger reducing agent and can displace a metal with a less negative (or more positive) reduction potential from its salt solution.Since $E^o_{Mg^{2+}/Mg} Therefore,$Zn$ cannot reduce $Mg^{2+}$ to $Mg$. Consequently,no reaction occurs when zinc dust is added to a solution of $MgCl_2$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Difficult

The standard electrode potentials at $25\,^oC$ for the following half-reactions are given:
$Zn^{2+} + 2e^- \to Zn, E^o = -0.762\,V$
$Mg^{2+} + 2e^- \to Mg, E^o = -2.37\,V$
When zinc dust is added to a solution of $MgCl_2$,what happens?

A
$ZnCl_2$ is formed
B
Zinc dissolves in the solution
C
No reaction takes place
D
$Mg$ is precipitated

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Electrochemistry

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Electrode potential and ECell

From the given values,which one is a strong oxidizing agent?
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

Easy

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Given the standard electrode potentials: $Fe^{2+}_{(aq)} + 2e^{-} \rightarrow Fe_{(s)}$ $(E^o = -0.44 \ V)$ and $Fe^{3+}_{(aq)} + e^{-} \rightarrow Fe^{2+}_{(aq)}$ $(E^o = 0.77 \ V)$. If $Fe^{2+}$,$Fe^{3+}$,and a piece of $Fe$ are kept together,what happens?

Difficult

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Which among the following reactions will take place spontaneously?

Difficult

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Which statement is correct for $\Delta G$ and $E_{cell}$ for a cell reaction?

MediumGUJCET 2025

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Consult the table of standard electrode potentials and suggest three substances that can oxidise ferrous ions under suitable conditions.

Medium

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The standard electrode potentials at $25\,^oC$ for the following half-reactions are given:$Zn^{2+} + 2e^- \to Zn, E^o = -0.762\,V$$Mg^{2+} + 2e^- \to Mg, E^o = -2.37\,V$When zinc dust is added to a solution of $MgCl_2$,what happens?

Similar Questions

From the given values,which one is a strong oxidizing agent?$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

Given the standard electrode potentials: $Fe^{2+}_{(aq)} + 2e^{-} \rightarrow Fe_{(s)}$ $(E^o = -0.44 \ V)$ and $Fe^{3+}_{(aq)} + e^{-} \rightarrow Fe^{2+}_{(aq)}$ $(E^o = 0.77 \ V)$. If $Fe^{2+}$,$Fe^{3+}$,and a piece of $Fe$ are kept together,what happens?

Which among the following reactions will take place spontaneously?

Which statement is correct for $\Delta G$ and $E_{cell}$ for a cell reaction?

Consult the table of standard electrode potentials and suggest three substances that can oxidise ferrous ions under suitable conditions.

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The standard electrode potentials at $25\,^oC$ for the following half-reactions are given:
$Zn^{2+} + 2e^- \to Zn, E^o = -0.762\,V$
$Mg^{2+} + 2e^- \to Mg, E^o = -2.37\,V$
When zinc dust is added to a solution of $MgCl_2$,what happens?

From the given values,which one is a strong oxidizing agent?
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$