(C) The strength of an oxidizing agent is directly proportional to its standard reduction potential $(E^o)$.Comparing the given values:$E^o(Cu^{+}/Cu)

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(C) The strength of an oxidizing agent is directly proportional to its standard reduction potential $(E^o)$.Comparing the given values:$E^o(Cu^{+}/Cu) = +0.52 \ V$$E^o(Fe^{3+}/Fe^{2+}) = +0.77 \ V$$E^o(\frac{1}{2} I_2/I^{-}) = +0.54 \ V$$E^o(Ag^{+}/Ag) = +0.88 \ V$Since $Ag^{+}$ has the highest reduction potential $(+0.88 \ V)$,it is the strongest oxidizing agent.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Difficult

Electrode potentials $(E^o)$ are given below:
$Cu^{+}/Cu = +0.52 \ V$
$Fe^{3+}/Fe^{2+} = +0.77 \ V$
$\frac{1}{2} I_{2(s)}/I^{-} = +0.54 \ V$
$Ag^{+}/Ag = +0.88 \ V$
Based on the above potentials,the strongest oxidizing agent will be:

JEE MAIN 2013 All JEE MAIN

A
$Cu^{+}$
B
$Fe^{3+}$
C
$Ag^{+}$
D
$I_2$

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$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-; E^o = -0.35 \ V$
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The standard reduction potential for $Li^{+}/Li$,$Zn^{2+}/Zn$,$H^{+}/H_2$ and $Ag^{+}/Ag$ is $-3.05$,$-0.762$,$0.00$ and $+0.80 \ V$. Which of the following has the highest reducing capacity?

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The standard cell potential of a cell consisting of copper and $Mg$ standard half-cells is $2.7 \ V$. If the standard reduction potential of the copper electrode is $+0.34 \ V$,what is the standard reduction potential of the magnesium electrode in volts?

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Calculate the standard potential of a cell having the following electrode reactions:
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$Zn_{(aq)}^{2+} + 2e^{-} \rightarrow Zn_{(s)}$ $E^{\circ} = -0.763 \ V$ (in $V$)

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Electrode potentials $(E^o)$ are given below:$Cu^{+}/Cu = +0.52 \ V$$Fe^{3+}/Fe^{2+} = +0.77 \ V$$\frac{1}{2} I_{2(s)}/I^{-} = +0.54 \ V$$Ag^{+}/Ag = +0.88 \ V$Based on the above potentials,the strongest oxidizing agent will be:

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On the basis of the following $E^o$ values,the strongest oxidizing agent is:$[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$

What is cell potential and $emf$? Explain with suitable examples.

The standard reduction potential for $Li^{+}/Li$,$Zn^{2+}/Zn$,$H^{+}/H_2$ and $Ag^{+}/Ag$ is $-3.05$,$-0.762$,$0.00$ and $+0.80 \ V$. Which of the following has the highest reducing capacity?

The standard cell potential of a cell consisting of copper and $Mg$ standard half-cells is $2.7 \ V$. If the standard reduction potential of the copper electrode is $+0.34 \ V$,what is the standard reduction potential of the magnesium electrode in volts?

Calculate the standard potential of a cell having the following electrode reactions:$Cd_{(aq)}^{2+} + 2e^{-} \rightarrow Cd_{(s)}$ $E^{\circ} = -0.403 \ V$$Zn_{(aq)}^{2+} + 2e^{-} \rightarrow Zn_{(s)}$ $E^{\circ} = -0.763 \ V$ (in $V$)

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Electrode potentials $(E^o)$ are given below:
$Cu^{+}/Cu = +0.52 \ V$
$Fe^{3+}/Fe^{2+} = +0.77 \ V$
$\frac{1}{2} I_{2(s)}/I^{-} = +0.54 \ V$
$Ag^{+}/Ag = +0.88 \ V$
Based on the above potentials,the strongest oxidizing agent will be:

On the basis of the following $E^o$ values,the strongest oxidizing agent is:
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-; E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-; E^o = -0.77 \ V$

Calculate the standard potential of a cell having the following electrode reactions:
$Cd_{(aq)}^{2+} + 2e^{-} \rightarrow Cd_{(s)}$ $E^{\circ} = -0.403 \ V$
$Zn_{(aq)}^{2+} + 2e^{-} \rightarrow Zn_{(s)}$ $E^{\circ} = -0.763 \ V$ (in $V$)