(C) The strength of a reducing agent is inversely proportional to its standard reduction potential $(E^0_{red})$. $A$ lower (more negative) $E^0_{red}

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(C) The strength of a reducing agent is inversely proportional to its standard reduction potential $(E^0_{red})$. $A$ lower (more negative) $E^0_{red}$ value indicates a stronger reducing agent. Comparing the given values: $E^0_{MnO_4^-/Mn^{2+}} = 1.51 \text{ V}$ $E^0_{Cl_2/Cl^{-}} = 1.36 \text{ V}$ $E^0_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \text{ V}$ $E^0_{Cr^{3+}/Cr} = -0.74 \text{ V}$ Since $E^0_{Cr^{3+}/Cr}$ has the lowest (most negative) value of $-0.74 \text{ V}$,the species $Cr$ acts as the strongest reducing agent.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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Using the data given below,find out the strongest reducing agent:
$E^0_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \text{ V}$,$E^0_{Cl_2/Cl^{-}} = 1.36 \text{ V}$,$E^0_{MnO_4^-/Mn^{2+}} = 1.51 \text{ V}$,$E^0_{Cr^{3+}/Cr} = -0.74 \text{ V}$

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A
$Cl^{-}$
B
$Cr^{3+}$
C
$Cr$
D
$Mn^{2+}$

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The $(\frac{\partial E}{\partial T})_P$ of different types of half cells are as follows:
$A$ $B$ $C$ $D$
$1 \times 10^{-4}$ $2 \times 10^{-4}$ $0.1 \times 10^{-4}$ $0.2 \times 10^{-4}$

(Where $E$ is the electromotive force)
Which of the above half cells would be preferred to be used as reference electrode?

$A$	$B$	$C$	$D$
$1 \times 10^{-4}$	$2 \times 10^{-4}$	$0.1 \times 10^{-4}$	$0.2 \times 10^{-4}$

DifficultJEE MAIN 2022

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If $Cu^{2+} + 2e^{-} \rightarrow Cu, E^{0} = 0.337 \ V$ and $Cu^{2+} + e^{-} \rightarrow Cu^{+}, E^{0} = 0.153 \ V$,then for the reaction $Cu^{+} + e^{-} \rightarrow Cu$,$E^{0}_{cell} =$ .............. $V$.

Medium

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What is the value of the standard electrode potential of a standard hydrogen electrode $(SHE)$ (in $V$)?

Easy

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Standard reduction potentials at $25^\circ C$ of $Li^{+}|Li$,$Ba^{2+}|Ba$,$Na^{+}|Na$,and $Mg^{2+}|Mg$ are $-3.05 \ V$,$-2.90 \ V$,$-2.71 \ V$,and $-2.37 \ V$ respectively. Which one of the following is the strongest oxidising agent?

MediumAIPMT 1994

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Given that $E^o_{K^{+}/K} = -2.93 \ V$,$E^o_{Fe^{2+}/Fe} = -0.44 \ V$,$E^o_{Zn^{2+}/Zn} = -0.76 \ V$,and $E^o_{Cu^{2+}/Cu} = 0.34 \ V$. Based on this data,which of the following is the strongest reducing agent?

DifficultAIIMS 2011

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Using the data given below,find out the strongest reducing agent: $E^0_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \text{ V}$,$E^0_{Cl_2/Cl^{-}} = 1.36 \text{ V}$,$E^0_{MnO_4^-/Mn^{2+}} = 1.51 \text{ V}$,$E^0_{Cr^{3+}/Cr} = -0.74 \text{ V}$

Similar Questions

The $(\frac{\partial E}{\partial T})_P$ of different types of half cells are as follows:$A$$B$$C$$D$$1 \times 10^{-4}$$2 \times 10^{-4}$$0.1 \times 10^{-4}$$0.2 \times 10^{-4}$(Where $E$ is the electromotive force)Which of the above half cells would be preferred to be used as reference electrode?

If $Cu^{2+} + 2e^{-} \rightarrow Cu, E^{0} = 0.337 \ V$ and $Cu^{2+} + e^{-} \rightarrow Cu^{+}, E^{0} = 0.153 \ V$,then for the reaction $Cu^{+} + e^{-} \rightarrow Cu$,$E^{0}_{cell} =$ .............. $V$.

What is the value of the standard electrode potential of a standard hydrogen electrode $(SHE)$ (in $V$)?

Standard reduction potentials at $25^\circ C$ of $Li^{+}|Li$,$Ba^{2+}|Ba$,$Na^{+}|Na$,and $Mg^{2+}|Mg$ are $-3.05 \ V$,$-2.90 \ V$,$-2.71 \ V$,and $-2.37 \ V$ respectively. Which one of the following is the strongest oxidising agent?

Given that $E^o_{K^{+}/K} = -2.93 \ V$,$E^o_{Fe^{2+}/Fe} = -0.44 \ V$,$E^o_{Zn^{2+}/Zn} = -0.76 \ V$,and $E^o_{Cu^{2+}/Cu} = 0.34 \ V$. Based on this data,which of the following is the strongest reducing agent?

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Using the data given below,find out the strongest reducing agent:
$E^0_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \text{ V}$,$E^0_{Cl_2/Cl^{-}} = 1.36 \text{ V}$,$E^0_{MnO_4^-/Mn^{2+}} = 1.51 \text{ V}$,$E^0_{Cr^{3+}/Cr} = -0.74 \text{ V}$