(A) The standard hydrogen electrode $(SHE)$ is used as a reference electrode.By convention,the standard electrode potential of $SHE$ is assigned a val

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Oxidation potential = $0.00 \ V$,Reduction potential = $0.00 \ V$

(A) The standard hydrogen electrode $(SHE)$ is used as a reference electrode.By convention,the standard electrode potential of $SHE$ is assigned a value of $0.00 \ V$ at all temperatures.Since the oxidation and reduction processes are reverse of each other,the potential values are equal in magnitude but opposite in sign.However,for $SHE$,both the standard oxidation potential and standard reduction potential are defined as $0.00 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Easy

What is the oxidation and reduction potential of standard hydrogen electrode?

A
Oxidation potential = $0.00 \ V$,Reduction potential = $0.00 \ V$
B
Oxidation potential = $1.00 \ V$,Reduction potential = $-1.00 \ V$
C
Oxidation potential = $-1.00 \ V$,Reduction potential = $1.00 \ V$
D
Oxidation potential = $0.00 \ V$,Reduction potential = $1.00 \ V$

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Electrode potential and ECell

$FeO_4^{2-}$ $\xrightarrow{2.0 \ V} Fe^{3+}$ $\xrightarrow{0.8 \ V} Fe^{2+}$ $\xrightarrow{-0.44 \ V} Fe^0$
In the above diagram,the standard electrode potentials are given in volts. The value of $E_{FeO_4^{2-}/Fe^{2+}}^{\Theta}$ is: (in $V$)

DifficultJEE MAIN 2025

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Standard electrode potential of $Ag^{+}/Ag$ and $Cu^{2+}/Cu$ is $+0.80 \ V$ and $+0.34 \ V$ respectively. These electrodes are joined together by a salt bridge. If:

Medium

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Given
$E^o_{Cl_2/Cl^-} = 1.36 \ V,$
$E^o_{Cr^{3+}/Cr} = -0.74 \ V,$
$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V,$
$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$
Among the following,the strongest reducing agent is:

MediumJEE MAIN 2017

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In a cell reaction
$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$
$E_{cell}^o = + 0.46 \ V$.
If the concentration of $Cu^{2+}$ ions is doubled,then $E_{cell}^o$ will be

Easy

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What is denoted by a negative $E^o$ and a positive $E^o$ value in electrochemistry?

Medium

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What is the oxidation and reduction potential of standard hydrogen electrode?

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$FeO_4^{2-}$ $\xrightarrow{2.0 \ V} Fe^{3+}$ $\xrightarrow{0.8 \ V} Fe^{2+}$ $\xrightarrow{-0.44 \ V} Fe^0$In the above diagram,the standard electrode potentials are given in volts. The value of $E_{FeO_4^{2-}/Fe^{2+}}^{\Theta}$ is: (in $V$)

Standard electrode potential of $Ag^{+}/Ag$ and $Cu^{2+}/Cu$ is $+0.80 \ V$ and $+0.34 \ V$ respectively. These electrodes are joined together by a salt bridge. If:

Given$E^o_{Cl_2/Cl^-} = 1.36 \ V,$$E^o_{Cr^{3+}/Cr} = -0.74 \ V,$$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V,$$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$Among the following,the strongest reducing agent is:

In a cell reaction$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$$E_{cell}^o = + 0.46 \ V$.If the concentration of $Cu^{2+}$ ions is doubled,then $E_{cell}^o$ will be

What is denoted by a negative $E^o$ and a positive $E^o$ value in electrochemistry?

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$FeO_4^{2-}$ $\xrightarrow{2.0 \ V} Fe^{3+}$ $\xrightarrow{0.8 \ V} Fe^{2+}$ $\xrightarrow{-0.44 \ V} Fe^0$
In the above diagram,the standard electrode potentials are given in volts. The value of $E_{FeO_4^{2-}/Fe^{2+}}^{\Theta}$ is: (in $V$)

Given
$E^o_{Cl_2/Cl^-} = 1.36 \ V,$
$E^o_{Cr^{3+}/Cr} = -0.74 \ V,$
$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V,$
$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$
Among the following,the strongest reducing agent is:

In a cell reaction
$Cu_{(s)} + 2Ag^{+}_{(aq)} \to Cu^{2+}_{(aq)} + 2Ag_{(s)}$
$E_{cell}^o = + 0.46 \ V$.
If the concentration of $Cu^{2+}$ ions is doubled,then $E_{cell}^o$ will be