Give the uses of the standard hydrogen electrode $(SHE)$.
(N/A) The standard hydrogen electrode $(SHE)$ is used as a reference electrode to measure the standard electrode potential of other half-cells.
$1$. It serves as a primary reference electrode with an assigned potential of $0.00 \ V$ at all temperatures.
$2$. It is used to determine the standard reduction potential of various metal/metal-ion couples by connecting them to the $SHE$ in an electrochemical cell.
$3$. It helps in constructing the electrochemical series by providing a baseline for comparison.
$1$. It serves as a primary reference electrode with an assigned potential of $0.00 \ V$ at all temperatures.
$2$. It is used to determine the standard reduction potential of various metal/metal-ion couples by connecting them to the $SHE$ in an electrochemical cell.
$3$. It helps in constructing the electrochemical series by providing a baseline for comparison.
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Similar Questions
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:
$E^o_{Cl_2/Cl^-} = 1.36 \ V,$
$E^o_{Cr^{3+}/Cr} = -0.74 \ V,$
$E^o_{Cr_2O_7^{2-}/Cr^{3+}} = 1.33 \ V,$
$E^o_{MnO_4^-/Mn^{2+}} = 1.51 \ V$
Among the following,the strongest reducing agent is:
Which one among the following is the strongest reducing agent?
$Fe^{2+} + 2e^- \to Fe \ (E^\circ = -0.44 \ V)$
$Ni^{2+} + 2e^- \to Ni \ (E^\circ = -0.25 \ V)$
$Sn^{2+} + 2e^- \to Sn \ (E^\circ = -0.14 \ V)$
$Fe^{3+} + e^- \to Fe^{2+} \ (E^\circ = +0.77 \ V)$
$Fe^{2+} + 2e^- \to Fe \ (E^\circ = -0.44 \ V)$
$Ni^{2+} + 2e^- \to Ni \ (E^\circ = -0.25 \ V)$
$Sn^{2+} + 2e^- \to Sn \ (E^\circ = -0.14 \ V)$
$Fe^{3+} + e^- \to Fe^{2+} \ (E^\circ = +0.77 \ V)$
Medium
View SolutionWhat will be the $EMF$ of the cell formed by the following half-cells in $V$?
$Mg^{2+} + 2e^- \to Mg_{(s)}; E = -2.37 \ V$
$Cu^{2+} + 2e^- \to Cu_{(s)}; E = +0.33 \ V$
$Mg^{2+} + 2e^- \to Mg_{(s)}; E = -2.37 \ V$
$Cu^{2+} + 2e^- \to Cu_{(s)}; E = +0.33 \ V$
Easy
View SolutionWhich of the following metals will not reduce $H_2O$?
Medium
View SolutionThe reaction $Zn^{2+} + 2e^{-} \to Zn$ has a standard electrode potential of $-0.76 \ V$. This means:
Easy
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