What is the procedure to determine the cell potential?
(N/A) Selection of reference electrode: The potential of an individual half-cell cannot be measured directly. We can only measure the difference between the potentials of two half-cells,which gives the $EMF$ of the cell.
$(b)$ Use of Standard Hydrogen Electrode $(SHE)$: To determine the potential of a single half-cell,it is coupled with a reference electrode whose potential is known. By convention,the Standard Hydrogen Electrode $(SHE)$ is used as the reference,and its potential is arbitrarily assigned a value of $0.00 \ V$ at all temperatures.
$(c)$ Calculation: When the half-cell is connected to the $SHE$,the measured $EMF$ of the resulting cell corresponds to the potential of that half-cell. If the half-cell acts as the cathode,its potential is positive; if it acts as the anode,its potential is negative relative to the $SHE$.
$(b)$ Use of Standard Hydrogen Electrode $(SHE)$: To determine the potential of a single half-cell,it is coupled with a reference electrode whose potential is known. By convention,the Standard Hydrogen Electrode $(SHE)$ is used as the reference,and its potential is arbitrarily assigned a value of $0.00 \ V$ at all temperatures.
$(c)$ Calculation: When the half-cell is connected to the $SHE$,the measured $EMF$ of the resulting cell corresponds to the potential of that half-cell. If the half-cell acts as the cathode,its potential is positive; if it acts as the anode,its potential is negative relative to the $SHE$.
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Similar Questions
The standard reduction potentials for $Al^{3+} | Al$,$Fe^{2+} | Fe$,and $Br_2 | Br^-$ are $-1.66 \ V$,$-0.45 \ V$,and $1.09 \ V$ respectively. What is the correct order of their reducing power?
Easy
View SolutionDiscuss the method to determine the cell potential of any cell when a standard hydrogen electrode is considered as the anode,with a suitable example.
Give the uses of the standard hydrogen electrode $(SHE)$.
Easy
View SolutionThe standard reduction potentials at $298 \ K$ for the following half-reactions are given:
$Zn^{2+}_{(aq)} + 2e^- \rightleftharpoons Zn_{(s)}; E^\circ = -0.762 \ V$
$Cr^{3+}_{(aq)} + 3e^- \rightleftharpoons Cr_{(s)}; E^\circ = -0.740 \ V$
$2H^+_{(aq)} + 2e^- \rightleftharpoons H_{2(g)}; E^\circ = 0.00 \ V$
$Fe^{3+}_{(aq)} + e^- \rightleftharpoons Fe^{2+}_{(aq)}; E^\circ = 0.770 \ V$
Which is the strongest reducing agent?
$Zn^{2+}_{(aq)} + 2e^- \rightleftharpoons Zn_{(s)}; E^\circ = -0.762 \ V$
$Cr^{3+}_{(aq)} + 3e^- \rightleftharpoons Cr_{(s)}; E^\circ = -0.740 \ V$
$2H^+_{(aq)} + 2e^- \rightleftharpoons H_{2(g)}; E^\circ = 0.00 \ V$
$Fe^{3+}_{(aq)} + e^- \rightleftharpoons Fe^{2+}_{(aq)}; E^\circ = 0.770 \ V$
Which is the strongest reducing agent?
MediumAIIMS 2013
View SolutionGiven $E^{0}_{Fe^{3+}|Fe} = -0.036 \, V$ and $E^{0}_{Fe^{2+}|Fe} = -0.439 \, V$,the standard electrode potential for the reaction $Fe^{3+}_{(aq)} + e^{-} \rightarrow Fe^{2+}_{(aq)}$ is ........... $V$.
Difficult
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