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 electrode potentials of the half-cells are given below:
$Zn^{2+} + 2e^- \to Zn$; $E^{\circ} = -0.76 \, V$
$Fe^{2+} + 2e^- \to Fe$; $E^{\circ} = -0.44 \, V$
The $EMF$ of the cell $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.
$Zn^{2+} + 2e^- \to Zn$; $E^{\circ} = -0.76 \, V$
$Fe^{2+} + 2e^- \to Fe$; $E^{\circ} = -0.44 \, V$
The $EMF$ of the cell $Fe^{2+} + Zn \to Zn^{2+} + Fe$ is ............ $V$.
Medium
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
View SolutionThe $E^o$ values of $Mg^{2+}/Mg$ is $-2.37 \ V$,$Zn^{2+}/Zn$ is $-0.76 \ V$,and $Fe^{2+}/Fe$ is $-0.44 \ V$. Which of the following statements is correct?
Easy
View SolutionGiven $E_{Cu^{2+}/Cu}^{\circ} = 0.34 \ V$ and $E_{Cu^{2+}/Cu^{+}}^{\circ} = 0.15 \ V$. Calculate the standard electrode potential $E_{Cu^{+}/Cu}^{\circ}$ in $V$.
Medium
View SolutionTwo half-cell reactions are given below:
$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$
$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$
The standard $EMF$ of a cell with a feasible redox reaction will be:
$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$
$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$
The standard $EMF$ of a cell with a feasible redox reaction will be:
MediumNEET 2022
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