If in a galvanic cell,the hydrogen half-cell is the anode on the left side,what is the sign of the standard potential of such a galvanic cell? Give an example.
(N/A) In a galvanic cell,if the hydrogen half-cell $(Pt, H_{2(g)} | H^{+}_{(aq)})$ is placed on the anode (left side),its oxidation potential is $0.00 \ V$.
Since $E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ}$ and $E_{anode}^{\circ} = 0 \ V$,then $E_{cell}^{\circ} = E_{cathode}^{\circ}$.
If the cathode has a positive standard reduction potential (like $Cu^{2+}/Cu$ where $E^{\circ} = +0.34 \ V$),the cell potential will be positive.
For the cell: $Pt, H_{2(g)} | H^{+}(1 \ M) || Cu^{2+}(1 \ M) | Cu_{(s)}$,the standard cell potential is $E_{cell}^{\circ} = +0.34 \ V - 0.00 \ V = +0.34 \ V$.
Since $E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ}$ and $E_{anode}^{\circ} = 0 \ V$,then $E_{cell}^{\circ} = E_{cathode}^{\circ}$.
If the cathode has a positive standard reduction potential (like $Cu^{2+}/Cu$ where $E^{\circ} = +0.34 \ V$),the cell potential will be positive.
For the cell: $Pt, H_{2(g)} | H^{+}(1 \ M) || Cu^{2+}(1 \ M) | Cu_{(s)}$,the standard cell potential is $E_{cell}^{\circ} = +0.34 \ V - 0.00 \ V = +0.34 \ V$.
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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?
| $A$ | $B$ | $C$ | $D$ |
|---|---|---|---|
| $1 \times 10^{-4}$ | $2 \times 10^{-4}$ | $0.1 \times 10^{-4}$ | $0.2 \times 10^{-4}$ |
(Where $E$ is the electromotive force)
Which of the above half cells would be preferred to be used as reference electrode?
DifficultJEE MAIN 2022
View SolutionGiven the following standard electrode potentials:
$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$
$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$
Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$
$Cu^{+2} + 2e^{-} \to Cu$,$E^{o} = X_{1}$
$Cu^{+} + e^{-} \to Cu$,$E^{o} = X_{2}$
Calculate the standard electrode potential $E^{o}$ for the reaction: $Cu^{+2} + e^{-} \to Cu^{+}$
Difficult
View SolutionGiven electrode potentials:
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = 0.771 \, V$
$I_2 + 2e^- \to 2I^-$; $E^o = 0.536 \, V$
$E^o_{\text{cell}}$ for the cell reaction
$2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$ is:
$Fe^{3+} + e^- \to Fe^{2+}$; $E^o = 0.771 \, V$
$I_2 + 2e^- \to 2I^-$; $E^o = 0.536 \, V$
$E^o_{\text{cell}}$ for the cell reaction
$2Fe^{3+} + 2I^- \to 2Fe^{2+} + I_2$ is:
Medium
View SolutionThe standard reduction potentials for two half-cell reactions are given below:
$Cd^{2+}_{(aq)} + 2e^{-} \rightarrow Cd_{(s)}, E^o = -0.40 \ V$
$Ag^{+}_{(aq)} + e^{-} \rightarrow Ag_{(s)}, E^o = 0.80 \ V$
What is the standard free energy change $\Delta G^o$ in $kJ$ for the reaction $2Ag^{+}_{(aq)} + Cd_{(s)} \rightarrow 2Ag_{(s)} + Cd^{2+}_{(aq)}$?
$Cd^{2+}_{(aq)} + 2e^{-} \rightarrow Cd_{(s)}, E^o = -0.40 \ V$
$Ag^{+}_{(aq)} + e^{-} \rightarrow Ag_{(s)}, E^o = 0.80 \ V$
What is the standard free energy change $\Delta G^o$ in $kJ$ for the reaction $2Ag^{+}_{(aq)} + Cd_{(s)} \rightarrow 2Ag_{(s)} + Cd^{2+}_{(aq)}$?
Medium
View SolutionGiven that the standard reduction potentials for $M^{+}/M$ and $N^{+}/N$ electrodes at $298 \ K$ are $0.52 \ V$ and $0.25 \ V$ respectively. Which of the following is correct in respect of the following electrochemical cell?
$M | M^{+} || N^{+} | N$
$M | M^{+} || N^{+} | N$
MediumAIIMS 2016
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