(D) In a Galvanic cell,the electrode with the higher reduction potential acts as the cathode (positive electrode),and the electrode with the lower red

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$2H^{+}_{(aq)} + 2e^{-} \longrightarrow H_{2(g)}$

(D) In a Galvanic cell,the electrode with the higher reduction potential acts as the cathode (positive electrode),and the electrode with the lower reduction potential acts as the anode (negative electrode). Given $E^{\circ}(Zn^{+2}/Zn) = -0.76 \ V$ and $E^{\circ}(H^{+}/H_2) = 0.00 \ V$. Since $0.00 \ V > -0.76 \ V$,the standard hydrogen electrode acts as the cathode (positive electrode). Reduction occurs at the cathode: $2H^{+}_{(aq)} + 2e^{-} \longrightarrow H_{2(g)}$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

For a Galvanic cell consisting of a zinc electrode and a standard hydrogen electrode,$E^{\circ}(Zn^{+2}_{(aq)} \mid Zn_{(s)}) = -0.76 \ V$. Identify the reaction that takes place at the positive electrode during the working of the cell.

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A
$Zn_{(s)} \longrightarrow Zn^{+2}_{(aq)} + 2e^{-}$
B
$Zn^{+2}_{(aq)} + 2e^{-} \longrightarrow Zn_{(s)}$
C
$H_{2(g)} \longrightarrow 2H^{+}_{(aq)} + 2e^{-}$
D
$2H^{+}_{(aq)} + 2e^{-} \longrightarrow H_{2(g)}$

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For a Galvanic cell consisting of a zinc electrode and a standard hydrogen electrode,$E^{\circ}(Zn^{+2}_{(aq)} \mid Zn_{(s)}) = -0.76 \ V$. Identify the reaction that takes place at the positive electrode during the working of the cell.

Similar Questions

$A$ galvanic cell consists of a copper electrode and a standard hydrogen electrode. If $E^\circ (Cu^{2+}_{(aq)} | Cu_{(s)}) = +0.34 \text{ V}$, identify the reaction taking place at the positive electrode during the working of the cell.

Which expression represents the cell potential $(E_{cell})$?

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:

For the following cell reaction,$Ag | Ag^{+} | AgCl | Cl^{-} | Cl_2, Pt$ $\Delta G_f^{\circ}(AgCl) = -109 \ kJ/mol$ $\Delta G_f^{\circ}(Cl^{-}) = -129 \ kJ/mol$ $\Delta G_f^{\circ}(Ag^{+}) = 78 \ kJ/mol$ $E^{\circ}$ of the cell is

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For the following cell reaction,$Ag | Ag^{+} | AgCl | Cl^{-} | Cl_2, Pt$
$\Delta G_f^{\circ}(AgCl) = -109 \ kJ/mol$
$\Delta G_f^{\circ}(Cl^{-}) = -129 \ kJ/mol$
$\Delta G_f^{\circ}(Ag^{+}) = 78 \ kJ/mol$
$E^{\circ}$ of the cell is