(B) $1$. In a galvanic cell, the electrode with the higher reduction potential acts as the cathode (positive electrode).$2$. The standard reduction po

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$Cu^{2+}_{(aq)} + 2e^- \longrightarrow Cu_{(s)}$

(B) $1$. In a galvanic cell, the electrode with the higher reduction potential acts as the cathode (positive electrode).$2$. The standard reduction potential of the standard hydrogen electrode $(SHE)$ is $E^\circ (H^+ | H_2) = 0.00 \text{ V}$.$3$. Since $E^\circ (Cu^{2+} | Cu) = +0.34 \text{ V} > 0.00 \text{ V}$, the copper electrode acts as the cathode.$4$. Reduction occurs at the cathode: $Cu^{2+}_{(aq)} + 2e^- \longrightarrow Cu_{(s)}$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

$A$ 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.

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A
$Cu_{(s)} \longrightarrow Cu^{2+}_{(aq)} + 2e^-$
B
$Cu^{2+}_{(aq)} + 2e^- \longrightarrow Cu_{(s)}$
C
$H_2(g) \longrightarrow 2H^+_{(aq)} + 2e^-$
D
$H^+_{(aq)} + 2e^- \longrightarrow H_2(g)$

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Calculate $E_{cell}^{\circ}$ for the following cell: $Zn_{(s)} | Zn^{2+}_{(1 \ M)} || Pb^{2+}_{(1 \ M)} | Pb_{(s)}$ given that $E^{\circ}_{Zn^{2+}/Zn} = -0.763 \ V$ and $E^{\circ}_{Pb^{2+}/Pb} = -0.126 \ V$. (in $V$)

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Given are $E^o$ values for some half reactions:
$I_2 + 2e^- \to 2I^{-}; E^o = 0.54 \ V$
$MnO_4^- + 8H^{+} + 5e^- \to Mn^{2+} + 4H_2O; E^o = 1.52 \ V$
$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.77 \ V$
$Sn^{4+} + 2e^- \to Sn^{2+}; E^o = 0.1 \ V$
The strongest reducant and oxidant respectively are:

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The relation between $\Delta G$ and $E$ for a cell is given by $\Delta G = -nFE$. Which of the following conditions must be satisfied for the cell reaction to be spontaneous?

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Which among the following species is reduced by tin easily?

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The standard reduction potentials for $Zn^{2+}/Zn$,$Ni^{2+}/Ni$ and $Fe^{2+}/Fe$ are $-0.76 \ V$,$-0.23 \ V$ and $-0.44 \ V$ respectively.
The reaction $X + Y^{2+} \rightarrow X^{2+} + Y$ will be spontaneous when:

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$A$ 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.

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Calculate $E_{cell}^{\circ}$ for the following cell: $Zn_{(s)} | Zn^{2+}_{(1 \ M)} || Pb^{2+}_{(1 \ M)} | Pb_{(s)}$ given that $E^{\circ}_{Zn^{2+}/Zn} = -0.763 \ V$ and $E^{\circ}_{Pb^{2+}/Pb} = -0.126 \ V$. (in $V$)

Given are $E^o$ values for some half reactions:$I_2 + 2e^- \to 2I^{-}; E^o = 0.54 \ V$$MnO_4^- + 8H^{+} + 5e^- \to Mn^{2+} + 4H_2O; E^o = 1.52 \ V$$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.77 \ V$$Sn^{4+} + 2e^- \to Sn^{2+}; E^o = 0.1 \ V$The strongest reducant and oxidant respectively are:

The relation between $\Delta G$ and $E$ for a cell is given by $\Delta G = -nFE$. Which of the following conditions must be satisfied for the cell reaction to be spontaneous?

Which among the following species is reduced by tin easily?

The standard reduction potentials for $Zn^{2+}/Zn$,$Ni^{2+}/Ni$ and $Fe^{2+}/Fe$ are $-0.76 \ V$,$-0.23 \ V$ and $-0.44 \ V$ respectively.The reaction $X + Y^{2+} \rightarrow X^{2+} + Y$ will be spontaneous when:

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Given are $E^o$ values for some half reactions:
$I_2 + 2e^- \to 2I^{-}; E^o = 0.54 \ V$
$MnO_4^- + 8H^{+} + 5e^- \to Mn^{2+} + 4H_2O; E^o = 1.52 \ V$
$Fe^{3+} + e^- \to Fe^{2+}; E^o = 0.77 \ V$
$Sn^{4+} + 2e^- \to Sn^{2+}; E^o = 0.1 \ V$
The strongest reducant and oxidant respectively are:

The standard reduction potentials for $Zn^{2+}/Zn$,$Ni^{2+}/Ni$ and $Fe^{2+}/Fe$ are $-0.76 \ V$,$-0.23 \ V$ and $-0.44 \ V$ respectively.
The reaction $X + Y^{2+} \rightarrow X^{2+} + Y$ will be spontaneous when: