Give the symbolic representation of the following half-cells (electrodes):
$(i)$ $Zn_{(s)} | Zn^{2+}_{(aq)} (1M)$
$(ii)$ $Cu^{2+}_{(aq)} (1M) | Cu_{(s)}$
$(iii)$ $Pt_{(s)} | H_{2(g)} (1 \text{ bar}) | H^+_{(aq)} (1M)$
$(i)$ $Zn_{(s)} | Zn^{2+}_{(aq)} (1M)$
$(ii)$ $Cu^{2+}_{(aq)} (1M) | Cu_{(s)}$
$(iii)$ $Pt_{(s)} | H_{2(g)} (1 \text{ bar}) | H^+_{(aq)} (1M)$
(N/A) The symbolic representation of half-cells follows the $IUPAC$ convention where the electrode is written on the left and the electrolyte on the right for oxidation,and vice versa for reduction.
$(i)$ $Zn_{(s)} | Zn^{2+}_{(aq)} (1M)$ represents an oxidation half-cell (Anode).
$(ii)$ $Cu^{2+}_{(aq)} (1M) | Cu_{(s)}$ represents a reduction half-cell (Cathode).
$(iii)$ $Pt_{(s)} | H_{2(g)} (1 \text{ bar}) | H^+_{(aq)} (1M)$ represents a standard hydrogen electrode $(SHE)$ acting as an oxidation half-cell.
$(i)$ $Zn_{(s)} | Zn^{2+}_{(aq)} (1M)$ represents an oxidation half-cell (Anode).
$(ii)$ $Cu^{2+}_{(aq)} (1M) | Cu_{(s)}$ represents a reduction half-cell (Cathode).
$(iii)$ $Pt_{(s)} | H_{2(g)} (1 \text{ bar}) | H^+_{(aq)} (1M)$ represents a standard hydrogen electrode $(SHE)$ acting as an oxidation half-cell.
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Similar Questions
Match the following:
List-$I$ List-$II$ $(A)$ Potential of hydrogen electrode at $pH = 10$ $(I)$ $0.76 \ V$ $(B)$ $Cu^{2+} | Cu$ $(II)$ $0.059$ $(C)$ $Zn | Zn^{2+}$ $(III)$ $-0.591 \ V$ $(D)$ $\frac{2.303 RT}{F}$ $(IV)$ $0.337 \ V$ $(V)$ $-0.76 \ V$
$A$ $B$ $C$ $D$
$(a)$ $(III)$ $(I)$ $(II)$ $(V)$
$(b)$ $(II)$ $(V)$ $(I)$ $(IV)$
$(c)$ $(III)$ $(IV)$ $(I)$ $(II)$
$(d)$ $(V)$ $(I)$ $(IV)$ $(II)$
| List-$I$ | List-$II$ |
|---|---|
| $(A)$ Potential of hydrogen electrode at $pH = 10$ | $(I)$ $0.76 \ V$ |
| $(B)$ $Cu^{2+} | Cu$ | $(II)$ $0.059$ |
| $(C)$ $Zn | Zn^{2+}$ | $(III)$ $-0.591 \ V$ |
| $(D)$ $\frac{2.303 RT}{F}$ | $(IV)$ $0.337 \ V$ |
| $(V)$ $-0.76 \ V$ |
$A$ $B$ $C$ $D$
$(a)$ $(III)$ $(I)$ $(II)$ $(V)$
$(b)$ $(II)$ $(V)$ $(I)$ $(IV)$
$(c)$ $(III)$ $(IV)$ $(I)$ $(II)$
$(d)$ $(V)$ $(I)$ $(IV)$ $(II)$
For the cell reaction $Mg_{(s)} + Zn^{2+}_{(aq)} (1M) \rightarrow Zn_{(s)} + Mg^{2+}_{(aq)} (1M)$,the $emf$ is $1.60 \ V$. The $E$ of the cell is ........ $V$.
Medium
View SolutionGiven $E_{Cu^{2+}/Cu^{+}}^o = 0.15 \, V$,$E_{Cu^{2+}/Cu}^o = 0.34 \, V$. The standard electrode potential for the half-cell $Cu^{+}/Cu$ is ............. $V$.
DifficultAIEEE 2012
View SolutionThe standard reduction potentials (in $V$) of a few metal ion/metal electrodes are given below: $Cr^{3+}/Cr = -0.74$; $Cu^{2+}/Cu = +0.34$; $Pb^{2+}/Pb = -0.13$; $Ag^{+}/Ag = +0.8$. The reducing strength of the metals follows the order:
MediumKVPY 2015
View SolutionWhat is the standard electrode potential $(E^o)$ for the electrode represented by $Pt, O_2(1 \, atm) | 2H^+(1 \, M)$?
Easy
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