If the standard reduction potentials of $Zn$, $Ni$, and $Fe$ are $-0.76 \text{ V}$, $-0.23 \text{ V}$, and $-0.44 \text{ V}$ respectively, determine the electrodes $X$ and $Y$ for the reaction $X(s) + Y^{+2}(aq) \rightarrow X^{+2}(aq) + Y(s)$ to be spontaneous.
- A$X = Ni, Y = Fe$
- B$X = Ni, Y = Zn$
- C$X = Fe, Y = Zn$
- D$X = Zn, Y = Ni$
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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:
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View SolutionIdentify which of the following cell reactions is spontaneous under standard state conditions.
DifficultMHT CET 2026
View SolutionFor the following cell,the standard electrode potential $E_{cell}^0$ is . . . . . . .
$E_{Zn^{2+}/Zn}^0 = -0.76 \ V, E_{Cu^{2+}/Cu}^0 = 0.34 \ V$
$Zn | Zn^{2+} || Cu^{2+} | Cu$ (in $V$)
$E_{Zn^{2+}/Zn}^0 = -0.76 \ V, E_{Cu^{2+}/Cu}^0 = 0.34 \ V$
$Zn | Zn^{2+} || Cu^{2+} | Cu$ (in $V$)
Which metal cannot produce $H_2$ gas by reaction with $HCl$ solution?
$E^0_{Fe^{2+}/Fe} = -0.44 \ V$
$E^0_{Cu^{2+}/Cu} = +0.34 \ V$
$E^0_{Ni^{2+}/Ni} = -0.25 \ V$
$E^0_{Zn^{2+}/Zn} = -0.76 \ V$
$E^0_{Fe^{2+}/Fe} = -0.44 \ V$
$E^0_{Cu^{2+}/Cu} = +0.34 \ V$
$E^0_{Ni^{2+}/Ni} = -0.25 \ V$
$E^0_{Zn^{2+}/Zn} = -0.76 \ V$
Calculate the standard free energy change for the reaction $\frac{1}{2}Cu_{(s)} + \frac{1}{2}Cl_{2(g)} \rightleftharpoons \frac{1}{2}Cu^{2+} + Cl^-$ taking place at $25\ ^oC$ in a cell whose standard e.m.f. is $1.02 \ V$ (in $J$).
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