The standard reduction potentials for Zn^{2+} | vedclass

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(D) For a spontaneous reaction,the standard cell potential $E^{\circ}_{cell}$ must be positive.The reaction is $X + Y^{2+} \rightarrow X^{2+} + Y$.$E^

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$X = Zn, Y = Ni$

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(D) For a spontaneous reaction,the standard cell potential $E^{\circ}_{cell}$ must be positive.The reaction is $X + Y^{2+} \rightarrow X^{2+} + Y$.$E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode} = E^{\circ}_{Y^{2+}/Y} - E^{\circ}_{X^{2+}/X}$.For $X = Zn$ and $Y = Ni$:$E^{\circ}_{cell} = E^{\circ}_{Ni^{2+}/Ni} - E^{\circ}_{Zn^{2+}/Zn} = -0.23 \ V - (-0.76 \ V) = +0.53 \ V$.Since $E^{\circ}_{cell} > 0$,the reaction is spontaneous.

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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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: