(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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(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.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

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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
$X = Ni, Y = Fe$
B
$X = Ni, Y = Zn$
C
$X = Fe, Y = Zn$
D
$X = Zn, Y = Ni$

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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:

Similar Questions

For a closed circuit Daniell cell, which of the following plots is the accurate one at a given temperature?

What is $emf$?

Using the standard reduction potentials of the electrodes $Li$,$Zn$,$Mg$,and $Ni$ as $-3.05 \ V$,$-0.76 \ V$,$-2.36 \ V$,and $-0.25 \ V$ respectively,identify the correct statement.

Which of the following expressions is correct for the standard Gibbs free energy change?

In which metal container can an aqueous solution of $CuSO_4$ be stored? $E^0_{Cu^{2+}/Cu} = 0.34 \ V$,$E^0_{Fe/Fe^{2+}} = 0.44 \ V$,$E^0_{Al/Al^{3+}} = 1.66 \ V$,$E^0_{Ni/Ni^{2+}} = 0.25 \ V$,$E^0_{Ag^{+}/Ag} = 0.80 \ V$

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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:

In which metal container can an aqueous solution of $CuSO_4$ be stored?
$E^0_{Cu^{2+}/Cu} = 0.34 \ V$,$E^0_{Fe/Fe^{2+}} = 0.44 \ V$,$E^0_{Al/Al^{3+}} = 1.66 \ V$,$E^0_{Ni/Ni^{2+}} = 0.25 \ V$,$E^0_{Ag^{+}/Ag} = 0.80 \ V$