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Given, $E_{{Ni}^{2 +} / Ni}^{\circ} = - 0 .25 V, E_{{Cu}^{2 +} / Cu}^{\circ} = 0 .34 V, E_{{Ag}^{+} / Ag}^{\circ} = 0 .80 V$ and $E_{{Zn}^{2 +} / Zn}^{\circ} = - 0 .76 V$
Which of the following reactions under standard condition will not take place in the specified direction?

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$Zn (s) + 2 H^{+} (aq) ⟶ {Zn}^{2 +} (aq) + H_{2} (g)$

${Ni}^{2 +} (aq) + Cu (s) ⟶ Ni (s) + {Cu}^{2 +} (aq)$

${Cu}^{+ 2} (aq) + H_{2} (g) ⟶ Cu (s) + 2 H_{(aq)}^{+}$

$Cu (s) + 2 {Ag}^{+} (aq) ⟶ {Cu}^{2 +} (aq) + 2 Ag (s)$

answer is A.

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Detailed Solution

Because $E_{cell}^{o}$ is negative only for the reaction.
$E_{cell}^{°} = E_{{Ni}^{+ 2} / Ni}^{°} - E_{{Cu}^{+ 2} / Cu}^{°}$

= -0.25-(+0.34)= -0.59V

cell reaction is not feasible in the given direction

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