Given that E^o_{Ni^{2+} | Ni} = -0.25 VE^o_{ | vedclass

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(A) reaction is spontaneous if the standard cell potential $E^o_{cell}$ is positive. $E^o_{cell} = E^o_{cathode} - E^o_{anode}$. For option $A$: $Ni^{

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$Ni^{2+}_{(aq.)} + Cu_{(s)} \longrightarrow Ni_{(s)} + Cu^{2+}_{(aq.)}$

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(A) reaction is spontaneous if the standard cell potential $E^o_{cell}$ is positive. $E^o_{cell} = E^o_{cathode} - E^o_{anode}$. For option $A$: $Ni^{2+} + Cu \longrightarrow Ni + Cu^{2+}$. $E^o_{cell} = E^o_{Ni^{2+}|Ni} - E^o_{Cu^{2+}|Cu} = -0.25 - 0.34 = -0.59 \ V$. Since $E^o_{cell} For option $B$: $2Ag^{+} + Cu \longrightarrow 2Ag + Cu^{2+}$. $E^o_{cell} = 0.80 - 0.34 = +0.46 \ V$. Since $E^o_{cell} > 0$,this reaction is spontaneous. For option $C$: $Zn + Cu^{2+} \longrightarrow Zn^{2+} + Cu$. $E^o_{cell} = 0.34 - (-0.76) = +1.10 \ V$. Since $E^o_{cell} > 0$,this reaction is spontaneous. For option $D$: $2H^{+} + Zn \longrightarrow H_2 + Zn^{2+}$. $E^o_{cell} = 0.00 - (-0.76) = +0.76 \ V$. Since $E^o_{cell} > 0$,this reaction is spontaneous.

Given that
$E^o_{Ni^{2+} | Ni} = -0.25 \ V$
$E^o_{Cu^{2+} | Cu} = 0.34 \ V$
$E^o_{Ag^{+} | Ag} = 0.80 \ V$
$E^o_{Zn^{2+} | Zn} = -0.76 \ V$
Which of the following reactions under standard condition will not take place in the specified direction?

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Given that $E^o_{Ni^{2+} | Ni} = -0.25 \ V$$E^o_{Cu^{2+} | Cu} = 0.34 \ V$$E^o_{Ag^{+} | Ag} = 0.80 \ V$$E^o_{Zn^{2+} | Zn} = -0.76 \ V$Which of the following reactions under standard condition will not take place in the specified direction?