The standard reduction potentials of {\Zn} and {\Ag} in water at 298 {\K} are, {\Zn}^{2+}+2 e^{-} \to {\Zn}, E^{\circ}=-0.76 {\V} \text{ and } {\Ag}^{+}+e^{-} ⟷ {\Ag} ; E^{\circ}=+0.80 {\V} \text{. } Which of the following reactions take place?

Correct Answer is : Zn(s)+2Ag+(aq)→Zn2+(aq)+2Ag(s)

{\Zn}^{2+}(a q)+2 {\Ag}(s) \to 2 {\Ag}^{+}(a q)+ {\Zn}(s)

{\Zn}(s)+2 {\Ag}^{+}(a q) \to {\Zn}^{2+}(a q)+2 {\Ag}(s)

{\Zn}^{2+}(a q)+ {\Ag}^{+}(a q) \to {\Zn}(s)+ {\Ag}(s)

{\Zn}(s)+ {\Ag}(s) \to {\Zn}^{2+}(a q)+ {\Ag}^{+}(a q)

0 For option (b), E'_{\cell}=(E"_{\red})_{\cathode}-(E"_{\red})_{\Anode} =0.80-(-0.76)=1.56V ∴ It will be sponteneous reaction ∵ E"_{\cell}>0" >

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