A) \[Z{{n}^{+2}}(aq)+2Ag(s)\xrightarrow{{}}2A{{g}^{+}}(aq)+Zn(s)\]
B) \[Zn(s)+2A{{g}^{+}}(aq)\xrightarrow{{}}Z{{n}^{+2}}(aq)+2Ag(s)\]
C) \[Z{{n}^{+2}}(aq)+A{{g}^{+}}(aq)\xrightarrow{{}}Zn(s)+Ag(s)\]
D) \[Zn(s)+Ag(s)\xrightarrow{{}}Z{{n}^{+2}}(aq)+A{{g}^{+}}(aq)\]
Correct Answer: B
Solution :
As the reduction potential of Zn is less than that of Ag, hence Zn will act as anode when a cell is made using them. Hence the correct cell reaction will be \[Zn(s)\xrightarrow{{}}Z{{n}^{2+}}(aq)+2{{e}^{-}}\] (oxidation) \[2A{{g}^{+}}(aq)+2{{e}^{-}}\xrightarrow{{}}2Ag(s)\] \[Zn(s)+2A{{g}^{+}}(aq)\xrightarrow{{}}Z{{n}^{2+}}(aq)+2Ag(s)\]You need to login to perform this action.
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