At 25oC, the standard oxidation potential of Zn and Ag in water are:
Zn(s)→Zn+2(aq)+2e−,E0=0.76V
and Ag(s)→Ag+(aq)+e−,E0=−0.80V.
Which of the following reaction actually takes place?
A
Zn2+(aq)+2Ag(s)→2Ag+(aq)+Zn(s)
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B
Zn(s)+2Ag+(aq)→Zn2+(aq)+2Ag(s)
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C
Zn2+(aq)+2Ag+(aq)→Zn(s)+2Ag(s)
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D
Zn(s)+Ag(s)→Zn2+(aq)+Ag+(aq)
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Solution
The correct option is CZn(s)+2Ag+(aq)→Zn2+(aq)+2Ag(s) Looking at the oxidation potential values of the reaction, Zn has a higher value compared to Ag. Thus, Zn gets more easily oxidised as compared to Ag.
∴Ag gets reduced and Zn gets oxidised. Hence, the reactions are as follows: