Question

Is the following reaction possible or not? Explain with reasons. \[Zn(NO_3)_2 + 2Ag \rightarrow 2AgNO_3 + Zn\]

Hint:

Zn is above Ag in the activity series; Ag cannot displace Zn. Check \(E^{\circ}_{cell}\) is negative.

Answer 1

Step 1: Rule for displacement. A more reactive metal pushes out a less reactive metal from its salt. So the question is simply: is silver more reactive than zinc?
Step 2: Position in the activity series. The order is \(Zn > Ag\); zinc lies well above silver. Silver is a noble metal that resists losing electrons, whereas zinc gives up electrons readily.
Step 3: Why it fails. Because silver is the weaker reducing agent, it cannot reduce \(Zn^{2+}\) to \(Zn\). Numerically the standard cell EMF for the written direction works out negative (\(-1.56\,V\)), confirming it will not proceed.
Step 4: The real direction. Nature runs the opposite way: metallic zinc displaces silver from silver nitrate, \(Zn + 2AgNO_3 \rightarrow Zn(NO_3)_2 + 2Ag\). Hence the given equation is impossible.
\[\boxed{\text{Not possible}}\]