What is the expected reaction when iron is placed in a solution of silver nitrate?

When iron is placed in a solution of silver nitrate, the expected reaction involves the oxidation of iron and the reduction of silver ions. In this reaction, iron serves as a more reactive metal compared to silver. As a result, iron will undergo oxidation, which means it loses electrons and forms iron ions (Fe²⁺ or Fe³⁺). Concurrently, the silver ions (Ag⁺) from the silver nitrate solution accept these electrons, leading to their reduction to metallic silver (Ag).

This process can be described in terms of the half-reactions:

1. Oxidation of iron:

[ \text{Fe} \rightarrow \text{Fe}^{2+} + 2\text{e}^- ]

2. Reduction of silver ions:

[ \text{Ag}^+ + \text{e}^- \rightarrow \text{Ag} ]

This overall reaction highlights the capability of iron to displace silver from its nitrate solution due to its higher reactivity. This is an example of a single displacement reaction where a more reactive metal (iron) displaces a less reactive metal (silver) from its compound.