When you react silver nitrate (AgNO₃) with iron (Fe), a single displacement reaction occurs. This means that the more reactive metal (iron) will displace the less reactive metal (silver) from its compound.

Here's what happens:

* Reaction: Fe(s) + 2AgNO₃(aq) → 2Ag(s) + Fe(NO₃)₂(aq)

* Explanation:

* Iron (Fe) is more reactive than silver (Ag) according to the reactivity series of metals.

* Iron atoms will donate electrons to silver ions (Ag⁺) in the silver nitrate solution.

* This results in the formation of iron(II) nitrate (Fe(NO₃)₂) and solid silver (Ag) is deposited as a coating on the iron.

* Observations:

* You will observe a grayish-white coating forming on the iron surface. This is the solid silver being deposited.

* The solution will turn pale green due to the formation of iron(II) nitrate.

Safety Precautions:

* Silver nitrate is corrosive and can cause skin irritation. Wear appropriate safety goggles and gloves when handling it.

* Iron(II) nitrate is also harmful. Avoid contact with skin and eyes.

* Conduct the experiment in a well-ventilated area.

In summary: The reaction between silver nitrate and iron is a classic example of a single displacement reaction, resulting in the formation of silver metal and iron(II) nitrate.