The reaction between lead and silver nitrate is a single displacement reaction where lead (Pb) displaces silver (Ag) from its compound. This is because lead is more reactive than silver in the reactivity series.

Here's the balanced chemical equation for the reaction:

Pb(s) + 2AgNO₃(aq) → Pb(NO₃)₂(aq) + 2Ag(s)

Explanation:

* Lead (Pb) is a solid metal.

* Silver nitrate (AgNO₃) is a colorless, soluble salt.

* Lead(II) nitrate (Pb(NO₃)₂) is also a soluble salt.

* Silver (Ag) is a solid metal.

Observations:

* When lead metal is added to a solution of silver nitrate, you will observe the following:

* Formation of a gray/white precipitate: This is the silver metal that is displaced from the solution.

* The solution will turn colorless: This is because the silver nitrate is consumed, and lead(II) nitrate is formed, which is also colorless.

Note: The reaction proceeds because lead is more reactive than silver, meaning it has a stronger tendency to lose electrons and form cations. This allows lead to displace silver from the silver nitrate solution.