Balance the following equations and identify the type of reaction: NaNO3 + PbO → Pb(NO3)2 + Na2O.

Steps to Solve

1. Identify Reactants and Products The reactants are sodium nitrate ($\text{NaNO}_3$) and lead(II) oxide ($\text{PbO}$). The products are lead(II) nitrate ($\text{Pb(NO}_3\text{)}_2$) and sodium oxide ($\text{Na}_2\text{O}$).

2. Count Atoms on Both Sides Count the number of each type of atom in the unbalanced equation:

   • Reactants:
     • Na: 1
     • N: 1
     • O: 3 (from NaNO3) + 1 (from PbO) = 4
     • Pb: 1
   • Products:
     • Pb: 1
     • N: 2 (from Pb(NO3)2)
     • O: 6 (from Pb(NO3)2) + 1 (from Na2O) = 7
     • Na: 2

3. Balance Sodium (Na) To balance sodium, place a coefficient of 2 before $\text{NaNO}_3$: $$ 2 \text{NaNO}_3 + \text{PbO} \rightarrow \text{Pb(NO}_3\text{)}_2 + \text{Na}_2\text{O} $$

4. Recount Atoms After Balancing Sodium Now recount the atoms:

   • Reactants:
     • Na: 2
     • N: 2
     • O: 6 (from 2NaNO3) + 1 (from PbO) = 7
     • Pb: 1
   • Products:
     • Pb: 1
     • N: 2
     • O: 6 (from Pb(NO3)2) + 1 (from Na2O) = 7
     • Na: 2

5. Confirm Balance Now both sides have:

   • Na: 2
   • N: 2
   • O: 7
   • Pb: 1

The equation is now balanced.

6. Identify the Type of Reaction This reaction is a double displacement reaction because it involves the exchange of ions between two compounds.