Step 1: Balanced equation for lead nitrate decomposition
\[
2\, \text{Pb(NO}_3)_2 \rightarrow 2\, \text{PbO} + 4\, \text{NO}_2 + \text{O}_2
\]
Step 2: Mole ratio from the equation
From the equation:
\[
2 \text{ moles of Pb(NO}_3)_2 \text{ produce } 1 \text{ mole of O}_2
\]
Step 3: Oxygen produced from 2 moles of Pb(NO\(_3\))\(_2\)
The question considers 2 moles of Pb(NO\(_3\))\(_2\) decomposition:
\[
\text{O}_2 \text{ produced} = 1 \text{ mole}
\]
\[
\boxed{\text{1 mole of O}_2 \text{ is formed from the decomposition of 2 moles of Pb(NO}_3)_2}
\]