# How would you balance this equation: ?Pb(NO_3)_2 → ?Pb + ?NO_2 + ?O_2?

Mar 14, 2017

$P b {\left(N {O}_{3}\right)}_{2} \rightarrow P b + O 2 + 2 N {O}_{2}$

#### Explanation:

To balance this reaction first we have to see the number of moles of each element.

$P b {\left(N {O}_{3}\right)}_{2} \rightarrow P b + {O}_{2} + N {O}_{2}$

(Pb = 1) (Pb = 1)

$\left(N = 2\right)$ $\left(O = {\cancel{4}}^{6}\right)$

(O = 6 ) $\left(N = {\cancel{1}}^{2}\right)$

First try adding 3 as the coefficient in front of ${O}_{2}$ and 2 in front of $N {O}_{2}$ but that will be wrong as 2NO2 has 4 oxygen atoms which we dont have, so to make a balanced equation we must remove 3 from O2 and add 2 in front of $N {O}_{2}$

= $P b {\left(N {O}_{3}\right)}_{2} \rightarrow P b + O 2 + 2 N {O}_{2}$