# Question #f8f8f

Jun 28, 2017

$2 {\text{NO"_ ((g)) + "O"_ (2(g)) -> 2"NO}}_{2 \left(g\right)}$

#### Explanation:

Nitric oxide, $\text{NO}$, reacts with oxygen gas to produce nitrogen dioxide, ${\text{NO}}_{2}$, according to the following unbalanced chemical equation

${\text{NO"_ ((g)) + "O"_ (2(g)) -> "NO}}_{2 \left(g\right)}$

To balance the chemical equation, start by multiplying the nitric oxide by $2$ to get

$2 {\text{NO"_ ((g)) + "O"_ (2(g)) -> "NO}}_{2 \left(g\right)}$

At this point, you have $2$ atoms of nitrogen and $4$ atoms of oxygen on the reactants' side and only $1$ atom of nitrogen and $2$ atoms of oxygen on the products' side, so multiply the nitrogen dioxide by $2$ to get the balanced chemical equation

$2 {\text{NO"_ ((g)) + "O"_ (2(g)) -> 2"NO}}_{2 \left(g\right)}$