# How would you balance _N2O5 -->_NO2+_O2?

Oct 21, 2015

${N}_{2} {O}_{5} \left(g\right) \rightarrow 2 N {O}_{2} \left(g\right) + \frac{1}{2} {O}_{2} \left(g\right)$

#### Explanation:

Can I have 1/2 a molecule of ${O}_{2} \left(g\right)$? How do I get rid of the $\frac{1}{2}$ coefficient? Is this a redox reaction?

Oct 21, 2015

${\text{2N"_2"O}}_{5}$$\rightarrow$${\text{4NO"_2+"O}}_{2}$

#### Explanation:

${\text{N"_2"O}}_{5}$$\rightarrow$${\text{NO"_2+"O}}_{2}$

Add coefficients in front of the formulas in order to balance the equation.

${\text{2N"_2"O}}_{5}$$\rightarrow$${\text{4NO"_2+"O}}_{2}$

There are now 4 atoms of N and 10 atoms of oxygen on both sides, and the equation is balanced.