45.4 L of dinitrogen reacted with 22.7 L of dioxygen and 45.4 L of nitrous oxide was formed. The reaction is given below.

$2{ \mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)⟶2{ \mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)$

Which law is being obeyed in this experiment?

$\underset{2\mathrm{V}}{2}{ \mathrm{N}}_2\left(\mathrm{g}\right)+\underset{1 \mathrm{V}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\underset{ }{⟶}\underset{2\mathrm{V}}{2{ \mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)}$

$\frac{45.4}{22.7}=2, \frac{22.7}{22.7}=1, \frac{45.4}{22.7}=2$

Hence, the ratio between the volumes of the reactants and the product in the given question is simple, i.e.2: I : 2, it proves the Gay Lussac's law of gaseous volumes, which states that when gases combine or are produced in a chemical reaction, they do so in a simple ratio by volume provided all gases are at the same temperature and pressure.