$45.4 \ L$ of dinitrogen reacts with $22.7 \ L$ of dioxygen to form $45.4 \ L$ of nitrous oxide. For the reaction $2N_{2(g)} + O_{2(g)} \to 2N_2O_{(g)}$,identify the law followed and state the law.

(A) The given reaction is: $2N_{2(g)} + O_{2(g)} \to 2N_2O_{(g)}$
Stoichiometric volumes: $2 \ V \quad 1 \ V \quad 2 \ V$
Given volumes: $45.4 \ L \quad 22.7 \ L \quad 45.4 \ L$
Dividing by $22.7 \ L$: $2 : 1 : 2$
Since the volumes of reactants and products bear a simple whole-number ratio $(2:1:2)$,this reaction follows Gay-Lussac's Law of Gaseous Volumes.
Gay-Lussac's Law states: "When gases react together,they do so in volumes which bear a simple ratio to one another and to the volume of the products,if gaseous,provided that all gases are at the same temperature and pressure."