Question

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

$2N_2\left(g\right)+O_2\left(g\right)\to 2N_{2}O\left(g\right)$

Which law is being obeyed in this experiment? write the statement of the law?

Answer 1

For the reaction, $\underset{2V}{2N_2\left(g\right)}+\underset{1V}{O_2\left(g\right)}⟶\underset{2V}{2N_{2}O\left(g\right)}$
$\frac{45.4}{22.7}=2\frac{22.7}{22.7}=1\frac{45.4}{22.7}=2$

Hence, the ratio between the volumes of the reactants and the product in the given question is simple i.e., 2 : 1 : 2. It proves the Gay-Lucssac's law of gaseous volumes.

Note Gay - Lussac's law of gaseous volumes, when gases combine or are produced in a chemical reaction, they do so in a simple ratio by volume provided all gases are at same temperature and pressure.

Gay - Lussac's discovery of the integer ratio in the volume relationship is actually the law of definite proportion. The law of definite proportion with respect to the mass.