45.6 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(g))+O_(2(g)) rarr 2N_(2)O_((g))`
Which law is being obeyed in this experiment ? Write the statement of the law ?

Explanation

For the reaction, `{:(2N_(2(g)),+,O_(2(g)),rarr,2N_(2)O_((g)),,),(2V,,1V,,2V,,):}`
`(45.4)/(22.7)=2 (22.7)/(22.7)= 1 (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 follows the Gay-Lussac.s law of gaseous solution.
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.