Question

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

2N2 (g) + O2 (g) -----------> 2N2O (g)

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

Answer 1

This experiment follows the Gay Lussac law.

Explanation:

Chemical equation:

2N₂ +  O₂   →   2N₂O

According to this law when gases are combined and undergo a chemical reaction in a simple whole number ratio by volume at the same temperature and pressure.

Mathematical expression:

V ∝ number of moles

The given reaction completely follow the Gay Lussac law. In this reaction dinitrogen and dioxygen combine to produce nitrous oxide at the same temperature and pressure. The two mole of dinitrogen and one mole of dioxygen combined and gives two mole of nitrous oxide followed  by the volume 45.4 L, 22.7 L and 45.4 L respectively. The ratio is 2 :1 :2 which is the simple whole number.

Answer 2

Answer:

Explanation:

2N2 (g) + O2 (g) -----------> 2N2O (g)

Gay lussac's law is being obeyed.