Solved Examples on Avogadro’s Law
Example 1: A puncture takes away half of the volume of a tire with 10 moles of air and a 40-liter volume. How much air is left in a tire that has been deflated?
Solution:
We know, V1/n1 = V2/n2
Here, initial volume = V1 = 40L
Initial number of moles = n1 = 10mole
Final volume= V2 = 20L
Final number of moles = n2 = x mole
Now, putting these values we get,
40/10 = 20/x
⇒ x = (20 ✖ 10)/40 = 200/40
⇒ x = 5mole
Example 2: 5L of gas is known to contain 0.90 mol. If the amount of gas is increased to 1.80 mol, what will be the new volume(at a constant temperature and pressure)?
Solution:
We know V1/n1 = V2/n2
Initial volume = V1 = 5L
Initial no. of moles = n1 = 0.90mole
Final volume = V2 = x L
Final no. of moles = n2 = 1.80mole
Now, putting these values we get,
5 ✖ 1.80 = x ✖ 0.90
⇒x = 10L
Avogadro’s Law
Avogadro’s Law was invented by Amedeo Carlo Avogadro in 1811. He was an Italian chemist and mathematician physicist. He said that, at constant temperature and pressure, two different ideal gases with similar volumes must contain an equal number of molecules. This law can be derived from the ideal gas equation.
In this article, we will discuss Avogadro’s law, its formula, derivation, application, and other aspects facts related to it in detail.