Avogadro's hypothesis:-
Consider two samples A and B of the gases each having volume V and pressure p.
Let m1 and m2 be the mass of each molecule of gas A and gas B respectively. N1 and N2 be the number of molecules of gas A and B respectively.
According to kinetic theory
p = {1mN}/{3V}C2 ....(i)
Therefore, for gas A, p = 1/3 {m1N1}/{V} C21,
where C1 = r.m.s. velocity of the molecules of gas A.
And for gas B, p = 1/3 {m2N2}/{V}C22 ....(ii)
where C2 = r.m.s. velocity of the molecule of gas B.
From (i) and (ii),
1/3 {m1N1}/{V} C12 = 1/3 {m2N2}/{V}C22
or, m1N1C12 = m2N2C22 ....(iii)
If the temperature of gas A and gas B is same, then their average K.E./ molecule is also same.
Thus, 1/2 m1C12 = 1/2 m2C22
or, m1C12 = m2C22 ...(iv)
Dividing (iii) by (iv), we have
N1 = N2 (Avogadro's hyppothesis)
Thus, equal volumes of all gases under similar conditions of temperature and pressure have the same number of molecules.