how gases don't have a fix volume, inspite that if we put it in a container than it will occupy that container fully ?

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Solution

The volume of container is fixed not gas. If we put same amount of gas in slightly bigger or smaller container then even the volume of gas would changed according to container. Because we are weighing the container.
Why volume of gas is not fixed ? Because gas has no fixed shape and volume. It occupies the shape of container hence volume changed accordingly.
Now in chemistry at higher level we specify the gas by number of moles, pressure volume and temperature. That is why 1 moles of any gas occupies a volume of 22.4 L at STP occupies .

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According to Avogadro's Law, "Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules". But how is this statement correct? How do we know that equal number of molecules are present in two gases taken in equal volumes?

Even if we consider equal volumes of any two gases(let's consider two gases for example) contain equal number of molecules, if we have the two gases in two containers of same volumes, we can add more gas to any one container and increase the density of the gas inside the container. In that case, the volume of the gas remains equal to the volume of the container but the number of gas molecules inside the container has increased and there is no chage to the number of molecules of the other gas we took inside a similar container. So now we have equal volumes of two gases but we have increased the number of molecules of one gas so now how can we say that the equal volumes of these two gases contain equal number of molecules?

If we take equal number of molecules of two gases and contain one of the gas in a container of some volume and the other gas in a container of a different volume, we will have unequal volumes of two gases having equal number of particles.

So how is Avogadro's Law explained?

Q. Two gases occupy two containers A and B the gas in A, of volume