We say that due to repulsive force present in real gases,volume occupied by the molecule is more than ideal gas that is,correction factor is given by (V-nb)but if we consider attractive force b/w the molecules it should actually pull the molecules and decrease its volume right but we dont consider attractive forces at all, why??

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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?

Assertion: Real gases do not obey the ideal gas equation.

Reason: In the ideal gas equation, the volume occupied by the molecules as well as the inter molecular forces are ignored.

Q. A gas at 350 K and 15 bar has molar volume 20 percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor (Z) is:

Q. Assertion :In van der Waals equation

[P + \frac{a}{V^{2}}] (V - b) = R T

pressure correction

(a / V^{2})

is due to the force of attraction between molecules. Reason: Volume of gas molecule cannot be neglected due to force of attraction.

Q. Consider the following statements.
I. Repulsive forces are significant when the molecules are close together on average.
II. Attractive intermolecular forces are important when the molecules are fairly close together but not necessarily touching.
III. Attractive forces are ineffective when the molecules arc for apart.
Select correct statements.

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