Question:

The gases show ideal behaviour when the volume occupied is large so that the volume of the molecules can be neglected in comparison to it. The behaviour of the gas becomes more ideal when pressure is very low.

Updated On: Jul 6, 2022

If both assertion and reason are true and reason is the correct explanation of assertion.
If both assertion and reason are true but reason is not the correct explanation of assertion.
If assertion is true but reason is false.
If both assertion and reason are false.

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The Correct Option is B

Solution and Explanation

For 1 mole of real gas, $\left(P+\frac{a}{V^{2}}\right)\left(V-b\right)=RT$ when $V$ is very large, the terms $b$ and $a/v^{2}$ are negligible and the van der Waals equation becomes ideal gas equation, $PV=RT$ hence, real gases behave like ideal gas.

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Notes on States of matter

Concepts Used:

States of Matter

The matter is made up of very tiny particles and these particles are so small that we cannot see them with naked eyes.

There are three States of Matter:

The three states of matter are as follows:

Solid State:

The solid-state is one of the fundamental states of matter.
Solids differ from liquids and gases by the characteristic of rigidity.
The molecules of solids are tightly packed because of strong intermolecular forces; they only oscillate about their mean positions.

Liquid State:

The molecules in a liquid are closely packed due to weak intermolecular forces.
These forces are weaker than solids but stronger than that of gases.
There is much space in between the molecules of liquids which makes their flowing ability easy.

Gaseous State:

In this state of matter, distances between the molecules are large (intermolecular distance is in the range of 10^-7-10^-5 cm.
The intermolecular forces experienced between them are negligible.
Thus, translatory, rotatory and vibratory motions are observed prominently in gases.