Question

Which of the following is not true about ideal gas molecules?

They do not have attractive forces
They move in random motion
They do not apply pressure
They have negligible size
All of these​

Answer 1

The most suitable option is C as ideal gases exert pressure.

What is an ideal gas?

• An ideal gas is one in which there are no attractive forces between the gas molecules.
• All the collisions between the atoms and molecules of these forces are 100% elastic.
• These gases do not have intermolecular attractions and the pressure they exert is directly proportional to the temperature.  

So, we conclude that statement c is not true about ideal gases.

Answer 2

The option which is not true about ideal gas molecules is that they do not apply pressure (3rd option).

• The ideal gas is a hypothetical gas that is claimed to have all of the properties of the ideal gas law.
• There are no interparticle forces of attraction or repulsion amongst ideal gas molecules.
• They travel at random and collide precisely elastically.
• Because gas molecules are point-sized particles, they are regarded to be of an insignificant size and have no volume of their own.
• They do, however, impose pressure that is temperature-dependent and can be estimated using the ideal gas equation PV=nRT (P= Pressure; V= Volume; n= moles of gas; R= gas constant; T= Temperature).
• As a result, the statement that perfect gas molecules do not exert pressure is incorrect.