Lecture 3 : Ideal gas equation ; Dalton’s law of partial pressure ; Kinetic molecular theory of gases

One of the assumptions of kinetic theory of gases is that there is no force of
attraction between the molecules of a gas.
State and explain the evidence that shows that the assumption is not applicable
for real gases.

Value of universal gas constant (R) is same for all gases. What is its physical
significance?

Two different gases ‘A’ and ‘B’ are filled in separate containers of equal capacity
under the same conditions of temperature and pressure. On increasing the
pressure slightly the gas ‘A’ liquefies but gas B does not liquify even on applying
high pressure until it is cooled. Explain this phenomenon.

What would be the SI unit for the quantity pV²T ²/n?

Pressure of 1 g of an ideal gas A at 27 °C is found to be 2 bar. When 2 g of another ideal gas B is introduced in the same flask at same temperature the pressure becomes 3 bar. Find a relationship between their molecular masses.

At 0°C, the density of a certain oxide of a gas at 2 bar is same as that of dinitrogen at 5 bar. What is the molecular mass of the oxide?