At the same temperature and pressure,which of the following gases will have the highest kinetic energy $(K.E)$ per mole?

Which of the following describes an ideal gas?
$(i)$ The volume occupied by a gas molecule is negligible.
$(ii)$ The collision between ideal gas molecules are elastic.
$(iii)$ Particles are very small compared to the distance between each other.

$A$ bottle of dry ammonia and a bottle of dry hydrogen chloride connected through a long tube are opened simultaneously at both ends. The white ammonium chloride ring first formed will be:

For a fixed amount of gas at constant volume,what is the reason for the increase in pressure with an increase in temperature?

Give two unfair assumptions of the Kinetic Molecular Theory of gases. Justify them.

The average kinetic energy of one molecule of an ideal gas at $27^{\circ} C$ and $1 \ atm$ pressure is