Kinetic Theory ...

The average energy per molecule of a triatomic gas at room temperature T is?

The value of universal gas constant is $$8.3\ J/mole/K$$, the mean kinetic energy of $$32gm$$ of oxygen at $$-73^oC$$ will be

The lowest pressure (the best vaccum) that can be created in laboratory at $$20^{\circ}C$$ is $$10^{-10}\ mm$$ of $$Hg$$. At this pressure, the number of ideal gas molecules per $$cm^{3}$$ will be

Under which of the following conditions is the law $$pV=RT$$ obeyed most closely by a real gas?

The S.I. unit of universal gas constant is

Which of the following is correct?
(Internal pressure in Van der Waal's equation)

Two gases, carbon monoxide $$(CO)$$ and nitrogen $$(N_2)$$ at the same temperature, have kinetic energies $$E_1$$ and $$E_2$$ respectively. Then :

At room temperature (27$$^0$$ C) the rms speed of the moleculesof certain diatomic gas is found to be 1920 ms$$^{-1}$$ then the molecule is:

At what temperature does the average transnational kinetic energy of a molecule in a gas become equal to kinetic energy of an electron accelerated from rest through a potential difference of $$1$$ volt? ($$k=1.38 \times 10^{-23}J/K)$$

Gas exerts pressure on the walls of container because the molecules-