Kinetic Molecular Theory of Gases

By what factor does the average velocity of a gaseous molecule increase when the temperature (in Kelvin) is doubled ?

If a gas expands at constant temperature, it indicated that:

Which of the following expressions correctly represents the relationship between the average molar kinetic energy  $\overline{KE}ofCOand{N}_2$ molecules at the same temperature ?

At STP, $0.50\text{mole}$  ${\mathrm{H}}_2$ gas and $\mathrm{1}.0\text{mole}\mathrm{He}$ gas

Which of the following is not true in case of an ideal gas ?

The root mean square speeds at STP for the gases  $H_2,N_2,O_{2}andHBr$ are in the order:

At what temperature (in kelvin) is the rms speed of hydrogen molecules the same as oxygen molecules at $1327\text{℃}$?

Which gas among the following is the easiest to liquify?

Among the following, identify the gas which has the greatest average speed of its molecules?

The Kinetic energy of one mole of any gas depends upon ______

At what temperature will the total kinetic energy of $0.30$ moles of $\mathrm{He}$ be same as the total kinetic energy of $0.40$ moles of $\mathrm{Ar}$ at $400 \mathrm{K} ?$

At what temperature (in kelvin) is the rms speed of hydrogen molecules the same as oxygen molecules at $1327\text{℃}$?

The average velocity (in cm/s) of hydrogen molecule at $27°\mathrm{C}$ will be

Which is not true in case of an ideal gas?

In a closed flask of 5 L, 1.0 g of ${\mathrm{H}}_2$ is heated from 300 to 600 K. Which option is incorrect?

The average root-mean-square speed of molecules in a sample of oxygen gas at $300 \mathrm{K}$ is $484 \mathrm{m} {\mathrm{s}}^{-1}$, respectively. The corresponding value at $600 \mathrm{K}$ is nearly (assuming ideal gas behaviour)

At what temperature (in kelvin) is the rms speed of hydrogen molecules the same as oxygen molecules at $1327\text{℃}$?

 On applying the pressure, the intermolecular spaces can be reduced. This assumption explains the

The theory that attempts to elucidate the behaviour of gases is known as of gases.