For a fixed number of moles of a gas at constant volume,the pressure of the gas increases with an increase in temperature because....

For a fixed number of moles of a gas at constant volume,the pressure of the gas increases with a rise in temperature due to:

Assertion $(A)$ At $300 \ K$,kinetic energy of $16 \ g$ of methane is equal to the kinetic energy of $32 \ g$ of oxygen.
Reason $(R)$ At constant temperature,kinetic energy of one mole of all gases is equal.

The mass of molecule $A$ is half the mass of molecule $B$. The $rms$ speed of $A$ is twice the $rms$ speed of $B$. If two samples of $A$ and $B$ contain the same number of molecules and are taken in two separate containers of equal volume,what will be the ratio of the pressure of $A$ to the pressure of $B$ $(P_A/P_B)$?

At $T$ $K$,the ratio of kinetic energies of $4$ $g$ of $H_{2(g)}$ and $8$ $g$ of $O_{2(g)}$ is

Which is not true in case of an ideal gas?