The energy of a gas per litre is $300 \ J$. Then its pressure will be:

The average translational kinetic energy of a hydrogen gas molecule at $NTP$ will be. [Boltzmann's constant $k_B = 1.38 \times 10^{-23} \text{ J/K}$]

The pressure of a gas is $6 \times 10^4 \ N/m^2$. What will be the kinetic energy per unit volume of the gas molecules?

$A$ gas is filled in a container at pressure ${P_0}$. If the mass of all molecules is halved and their $rms$ speed is doubled,what will be the new pressure?

If the average kinetic energy of $O_2$ (molar mass $32$) is $0.048 \ eV$,what is the average kinetic energy of $N_2$ (molar mass $28$) at the same temperature (in $eV$)?

Assertion $(A)$: The temperature of a gas is a result of the kinetic energy of its molecules.
Reason $(R)$: Due to kinetic energy,the molecules collide with each other to produce thermal energy.