Find the average kinetic energy for $1$ gram-mole of a monatomic gas.

The energy (in $eV$) possessed by a neon atom at $77^{\circ} C$ is (Boltzmann constant,$K_{B} = 1.38 \times 10^{-23} \,J \,K^{-1}$)

At which of the following temperatures would the molecules of a gas have twice the average kinetic energy they have at $20^{\circ}C$ (in $^{\circ}C$)?

The temperature of a gas is $-73^{\circ}C$. To what temperature in $^{\circ}C$ should the gas be heated so that the average kinetic energy of its molecules becomes doubled?

$10^{23}$ molecules of a gas, each having a mass of $3 \times 10^{-27} \,kg$, strike per second per $cm^2$ of a rigid wall at an angle of $60^{\circ}$ with the normal and rebound with a velocity of $500 \,m/s$. The pressure exerted by the gas molecules on the wall is: (in $\,N/m^2$)

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