Pressure of an ideal gas is increased by keeping temperature constant. What is the effect on the kinetic energy of molecules?

The average translational kinetic energy of a molecule in a gas becomes equal to $0.69 \ eV$ at a temperature of about,[Boltzmann's constant $= 1.38 \times 10^{-23} \ J \ K^{-1}$] (in $^{\circ} C$)

Helium and argon are placed in a flask at the same room temperature $(300 \ K)$. What is the ratio of the average kinetic energies (per molecule) of helium and argon?

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

$A$ gas has volume $V$ and pressure $P$. The total translational kinetic energy of all the molecules of the gas is

If the temperature of a gas is increased from $27^{\circ}C$ to $927^{\circ}C$,what will be the change in its kinetic energy?