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(A) The average kinetic energy per molecule of an ideal gas is given by the formula: $K = \frac{3}{2} kT$,where $k$ is the Boltzmann constant and $T$

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(A) The average kinetic energy per molecule of an ideal gas is given by the formula: $K = \frac{3}{2} kT$,where $k$ is the Boltzmann constant and $T$ is the absolute temperature.Since both gases are in the same flask,they are at the same temperature $T = 30^{\circ} C = 303 	ext{ K}$.The average kinetic energy per molecule depends only on the temperature of the gas and is independent of the mass or the nature of the gas molecules.Therefore,the ratio of the average kinetic energy per molecule of Argon to that of Hydrogen is:$\frac{K_{	ext{argon}}}{K_{	ext{hydrogen}}} = \frac{\frac{3}{2} kT}{\frac{3}{2} kT} = 1$.

$A$ flask contains Hydrogen and Argon in the ratio $2:1$ by mass. The temperature of the mixture is $30^{\circ} C$. The ratio of average kinetic energy per molecule of the two gases $(K_{\text{argon}} / K_{\text{hydrogen}})$ is: (Given: Atomic weight of $Ar = 39.9$)

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