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

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$1: 1$

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(B) The average kinetic energy per molecule of an ideal gas is given by the formula $K_{av} = \frac{3}{2} kT$,where $k$ is the Boltzmann constant and $T$ is the absolute temperature.Since both hydrogen and oxygen are in the same flask,they are at the same temperature $T = 27^{\circ} C = 300 \ K$.The average kinetic energy per molecule depends only on the temperature $T$ and is independent of the mass or the nature of the gas molecules.Therefore,the ratio of the average kinetic energy per molecule of hydrogen to that of oxygen is $\frac{K_{H_2}}{K_{O_2}} = \frac{\frac{3}{2} kT}{\frac{3}{2} kT} = 1: 1$.

$A$ flask contains hydrogen and oxygen in the ratio of $2: 1$ by mass at temperature $27^{\circ} C$. The ratio of average kinetic energy per molecule of hydrogen and oxygen respectively is:

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