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(A) The root mean square $(rms)$ velocity of a gas molecule is given by the formula $v_{rms} = \sqrt{\frac{3RT}{M}}$,where $R$ is the universal gas co

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$H_2$ has a higher $rms$ velocity.

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(A) The root mean square $(rms)$ velocity of a gas molecule is given by the formula $v_{rms} = \sqrt{\frac{3RT}{M}}$,where $R$ is the universal gas constant,$T$ is the absolute temperature,and $M$ is the molar mass of the gas.Since the temperature $T$ is the same for both gases,$v_{rms} \propto \frac{1}{\sqrt{M}}$.The molar mass of $H_2$ $(M_{H_2} = 2 \ g/mol)$ is much smaller than the molar mass of $O_2$ $(M_{O_2} = 32 \ g/mol)$.Therefore,$v_{rms}$ of $H_2$ is greater than $v_{rms}$ of $O_2$.Regarding average kinetic energy,the formula is $K_{avg} = \frac{3}{2}kT$,which depends only on temperature. Since both gases are at the same temperature,their average kinetic energies are equal.

If a container is filled with a mixture of $H_2$ and $O_2$ gases at the same temperature,then:

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