At identical temperatures, the rms speed of hydrogen molecules is $4$ times that for oxygen molecules. In a mixture of these in mass ratio $H_{2} : O_{2} = 1 : 8$ , the rms speed of all molecules is n times the rms speed of $O_{2}$ , molecules, where n is

3

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\frac{4}{3}

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{(\frac{8}{3})}^{1 / 2}

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(11)^{1 / 2}

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Solution

The correct option is D $(11)^{1 / 2}$
Molecule number ratio in the mixture is $H_{2} : O_{2} = \frac{1}{2} : \frac{8}{32}$
$= \frac{2}{3} : \frac{1}{3}$
Thus $c_{r m s}^{2} = 16 (\frac{2}{3}) + 1 (\frac{1}{3})$ times that of oxygen.
$⟹ c_{r m s} = \sqrt{11}$ times that of oxygen.

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At identical temperatures, the rms speed of hydrogen molecules is 4 times that for oxygen molecules. In a mixture of these in mass ratio H2:O2=1:8 , the rms speed of all molecules is n times the rms speed of O2, molecules, where n is

The correct option is D (11)1/2Molecule number ratio in the mixture is H2:O2=12:832=23:13Thus c2rms=16(23)+1(13) times that of oxygen.⟹crms=√11 times that of oxygen.

At identical temperatures, the rms speed of hydrogen molecules is $4$ times that for oxygen molecules. In a mixture of these in mass ratio $H_{2} : O_{2} = 1 : 8$ , the rms speed of all molecules is n times the rms speed of $O_{2}$ , molecules, where n is

The correct option is D $(11)^{1 / 2}$
Molecule number ratio in the mixture is $H_{2} : O_{2} = \frac{1}{2} : \frac{8}{32}$
$= \frac{2}{3} : \frac{1}{3}$
Thus $c_{r m s}^{2} = 16 (\frac{2}{3}) + 1 (\frac{1}{3})$ times that of oxygen.
$⟹ c_{r m s} = \sqrt{11}$ times that of oxygen.