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The rms velocity of hydrogen is $\sqrt{7}$ times to that of nitrogen. If T is temperature of the gas, then

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answer is C.

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Detailed Solution

\large {\left( {{C_{RMs}}} \right)_{{H_2}}} = \sqrt 7 {\left( {{C_{RMS}}} \right)_{{N_2}}}

\large \sqrt{\frac{3RT_{H_{2}}}{2}}\;=\sqrt{7}\sqrt{\frac{3RT_{N_{2}}}{28}}

\large \frac{T_{H_{2}}}{2}\;=7\frac{T_{N_{2}}}{28}

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