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The rms velocity of hydrogen is \( \sqrt{7} \) times the \( \mathrm{rms} \)
P velocity of nitrogen. If \( T \) is the temperature of the gas:

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(1) \( \mathrm{T}\left(\mathrm{H}_{2}\right)=\mathrm{T}\left(\mathrm{N}_{2}\right) \)
(2) \( \mathrm{T}\left(\mathrm{H}_{2}\right)\mathrm{T}\left(\mathrm{N}_{2}\right) \)
(3) \( \mathrm{T}\left(\mathrm{H}_{2}\right)\mathrm{T}\left(\mathrm{N}_{2}\right) \)
(4) \( \mathrm{T}\left(\mathrm{H}_{2}\right)=\sqrt{7} \mathrm{~T}\left(\mathrm{~N}_{2}\right) \)
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