The ratio between the RMS velocity of N_2 at | vedclass

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(D) The formula for $RMS$ velocity is $v_{rms} = \sqrt{\frac{3RT}{M}}$.Here, $R$ is the molar gas constant, $T$ is the temperature in Kelvin, and $M$

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$0.5$

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(D) The formula for $RMS$ velocity is $v_{rms} = \sqrt{\frac{3RT}{M}}$.Here, $R$ is the molar gas constant, $T$ is the temperature in Kelvin, and $M$ is the molar mass.Given $M_{(N_2)} = 28 \ g \ mol^{-1}$ and $M_{(CO)} = 28 \ g \ mol^{-1}$.Since the molar masses are equal, the ratio of $RMS$ velocities depends only on the square root of the temperatures:$\frac{v_{rms}(N_2)}{v_{rms}(CO)} = \sqrt{\frac{T_{(N_2)}}{T_{(CO)}}} = \sqrt{\frac{200}{800}}$.$\frac{v_{rms}(N_2)}{v_{rms}(CO)} = \sqrt{\frac{1}{4}} = \frac{1}{2} = 0.5$.

The ratio between the $RMS$ velocity of $N_2$ at $200 \ K$ and that of $CO$ at $800 \ K$ is (molecular mass of $N_2 = 28 \ g \ mol^{-1}$, molecular mass of $CO = 28 \ g \ mol^{-1}$)

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