Calculate rms speed (MM of CO is 28.01 g/mol):

$\overline{){{\mathbf{\mu}}}_{{\mathbf{rms}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\sqrt{\frac{\mathbf{3}\mathbf{RT}}{\mathbf{M}}}}\phantom{\rule{0ex}{0ex}}{\mathbf{\mu}}_{\mathbf{rms}}\mathbf{}\mathbf{=}\mathbf{}\sqrt{\frac{\mathbf{3}\mathbf{(}\mathbf{8}\mathbf{.}\mathbf{314}\mathbf{}{\displaystyle \frac{\mathbf{J}}{\overline{)\mathbf{mol}}\mathbf{}\overline{)\mathbf{K}}}}\mathbf{)}\mathbf{(}\mathbf{315}\mathbf{}\overline{)\mathbf{K}}\mathbf{)}}{(28.01\overline{){\displaystyle \frac{g}{\mathrm{mol}}}})\left({\displaystyle \frac{1\mathrm{kg}}{1x{10}^{3}\overline{)g}}}\right)}}$

Calculate the rms speed of CO molecules at 315 K .

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Our tutors have indicated that to solve this problem you will need to apply the Root Mean Square Speed concept. You can view video lessons to learn Root Mean Square Speed. Or if you need more Root Mean Square Speed practice, you can also practice Root Mean Square Speed practice problems.

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Based on our data, we think this problem is relevant for Professor Bindell's class at UCF.