Problem: Calculate the root mean square velocities of CH4(g) and N2(g) molecules at 273 K and 546 K.

root mean square speed (C_rms):

$C_{rms} = \sqrt{\frac{3 RT}{M}}$

µ_rms = rms speed,
R = 8.314 J/(mol·K)
T = temperature, K
M = molar mass, kg/mol

MM of CH₄ → 16.04 g/mol

MM of N₂ → 28 g/mol

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Calculate the root mean square velocities of CH₄(g) and N₂(g) molecules at 273 K and 546 K.

What scientific concept do you need to know in order to solve this problem?

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 Antonacci's class at SHU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.