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Answers without the blur. Sign up and see all textbooks for free! Q. 1.18

Expert-verified Found in: Page 13 ### An Introduction to Thermal Physics

Book edition 1st
Author(s) Daniel V. Schroeder
Pages 356 pages
ISBN 9780201380279 # Calculate the rms speed of a nitrogen molecule at room temperature.

Root mean square speed is 515.9m/s.

See the step by step solution

## Step1: Given information

Gas is Nitrogen.

Temp = room temp = 25oC= 298 K

## Step2: Explanation

The root mean square velocity is calculated as

$v=\sqrt{\frac{3kT}{m}}............................\left(1\right)$

where

T = temperature

k = Boltzmann constant

m = mass

Mass of Nitrogen is calculated as

$m=28\mathrm{u}\phantom{\rule{0ex}{0ex}}=28×1.6×{10}^{-27}\mathrm{kg}\phantom{\rule{0ex}{0ex}}=4.65×{10}^{-26}\mathrm{kg}$

Boltzmann constant is $=1.38×{10}^{-23}{\mathrm{m}}^{2}{\mathrm{kgs}}^{-2}{\mathrm{K}}^{-1}$

Substitute the values in equation (1), we get

$v=\sqrt{\frac{3×\left(1.38×{10}^{-23}{m}^{2}kg{s}^{-2}{K}^{-1}\right)×\left(298K\right)}{4.65×{10}^{-26}kg}}\phantom{\rule{0ex}{0ex}}v=515.9{\mathrm{ms}}^{-1}$

Root mean square speed is 515.9m/s. ### Want to see more solutions like these? 