Physics: Principles with Applications (7th Edition)

Published by Pearson
ISBN 10: 0-32162-592-7
ISBN 13: 978-0-32162-592-2

Chapter 13 - Temperature and Kinetic Theory - Problems - Page 386: 27

Answer

a. 22.8 cubic meters. b. $2.15\times10^5\;Pa$.

Work Step by Step

a. Find the number of moles of nitrogen in 28.5 kg. $$n=\frac{28.5\;kg}{28.0\times10^{-3}kg/mol}=1018\;mol$$ Use the ideal gas model for nitrogen to calculate the volume of the gas. $$V=\frac{nRT}{P}=\frac{(1018\;mol)(8.314)(273\;K)}{1.013\times10^5\;Pa}\approx 22.8\;m^3$$ b. Find the new number of moles. $$n=\frac{28.5+32.2\;kg}{28.0\times10^{-3}kg/mol}=2168\;mol$$ Use the ideal gas model for nitrogen to calculate the pressure of the gas. $$P=\frac{nRT}{V}=\frac{(2168\;mol)(8.314)(273\;K)}{22.8\;m^3 }\approx 2.15\times10^5\;Pa $$
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