Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 10 - Gases - Exercises: 10.38b

Answer

1.96 x 10^19 molecules of CO2

Work Step by Step

We are given the volume (2L of sample), the pressure (1atm) and the temperature of the atmosphere (27C and then we add 273 to have 300K). We can then find the number of moles by using the ideal gas law: PV = nRT so n = PV/RT = (1atm * 2L) / (0.0821 * 300K) = 0.0812 moles Then to find the number of molecules, we multiply by Avogadro's number, 6.022 x 10^23, which gives 4.89 x 10^22 molecules. Since the atmosphere is 0.04% of the atmosphere we take 4.89 x 10^22 * (0.04/100) = 1.96 x 10^19 molecules of CO2
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