Chemistry: The Central Science (13th Edition)

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

Chapter 10 - Gases - Exercises: 10.39a


91.22 atm

Work Step by Step

We are given the mass of Oxygen in kg so we must first convert this to moles to be able to use the ideal gas law. The molar mass of O2 is 2 * 16 = 32 g/mol. This means we have: 0.29kg * (1000g/1kg) * (1mol/32g) = 9.0625 moles We are told the volume is 2.3L and the temperature is 9C (we add 273 to find Kelvin) or 282K. We can then use ideal gas law to find the pressure: PV = nRT so P = nRT/V = (9.0625 moles * 0.0821 * 282K) / 2.3L = 91.22 atm
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