Introductory Chemistry (5th Edition)

Published by Pearson
ISBN 10: 032191029X
ISBN 13: 978-0-32191-029-5

Chapter 11 - Gases - Exercises - Problems - Page 403: 63


There are $1.444 mols$ of the gas.

Work Step by Step

Using the ideal gas law $PV = nRT$ where "P" is the pressure the gas exerts, "V" is the volume the gas occupies, "n" represents the number of moles of the gas, "R" is the ideal gas constant and "T" represents the temperature, we can solve many gaseous questions that behave in ideal conditions. In this question we must also convert the pressure from "psi" to atm since the gas constant we are using is in terms of atm from the conversion factor below: $44 psi \times\frac{1 atm}{14.6959 psi} = 2.994 atm$ Also we must convert the temperature into Kelvin by simply adding 273.15 to the Celsius value: $T = 25^{\circ}C+273.15 = 298.15 K$ The question asks for $n$ so we must isolate for the volume from the ideal gas equation to obtain $n = \frac{PV}{RT}$ $n = \frac{2.994 atm \times 11.8 L}{298.15 K \times 0.08206 \frac{L\times atm}{mol\times K}} = 1.444 mols $
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