Chemistry: The Central Science (13th Edition)

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

Chapter 10 - Gases - Exercises: 10.54

Answer

74 g/mol

Work Step by Step

We are given that the mass of vapor is0.846g, the volume of the bulb is 354 $cm^3$, the pressure is 752 torr and the temperature is 100C. To find the molar mass, we can use the formula M = dRT/P, but first we need to find the density. Given that 0.846g takes up a volume of 354$cm^3$ we need to convert the 354 $cm^3$ in to Liters. Given that a cubic centimeter, or cc ($cm^3$) is equivalent to a mL, then we have 354mL, which is 0.354L. Then we have 0.846g/0.354L =2.390g/L. We now convert the pressure from torr to atm: 752 torr * (1 atm/ 760torr) = 0.989 atm and the temperature to Kelvin by adding 273, which is 373K Last we have M = dRT/P = (2.390 g/L * 0.0821 * 373K) / 0.989 atm = 74 g/mol
Update this answer!

You can help us out by revising, improving and updating this answer.

Update this answer

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.