   Chapter 13, Problem 154CP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
1 views

# large flask with a volume of 936 mL is evacuated and found to have a mass of 134 . 66 g . It is then filled to a pressure of 0. 967 am at 31  ° C with a gas of unknown molar mass and then reweighed to give a new mass of 135 . 87 g . What is the molar mass of this gas?

Interpretation Introduction

Interpretation:

To determine the molar mass of gas filled in the flask with the given information.

Concept Introduction:

Gases follow the ideal gas equation that shows the relation between pressure, volume and temperature. We can calculate any one of this property along with moles with the help of this equation.

PV = nRT.

Explanation

Given information:

Volume = 936 mL = 0.936 L

Pressure = 0.967 atm

Temperature = 31 Â°C = 31+273 = 304 K

The mass of gas must be calculated with the difference in the mass of flask and mass of gas. Then we have to use the ideal gas equation to calculate the molar mass of gas with the help of given temperature, pressure and volume.

Mass of gas = Mass of flask after filling the gas − Mass of empty flask

= 135.87 -134.66 = 1.21 g

Number of moles of gas = massmolar mass

Plug the values in the given ideal gas equation:

PV = nRT

0

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