Explanation Given: Mass of flask = 143.187 g Volume of an evacuated flask = 255 mL = 255 1000 = 0.255 L Mass of flask after filled with an unknown gas = 143.289 g So, the final mass of the gas filled in the flask = 143.289 g - 143.187g = 0.102 g Pressure in the flask = 267 torr Temperature = 298K Calculation: As we know that 1 atm = 760 torr. Therefore, converting 267 torr to atmospheric units 267 torr × 1 atm 760 torr = 0.3513 atm Now here we have to identify the number of moles of gas obtained using the ideal gas equation → PV = nRT n = P × V R × T 0 ...

Modified Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: Structure and Properties (2nd Edition)

2nd Edition

ISBN: 9780134565613

Author: Nivaldo J. Tro

Publisher: PEARSON

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Chapter 10, Problem 97E

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To determine: The molar mass of the unknown gas.

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Chapter 10, Problem 96E

Chapter 10, Problem 98E

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Modified Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: Structure and Properties (2nd Edition)

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The molar mass of the unknown gas.

Solution Summary: The author explains how to determine the molar mass of the unknown gas using the ideal gas equation.

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To determine: The molar mass of the unknown gas.

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Chapter 10 Solutions