Explanation As per the given information, a gaseous mixture made up of 106 g of cyclopropane, 12.2 g of chloroform and 5.23 g of methane is filled in a 78 L tank at 20 0 C . The whole pressure exerted by the gas mixture is the product of partial pressure of gas and its mole fraction: P t o t = X 1 P 1 Now, calculating the mole fraction using the following formula: X 1 = n 1 n t o t Again, calculating the mole number of cyclopropane: n C 3 H 6 = mass of C 3 H 6 molar mass ofC 3 H 6 = 10 .6 g 42 .08 g/mol =0 .252 mol Now, calculating the mole number of chloroform: n CHCl 3 = mass of CHCl 3 molar mass of CHCl 3 = 12 .2 g 119 .38 g/mol =0 .102 mol Again, calculating the mole number of methane: n CH 4 = mass of CH 4 molar mass of CH 4 = 5 .23 g 16 .04 g/mol =0 .326 mol The total number of moles of gas is calculated using the following formula: n total = n C 3 H 6 +n CHCl 3 +n CH 4 = 0 .252 mol+0 .102 mol+0

8th Edition

ISBN: 9781305079373

Author: William L. Masterton, Cecile N. Hurley

Publisher: Cengage Learning

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Question

Chapter 5, Problem 41QAP

Interpretation Introduction

Interpretation:

The pressure exerted by the gaseous mixture in a tank and the highest partial pressure of the gas needs to be calculated.

Concept introduction:

To solve the question, we have to use Dalton’s Law of partial pressure of gases.

Dalton’s Law of partial pressure of gases: The sum of the partial pressures exerted by a mixture of non-reacting gases is equal to the total pressure.

Expert Solution & Answer

Chapter 5 Solutions

Chemistry: Principles and Reactions

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