CHEMISTRY >CUSTOM<
CHEMISTRY >CUSTOM<
14th Edition
ISBN: 9781259137815
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 24, Problem 79QP
Interpretation Introduction

Interpretation:

The volume of chlorine gas required to oxidize all the bromide ions is to be calculated.

Concept introduction:

A balanced chemical equation must contain an equal number of similar atoms on each side.

The ideal gas equation is given as follows:

PV=nRT

Here, P,V,n,R,andT are pressure, volume, number of moles, gas constant, and temperature, respectively.

The moles of a substance are calculated by the ratio of the mass of the substance to the molar mass of the substance.

Number of moles = Given massMolar mass

The mass of compound can be calculated as: m=n×M

Here, n is the number of moles, m is the mass, and M is the molar mass.

The number of moles of chlorine needed is calculated as:

number of moles of chlorine = givenmassofbrominemolarmassofbromine×1molchlorine2molbromine

Expert Solution & Answer
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Answer to Problem 79QP

Solution: 25.3L

Explanation of Solution

The balanced chemical reaction is as follows:

2Br(g) + Cl2(g) 2Cl(aq) + Br2(l)

2molesofbrominereactswith1moleofchlorine

The number of moles of chlorine needed is calculated as follows:

number of moles of chlorine = givenmassofbrominemolarmassofbromine×1molchlorine2molbromine

(167gBr)×(1molBr79.90gBr)×(1molCl22molBr)=1.05molCl2(g)

The volume of chlorine gas needed is calculated by using the ideal gas equation as follows:

VCl2=nRTP=(1.05mol)(0.0821atm/K×mol)(293K)(1atm)25.3L

Conclusion

The volume of chlorine gas required to oxidize all the bromide ions is 25.3 L.

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Chapter 24 Solutions

CHEMISTRY >CUSTOM<

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