Chemistry: An Atoms-Focused Approach
Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
Question
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Chapter 10, Problem 10.148QA
Interpretation Introduction

To find:

a. Whether the volume of gases collected can be used to distinguish the pathways of two reactions.

b. If the gas produced during thermal decomposition is N2O or a mixture of N2and O2.

Expert Solution & Answer
Check Mark

Answer to Problem 10.148QA

Solution:

a. The volume of gases collected can be used to distinguish the pathways of two reactions.

b. The gas produced during the thermal decomposition is  N2O gas.

Explanation of Solution

Explanation: 1) Concept:

a. The given two decomposition reactions at two different temperatures produce different number of moles of products. Using this information, we can say that the volume of gases collected can be used to distinguish the pathways of two reactions.

b. As the gaseous products are collected over water, we can get the number of moles of gaseous products N2 and O2 for the first reaction and N2O for the second reaction. Using the moles of gas, the given temperature, and pressure for both the reaction products, we can calculate the volume. If this volume is the same as that of the given volume, then we can determine whether it is N2O  or a mixture of N2 and O2.

2) Formula:  P×V=n×R×T      3) Given:

Reactions:

NH4NO3s3000C N2g+12O2g+2H2Og

NH4NO3s200-2600C N2Og+2H2Og

For part b)

i) mass of NH4NO3=0.256 g

ii) V=79 mL=0.0079 L

iii) T=200C

iv) P=760 mm Hg

v) R=0.08206 atm. L/(mol.K)

4) Calculations:

a. The decomposition of ammonium nitrate at 3000C, produces one mole of gaseous  N2, half mole of gaseous O2, and two moles of gaseous water. So, the total 3.5 moles of gaseous species produce at  3000C while the same reaction at 200-2600C produces one mole of gaseous N2O, and two moles of gaseous water. So, only 3 gaseous moles produced by this reaction at 200-2600C. Therefore, we can say that the volume of gases collected can be used to distinguish the pathways of two reactions

b. Finding which gas is produced.

T=200C=20+273 K=293 K

P=760 mm Hg=1 atm

Calculation for moles of NH4NO3

0.256 g NH4NO3×1 mol NH4NO380.04 g NH4NO3=0.003198 mol NH4NO3

For first reaction, the number of gaseous moles =1 mol N2+12mol of O2=1.5  moles of the mixture of  N2 and O2.

0.003198 mol NH4NO3×1.5 mol mixture of N2 and O21 mol NH4NO3

=0.004798 mol mixture of N2 and O2=n

Therefore, volume calculation for first reaction is

1 atm×V=0.004798 mol×0.08206 atm.Lmol.K×293 K

V=0.004798 mol×0.08206 atm.Lmol.K×293 K1 atm

V=0.115 L

For second reaction, n=1 mol of N2O,

0.003198 mol NH4NO3×1 mol N2O1 mol NH4NO3=0.003198 mol N2O=n

Therefore, volume calculation for second reaction is

1 atm×V=0.003198 mol×0.08206 atm.Lmol.K×293 K

V=0.0032 mol×0.08206 atm.Lmol.K×293 K1 atm

V=0.0769 L

Second reaction’s volume is nearly the same as the given volume. Therefore, the gas produced is N2O.

Conclusion:

a.  The number of the gaseous moles of the product are different for both the reaction. So we can say that their volumes collected can be used to distinguish their pathways.

b. The volume of the product produced by the given amount of ammonium nitrate can help to get which gas is produced.

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Chapter 10 Solutions

Chemistry: An Atoms-Focused Approach

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