   # As NH 3 (g) is decomposed into nitrogen gas and hydrogen gas at constant pressure and temperature, the volume of the product gases collected is twice the volume of NH 3 reacted. Explain. As NH 3 (g) is decomposed into nitrogen gas and hydrogen gas at constant volume and temperature, the total pressure increases by some factor. Why the increase in pressure and by what factor does the total pressure increase when reactants are completely converted into products? How do the partial pressures of the product gases compare to each other and to the initial pressure of NH 3 ? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 8, Problem 31Q
Textbook Problem
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## As NH3(g) is decomposed into nitrogen gas and hydrogen gas at constant pressure and temperature, the volume of the product gases collected is twice the volume of NH3 reacted. Explain. As NH3(g) is decomposed into nitrogen gas and hydrogen gas at constant volume and temperature, the total pressure increases by some factor. Why the increase in pressure and by what factor does the total pressure increase when reactants are completely converted into products? How do the partial pressures of the product gases compare to each other and to the initial pressure of NH3?

Interpretation Introduction

Interpretation:

For the given decomposition reaction of NH3 the volume of product gases is twice the volume of NH3 at constant pressure and temperature should be explained, the increment of total pressure at constant volume and temperature after the completion reaction should be determine and explain the reason for increment and the comparison between the partial pressures of product gases and initial pressure of NH3 should be determined.

Concept introduction:

• Balanced equation of a reaction is written according to law of conservation of mass.
• According to Avogadro’s law of gas molecules,

If the number of moles of gases in a container is increased then the volume will increase at constant temperature and pressure.

Vinitialninitial=Vfinalnfinal

• According to ideal gas law: the pressure of gas is directly proportional to the number of moles of gas at constant volume and temperature.

Pn=RTV, P and n are proportional.

Mathematically, for two gases (1 and 2) at constant V and T,

P1n1=P2n2P1P2=n1n2

• Mole ratios between the reactant and products of a reaction are depends upon the coefficients of respective reactant in a balanced chemical equation.
• Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone.

### Explanation of Solution

Explanation

The decomposition reaction of NH3 is producing N2 and H2 gases.

Therefore,

The chemical equation of the reaction given is,

NH3N2+H2

This equation is not balanced, Balanced equation is the chemical equation of a reaction which is written according to law of conservation of mass the mass of reactant molecules should conserve in product molecules.

The balanced chemical equation of the given reaction is,

Balance the molecules in both sides of arrow in order of atoms other than hydrogen then hydrogen atoms.

Therefore, the balanced chemical equation of the given decomposition reaction of NH3 will be,

2NH3N2+3H2

Hence,

The balanced chemical equation for the given decomposition reaction of NH3 is, 2NH3N2+3H2.

By using Avogadro’s law of gas molecules, if the number of moles of product gases as compared to reactants is doubled, then the volume will be doubled at constant pressure and temperature.

The balanced chemical equation for the given decomposition reaction of NH3 is, 2NH3N2+3H2.

Here 2 mole of NH3 is producing 1 mole of N2 and 3 mole of H2. That means, in initial 2 moles of molecules are presented and at final 1+3=4 moles molecules are produced.

According to Avogadro’s law of gas molecules,

If the number of moles of gases in a container is increased then the volume will increase at constant temperature and pressure.

Vinitialninitial=Vfinalnfinal

Therefore,

For the given decomposition reaction of NH3,

VinitialVfinal=ninitialnfinal2mol4mol=12

Hence,

By using Avogadro’s law of gas molecules, if the number of moles of product gases as compared to reactants is doubled, then the volume will be doubled at constant pressure and temperature.

By using ideal gas equation, the total pressure at constant volume and temperature after the completion of reaction will be doubled because the number of moles of product gases as compared to reactants is doubled.

The balanced chemical equation for the given decomposition reaction of NH3 is, 2NH3N2+3H2.

Here 2 mole of NH3 is producing 1 mole of N2 and 3 mole of H2. That means, in initial 2 moles of molecules are presented and at final 1+3=4 moles molecules are produced.

The reaction is at constant volume and temperature.

According to ideal gas law, the pressure of gas is directly proportional to the number of moles of gas at constant volume and temperature.

Pn=RTV, P and n are proportional.

Mathematically, for two gases (1 and 2) at constant V and T,

P1n1=P2n2P1P2=n1n2

Therefore,

For the given decomposition reaction of NH3,

PinitialPfinal=ninitialnfinal=2mol4mol=12

Hence, by using ideal gas equation, the total pressure at constant volume and temperature after the completion of reaction will be doubled because the number of moles of product gases as compared to reactants is doubled

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