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Consider the decomposition equilibrium for dinitrogen pentoxide: 2 N 2 O 5 ( g ) ⇌ 4 NO 2 ( g ) + O 2 ( g ) At a certain temperature and a total pressure of 1.00 atm, the N 2 O 5 is 0.50% decomposed (by moles) at equilibrium. a . If the volume is increased by a factor of 10.0. will the mole percent of N 2 O 5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N 2 O 5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.

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Chemistry: An Atoms First Approach

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

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 12, Problem 108CP
Textbook Problem
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Consider the decomposition equilibrium for dinitrogen pentoxide:

2 N 2 O 5 ( g ) 4 NO 2 ( g ) + O 2 ( g )

At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium.

a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer.

b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.

(a)

Interpretation Introduction

Interpretation: For the given decomposition equilibrium reaction if the volume increased by a factor of 10 then the effect on mole percent is to be stated and explained. The decomposed mole percent of N2O5 at equilibrium is to be calculated.

Concept introduction: The equilibrium constant K describes the ratio of the reactant to the product on the equilibrium conditions in terms of molar concentration.

The equilibrium constant depends upon temperature.

Law of mass action is applicable on the equilibrium reactions.

The Le Chatelier’s principle states that the addition of the reactants shifts the equilibrium to the right while the addition of product shifts the equilibrium to the left at constant temperature.

To determine: The effect on mole percent of N2O5 if volume is increased by a factor of 10.

Explanation of Solution

Explanation

Given

The reaction is given as,

2N2O5(g)4NO2(g)+O2(g)

The pressure at equilibrium is 1.00atm . The decomposed moles at equilibrium is 0.50%

In the given reaction the number of moles of reactants is two and number of moles of products is five. According to the given condition if the volume of gaseous reaction is increased, the pressure of gaseous molecules will decrease. Therefore, the effect of increase of volume is equivalent to the effect of decrease of pressure.

If the pressure is decreased then according to the Le Chatelier’s principle, the equilibrium shifts in the direction which nullifies the effect of pressure that is increase the number of moles

(b)

Interpretation Introduction

Interpretation: For the given decomposition equilibrium reaction if the volume increased by a factor of 10 then the effect on mole percent is to be stated and explained. The decomposed mole percent of N2O5 at equilibrium is to be calculated.

Concept introduction: The equilibrium constant K describes the ratio of the reactant to the product on the equilibrium conditions in terms of molar concentration.

The equilibrium constant depends upon temperature.

Law of mass action is applicable on the equilibrium reactions.

The Le Chatelier’s principle states that the addition of the reactants shifts the equilibrium to the right while the addition of product shifts the equilibrium to the left at constant temperature.

To determine: The decomposed mole percent of N2O5 at equilibrium if volume is increased by a factor of 10.

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Chapter 12 Solutions

Chemistry: An Atoms First Approach
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