   # At a particular temperature, 12.0 moles of SO 3 is placed into a 3.0-L rigid container, and the SO 3 dissociates by the reaction 2 SO 3 ( g ) ⇌ 2 SO 2 ( g ) + O 2 ( g ) At equilibrium. 3.0 moles of SO 2 is present Calculate K for this reaction. ### 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 12, Problem 47E
Textbook Problem
1 views

## At a particular temperature, 12.0 moles of SO3 is placed into a 3.0-L rigid container, and the SO3 dissociates by the reaction 2 SO 3 ( g ) ⇌ 2 SO 2 ( g ) + O 2 ( g ) At equilibrium. 3.0 moles of SO2 is present Calculate K for this reaction.

Interpretation Introduction

Interpretation:  A 3.0L rigid container filled with 12.0moles of gaseous SO3 is given. The reaction that takes place is stated. The value of the equilibrium constant is to be calculated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction. When the equilibrium constant is expressed in terms of concentration, it is represented as K .

To determine: The equilibrium constant (K) for the given reaction.

### Explanation of Solution

Given

The stated reaction is,

2SO3(g)2SO2(g)+O2(g)

The volume of the container is 3.0L .

Initial moles of SO3 are 12.0moles .

The moles of SO2 present at equilibrium are 3.0moles .

At equilibrium, the equilibrium ratio is expressed by the formula,

K=ConcentrationofproductsConcentrationofreactants

Where,

• K is the equilibrium constant.

The equilibrium ratio for the given reaction is,

K=[SO2]2[O2][SO3]2 (1)

The concentration of a reactant is calculated by the formula,

Concentration=MolesVolume(L)

The initial concentration of SO3 is calculated by the formula,

Substitute the given values of the number of moles of SO3 and the volume of the flask in the above expression.

InitialconcentrationofSO3=12moles3.0L=4.0M

The initial concentration of SO2 and O2 is zero.

The number of moles of SO3 consumed are assumed to be x .

The equilibrium concentrations are represented as,

2SO3(g)2SO2(g)+O2(g)Initial4.000Change-2x+2xxEquilibrium(4.0-2x)+2xx

The moles of SO2 present at equilibrium are 3.0moles .

The concentration of SO2 at equilibrium is calculated by the formula,

Substitute the given values of the number of moles of NO and the volume of the flask in the above expression

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