9th Edition
Steven S. Zumdahl
ISBN: 9781133611097




9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

A 1.00-L flask was filled with 2.00 moles of gaseous SO2 and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, it was found that 1.30 moles of gaseous NO was present. Assume that the reaction

SO 2 ( g ) + NO 2 ( g ) SO 3 ( g ) + NO ( g )

occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction.

Interpretation Introduction

Interpretation:  A 1.00L flask filled with 2.00moles of gaseous SO2 and 2.00moles of gaseous NO2 is given. The reaction that takes place between these 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.



The stated reaction is,


The volume of the flask is 1.00L .

Initial moles of SO2 are 2.00moles .

Initial moles of NO2 are 2.00moles .

The moles of NO present at equilibrium are 1.30moles .

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



  • K is the equilibrium constant.

The equilibrium ratio for the given reaction is,

K=[SO3][NO][SO2][NO2] (1)

The number of moles of SO2 and NO2 consumed are assumed to be x .

The equilibrium concentrations are represented as,


The moles of NO present at equilibrium are 1.30moles .

The concentration of a reactant is calculated by the formula,


The concentration of NO 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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