   Chapter 13, Problem 37E

Chapter
Section
Textbook Problem

# Consider the following reaction at a certain temperature: 4 Fe ( s ) + 3 O 2 ( g ) ⇌ 2 Fe 2 O 3 ( s ) An equilibrium mixture contains 1.0 mole of Fe, 1.0 × 10-3 mole of O2, and 2.0 moles of Fe2O3 all in a 2.0-L container. Calculate the value of K for this reaction.

Interpretation Introduction

Interpretation: The number of moles of Fe , O2 and Fe2O3 at a particular temperature are given. The value of the equilibrium constant (K) value for the given reaction 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 K .

To determine: The concentrations of Fe , O2 and Fe2O3 for the given reaction.

Explanation

Given

The stated reaction is,

4Fe(s)+3O2(g)2Fe2O3(s)

The number of moles Fe is 1.0mole .

The number of moles O2 is 1.0×103mole .

The number of moles Fe2O3 is 2.0mole .

The given volume of the flask is 2.00L .

The concentration of a reactant is calculated by the formula,

Concentration=MolesVolume(L)

For Fe ,

The concentration of Fe is calculated by the formula,

Substitute the values of the number of moles of Fe and the volume of the flask in the above expression in the above

ConcentrationofFe=1.0mole2.0L=0.5M_

For O2 ,

The concentration of O2 is calculated by the formula,

Substitute the values of the number of moles of O2 and the volume of the flask in the above expression in the above

ConcentrationofO2=1.0×103mole2.0L=5

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