   # At a particular temperature, K = 1.00 × 10 2 for the reaction H 2 ( g ) + I 2 ( g ) ⇌ 2 HI ( g ) In an experiment, 1.00 mole of H 2 , 1.00 mole of I 2 , and 1.00 mole of HI are introduced into a 1.00-L container. Calculate the concentrations of all species when equilibrium is reached. ### 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 52E
Textbook Problem
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## At a particular temperature, K = 1.00 × 102 for the reaction H 2 ( g ) + I 2 ( g ) ⇌ 2 HI ( g ) In an experiment, 1.00 mole of H2, 1.00 mole of I2, and 1.00 mole of HI are introduced into a 1.00-L container. Calculate the concentrations of all species when equilibrium is reached.

Interpretation Introduction

Interpretation: The value of the equilibrium constant for the reaction between H2 and I2 and the initial number of moles of the species involved are given. The equilibrium concentrations of the three gases involved in the system are 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 concentrations of the three gases involved in the system.

### Explanation of Solution

Given

The stated reaction is,

H2(g)+I2(g)2HI(g)

The initial number of moles of H2(g) is 1.00mole .

The initial number of moles of I2(g) is 1.00mole .

The initial number of moles of HI(g) is 1.00mole .

The equilibrium constant (K) value is 1.00×102 .

The volume of the container is 1.00L .

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=[HI]2[H2][I2] (1)

Formula

The concentration of a reactant is calculated by the formula,

Concentration=MolesVolume(L)

The initial concentration of H2 is calculated by the formula,

Substitute the given values of the number of moles of H2 and the volume of the flask in the above expression.

ConcentrationofH2=1.00moles1.00L=1.00M

The initial concentration of I2 is calculated by the formula,

Substitute the given values of the number of moles of I2 and the volume of the flask in the above expression.

ConcentrationofI2=1.00moles1.00L=1.00M

The initial concentration of HI is calculated by the formula,

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

ConcentrationofHI=1.00moles1.00L=1.00M

The concentration of H2 and I2 consumed is assumed to be x .

The equilibrium concentrations are represented as,

H2(g)+I2(g)2HI(g)Initialconcentration1.01.01.0Change-x-x+2xEquilibriumconcentration1

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