   Chapter 15, Problem 36GQ

Chapter
Section
Textbook Problem

Equal numbers of moles of H2 gas and I2 vapor are mixed in a flask and heated to 700 °C. The initial concentration of each gas is 0.0088 mol/L, and 78.6% of the I2 is consumed when equilibrium is achieved according to the equationH2(g) + I2(g) ⇄ 2 HI(g)Calculate Kc for this reaction.

Interpretation Introduction

Interpretation: The equilibrium constant for the given reaction has to be determined.

Concept introduction:

Equilibrium constant: At equilibrium the ratio of products to reactants has a constant value. And it is represented by the letter K.

For a general reaction, aA+bBcC+dD

The equilibrium constant Kc=[C]c[D]d[A]a[B]b    a, b, c and d are the stoichiometric coefficients of reactant and product in the reaction. Concentration value for solid substance is 1.

If the value of Kc and the concentration of any of the reactant of a reaction is known then the concentration of product can be determined by multiplying Kc with the concentration of reactant.

Explanation

The balanced equation for the given reaction is,

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

The initial concentration of H2andI2 are both 0.0088mol/L

When the equilibrium is achieved 78.6%oftheI2 is consumed.

From this percentage value the concentration of I2 can be determined.

78.6×0.0088100=0.00692mol/L

The concentration of H2andI2left is,

0

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