   Chapter 15, Problem 6PS

Chapter
Section
Textbook Problem

The equilibrium constant Kc, for the reaction2 NOCI(g) ⇄ 2 NO(g) + Cl2(g)is 3.9 × 10−3 at 300 °C. A mixture contains the gases at the following concentrations: [NOCl] = 5.0 × 10−3 mol/L, [NO] = 2.5 × 10−3 mol/L, and [Cl2] = 2.0 × 10−3 mol/L. Is the reaction at equilibrium at 300 °C? If not, in which direction does the reaction proceed to come to equilibrium?

Interpretation Introduction

Interpretation:

The given reaction is in equilibrium or not has to be determined and way to proceed to reach equilibrium has to be identified.

Concept Introduction: For a reaction, aA+bBcC+dD ,

The reaction quotient,Q=[C]c[D]d[A]a[B]b

Q<K, means some reactants must convert to products for the reaction to reach equilibrium. This will decrease concentration of the reactant and will increase concentration of the products.

Q>K, means some products must convert to reactants for the reaction to reach equilibrium. This will increase concentration of the reactant and will decrease concentration of the products.

Explanation

Given Kc=3.9×10-3

The reaction quotient,Q=(5.0×10-3mol/L)2(2.5×10-3mol/L)2(2

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