   Chapter 15, Problem 4PS

Chapter
Section
Textbook Problem

The reaction2 NO2(g) ⇄ N2O4(g)has an equilibrium constant, Kc, of 170 at 25 °C. If 2.0 × 10−3 mol of NO2 is present in a 10.-L. Flask along with 1.5 × 10−3 mol of N2O4, is the system at equilibrium? If it is not at equilibrium, does the concentration of NO2 increase or decrease as the system proceeds 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=5.88×10-3mol

The reaction quotient,Q=(2.0×10-3mol)21.5×10-3mol= 2

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