Chapter 15, Problem 15.147QP

Interpretation Introduction

Interpretation:

To derive the equilibrium pressure (Kp) with supporting of Le Chatelier’s principle given the ${\text{N}}_{\text{2}}{\text{O}}_{\text{4}}$ converted into ${\text{NO}}_{\text{2}}$ equilibrium formation process.

Concept Introduction:

Equilibrium pressure: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Kp and Kc: This equilibrium constants of gaseous mixtures, these difference between the two constants is that Kc is defined by molar concentrations, whereas Kp is defined by the partial pressures of the gasses inside a closed system.

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.