Chapter 14, Problem 14.138CP

Interpretation Introduction

Interpretation:

In the following reaction of formation of N₂O₃.

$NO\left(g\right)+N{O}_2\left(g\right)\rightleftharpoons N_2{O}_3\left(g\right)$

A mixture at temperature 298K and total pressure 1.65 atm is prepared with 2.0 mol NO and 3.0 mol NO₂. Calculate:

1. The equilibrium partial pressure NO and NO₂
2. Volume of the container.

Concept introduction:

Equilibrium is the process in which temperature, pressure, concentration of reactant and product do not show any change with respect to time.
There are two types of equilibrium.

1. Physical equilibrium: In this, the physical state of the reactant and the product does not change when dynamic equilibrium occurred.
2. Chemical equilibrium: In this, the chemical composition of reactant and product does not change when dynamic equilibrium occurred. There are two types of reaction occurred in this.

(a) Reversible reactions: In this reaction, reaction can occur in two ways, where reactant can convert to product as well as product can convert back to reactant.
(b) Irreversible reaction: In this reaction, reaction cannot occur in two ways where reactant can convert to product, but product cannot convert back to reactant.

Equilibrium constant $K_c$ is defined as the ratio of the concentrations of the products raised to the power of their stoichiometric coefficients and reactants raised to the power of their stoichiometric coefficients.
Reaction quotient Q is defined as the ratio at any point of the reaction of the concentration of the product raised to the power of their stoichiometric coefficients and reactant raised to the power of their stoichiometric coefficients.

$\begin{array}{l}aA+bB\to cC+dD\\ K_c=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b},equilibrium\\ Q=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}\end{array}$

To calculate:

The partial pressure of NO and NO₂ at equilibrium and volume.