Chapter 6, Problem 92AE

(a)

Interpretation Introduction

Interpretation: The below table for reaction is to be completed.

  $\begin{array}{cccccc}& \text{2NOCl}\left(g\right)& \rightleftharpoons & \text{NO}\left(g\right)& +& {\text{Cl}}_{\text{2}}\left(g\right)\\ \text{Initial}& & & & & \\ \text{Change}& & & & & \\ \text{Equilibrium}& 2.6-2x& & & & \end{array}$

Concept introduction:

(b)

Interpretation Introduction

Interpretation: The equilibrium concentration of all species in below reaction is to be calculated.

  $\text{2NOCl}\left(g\right)\to 2\text{NO}\left(g\right)+{\text{Cl}}_2\left(g\right)$

Concept introduction:Equilibrium constant is denoted by $K_{\text{eq}}$ and it is a ratio of concentration of product to reactant. Consider an equilibrium reaction as below.

  $\text{A}\rightleftharpoons \text{B}$

The expression used to calculate $K_{\text{eq}}$ is as follows:

  $K_{\text{eq}}=\frac{\left[\text{B}\right]}{\left[\text{A}\right]}$

Where,

  $K_{\text{eq}}$ is equilibrium constant.

  $\left[\text{B}\right]$ is concentration of B (product).

  $\left[\text{A}\right]$ is concentration of A (reactant).