Chapter 17, Problem 17.92P

Interpretation Introduction

Interpretation:

The number of moles of each substance that will be present in scene B when the mixture reaches equilibrium has to be calculated.

The given reaction is

  ${\text{M}}_{\text{2}}{\text{+ N}}_{\text{2}}\rightleftharpoons \text{2MN}$

Figure 1

Scene A represents mixture at equilibrium with M black and N orange.  Each molecule represents $\text{0}\text{.10 mol}$ and the volume is $\text{1}\text{.0 L}$.

Concept Introduction:

Equilibrium constant:

The relationship between the concentration of products and concentration of reactants in a chemical reaction at equilibrium is said to be equilibrium constant.  It is denoted by $\text{K}$.

For a reaction,

  $\text{xX + yY }\rightleftharpoons \text{ zZ}$

The expression of $\text{K}$ can be given as

  $\begin{array}{l}{\text{K}}_{\text{c}}\text{ = }\frac{{\text{[Z]}}^{\text{z}}}{{\text{[X]}}^{\text{x}}{\text{[Y]}}^{\text{y}}}\\ \\ \text{where,}\text{[X] = equilibrium concentration of X}\\ \\ \text{[Y] = equilibrium concentration of Y}\\ \\ \text{[Z] = equilibrium concentration of Z}\end{array}$