Chapter 15, Problem 15.1QP

Interpretation Introduction

Interpretation:

The definition for equilibrium and two examples for dynamic equilibrium should be explained.

Concept Introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved when the concentrations of reactants and products become constant.

Forward Reaction: This type of reaction has involved irreversible, if obtained product cannot be converted back in to respective reactants under the same conditions. Backward Reaction: This type of reaction process involved a reversible, if the products can be converted into a back to reactants.

Equilibrium expression: The equilibrium expression is equal to the concentration of each product raised to its coefficient in a balanced chemical equation and multiplied together, divides by the concentrate ions of the product of reactants to the power of their coefficient.

Homogeneous equilibrium: A homogeneous equilibrium involved has a everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.

Heterogeneous equilibrium: This equilibrium reaction does not depend on the amounts of pure solid and liquid present, in other words heterogeneous equilibrium, substances are in different phases.

Dynamic equilibrium: Both the forward and the backward reaction tends to occur without any net change in the concentrations of both reactant and the product.

Answer to Problem 15.1QP

The chemical equilibrium is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved when the concentrations of reactants and products become constant.

Examples for dynamic equilibrium are as follows,

${\text{N}}_{\text{2}}{\text{O}}_{\text{4}}{}_{\left(g\right)}\stackrel{}{\to }{\text{NO}}_{\text{2}}{}_{\left(g\right)}$

${\text{CO}}_{\left(g\right)}+{\text{Cl}}_{\text{2}}{}_{\left(g\right)}\stackrel{}{\to }{\text{COCl}}_{\text{2}}{}_{\left(g\right)}$

Explanation of Solution

The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved when the concentrations of reactants and products become constant.

The equilibrium is a dynamic state where both the forward and the backward occur simultaneously without any change in the concentrations of the reactant and the product.

The examples for the dynamic equilibrium are as follows,

The reaction ${\text{N}}_{\text{2}}{\text{O}}_{\text{4}}{}_{\left(g\right)}\stackrel{}{\to }{\text{NO}}_{\text{2}}{}_{\left(g\right)}$ is perfect example for dynamic equilibrium since the after the product form it decomposes to give the reactants and once the reactants are formed they results to give the product at the right side therefore, rate of forward and the backward rate are equal.

Similarly the reaction between carbon monoxide and chlorine also serves as example for dynamic equilibrium ${\text{CO}}_{\left(g\right)}+{\text{Cl}}_{\text{2}}{}_{\left(g\right)}\stackrel{}{\to }{\text{COCl}}_{\text{2}}{}_{\left(g\right)}$ where the forward and the backward rate are equal.

Conclusion

The definition for chemical equilibrium and the examples for dynamic equilibrium are determined.