# 19.2: Chemical Equilibrium

A tug of war involves two teams at the ends of a rope. The goal is to pull the other team over a line in the middle. At first, there is a great deal of tension on the rope, but no apparent movement. A bystander might think that there is nothing happening. In reality, there is a great deal of tension on the rope as the two teams pull in opposite directions at the same time.

### Chemical Equilibrium

Hydrogen and iodine gases react to form hydrogen iodide according to the following reaction:

$\ce{H_2} \left( g \right) + \ce{I_2} \left( g \right) \rightleftharpoons 2 \ce{HI} \left( g \right)$

$\text{Forward reaction:} \: \: \: \ce{H_2} \left( g \right) + \ce{I_2} \left( g \right) \rightarrow 2 \ce{HI} \left( g \right)$

$\text{Reverse reaction:} \: \: \: 2 \ce{HI} \left( g \right) \rightarrow \ce{H_2} \left( g \right) + \ce{I_2} \left( g \right)$

Initially, only the forward reaction occurs because no $$\ce{HI}$$ is present. As soon as some $$\ce{HI}$$ has formed, it begins to decompose back into $$\ce{H_2}$$ and $$\ce{I_2}$$. Gradually, the rate of the forward reaction decreases while the rate of the reverse reaction increases. Eventually the rate of combination of $$\ce{H_2}$$ and $$\ce{I_2}$$ to produce $$\ce{HI}$$ becomes equal to the rate of decomposition of $$\ce{HI}$$ into $$\ce{H_2}$$ and $$\ce{I_2}$$. When the rates of the forward and reverse reactions have become equal to one another, the reaction has achieved a state of balance. Chemical equilibrium is the state of a system in which the rate of the forward reaction is equal to the rate of the reverse reaction.

Figure 19.2.1: Equilibrium in reaction: $$\ce{H_2} \left( g \right) + \ce{I_2} \left( g \right) \rightleftharpoons 2 \ce{HI} \left( g \right)$$.

Chemical equilibrium can be attained whether the reaction begins with all reactants and no products, all products and no reactants, or some of both. The figure below shows changes in concentration of $$\ce{H_2}$$, $$\ce{I_2}$$, and $$\ce{HI}$$ for two different reactions. In the reaction depicted by the graph on the left (A), the reaction begins with only $$\ce{H_2}$$ and $$\ce{I_2}$$ present. There is no $$\ce{HI}$$ initially. As the reaction proceeds towards equilibrium, the concentrations of the $$\ce{H_2}$$ and $$\ce{I_2}$$ gradually decrease, while the concentration of the $$\ce{HI}$$ gradually increases. When the curve levels out and the concentrations all become constant, equilibrium has been reached. At equilibrium, concentrations of all substances are constant. In reaction B, the process begins with only $$\ce{HI}$$ and no $$\ce{H_2}$$ or $$\ce{I_2}$$. In this case, the concentration of $$\ce{HI}$$ gradually decreases while the concentrations of $$\ce{H_2}$$ and $$\ce{I_2}$$ gradually increase until equilibrium is again reached. Notice that in both cases, the relative position of equilibrium is the same, as shown by the relative concentrations of reactants and products. The concentration of $$\ce{HI}$$ at equilibrium is significantly higher than the concentrations of $$\ce{H_2}$$ and $$\ce{I_2}$$. This is true whether the reaction began with all reactants or all products. The position of equilibrium is a property of the particular reversible reaction and does not depend upon how equilibrium was achieved.

Figure 19.2.2: Equilibrium between reactants and products.

### Conditions for Equilibrium

It may be tempting to think that once equilibrium has been reached, the reaction stops. Chemical equilibrium is a dynamic process. The forward and reverse reactions continue to occur even after equilibrium has been reached. However, because the rates of the reactions are the same, there is no change in the relative concentrations of reactants and products for a reaction that is at equilibrium. The conditions and properties of a system at equilibrium are summarized below.

1. The system must be closed, meaning no substances can enter or leave the system.
2. Equilibrium is a dynamic process. Even though we don't necessarily see the reactions, both the forward and reverse reactions are taking place.
3. The rates of the forward and reverse reactions must be equal.
4. The amount of reactants and products do not have to be equal. However, after equilibrium is attained, the amounts of reactants and products will be constant.

The description of equilibrium in this concept refers primarily to equilibrium between reactants and products in a chemical reaction. Other types of equilibrium include phase equilibrium and solution equilibrium. A phase equilibrium occurs when a substance is in equilibrium between two states. For example, a stoppered flask of water attains equilibrium when the rate of evaporation is equal to the rate of condensation. A solution equilibrium occurs when a solid substance is in a saturated solution. At this point, the rate of dissolution is equal to the rate of recrystallization. Although these are all different types of transformations, most of the rules regarding equilibrium apply to any situation in which a process occurs reversibly.

### Summary

• The concept of chemical equilibrium is described.
• Conditions for chemical equilibrium are listed.

### Contributors

• CK-12 Foundation by Sharon Bewick, Richard Parsons, Therese Forsythe, Shonna Robinson, and Jean Dupon.