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# Chemical Equilibrium

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Practice Chemical Equilibrium
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Chemical Equilibrium

Pull hard

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:

$\text{H}_2(g)+\text{I}_2(g) & \rightleftarrows 2\text{HI}(g) \\\text{Forward reaction:} & \quad \text{H}_2(g)+\text{I}_2(g) \rightarrow 2\text{HI}(g) \\\text{Reverse reaction:} & \quad 2\text{HI}(g) \rightarrow \text{H}_2(g)+\text{I}_2(g)$

Initially, only the forward reaction occurs because no HI is present. As soon as some HI has formed, it begins to decompose back into H 2 and I 2 . Gradually, the rate of the forward reaction decreases while the rate of the reverse reaction increases. Eventually the rate of combination of H 2 and I 2 to produce HI becomes equal to the rate of decomposition of HI into H 2 and 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.

Equilibrium in reaction: H 2 (g) + I 2 (g) → 2HI(g).

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 H 2 , I 2 , and HI for two different reactions. In the reaction depicted by the graph on the left (A), the reaction begins with only H 2 and I 2 present. There is no HI initially. As the reaction proceeds towards equilibrium, the concentrations of the H 2 and I 2 gradually decrease, while the concentration of the 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 HI and no H 2 or I 2 . In this case, the concentration of HI gradually decreases while the concentrations of H 2 and 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 HI at equilibrium is significantly higher than the concentrations of H 2 and 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.

Equilibrium between reactants and products.

#### Conditions for Equilibrium and Types of 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 forward and reverse 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.

#### Summary

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

#### Practice

1. What is a closed system?
2. What is a dynamic system?
3. What happens if you change the relative rates of the forward and back reactions?

#### Review

1. What is chemical equilibrium?
2. In the reaction illustrated in the text, does the equilibrium concentration of HI equal the equilibrium concentrations of H 2 and I 2 ?
3. Does the position at equilibrium depend upon how the equilibrium was reached?