### All College Chemistry Resources

## Example Questions

### Example Question #31 : Reactions

Consider the following reaction:

Give the expression for the equilibrium constant for this reaction.

**Possible Answers:**

**Correct answer:**

Recall how to find the expression of the equilibrium constant for the simplified equation:

Since the given equation has gases, we will only consider the partial pressures of each gas in the expression for the equilibrium constant. Remember that only molecules in aqueous and gas forms are included in this expression. Pure solids and pure liquids are excluded.

Thus, we can then write the following equilibrium constant for the given equation:

### Example Question #32 : Reactions

Consider the following reaction:

The reaction mixture at initially contains and . At equilibrium, . What is the equilibrium constant for the reaction?

**Possible Answers:**

**Correct answer:**

Start by writing the equilibrium expression:

Now, create a chart like the following to keep track of the changes in concentration.

Initial | 0.750 | 2.00 | 0.00 |

Change | -0.100 | -0.025 | 0.200 |

Equilibrium | 0.650 | 19.75 | 0.200 |

Since we know that the concentration of HCl decreased by , we can use the stoichiometric ratios to deduce the amount of change for the oxygen gas and the chlorine gas.

Plug in the equilibrium concentrations into the expression for the equilibrium constant.

### Example Question #36 : Reactions

Calculate the equilibrium constant at for the reaction by using free energies of formation.

**Possible Answers:**

**Correct answer:**

Start by using the free energies of formation to find .

,

Recall the equation that links together with the equilibrium constant, .

Plug in the given information and solve for .

### Example Question #37 : Reactions

Consider a reaction mixture using the equation shown. At equilibrium the partial pressure of is and the partial pressure of _{ }is . What is the partial pressure of _{ }in this mixture if at ?

**Possible Answers:**

or

or

or

or

**Correct answer:**

or

Use algebra to solve for the partial pressure of .

### Example Question #33 : Reactions

Considering the reaction shown, if the partial pressures of , , and are each, is the mixture at equilibrium? If not which direction will the reaction proceed to reach equilibrium if ?

**Possible Answers:**

No, reaction will proceed right towards the products.

Yes, the reaction will move towards the products.

No, the reaction will proceed left towards the reactants.

Yes

**Correct answer:**

No, reaction will proceed right towards the products.

Since the reaction is not at equilibrium. This means that at equilibrium, the ratio of products to reactants is greater than at the given conditions. Thus, the reaction will move right towards the products to reach equilibrium.

### Example Question #39 : Reactions

In the laboratory of and of are reacted in a beaker. At equilibrium of remain. Using the equation shown calculate the equilibrium constant.

**Possible Answers:**

**Correct answer:**

Use an ice table and the _{ }equation to solve.

_{ }

Initial

Change

Equilibrium

### Example Question #40 : Reactions

Find the _{ }of the reaction if you start with and end with at .

**Possible Answers:**

**Correct answer:**

Use an ICE table and the equation to solve.

Initial

Change

Equilibrium

### Example Question #41 : Reactions

Hypobromous acid will dissociate in water at with a . What is the for this dissociation process?

**Possible Answers:**

**Correct answer:**

For this question, we're given the acid dissociation constant for a reaction that occurs at a given temperature. We're asked to find the standard free energy change for the reaction.

First, we're going to need to use an equation that relates standard free energy changes with an equilibrium constant, which is shown as follows.

With regards to the temperature, we will need to convert the units given in the question stem into units of Kelvin.

Knowing that is the ideal gas constant, we have all the information we need to solve for the value of .

### Example Question #42 : Reactions

Determine the acid dissociation constant expression for the given reaction.

**Possible Answers:**

**Correct answer:**

Acid dissociation constant which is denoted as is the equilibrium constant for the ionization of an acid. Therefore, the numerator contains the product of the concentrations of the substances on the product side of the chemical equation. The denominator contains the product of the concentrations of the substances on the reactant side of the chemical equation. is omitted in the acid dissociation constant expression because as the solvent it is in excess and therefore the change in its concentration is negligible in comparison to the other substances in solution.