AP Chemistry : AP Chemistry

Study concepts, example questions & explanations for AP Chemistry

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Example Questions

Example Question #1 : Le Chatelier's Principle

Figure 1: Ammonia gas formation and equilibrium

 

What would most likely happen if a scientist decreased the volume of the container in which the reaction occurs?

Possible Answers:

A violent explosion would occur

More NH3 would form

More N2 would form

Less NH3 would form

More H2 would form

Correct answer:

More NH3 would form

Explanation:

Le Chatelier's principle states that changes in pressure are attributable to changes in volume. If we increase the volume, the reaction will shift toward the side that has more moles of gas. If we decrease the volume, the reaction will shift toward the side that has less moles of gas. Since the product side has only two moles of gas, compared to the reactant side with four moles, the reaction would shift toward the product side, and more NH3 would form.

Example Question #261 : Ap Chemistry

Which of the following reactions will be favored when the pressure in a system is increased?

I.

II.

III.

Possible Answers:

II and III only

I only

I and II only

I, II, and III

II only

Correct answer:

II only

Explanation:

With increased pressure, each reaction will favor the side with the least amount of moles of gas. In this problem we are looking for the reactions that favor the products in this scenario. I will favor reactants, II will favor products, III will favor reactants.

Example Question #7 : Le Chatelier's Principle

Consider the following reaction system, which has a Keq of 1.35 * 104, taking place in a closed vessel at constant temperature.

Which of the following is NOT true about this system at equilibrium?

Possible Answers:

Increasing the pressure will produce more AX5

Increasing the volume will produce more AX5

AX5 is the main compound present

The rate of formation of AX5 equals the rate of formation of AX3 and X2

Correct answer:

Increasing the volume will produce more AX5

Explanation:

An increase in volume will result in a decrease in pressure at constant temperature. As a result, the equilibrium will shift toward the side with the greater total moles of gas, according to Le Chatelier's Principle. This will result in less AX5 being produced.

The Keq tells us that the reaction favors the products because it is greater than 1. The definition of equilibrium is that the rate of formation of products equals the rate of formation of reactants.

Example Question #5 : Le Chatelier's Principle

What would happen to the Ksp if NH3 was added to an existing solution of Na2SO4?

Possible Answers:

It woud remain unchanged.

It is impossible to determine.

It would increase.

It would decrease.

Correct answer:

It woud remain unchanged.

Explanation:

Ksp is dependent only on the species itself and the temperature of the solution. Adding another compound or stressing the system will not affect Ksp.

Example Question #1 : Le Chatelier's Principle

Which of the following would occur if NH3 was added to an existing solution of Na2SO4?

Possible Answers:

No effect

Additional Na2SO4 will precipitate

Na2SO4 will dissolve more

It is impossible to determine

Correct answer:

Additional Na2SO4 will precipitate

Explanation:

Both Na2SO4 and ammonia are slightly basic compounds. Thus, adding ammonia will create a common ion effect, where less sodium sulfate will be able to dissolve and some would precipitate out of solution. 

Example Question #31 : Chemical Equilibrium

Which of the following stresses to a system at equilibrium cause an increase in the production of CH3OH ? CO(g)+ 2H2(g) → CH3OH(g)
(a) H2 is added. (b) The volume is increased. (c) Argon is added. (d) Removing CO.

Possible Answers:

(a)

(a), (b), (c), (d)

(a), (c), (d)

(b)

(a), (d)

Correct answer:

(a)

Explanation:

LeChatelier’s principle states that if a stress is applied to a rxn mixture at equilibrium,
reaction occurs in the direction that relieves the stress. Therefore, adding H2 will produce
more methanol. By increasing the volume and decreasing the pressure, there will be a net
reaction in the direction that increases the number of moles of gas. So since there are 3
moles of gas on the products side and only 1 mole of gas on the reactants side, if the volume  is increased less methanol will be produced. Since Ar is an inert, it will have no effect on the amount of methanol produced. Removing CO will cause a shift in the reaction from right to left causing less methanol to be produced.

Example Question #261 : Ap Chemistry

 

Figure 1: Ammonia gas formation and equilibrium

Experimental data shows that the reaction shifts to the left at very cold temperatures. Using this information, what type of reaction is shown in Figure 1?

Possible Answers:

Endothermic

Boltzmann-like

Exothermic

Exergonic

Endergonic

Correct answer:

Endothermic

Explanation:

This is an application of Le Chatlier's Principle. When you take away heat from the reaction, the reaction shifts toward the left in order to compensate from the heat loss. The reaction may then be rewritten to include energy as a reactant.

Since the energy is on the reactant side, the reaction is endothermic.

Example Question #13 : Le Chatelier's Principle

Which of the following will not shift the equilibrium of a reaction?

Possible Answers:

Adding more products

Adding a catalyst

Taking away products

Increasing the temperature

Adding more reactants

Correct answer:

Adding a catalyst

Explanation:

A catalyst does not change the equilibrium of a reaction. Catalysts will affect reaction rate by lowering activation energy, but will ultimately have no effect on the amount of reactants and products present when equilibrium is reached.

Adding or removing reactants or products will result in a shift in equilibrium according to Le Chatelier's principle. Similarly, changing the temperature of a reaction will affect equilibrium in different ways depending on the enthalpy of reaction; increasing the temperature of an exothermic reaction will increase the reactant concentration, while increasing the temperature of an endothermic reaction will increase the products.

Example Question #41 : Chemical Equilibrium

Consider the following balanced chemical equation:

 

What will be the effect on the concentration of  if the overall pressure of the system increases, but the volume remains constant? Why?

Possible Answers:

The concentration of  will decrease because that will counteract the increased pressure

The concentration of  will decrease because of added heat

There will be no effect on  because the number of molecules of gas is the same on both sides

The concentration of  will increase because that will counteract the increased pressure

The concentration of  will increase because of added heat

Correct answer:

The concentration of  will increase because of added heat

Explanation:

To answer this question we need to combine our knowledge of a few different subjects. Under normal cicrumstances, when determining the effects of a system pressure change, we compare the number of moles of gas on either side of the equilibrium. In this case, there are 2 moles of gas on either side, which means that neither side is favored in terms of pressure changes.



However, we consider that in this case, the pressure is increasing while the volume remains constant. Since the total moles of gas cannot be changed in a closed system, we have to conclude that increased pressure results in increased temperature. If  is greater than , then  must also be greater than .

Since this reaction is exothermic, increasing the temperature (i.e. adding heat) causes the reaction to shift to the left; therefore, the concentration of  increases.

Example Question #81 : Reactions And Equilibrium

Consider the following reaction: 

What will happen to the equilibrium constant if the concentration of  is increased? Why?

Possible Answers:

The equilibrium constant will increase because the concentration of  has increased

None of the other answers

The equilibrium constant will decrease because the reaction will shift towards the reactants

Nothing, because the equilibrium constant is not affected by concentration changes

The equilibrium constant will go through an unclear change because it is temperature dependent

Correct answer:

The equilibrium constant will go through an unclear change because it is temperature dependent

Explanation:

By Le Chatelier's principle, when a concentration on the right side increases, the reaction shifts towards the left side in order to balance out the disturbance to equilibrium. In doing so, heat will be consumed along with , which will lower the temperature of the system. Since the equilibrium constant is temperature dependent its value will change, but without experimental observation it is not entirely clear how it will change. 

It is true that concentration changes normally do not affect the equilibrium constant, but because in this case temperature is affected by concentration changes, that rule does not hold. 

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