AP Chemistry : Equilibrium

Study concepts, example questions & explanations for AP Chemistry

Example Questions

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Example Question #1 : Equilibrium

Suppose that a rxn has ∆H = -28 kJ and ∆S= -60 J/K. At what temperature will it
change from spontaneous to non-spontaneous?

Possible Answers:

500 K

50

467 K

46.7 K

Correct answer:

467 K

Explanation:

Approximately 467 K. ∆G=∆H-T∆S and a rxn proceeds spontaneously when ∆G < 0
and is non-spontaneous when ∆G > 0. So if we set ∆G=0 and solve the equation for T, we will see that the crossover from spontaneous to non-spontaneous occurs when T=467K.

Example Question #2 : Equilibrium

If the reaction quotient (Q) is greater than the equilibrium constant (K), what is true about the Gibbs free energy?

Possible Answers:

It is greater than zero.

More information is needed to determine the gibbs free energy.

It is less than zero.

It is equal to zero.

Correct answer:

It is greater than zero.

Explanation:

If Q is greater than K, the reaction has exceeded the equilibrium state. It will proceed nonspontaneously (since equilibrium has already been reached), and this must mean that the ΔG (gibbs free energy) must be positive, or greater than zero. 

Example Question #3 : Equilibrium

Which of the following is true when the reaction quotient (Q) equals the equilibrium constant (K)?

Possible Answers:

The change in free energy is less than zero.

The change in free energy is greater than zero.

The reaction stops completely.

Change in free energy = 0.

Correct answer:

Change in free energy = 0.

Explanation:

When Q = K, the reaction has reached equilibrium and is in a state of dynamic equilibrium, where the forward and reverse reactions are occurring at the same rate. Since there is no net change in concentration, the free energy is zero. 

Example Question #4 : Equilibrium

The entropy and enthalpy of a reaction are both negative. Is the reaction spontaneous?

Possible Answers:

The reaction is spontaneous

The reaction will be spontaneous if and only if the magnitude of the enthalpy is greater than the magnitude of the entropy

The reaction will be spontaneous if and only if the magnitude of the enthalpy is greater than the magnitude of the entropy times the temperature

The reaction is not spontaneous

The reaction will be spontaneous if and only if the magnitude of the entropy is greater than the magnitude of the enthalpy times the temperature

Correct answer:

The reaction will be spontaneous if and only if the magnitude of the enthalpy is greater than the magnitude of the entropy times the temperature

Explanation:

A reaction is spontaneous if the Gibb's Free Energy of the reaction is negative.

If , the enthalpy, and , the entropy, are both negative, then the reaction will be spontaneous if and only if the magnitude of the enthalpy is greater than the magnitude of the entropy times the temperature.

Example Question #5 : Equilibrium

If delta G for a certain reaction is found to be -4955 J/mol, what is the equilibrium constant (Keq) for this reaction?

Possible Answers:

100

7.4

55.6

80.9

5.9

Correct answer:

7.4

Explanation:

Given the equation delta G = -RTln(Keq), plugging in the correct values for the variables will lead us to the correct answer. Using e = 2.7, R = 8.314 J/molK, T= 298 K, and G = -4955 J, we can calculate that K = 7.4.

Example Question #6 : Equilibrium

A system with __________ and __________ will never be spontaneous.

Possible Answers:

positive enthalpy . . . positive entropy

negative enthalpy . . . negative entropy

negative enthalpy . . . positive entropy

positive enthalpy . . . negative entropy

Correct answer:

positive enthalpy . . . negative entropy

Explanation:

The Gibb's free energy equation is used to determine the spontaneity of a reaction and is written as follows: .

is Gibb's free energy,  is enthalpy, and  is entropy. In order for a reaction to be spontaneous, Gibb's free energy must have a negative value. Based on the equation, we can see that a positive enthalpy in combination with a negative entropy will always result in a positive value for Gibb's free energy.

This means these are the conditions that will always result in a nonspontaneous reaction. 

Example Question #7 : Equilibrium

A chemical reaction has the following changes in enthalpy and entropy.

What is the temperature range for this reaction that allow it to be spontaneous? 

Possible Answers:

The reaction is always spontaneous

Correct answer:

Explanation:

A reaction is spontaneous when Gibb's free energy is negative. As a result, we need to determine the temperature range where Gibb's free energy is less than zero. Since we know the values for changes in enthalpy and entropy, we can plug them into the Gibb's free energy equation, and set it equal to zero.

437K is the temperature at which Gibb's free energy is zero. Since entropy is positive for this reaction, increasing the temperature will result in a more negative value for Gibb's free energy.

As a result, any temperature that is greater than 437K will make this reaction spontaneous.

Example Question #8 : Equilibrium

Consider the following reaction in a galvanic cell:

    

Which if the following statements about the reaction is false?

Possible Answers:

Gibb's free energy is positive

The equilibrium constant is greater than one

The cell potential is positive

The reaction is spontaneous

Correct answer:

Gibb's free energy is positive

Explanation:

A galvanic cell results in a positive cell potential from a spontaneous reaction. Spontaneous reactions always have a negative Gibb's free energy.

An equilibrium constant greater than one would indicate that the equilibrium concentration of products is greater than the equilibrium concentration of reactants, consistent with a spontaneous reaction.

Example Question #9 : Equilibrium

Consider the following reaction in a galvanic cell:

    

What is the Gibb's free energy for the reaction under standard conditions?

Possible Answers:

Correct answer:

Explanation:

You can find the Gibb's free energy of a galvanic cell by using the following equation:

 is the number of moles of electrons that are transferred in the reaction,  is Faraday's constant, and  is the potential of the cell.

We are given the constant value and the cell potential. The moles of electrons transferred is equal to the change in charge on the atoms in the reaction. In this reaction, copper is reduced from a charge of to zero, requiring that is gained two moles of electrons.

Using these values, we can find Gibb's free energy for the cell.

Notice that the value is negative. Galvanic cells are spontaneous, and will have negative Gibb's free energies at standard conditions.

 

Example Question #10 : Equilibrium

If the reaction quotient (Q) is less than the equilibrium constant (K), what is true about the Gibbs free energy?

Possible Answers:

We must know the reaction enthalpy to determine the answer

It is less than zero

It is equal to zero

We must know the reaction temperature to determine the answer

It is greater than zero

Correct answer:

It is less than zero

Explanation:

If Q is less than K, then the reaction has not yet reached the equilibrium state. It will proceed spontaneously in the forward direction. Since it is proceeding spontaneously in the forward direction, this must mean that the ΔG (Gibbs free energy) must be negative, or less than zero.

Enthalpy and temperature are necessary when mathematically evaluating Gibbs free energy, but the reaction quotient and equilibrium constant provide enough information to qualitatively determine that the reaction is proceeding spontaneously.

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