### All Physical Chemistry Resources

## Example Questions

### Example Question #1 : Thermodynamics

For Constant Temperature, Gibbs Free Energy is defined as:

Where , is the change in Gibbs Free Energy, is the change in enthalpy, is temperature, and is the change in entropy.

Which of the following scenarios is not possible?

**Possible Answers:**

**Correct answer:**

The following condition is not possible:

This is because if enthalpy is positive, and entropy is negative, the negative sign in front of the temperature term in the formula becomes positive. Addition of 2 positive numbers can not be negative. Plugging in arbitrary numbers into the other conditions can show they are all possible.

Take the following condition:

Then Gibbs free energy can either be positive or negative, depending on the magnitude of enthalpy, entropy, and temperature. (If enthalpy is much larger than entropy and temperature, then the difference will be positive, but if entropy * is greater than the enthalpy, then the difference will be negative).

### Example Question #1 : Gibbs Free Energy

For constant temperature, Gibbs free energy is defined as:

Where , is the change in Gibbs free energy, is the change in enthalpy, is temperature, and is the change in entropy.

Given that a system is spontaneous, which of the following states are possible?

I.

II.

III.

IV.

**Possible Answers:**

I, II, and III

I, II, III, and IV

IV only

I and III

II and III

**Correct answer:**

I and III

Condition I is always true. Condition II is never true, as Gibbs free energy cannot be negative if enthalpy is positive and entropy is negative. Condition III may be true if temperature is very high (this is the scenario when the term dominates the term. Condition IV is not possible because and we were given a system with a Gibbs free Energy that is (we were told the system was spontaneous).

### Example Question #1 : Thermochemistry And Thermodynamics

The enthalpy of a reaction is and the entropy of a reaction is . Which of the following is the Gibbs free energy (in ) of this reaction?

**Possible Answers:**

Cannot be determined from the given information

**Correct answer:**

Cannot be determined from the given information

Gibbs free energy of a system can be solved using the following equation.

where is change in Gibbs free energy, is change in enthalpy, is temperature in Kelvins and is change in entropy. To solve for we need all three of the variables. We are not given the temperature; therefore, we cannot solve for Gibbs free energy.

### Example Question #1 : Thermodynamics

In an exergonic reaction, products will have __________ Gibbs free energy and the reaction is __________.

**Possible Answers:**

higher . . . nonspontaneous

lower . . . spontaneous

higher . . . spontaneous

lower . . . nonspontaneous

**Correct answer:**

lower . . . spontaneous

Exergonic reaction suggests that the Gibbs free energy is negative. Since the change in Gibbs free energy is defined as Gibbs free energy of products - Gibbs free energy of reactants, a negative change in Gibbs free energy suggests that the products have a lower Gibbs free energy than reactants. A reaction is spontaneous if it has negative Gibbs free energy; therefore, exergonic reactions are always spontaneous. This is because the reaction is producing a more stable product (lower energy) from a less stable reactant (higher energy).

### Example Question #1 : Thermodynamics

Which of the following is true regarding enthalpy and entropy?

**Possible Answers:**

The enthalpy of liquid water is nonzero whereas enthalpy of hydrogen gas is zero

None of these are true

Both of these are true

The entropy of liquid water is higher than the entropy of hydrogen gas

**Correct answer:**

The enthalpy of liquid water is nonzero whereas enthalpy of hydrogen gas is zero

Enthalpy is the amount of internal energy contained in a compound whereas entropy is the amount of intrinsic disorder within the compound. Enthalpy is zero for elemental compounds such hydrogen gas and oxygen gas; therefore, enthalpy is nonzero for water (regardless of phase). Entropy, or the amount of disorder, is always highest for gases and lowest for solids. This is because gas molecules are widely spread out and, therefore, are more disordered than solids and liquids. Hydrogen gas will have a higher entropy than liquid water.

### Example Question #2 : Thermodynamics

According to the law of thermodynamics, which of the following statement(s) is/are true?

I. Enthalpy of a system is always increasing

II. Entropy of a system is always increasing

III. Absolute entropy can never be negative

**Possible Answers:**

II only

III only

I and II

II and III

**Correct answer:**

III only

The first law of thermodynamics states that the energy of the universe is always constant, which implies that energy cannot be created or destroyed. The energy lost by a system is gained by surroundings and vice versa; however, the total energy of the universe is always constant. The second law of thermodynamics states that the entropy, or the amount of disorder in the universe, is always increasing. This suggests that the universe is always going towards a more disordered state. Based on these two laws, we can determine that statement I and statement II are false. Note that these two statements are talking about the system, rather than the universe. The energy (in the form of enthalpy) and entropy can increase or decrease in a system. The surroundings will compensate accordingly to keep the energy of universe constant and increase the entropy. Absolute entropy of a system, surroundings or the universe can never be negative because it isn’t possible to have negative disorder (this is due to the definition of entropy; just remember that entropy can never be negative). Note that the change in entropy can, however, be negative.

### Example Question #3 : Thermodynamics

A newly discovered element has been determined to have a standard entropy of in its pure form. This value is highly unlikely because it violates the __________.

**Possible Answers:**

Zeroth Law of Thermodynamics

First Law of Equivalent Exchange

Second Law of Thermodynamics

Third Law of Thermodynamics

First Law of Thermodynamics

**Correct answer:**

Third Law of Thermodynamics

The Third Law of Thermodynamics states that a pure crystalline substance at absolute zero has an entropy of . Mathematically, this formula is expressed as:

where is the Boltzmann constant and W is the number of microstates of a gaseous atom in the system. Because microstates are used to describe this gaseous atom, there has to be at least one or more.

If only one microstate exists for the system, then the entropy is zero , and can only increase from this point. It is therefore mathematically impossible for any element to have a negative standard entropy.

Remark: keep in mind that entropy **changes** can be negative, but the entropy of pure compounds cannot be negative.

### Example Question #1 : Thermodynamics

A chemical reaction is run in which of work is done by the system and the internal energy changes by . What is the total amount of heat transferred?

**Possible Answers:**

**Correct answer:**

The First Law of thermodynamics states that for a system that only exchanges energy by heat or work:

Work is done *by* the system, therefore

### Example Question #1 : Thermochemistry And Thermodynamics

An automobile engine provides of work to push the pistons and generates of heat that must be carried away by the cooling system. What is the change in the internal energy of the engine?

**Possible Answers:**

**Correct answer:**

The First Law of thermodynamics states that for a system that only exchanges energy by heat or work:

The heat is given off by the system, so . Similarly, work is being done by the system, so

### Example Question #4 : Thermodynamics

A chemical reaction is run in which of heat is absorbed and the internal energy changes by . What is the amount of work done?

**Possible Answers:**

**Correct answer:**

The First Law of thermodynamics states that for a system that only exchanges energy by heat or work:

Heat is *absorbed* by the system, therefore

So

done by the system.