Question 1

Which of the following statements best describes a spontaneous process?

Accepted Answer

A process that occurs without any continuous outside intervention.

Question 2

According to the First Law of Thermodynamics, which equation correctly represents the change in internal energy of a system?

Accepted Answer

$$\Delta U = q + w$$

Question 3

Which of the following is NOT a feature of a spontaneous process?

Accepted Answer

It is always spontaneous in both directions.

Question 4

Ice melting at $$T \u003e 0\ ^\circ \mathrm{C} is an $$example of:

Accepted Answer

A spontaneous, endothermic process.

Question 5

What is the common characteristic of all spontaneous processes according to the Second Law of Thermodynamics?

Accepted Answer

An increase in entropy.

Question 6

Which of the following best defines entropy ($$S$$)?

Accepted Answer

A thermodynamic quantity that increases with the number of energetically equivalent ways to arrange the components of a system.

Question 7

Ludwig Boltzmann related entropy to the number of possible arrangements of molecules in a system. Which equation expresses this relationship?

Accepted Answer

$$S = k \ln W$$

Question 8

Why does a gas spontaneously expand to evenly fill a container?

Accepted Answer

Because it increases the system's entropy by maximizing the number of possible arrangements (microstates).

Question 9

How many macrostates are possible for three molecules in a two-bulbed container?

Accepted Answer

4

Question 10

How many microstates are possible for the macrostate where there are 2 molecules in the left bulb and one in the right bulb (for three molecules in total)?

Accepted Answer

3

Question 11

Which of the following changes will increase the number of available energy levels (microstates) for a system?

Accepted Answer

Increasing the volume.

Question 12

According to the atomic/molecular view of entropy, what does a macrostate represent?

Accepted Answer

The total energy of the atom or molecule under a given set of conditions.

Question 13

The Second Law of Thermodynamics states that for a spontaneous process:

Accepted Answer

The total entropy of a system and its surroundings always increases.

Question 14

Which of the following best describes the relationship between enthalpy change ($$\Delta H) in $$the system and the entropy change in the surroundings ($$\Delta S_{surr}$$)?

Accepted Answer

$$\Delta S_{surr} is $$inversely proportional to temperature.

Question 15

How is the magnitude of $$\Delta S_{surr}$$ affected by temperature?

Accepted Answer

It decreases as temperature increases.

Question 16

Which of the following scenarios would result in the greatest increase in entropy?

Accepted Answer

Sublimation of dry ice (solid CO$$_2) to CO$_2$$ gas.

Question 17

Which of the following is a correct statement about microstates?

Accepted Answer

A microstate is a specific arrangement of the energy of each molecule in a system.

Question 18

Which of the following processes is NOT spontaneous under standard conditions?

Accepted Answer

Water freezing at $$T \u003e 0\ ^\circ \mathrm{C}.$$

Chapter 17: Gibbs Energy and Thermodynamics – Spontaneous Processes and Entropy

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