9.1 Introduction to Entropy

• What is the name of the equation that relates entropy to the number of microstates in a system?

  Boltzmann's equation
• A higher number of microstates corresponds to greater entropy.


  True
• Natural processes are irreversible because they increase the system's disorder.


  True
• Match the system property with its state in ordered or disordered systems:

  Entropy ↔️ Low in ordered systems

  Microstates ↔️ Many in disordered systems
• What is a spontaneous process?

  A natural process
• Spontaneous processes are reversible.

  False
• Match the process type with its entropy change and reversibility:

  Spontaneous ↔️ Increases entropy, irreversible

  Non-spontaneous ↔️ Decreases entropy, reversible
• Order the factors affecting entropy from lowest to highest effect on entropy:

  1️⃣ Lower temperature

  2️⃣ Smaller volume

  3️⃣ Freezing

  4️⃣ Boiling
• What is the name of the equation used to calculate entropy changes?

  Boltzmann's equation
• What is entropy a measure of in a system?

  Disorder or randomness
• Why do spontaneous processes occur without external intervention?

  They increase entropy
• Match the process type with its entropy change and reversibility:

  Spontaneous ↔️ Increases, No

  Non-spontaneous ↔️ Decreases, Yes
• Match the factor affecting entropy with its effect:

  Temperature ↔️ Higher temperature leads to higher entropy

  Volume ↔️ Larger volume leads to higher entropy

  Phase Changes ↔️ Melting and boiling increase entropy
• Arrange the steps to calculate entropy changes using Boltzmann's equation:

  1️⃣ Identify the number of microstates (W)

  2️⃣ Use Boltzmann's constant (k)

  3️⃣ Apply the equation S = k ln W

  4️⃣ Calculate the entropy (S)
• The number of microstates in Boltzmann's equation is represented by the symbol W
• What is the Gibbs free energy equation?

  $G =$$H - TS$
• If ΔG = 0, the process is at equilibrium
• Entropy is a measure of the disorder or randomness within a system.
• Entropy quantifies the number of possible microstates that a system can occupy.
• What does the Second Law of Thermodynamics state about the total entropy of an isolated system?

  It increases
• What happens to entropy in a reversible process?

  It remains constant
• Natural processes are irreversible because they increase the system's disorder.
• What happens to entropy in a reversible process?

  Remains constant
• Why are spontaneous processes irreversible?

  No external energy input
• Match the system property with its description:

  Ordered system ↔️ Low entropy, few microstates

  Disordered system ↔️ High entropy, many microstates
• The Second Law of Thermodynamics states that the total entropy of an isolated system decreases during any natural process.

  False
• Spontaneous processes, such as the diffusion of a gas, increase the entropy
• The Second Law of Thermodynamics states that the total entropy of an isolated system increases
• Higher temperature increases the disorder and randomness of a system, leading to higher entropy
• In Boltzmann's equation, S represents the entropy
• Boltzmann's constant is approximately 1.38 × 10^-23 J/K.


  True
• Increasing the volume of a system generally increases its entropy.

  True
• In the Gibbs free energy equation, H represents the enthalpy
• Increasing temperature makes spontaneous processes more favorable.

  True
• Boltzmann's constant is approximately 1.38 × 10^-23 J/K.


  True
• Order the following systems from lowest to highest entropy:

  1️⃣ Crystalline lattice

  2️⃣ Ordered solid

  3️⃣ Liquid

  4️⃣ Gas
• It is impossible to convert heat completely into work in a cyclical process without producing entropy.
• The Second Law of Thermodynamics applies only to isolated systems.

  True
• The Second Law of Thermodynamics explains why spontaneous processes occur.


  True
• The Second Law of Thermodynamics states that the total entropy of an isolated system increases during any natural process