Question

Match. prompt

1. δsᵤₙᵢᵥ < 0
2. s = k(ln w) where k = 1.38 x 10⁻²³ j/k
3. a particular combination of motions and locations of the atoms and molecules of a system at a particular instant
4. δsᵤₙᵢᵥ > 0
5. δsᵤₙᵢᵥ = 0
6. energy can be converted from one form to another, but cannot be created or destroyed
7. for any irreversible and spontaneous process, the entropy of the universe increases.
8. the entropy of a pure, perfect crystalline substance at absolute zero (0 k) is zero.
9. thermodynamic state function that is associated with the extent of disorder in a system or how energ

a. δsᵤₙᵢᵥ = 0
b. δsᵤₙᵢᵥ > 0
c. δsᵤₙᵢᵥ < 0
d. a particular combination of motions and locations of the atoms and molecules of a system at a particular instant
e. Thermodynamic state function that is associated with the extent of disorder in a system or how energy is dispersed.
f. s = k(ln w) where k = 1.38 x 10⁻²³ j/k
g. for any irreversible and spontaneous process, the entropy of the universe increases.
h. energy can be converted from one form to another, but cannot be created or destroyed
i. the entropy of a pure, perfect crystalline substance at absolute zero (0 k) is zero.

Answer 1

Entropy is a thermodynamic function indicating disorder within a system and is central to understanding spontaneous processes as described by the second and third laws of thermodynamics. The third law sets the zero point for entropy at a perfect crystalline solid at absolute zero. Changes in entropy help predict the spontaneity of physical and chemical processes.

Step-by-step explanation:

The entropy of a system is a measure of the disorder or randomness in the system, and it is a central concept in thermodynamics, particularly concerning the second and third laws. Entropy is denoted by the symbol S and can be calculated using various formulas, such as S = k(ln w), where k is Boltzmann's constant and w represents the number of microstates of the system. The third law of thermodynamics states that the entropy of a perfect crystalline substance at absolute zero is zero because there is only one microstate available.

When a process occurs that results in a positive change in the entropy of the universe (δSᵣᵒᵩᵖ > 0), we interpret this as a spontaneous process. Conversely, a negative entropy change of the universe (δSᵣᵒᵩᵖ < 0) indicates a nonspontaneous process, and if δSᵣᵒᵩᵖ = 0, the system is in equilibrium. Spontaneous processes are also related to the second law of thermodynamics, which states that the total entropy of a system and its surroundings always increases for a spontaneous process.

Specific examples of entropy changes include the transition of matter from solid to liquid to gas, with each phase change involving an increase in entropy. In solutions, entropy can also increase when substances mix and disperse energy more widely. The enthalpy change during a process is also crucial as certain processes that release substantial amounts of energy can occur spontaneously. Ultimately, evaluating the spontaneity of a reaction involves looking at both enthalpy and entropy changes.