16.3 The Second and Third Laws of Thermodynamics

16.3 The Second and Third Laws of Thermodynamics

• There is a reason for your prediction.

• We have identified a promising candidate for a property that can reliably predict the nature of a process.
• The examples to the contrary are plentiful.

• Consider the process of heat flow between two objects, one identified as the system and the other as the surroundings.

• The hotter the object, the hotter the heat flows from it to the cooler object.

• The increase in the universe's entropy is the result of this process.

• The objects are cooler than the hotter one, and the heat goes from the cooler to the hotter one.

• A decrease in the universe's instument is involved.

• See the discussion from the previous section.
• There is no change in the universe's entropy.

• Table 16.1 has a summary of these three relations.

• In comparison to the system, the surroundings are vast.
• The heat gained or lost by the surroundings as a result of some process is a very small fraction of the total thermal energy.
• Transferring heat from a system to surroundings that are larger than the earth's atmosphere is one way in which a fuel can be burned.

• The process can be assessed by calculating the change of the universe.

• This information can be used to determine if liquid water will spontaneously freeze.

• Entropy is a state function and freezing is not.
• At -10.00 degC nonspontaneous, +0.7 J/K.

• The previous section described the contributions of matter and energy to the system.
• At a temperature of absolute zero, 0 K, the entropy of a pure, perfectly crystalline solid is zero.
• The Boltzmann equation states that the system is zero.

• calorimetric measurements can be made to determine the temperature dependence of a substance and to derive absolute entropy values.
• The balanced equation represents the process.