Problem Set #16: Entropy and Thermodynamics

University:
The Pennsylvania State University
Course:
CHEM 450 | Thermodynamics
Academic year:

2024
Views:

162

Pages:

1
Author:

Alexis H.

Problem Set #16 Assigned: February 12, 2024 Due: Feb. 14, 2023 at 2:30 pm 1. The formation of a living organism involves the organization of a large number of biochemical molecules into very specific configurations. This represents far lower entropy than if the same molecules were disorganized. Why is it possible to do this? 2. What do “dispersal” and “disorder” mean in the context of the Second Law of Thermodynamics? 3. Consider a process in which the entropy of the system increases by 125 J/K and entropy of the surroundings decreases by 125 J/K. Is this process spontaneous? 4. Consider a process in which 1000 kJ of energy is transferred reversibly and isothermally as heat to a large block of copper. Find the change in entropy if the process takes place at 0 °C and at 50 °C. Which one is larger? 1. The formation of living organisms is a very organized process with many parts where that organization is very important, while the second law of thermodynamics states that things tend towards disorder, the greater the disorder the greater the entropy. Since the formation of living organisms is so ordered it has a lower value of entropy. 2. Disorder is what is used to test the entropy of a system while dispersal means that something spreads out 3. No the process is not spontaneous because ¢Stot = Ssys + Ssurr ¢Stot = 125J=k + (¡125J=·) ¢Stot = 0J=K 4. qrev T 1000 ¢ 103 ¢S = 273 ¢S = 3663:0J=K ¢S = qrev T 1000 ¢ 103 ¢S = 323 ¢S = 3095:9J=K ¢S = the lower temperature has higher entropy