ENTROPY, MICROSTATES, AND PROBABILITY Overview Expansion of a gas at the molecular level is explained in terms of particle motion and probability. Learning Objectives At the end of the activity I am able to: 1. Explain a spontaneous process - such as air rushing in to an evacuated chamber - using particle motion at the molecular level; 2. Distinguish between spontaneous and non-spontaneous processes, and connect these to a probabilistic description of matter; 3. Explain how a large number of microstates can produce the same macro-state; 4. Use particle motion and probability to explain heat transfer. Procedure Direction: This is a guided inquiry activity. Visit the links suggested and observe. Answer the questions in the space provided. Air Entering an Evacuated Chamber Image CC BY censed from H. Grobe via Wikimedia Figure 1: Air Moving into an Evacuated Chamber. Figure 1 shows a vacuum pump has been removing air form the glass chamber. Q4. Research the meaning of the phrase "Nature abhors a vacuum". What does this physically means to you?

ENTROPY, MICROSTATES, AND PROBABILITY Overview Expansion of a gas at the molecular level is explained in terms of particle motion and probability. Learning Objectives At the end of the activity I am able to: 1. Explain a spontaneous process - such as air rushing in to an evacuated chamber - using particle motion at the molecular level; 2. Distinguish between spontaneous and non-spontaneous processes, and connect these to a probabilistic description of matter; 3. Explain how a large number of microstates can produce the same macro-state; 4. Use particle motion and probability to explain heat transfer. Procedure Direction: This is a guided inquiry activity. Visit the links suggested and observe. Answer the questions in the space provided. Air Entering an Evacuated Chamber Image CC BY censed from H. Grobe via Wikimedia Figure 1: Air Moving into an Evacuated Chamber. Figure 1 shows a vacuum pump has been removing air form the glass chamber. Q4. Research the meaning of the phrase "Nature abhors a vacuum". What does this physically means to you?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter13: Spontaneous Processes And Thermodynamic Equilibrium

Section: Chapter Questions

Problem 35P

See similar textbooks

Similar questions

In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
List the sets of conditions that allow dS, dU, and dH of a process in a system act as a spontaneity condition.
For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
Why isnt the entropy of elements in their standard pressure at normal that is, room temperatures equal to zero?
Explain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.
The synthesis of glucose directly from CO2 and H2O and the synthesis of proteins directly from amino acids are both non-spontaneous processes under standard conditions. Yet it is necessary for these to occur for life to exist. In light of the second law of thermodynamics, how can life exist?
Plants take in CO2(g) and H2O(l) and make glucose, C6H12O6(s), and O2(g). Determine the standard entropy change for the overall reaction.
Try to find one additional example of a spontaneous process that is in fact endothermic that is, it occurs with an absorption of heat.
Many plastic materials are organic polymers that contain carbon and hydrogen. The oxidation of these plastics in air to farm carbon dioxide and water is a spontaneous process; however, plastic materials tend to persist in the environment. Explain.
Consider the system shown in Figure 16.9. What is the change in entropy for the process where the energy is initially associated only with particle A, but in the final state the energy is distributed between two different particles?
Explain why absolute entropies can be measured.
Limestone is predominantly CaCO3, which can undergo the reaction CaCO3(s)CaO(s)+CO2(g). We know from experience that this reaction is not spontaneous, yet S for the reaction is positive. How can the second law of thermodynamics explain that this reaction is not spontaneous?