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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?

$2.47 \times 10^{-23} J/K$

Chemistry 102

Chapter 16

Thermodynamics

Carleton College

University of Central Florida

Lectures

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question. Number 10 is a change in entropy equation using the Ludwig Bolts Hman equation and the number of potential micro states. If we have all of the energy to units of energy on just the Adam A, as shown in figure 16 9, then there's only one initial micro state. But then, if those two units of energy and that being distributed between two different particles than the possible micro states that can exist, are one unit of energy on a one unit of energy and be that's one micro state. One unit of energy on A when went on C one on a one on D one on B one and C one on B one and D and one on C one on the That's a total of six Micro States after the energy has been distributed, so we'll use the left with Holzmann equation. Delta's is equal to bolt cement constant 1.38 times 10. The negative three jewels per kelvin, multiplied by the natural log of our six micro states is the final over the initial one micro state, and we get 2.47 times 10 to the negative 23 jewels per Calvin

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