Suppose we have two identical boxes of matter, A and B, that are in thermal contact but cannot exchange materials. They come to thermal equilibrium. System 1 consists of box A alone, while system 2 consists of both boxes A and B. What can you say about the entropy of the two systems? Choose all correct answers.
a. The entropy of system 2 is twice as high as that of system 1.b. The entropy of system 2 is a lot more than twice as high compared to system 1.c. The number of microstates of system 2 is twice as high as those of system 1.d. The number of microstates of system 2 is a lot more than twice as high as those of system 1.e. You cant tell anything about the comparative entropy of the two systems without more information.

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Answer:

Explanation:

a) The entropy of system 2 is twice as high as that of system 1.

d) The number of microstates of system 2 is a lot more than twice as high as those of system 1

Option (a) and (d) are the correct answers.

The correct answer is option (c) the number of microstates of system 2 is twice as high as those of system 1.

The answer can be explained using the second law of thermodynamics.

  • Given that both the boxes are in thermal equilibrium. This means that there is no energy exchange between the systems.
  • According to the second law of thermodynamics, we can say that the entropy of a thermally isolated system in equilibrium will be at a maximum and constant value.
  • As both the boxes are in thermal equilibrium, we can say that the entropy of system 1 and system 2 are equal.
  • But both systems can have a specific number of microstates.

System 1 = [tex]A[/tex]

System  2 = [tex]A+B[/tex]

Given that, both the boxes are identical.

  • Therefore, [tex]System\,2 = 2\times(System\,1)[/tex]
  • So, the number of microscopic configurations for system 2 will be twice as much as that of system 2.
  • [tex]P(System\,2) = P(A+B) = P(2A)[/tex]

So, we can say that the number of microstates of system 2 is twice as high as those of system 1.

Learn more about entropy and microstates here:

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