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Ch.19 - Chemical Thermodynamics

Chapter 19, Problem 30a

(a) What is the difference between a state and a microstate of a system?

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Hello everyone today. We are being given the following problem, differentiate a micro state of a system from a state of a system. So what we want to do is we want to recall a state and the state is going to describe the macro scope pick view of a system. So it's going to look at a big scale big scale factors such as pressure and temperature immediately that gets rid of answer choices, see indeed since they state that a state of a system describes the microscopic view and that is incorrect because we stated that it is a macroscopic view. Next you wanna recall the definition of a micro state and in a micro state right here in a micro state we're gonna have a micro scalp pick view of the systems atoms that corresponds to a systems given state. And so as we said before, this is going to be a specific write this in the beginning, it's a specific microscopic view. And so that only leaves answer choice B as being the correct answer. So once again, the micro state of a system is the specific microscopic arrangement of the atoms or molecules of the system. Whereas a state of a system describes the macroscopic view of the system at a specific time. And with that we've answered the question. I hope this helped. And until next time
Related Practice
Textbook Question

(c) During a certain reversible process, the surroundings undergo an entropy change, ΔSsurr = -78 J/K. What is the entropy change of the system for this process?

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Textbook Question

(a) What sign for Δ𝑆 do you expect when the pressure on 0.600 mol of an ideal gas at 350 K is increased isothermally from an initial pressure of 0.750 atm?

(b) If the final pressure on the gas is 1.20 atm, calculate the entropy change for the process.

(c) Which of the following statements about this process are true? (i) The entropy change you calculated will be the same for at any other constant temperature. (ii) The value of Δ𝑆 you calculated is valid only if the compression is done irreversibly. (iii) If the number of moles of gas being compressed were decreased by a factor of three, the entropy change would increase by a factor of three.

Textbook Question

For the isothermal expansion of a gas into a vacuum, ΔE = 0, q = 0, and w = 0. (b) Explain why no work is done by the system during this process.

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Textbook Question

(b) As a system goes from state A to state B, its entropy decreases. What can you say about the number of microstates corresponding to each state?

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Textbook Question

(c) In a particular spontaneous process, the number of microstates available to the system decreases. What can you conclude about the sign of ΔSsurr?

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Textbook Question

Would each of the following changes increase, decrease, or have no effect on the number of microstates available to a system: (b) decrease in volume

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