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Ch.19 - Chemical Thermodynamics
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All textbooksBrown 14th EditionCh.19 - Chemical ThermodynamicsProblem 30c

Chapter 19, Problem 30c

(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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Hello. In this problem, we are told for a given process, the number of micro states increased. We wanna know how is this related to the change in entropy of the system we call the bolts Mons equation then relates the entropy to the number of micro states K is called Holtzman's constant. And the number of micro states is given by W. So as the number of micro states increases, so will the entropy and so our change in entropy or the system will be positive in sign. This then corresponds to answer a thanks for watching. Hope this helps.
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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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Indicate whether each statement is true or false. (a) Unlike enthalpy, where we can only ever know changes in H, we can know absolute values of S. (b) If you heat a gas such as CO2, you will increase its degrees of translational, rotational and vibrational motions. (c) CO2(g) and Ar(g) have nearly the same molar mass. At a given temperature, they will have the same number of microstates.

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