For a particular spontaneous process the entropy change of the system, ΔSsys, is −62.0 J/K. What does this mean about the change in entropy of the surroundings, ΔSsurr?

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To understand what the given ΔSsys = −62.0 J/K implies for the surroundings, we need to apply the second law in terms of total entropy change.
First, recall that for a spontaneous (irreversible) process, the total entropy change ΔStotal = ΔSsys + ΔSsurr must be greater than zero.
If the system loses entropy by 62 J/K (ΔSsys = −62 J/K), the surroundings must compensate by increasing their entropy by at least more than 62 J/K to make the sum positive. In other words, ΔSsurr must be greater than +62 J/K.
Now evaluate the options one by one:
- Option A: ΔSsurr > +62 J/K. This matches the requirement that ΔSsys + ΔSsurr > 0 given ΔSsys = −62 J/K, since any ΔSsurr larger than +62 J/K yields a positive total entropy change. This option is consistent with the second law for a spontaneous process.
- Option B: ΔSsurr = −62 J/K. If the surroundings also decreased by 62 J/K, the total would be ΔStotal = −124 J/K, which is negative and corresponds to a non-spontaneous or irreversible constraint not allowed for a spontaneous process.
- Option C: I am unsure and need to study this concept to prepare for the exam. This reflects a lack of understanding of the entropy balance concept; it is not an evaluative statement about the thermodynamics, but an uncertainty about the principle.
- Option D: ΔSsurr < −62 J/K. Here the surroundings lose even more entropy than the system gains, leading to an overall negative ΔStotal, which would imply a non-spontaneous or externally driven process, contradicting the spontaneous process scenario described.
- Option E: ΔSsurr = +62 J/K. With equality, the total entropy change would be ΔStotal = 0, which characterizes a system at equilibrium, not a spontaneous process. Since the problem specifies spontaneity, this equality does not fit.
In summary, the only choice that satisfies the condition for spontaneity given a negative ΔSsys of −62 J/K is a surplus positive entropy change in the surroundings greater than +62 J/K, while the other options fail to meet the required total entropy criterion or describe equilibrium or non-interpretations.

CHEM 1220 SP2025 (18215) CHEM 1220 Practice Exam #4 v1 (17.4 - 17.6, 19, 20.1 - 20.5)- Requires Respondus LockDown Browser

For a particular spontaneous process the entropy change of the system, ΔSsys, is −62.0 J/K. What does this mean about the change in entropy of the surroundings, ΔSsurr?

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