Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

19. Chemical Thermodynamics

Spontaneous vs Nonspontaneous Reactions

General Chemistry

19. Chemical Thermodynamics

Spontaneous vs Nonspontaneous Reactions

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Multiple Choice

Which of the following is a true statement about ΔS_surroundings?

ΔS_surroundings is positive when the system absorbs heat from the surroundings.

ΔS_surroundings will decrease as a result of an exothermic process.

ΔS_surroundings is always positive when ΔS_univ is positive.

ΔS_surroundings is independent of the heat released or absorbed by the system.

ΔS_surroundings is always positive when ΔS_system is negative for a spontaneous process.

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Verified step by step guidance

Understand the concept of entropy (S) and how it relates to the surroundings and the system. Entropy is a measure of disorder or randomness in a system.

Recall that the change in entropy of the surroundings (ΔS_surroundings) is related to the heat exchanged with the surroundings and the temperature at which the exchange occurs. For an exothermic process, the system releases heat to the surroundings, increasing the entropy of the surroundings.

Consider the relationship between the system and the surroundings in terms of entropy. For a spontaneous process, the total entropy change of the universe (ΔS_univ) is positive, which means ΔS_system + ΔS_surroundings > 0.

Analyze each statement: ΔS_surroundings is positive when the system absorbs heat from the surroundings is incorrect because it would decrease the surroundings' entropy. ΔS_surroundings will decrease as a result of an exothermic process is incorrect because it increases. ΔS_surroundings is always positive when ΔS_univ is positive is not necessarily true as ΔS_system could be negative. ΔS_surroundings is independent of the heat released or absorbed by the system is incorrect as it directly depends on it.

Conclude that the correct statement is: ΔS_surroundings is always positive when ΔS_system is negative for a spontaneous process, as this ensures that ΔS_univ is positive, satisfying the condition for spontaneity.