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

Calculate ΔS_surr (in units of J/K) for the process in which 2.00 mol of water are placed into a freezer at −10.0℃.

−22.8 J/K

−44.1 J/K

−45.8 J/K

+22.8 J/K

+45.8 J/K

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Verified step by step guidance

Identify the process: The problem involves calculating the change in entropy of the surroundings (ΔS_surr) when 2.00 mol of water is placed into a freezer at -10.0°C.

Understand the relationship: The change in entropy of the surroundings (ΔS_surr) is related to the heat exchanged with the surroundings (q_surr) and the temperature (T) by the formula: ΔS_surr = -q_sys / T, where q_sys is the heat absorbed or released by the system.

Determine the heat exchange: Since the water is being frozen, it releases heat to the surroundings. The heat released (q_sys) can be calculated using the formula q = n * ΔH_fusion, where n is the number of moles and ΔH_fusion is the enthalpy of fusion for water.

Convert temperature: Ensure the temperature is in Kelvin for the calculation. Convert -10.0°C to Kelvin by adding 273.15, resulting in 263.15 K.

Substitute values into the formula: Use the calculated q_sys and the converted temperature to find ΔS_surr using the formula ΔS_surr = -q_sys / T. This will give you the change in entropy of the surroundings in J/K.