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

8. Thermochemistry

Thermal Equilibrium

General Chemistry

8. Thermochemistry

Thermal Equilibrium

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Multiple Choice

How much heat is released when 125.0 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol·°C).

30.1 kJ

60.5 kJ

45.2 kJ

75.3 kJ

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Verified step by step guidance

Calculate the number of moles of water using the formula: \( n = \frac{m}{M} \), where \( m \) is the mass of the water (125.0 g) and \( M \) is the molar mass of water (18.02 g/mol).

Determine the heat released during the condensation of steam to liquid water at 100.0°C using the formula: \( q_1 = n \times \Delta H_{vap} \), where \( \Delta H_{vap} \) is the enthalpy of vaporization (40.67 kJ/mol).

Calculate the heat released when the liquid water cools from 100.0°C to 0.0°C using the formula: \( q_2 = n \times C_{p,water} \times \Delta T \), where \( C_{p,water} \) is the molar heat capacity of liquid water (75.4 J/(mol·°C)) and \( \Delta T \) is the temperature change.

Determine the heat released during the freezing of water at 0.0°C using the formula: \( q_3 = n \times \Delta H_{fus} \), where \( \Delta H_{fus} \) is the enthalpy of fusion (6.01 kJ/mol).

Calculate the heat released when the ice cools from 0.0°C to -15.0°C using the formula: \( q_4 = n \times C_{p,ice} \times \Delta T \), where \( C_{p,ice} \) is the molar heat capacity of ice (approximately 36.6 J/(mol·°C)). Sum all the heat changes: \( q_{total} = q_1 + q_2 + q_3 + q_4 \) to find the total heat released.