Table of contents

1. Introduction to Anatomy & Physiology5h 43m
2. Cell Chemistry & Cell Components12h 36m
3. Energy & Cell Processes10h 6m
4. Tissues & Histology10h 3m
5. Integumentary System2h 20m
6. Bones & Skeletal Tissue2h 16m
7. The Skeletal System2h 35m
8. Joints2h 17m
9. Muscle Tissue2h 33m
10. Muscles1h 11m
11. Nervous Tissue and Nervous System1h 35m
12. The Central Nervous System1h 6m
- Introduction to the Central Nervous System
  18m
- The Cerebrum
  48m
13. The Peripheral Nervous System1h 26m
14. The Autonomic Nervous System1h 38m
15. The Special Senses2h 41m
16. The Endocrine System2h 48m
17. The Blood3h 22m
18. The Heart3h 42m
19. The Blood Vessels3h 35m
20. The Lymphatic System3h 16m
21. The Immune System14h 37m
22. The Respiratory System3h 20m
23. The Digestive System2h 5m
24. Metabolism and Nutrition4h 0m
25. The Urinary System2h 39m
26. Fluid and Electrolyte Balance, Acid Base Balance37m
27. The Reproductive System2h 5m
28. Human Development1h 21m
29. Heredity3h 32m

2. Cell Chemistry & Cell Components

Properties of Water- Thermal

Anatomy & Physiology

2. Cell Chemistry & Cell Components

Properties of Water- Thermal

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Multiple Choice

Which action would involve the greatest transfer of heat?

Changing the temperature of 1 g of water from 10°C to 90°C

Cooling 10 g of water from 80°C to 40°C

Evaporating 1 g of water at 25°C

Condensing 5 g of steam to liquid water

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Verified step by step guidance

Understand that heat transfer involves changes in temperature or phase of a substance. In this problem, we are comparing the heat transfer involved in changing temperature and phase of water.

Calculate the heat required to change the temperature of 1 g of water from 10°C to 90°C using the formula: \( q = m \cdot c \cdot \Delta T \), where \( q \) is the heat absorbed or released, \( m \) is the mass, \( c \) is the specific heat capacity of water (4.18 J/g°C), and \( \Delta T \) is the change in temperature.

Calculate the heat released when cooling 10 g of water from 80°C to 40°C using the same formula: \( q = m \cdot c \cdot \Delta T \).

Calculate the heat required to evaporate 1 g of water at 25°C using the formula: \( q = m \cdot L_v \), where \( L_v \) is the latent heat of vaporization for water (approximately 2260 J/g).

Compare the calculated heat values for each process. The process with the greatest heat transfer will involve the largest value of \( q \). Note that condensing steam to liquid water involves a phase change, which typically involves a significant amount of heat transfer due to the latent heat of condensation.