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 Heart2h 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

3. Energy & Cell Processes

Chemical Reactions

Anatomy & Physiology

3. Energy & Cell Processes

Chemical Reactions

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Multiple Choice

Molecules A and B contain 110 kcal/mol of free energy, and molecules B and C contain 150 kcal/mol of energy. A and B are converted to C and D. What can be concluded?

A and B will be converted to C and D with a net release of energy.

The conversion of A and B to C and D is exergonic; the products are less organized than the reactants.

The conversion of A and B to C and D is spontaneous.

The entropy in the products, C and D, is higher than in the reactants, A and B.

The reaction that proceeds to convert A and B to C and D is endergonic; the products are more organized than the reactants.

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Verified step by step guidance

Begin by understanding the concept of free energy in chemical reactions. Free energy, often denoted as Gibbs free energy (G), is the energy available to do work. In a chemical reaction, the change in free energy (ΔG) determines whether the reaction is spontaneous or requires energy input.

Calculate the total free energy of the reactants (A and B) and the products (C and D). Molecules A and B together contain 110 kcal/mol of free energy, while molecules B and C contain 150 kcal/mol. Since B is common in both pairs, focus on the net change in energy.

Determine the change in free energy (ΔG) for the reaction. The formula for ΔG is: ΔG = G_products - G_reactants. Substitute the values: ΔG = (energy of C and D) - (energy of A and B).

Analyze the sign of ΔG. If ΔG is positive, the reaction is endergonic, meaning it requires energy input and the products are more organized than the reactants. If ΔG is negative, the reaction is exergonic, meaning it releases energy and the products are less organized.

Conclude based on the calculated ΔG. Since the problem states that the reaction is endergonic, it implies that the products (C and D) are more organized than the reactants (A and B), and the reaction requires an input of energy.