Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

21. The Generation of Biochemical Energy

Intro to Metabolism

GOB Chemistry

21. The Generation of Biochemical Energy

Intro to Metabolism

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3:27 minutes

Problem 29

Textbook Question

Why is ∆G a useful quantity for predicting the favorability of biochemical reactions?

Verified step by step guidance

Understand that ∆G, or Gibbs free energy change, is a thermodynamic quantity that combines enthalpy (∆H), entropy (∆S), and temperature (T) to determine the spontaneity of a reaction. The formula is:

Δ G = Δ H - T Δ S

Recognize that a negative ∆G value indicates a spontaneous reaction under the given conditions, meaning the reaction is thermodynamically favorable and can proceed without external energy input.

Note that ∆G provides insight into both the energy changes (enthalpy) and the disorder (entropy) of a system, making it particularly useful for understanding complex biochemical reactions where both factors are important.

Understand that in biochemical systems, ∆G can predict whether a reaction will occur under physiological conditions, which is critical for processes like metabolism, enzyme activity, and energy transfer.

Realize that ∆G also helps in determining equilibrium positions and the extent to which a reaction will proceed, which is essential for understanding reaction dynamics in living organisms.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Gibbs Free Energy (∆G)

Gibbs Free Energy (∆G) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. It is a crucial indicator of the spontaneity of a reaction; a negative ∆G value suggests that a reaction can occur spontaneously, while a positive value indicates that the reaction is non-spontaneous under standard conditions.

Spontaneity of Reactions

The spontaneity of a reaction refers to its tendency to proceed without external influence. This is determined by the sign of ∆G: reactions with a negative ∆G are spontaneous, meaning they can occur naturally, while those with a positive ∆G require energy input to proceed. Understanding spontaneity helps predict whether a biochemical reaction will occur in living organisms.

Thermodynamic Equilibrium

Thermodynamic equilibrium is the state in which a system's macroscopic properties remain constant over time, indicating that the forward and reverse reactions occur at equal rates. At equilibrium, ∆G equals zero, meaning there is no net change in the concentrations of reactants and products. This concept is essential for understanding how biochemical reactions can shift in response to changes in conditions, such as concentration and temperature.

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