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

Endothermic & Exothermic Reactions

General Chemistry

8. Thermochemistry

Endothermic & Exothermic Reactions

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Multiple Choice

What is the basic difference between exergonic and endergonic reactions?

Exergonic reactions require a catalyst, while endergonic reactions do not.

Exergonic reactions occur only at high temperatures, while endergonic reactions occur at low temperatures.

Exergonic reactions increase entropy, while endergonic reactions decrease entropy.

Exergonic reactions release energy, while endergonic reactions absorb energy.

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Verified step by step guidance

Understand the terms: Exergonic and Endergonic reactions are terms used to describe the energy changes in chemical reactions.

Exergonic reactions are characterized by the release of energy. This means that the products of the reaction have less free energy than the reactants, indicating that energy is released to the surroundings.

Endergonic reactions, on the other hand, absorb energy. In these reactions, the products have more free energy than the reactants, meaning that energy is absorbed from the surroundings.

The key difference lies in the direction of energy flow: Exergonic reactions release energy (often in the form of heat or light), while endergonic reactions require an input of energy to proceed.

This energy change can be represented by the Gibbs free energy change (ΔG). For exergonic reactions, ΔG is negative, indicating a release of energy. For endergonic reactions, ΔG is positive, indicating an absorption of energy.