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

Which of the following statements is true regarding endergonic reactions?

Endergonic reactions release energy to the surroundings.

Endergonic reactions have a negative Gibbs free energy change.

Endergonic reactions occur spontaneously.

Endergonic reactions have a positive Gibbs free energy change.

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Verified step by step guidance

Begin by understanding the concept of Gibbs free energy (ΔG), which is a thermodynamic quantity used to predict the spontaneity of a reaction. It combines enthalpy (ΔH), temperature (T), and entropy (ΔS) in the equation:

Δ G = Δ H - T Δ S

Recognize that endergonic reactions are characterized by a positive Gibbs free energy change (

Δ G > 0

). This indicates that the reaction requires an input of energy from the surroundings to proceed.

Understand that because endergonic reactions have a positive ΔG, they are non-spontaneous under standard conditions. This means they do not occur without external energy input.

Clarify that endergonic reactions do not release energy to the surroundings; instead, they absorb energy. This is the opposite of exergonic reactions, which release energy and have a negative ΔG.

Conclude that the correct statement regarding endergonic reactions is that they have a positive Gibbs free energy change, which is why they require energy input to proceed.