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

19. Chemical Thermodynamics

Spontaneous vs Nonspontaneous Reactions

General Chemistry

19. Chemical Thermodynamics

Spontaneous vs Nonspontaneous Reactions

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

The reaction between carbon tetrachloride (CCl4) and water (H2O) to form carbon dioxide (CO2) and hydrogen chloride (HCl) has a ΔG° value of -232 kJ/mole, indicating it is thermodynamically favored. However, when you mix carbon tetrachloride with water, what occurs?

No reaction occurs because the activation energy is too high.

The reaction proceeds rapidly at room temperature.

The reaction occurs slowly, producing a small amount of products.

The reaction requires a catalyst to proceed.

Previous problemNext problem

Verified step by step guidance

Understand the concept of Gibbs free energy (ΔG°): A negative ΔG° value indicates that a reaction is thermodynamically favored, meaning it can occur spontaneously under standard conditions. However, this does not provide information about the rate of the reaction.

Consider the role of activation energy: Even if a reaction is thermodynamically favored, it may not occur if the activation energy is too high. Activation energy is the energy barrier that must be overcome for a reaction to proceed.

Analyze the given reaction: The reaction between carbon tetrachloride (CCl4) and water (H2O) to form carbon dioxide (CO2) and hydrogen chloride (HCl) has a ΔG° of -232 kJ/mole, suggesting it is favorable. However, the high activation energy can prevent the reaction from occurring at a noticeable rate.

Evaluate the conditions: At room temperature, without any additional energy input or catalyst, the high activation energy can prevent the reaction from proceeding, despite the favorable ΔG°.

Conclude based on the options: Since the activation energy is too high for the reaction to occur spontaneously at room temperature, the correct interpretation is that no reaction occurs under these conditions without a catalyst.