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

8. Gases, Liquids and Solids

Kinetic Molecular Theory

GOB Chemistry

8. Gases, Liquids and Solids

Kinetic Molecular Theory

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Multiple Choice

Which of the following statements would correctly explain the non-ideal behavior of a gas based on the Kinetic Molecular Theory (KMT)?

At high temperatures the attractive forces between molecules becomes negligible.

At high pressure the volume of gas molecules become significant.

An increase or decrease in the moles of gas causes the gas constant value to change.

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Verified step by step guidance

Begin by understanding the Kinetic Molecular Theory (KMT), which assumes that gas particles are in constant random motion and that they occupy negligible volume compared to the container they are in.

Recognize that KMT assumes no intermolecular forces between gas particles, meaning they do not attract or repel each other under ideal conditions.

Identify the conditions under which gases deviate from ideal behavior: high pressure and low temperature. At high pressure, the volume occupied by gas molecules becomes significant compared to the container volume.

Understand that at high pressure, the assumption that gas particles have negligible volume is no longer valid, leading to non-ideal behavior as the particles occupy a larger fraction of the container's volume.

Note that the gas constant value (R) does not change with the number of moles of gas; it is a constant in the ideal gas law equation, which is another reason why the statement about moles affecting the gas constant is incorrect.