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

6. Chemical Reactions & Quantities

Mole Concept

GOB Chemistry

6. Chemical Reactions & Quantities

Mole Concept

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1:50 minutes

Problem 85a

Textbook Question

What is the mass (in amu and in grams) of a single atom of Carbon-12?

Verified step by step guidance

Understand the problem: Carbon-12 is an isotope of carbon with a mass number of 12. The mass of a single atom of Carbon-12 is defined as exactly 12 atomic mass units (amu) by definition of the atomic mass unit.

To express the mass in grams, recall the relationship between amu and grams: 1 amu = 1.660539066 × 10⁻²⁴ grams.

Multiply the mass of the Carbon-12 atom in amu (12 amu) by the conversion factor to convert it to grams: \( \text{Mass in grams} = 12 \times 1.660539066 \times 10^{-24} \).

Perform the multiplication to determine the mass of a single Carbon-12 atom in grams. This step involves basic arithmetic with scientific notation.

Summarize the results: The mass of a single Carbon-12 atom is 12 amu by definition, and the calculated value in grams will be the result of the multiplication in the previous step.

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Key Concepts

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

Atomic Mass Unit (amu)

The atomic mass unit (amu) is a standard unit of mass used to express atomic and molecular weights. It is defined as one twelfth of the mass of a carbon-12 atom, which is approximately 1.66 x 10^-27 kilograms. This unit allows for easier comparison of the masses of different atoms and molecules, as they are typically very small.

Carbon-12 Isotope

Carbon-12 is one of the most common isotopes of carbon, consisting of 6 protons and 6 neutrons in its nucleus. It is used as a standard for atomic mass measurements and has an atomic mass of exactly 12 amu. Understanding isotopes is crucial for calculations involving atomic mass, as different isotopes of an element can have varying masses.

Conversion between amu and grams

The conversion between atomic mass units (amu) and grams is essential for expressing atomic masses in a more practical unit. One amu is equivalent to 1.66053906660 x 10^-24 grams. This relationship allows scientists to convert the mass of an atom from amu to grams, facilitating calculations in chemistry and physics.