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

Empirical Formula

GOB Chemistry

6. Chemical Reactions & Quantities

Empirical Formula

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Multiple Choice

Elemental analysis of a sample of an ionic compound showed 2.82 g of Na, 4.35 g of Cl, and 7.83 g of O. What is the empirical formula of the compound?

NaClO

NaClO₂

NaClO₃

NaClO₄

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Verified step by step guidance

Step 1: Determine the number of moles of each element in the compound. Use the molar mass of each element: Na (22.99 g/mol), Cl (35.45 g/mol), and O (16.00 g/mol). Calculate the moles of Na, Cl, and O by dividing the given mass of each element by its molar mass.

Step 2: Calculate the moles of sodium (Na) by dividing 2.82 g by 22.99 g/mol.

Step 3: Calculate the moles of chlorine (Cl) by dividing 4.35 g by 35.45 g/mol.

Step 4: Calculate the moles of oxygen (O) by dividing 7.83 g by 16.00 g/mol.

Step 5: Determine the simplest whole number ratio of moles of each element by dividing each mole value by the smallest number of moles calculated in the previous steps. This will give you the empirical formula of the compound.