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

Previous problemNext problem

Struggling with GOB Chemistry?

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

Multiple Choice

A compound that contains only carbon, hydrogen, and oxygen is composed of 48.64% C and 43.2% O by mass. What is the empirical formula of this compound?

C₃H₆O₂

CH₂O₂

CH₄O

C₂H₆O₂

Previous problemNext problem

Verified step by step guidance

Step 1: Begin by assuming you have 100 grams of the compound. This assumption simplifies calculations because the percentage of each element can be directly converted to grams. Therefore, you have 48.64 grams of carbon, 43.2 grams of oxygen, and the remainder will be hydrogen.

Step 2: Calculate the mass of hydrogen. Since the total mass is 100 grams, subtract the mass of carbon and oxygen from 100 grams to find the mass of hydrogen: 100 - 48.64 - 43.2 = 8.16 grams of hydrogen.

Step 3: Convert the mass of each element to moles using their respective molar masses. The molar mass of carbon (C) is approximately 12.01 g/mol, hydrogen (H) is about 1.01 g/mol, and oxygen (O) is roughly 16.00 g/mol. Calculate the moles for each element: moles of C = 48.64 g / 12.01 g/mol, moles of H = 8.16 g / 1.01 g/mol, moles of O = 43.2 g / 16.00 g/mol.

Step 4: Determine the mole ratio of the elements by dividing the moles of each element by the smallest number of moles calculated in Step 3. This will give you the simplest whole number ratio of the elements.

Step 5: Use the mole ratio to write the empirical formula. The empirical formula is the simplest whole number ratio of atoms in the compound. Adjust the ratios to the nearest whole numbers to find the empirical formula.