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

3. Chemical Reactions

Empirical Formula

General Chemistry

3. Chemical Reactions

Empirical Formula

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Multiple Choice

A compound consists of 36.33% carbon, 6.11% hydrogen, 21.20% nitrogen, and 36.31% oxygen. What is the empirical formula for this compound?

C4H8N4O4

C3H6N3O3

CH2NO

C2H4N2O2

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Verified step by step guidance

Step 1: Begin by assuming you have 100 grams of the compound. This assumption allows you to directly convert the percentage of each element to grams. Therefore, you have 36.33 grams of carbon, 6.11 grams of hydrogen, 21.20 grams of nitrogen, and 36.31 grams of oxygen.

Step 2: 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 1.01 g/mol, nitrogen (N) is 14.01 g/mol, and oxygen (O) is 16.00 g/mol. Use the formula: \( \text{moles} = \frac{\text{mass in grams}}{\text{molar mass}} \).

Step 3: Calculate the moles for each element: \( \text{moles of C} = \frac{36.33}{12.01} \), \( \text{moles of H} = \frac{6.11}{1.01} \), \( \text{moles of N} = \frac{21.20}{14.01} \), \( \text{moles of O} = \frac{36.31}{16.00} \).

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

Step 5: Use the mole ratios to write the empirical formula. The empirical formula is the simplest whole number ratio of atoms in the compound, which corresponds to the ratios calculated in the previous step.