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

Molecular Formula

General Chemistry

3. Chemical Reactions

Molecular Formula

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Multiple Choice

Determine the molecular formula for the compound with a molar mass of 46.08 g/mol and the following percent composition: C: 26.06%, H: 13.13%, N: 60.81%.

CH4N2

CH3NO

C2H6N

C2H4N2

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Verified step by step guidance

Step 1: Convert the percentage composition of each element to grams, assuming you have 100 grams of the compound. This means you have 26.06 grams of Carbon (C), 13.13 grams of Hydrogen (H), and 60.81 grams of Nitrogen (N).

Step 2: Calculate the number of moles of each element using their atomic masses. Use the formula: \( \text{moles} = \frac{\text{mass in grams}}{\text{atomic mass}} \). The atomic masses are approximately: C = 12.01 g/mol, H = 1.01 g/mol, N = 14.01 g/mol.

Step 3: Determine the mole ratio of the elements by dividing the moles of each element by the smallest number of moles calculated in Step 2. This will give you the empirical formula.

Step 4: Calculate the molar mass of the empirical formula obtained in Step 3 and compare it to the given molar mass of 46.08 g/mol. If they match, the empirical formula is also the molecular formula.

Step 5: If the molar mass of the empirical formula does not match the given molar mass, multiply the subscripts in the empirical formula by a whole number to obtain the molecular formula that matches the given molar mass.