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 of a compound that has a molar mass of 92.0 g/mol and an empirical formula of NO₂.

NO₂

N₂O₄

N₂O

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Verified step by step guidance

First, calculate the molar mass of the empirical formula NO₂. The atomic mass of nitrogen (N) is approximately 14.01 g/mol, and the atomic mass of oxygen (O) is approximately 16.00 g/mol. Therefore, the molar mass of NO₂ is calculated as:

14.01 + 2 \times 16.00

g/mol.

Next, determine the ratio of the molar mass of the compound to the molar mass of the empirical formula. This is done by dividing the given molar mass of the compound (92.0 g/mol) by the molar mass of the empirical formula calculated in the previous step.

The result from the division in the previous step will give you a whole number or a number very close to a whole number. This number represents how many times the empirical formula must be multiplied to obtain the molecular formula.

Multiply the subscripts in the empirical formula NO₂ by the whole number obtained in the previous step to find the molecular formula. This involves multiplying each subscript in NO₂ by the whole number.

Finally, write the molecular formula using the new subscripts obtained from the multiplication. This will give you the molecular formula of the compound.