Table of contents

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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

Mass Percent

General Chemistry

3. Chemical Reactions

Mass Percent

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Multiple Choice

The following data were collected when analyzing a compound used in dentistry as a cement to repair teeth:

50.82% Zn;16.04% P;33.14% O

What is the empirical formula of the compound?

Zn₃PO₂

Zn₁₆P₅O₁₀

Zn₆P₂O₄

Zn₃P₂O₈

Zn₅P₁₆O₃₃

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Verified step by step guidance

Step 1: Assume you have 100 grams of the compound. This means you have 50.82 grams of Zn, 16.04 grams of P, and 33.14 grams of O.

Step 2: Convert the mass of each element to moles by dividing by their respective molar masses. Use the molar masses: Zn = 65.38 g/mol, P = 30.97 g/mol, O = 16.00 g/mol.

Step 3: Calculate the moles of each element: Zn: \( \frac{50.82}{65.38} \), P: \( \frac{16.04}{30.97} \), O: \( \frac{33.14}{16.00} \).

Step 4: Determine the mole ratio by dividing each element's mole value by the smallest number of moles calculated in the previous step.

Step 5: Round the ratios to the nearest whole number to find the empirical formula. If necessary, multiply all ratios by the same factor to get whole numbers.