Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 36m
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

Previous problemNext problem

Struggling with General Chemistry?

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

Multiple Choice

What is the empirical formula for a compound containing 34.4% ethylenediamine, 2.101% Ni, 3.44% sulfate, and 60.06% water by mass?

C2H8N2Ni(SO4)2·6H2O

C2H8N2NiSO4·6H2O

C2H8N2NiSO4·4H2O

C2H4N2NiSO4·6H2O

Previous problemNext problem

Verified step by step guidance

Step 1: Convert the percentage composition of each component to grams, assuming you have 100 grams of the compound. This means you have 34.4 grams of ethylenediamine, 2.101 grams of Ni, 3.44 grams of sulfate, and 60.06 grams of water.

Step 2: Calculate the moles of each component. Use the molar mass of each component: ethylenediamine (C2H8N2), Ni, sulfate (SO4), and water (H2O). For example, moles of ethylenediamine = 34.4 g / molar mass of C2H8N2.

Step 3: Determine the simplest whole number ratio of moles of each component. Divide the moles of each component by the smallest number of moles calculated in the previous step.

Step 4: Use the whole number ratios to write the empirical formula. The empirical formula is the simplest ratio of the elements in the compound.

Step 5: Verify the empirical formula by checking if the calculated formula matches one of the given options. Consider the hydration number (number of water molecules) in the formula as well.