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

Combustion Analysis

General Chemistry

3. Chemical Reactions

Combustion Analysis

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

Combustion analysis of 63.8 mg of a compound containing carbon, hydrogen, and oxygen produced 145.0 mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound?

C4H10O

C3H8O

C2H4O

C3H6O2

Previous problemNext problem

Verified step by step guidance

Start by determining the amount of carbon in the compound. Use the mass of CO2 produced to find the mass of carbon. The molar mass of CO2 is 44.01 g/mol, and the molar mass of carbon is 12.01 g/mol. Calculate the moles of CO2 using the formula:

\frac{145.0}{44.01}

. Then, use the ratio of carbon in CO2 to find the mass of carbon:

\frac{12.01}{44.01}

Next, determine the amount of hydrogen in the compound using the mass of H2O produced. The molar mass of H2O is 18.02 g/mol, and the molar mass of hydrogen is 1.01 g/mol. Calculate the moles of H2O using the formula:

\frac{59.38}{18.02}

. Then, use the ratio of hydrogen in H2O to find the mass of hydrogen:

\frac{2.02}{18.02}

Calculate the mass of oxygen in the compound. Subtract the mass of carbon and hydrogen from the total mass of the compound to find the mass of oxygen:

63.8 - mass of carbon - mass of hydrogen

Convert the masses of carbon, hydrogen, and oxygen to moles using their respective molar masses: Carbon:

\frac{mass of carbon}{12.01}

, Hydrogen:

\frac{mass of hydrogen}{1.01}

, Oxygen:

\frac{mass of oxygen}{16.00}

Determine the empirical formula by finding the simplest whole number ratio of moles of carbon, hydrogen, and oxygen. Divide each mole value by the smallest number of moles calculated in the previous step to get the ratio. Adjust the ratio to the nearest whole number to find the empirical formula.