Ch.3 - Chemical ReactionsSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Combustion analysis is a technique where an organic compound is combusted (exploded!!!) and the products are quantitatively measured. 

Understanding Combustion Analysis

Concept #1: Combustion Analysis Determination 

In a combustion reaction an organic compound made of carbon and hydrogen or carbon, hydrogen and oxygen is combusted to form carbon dioxide and water as products. 

Example #1: A 0.2500 g sample contains carbon, hydrogen and oxygen and undergoes complete combustion to produce 0.3664 g of CO2 and 0.1500 g of H2O. What is the empirical formula of the compound?

Additional Problems
If 3.25 g of butane (C4H10, M = 58.14) is burned (combusted) in the presence of excess O2, what is the mass of CO2 that forms, in g? Enter your answer with 2 decimal places and no units.
Para-cresol is used as a disinfectant. A 0.3654 g sample of this compound that contains only C, H, and O, gave 1.0420 g CO2 and 0.2437 g H2O in a combustion analysis. Its molecular mass is 108.1g/mol. What is its molecular formula? a. C7H8Ob. C6H7Oc. C7H7O2d. C6H7O2e. C7H8O2
Combustion analysis of a 12.01 g sample of tartaric acid, which contains only  carbon, hydrogen, and oxygen, produced 14.08 g CO2 and 4.32 g H2O. a) What is the empirical formula of tartaric acid?             b) If 0.250 moles of the compound weighs 37.52 g, what is the molecular formula of the compound?  
The combustion of 4.16 grams of a compound which contains only C,H,O and F yields 7.7 g CO2 and 2.52 g H2O. Another sample of the compound with a mass of 3.63 g is found to contain 0.58 g F. What is the empirical formula of the compound? A. C3H8O2FB. C4H10OFC. C4H8OFD. C5H8O2F
A 4.05 g sample of a compound containing only C, H, and O was burned completely. The only combustion products were 10.942 g CO2 and 4.476 g H2O. What is the empirical formula of the compound?A) C7H7OB) C7H14O7C) CH2OD) C7H14OE) C6H12O
Combustion analysis of an unknown compound containing only carbon and hydrogen produced 4.554 g of CO2 and 2.322 g of H2O. What is the empirical formula of the compound?A) C4H10B) CH2 C) C2H5D) C5H2
Combustion analysis of 2.400 g of an unknown compound containing carbon, hydrogen, and oxygen produced 4.171 g of CO2 and 2.268 g of H2O. What is the empirical formula of the compound?A) C2H5O2B) C2H5OC) C2H10O3 D) C3H8O2
Isoeugenol is the compound which gives the characteristic odor to nutmeg and contains carbon, hydrogen, and oxygen. If a 0.500 g sample of isoeugenol is combusted it gives 1.341 g of CO2 and 0.329 g of H2O. Isoeugenol has a molecular weight of 164 g/mol. What is the molecular formula of isoeugenol?A) C8H4O4B) C10H12O2 C) C2HOD) C5H6O
A strip of pure copper metal weighing 3.178 g is heated in the presence of oxygen gas. In the process, all of the copper reacts with oxygen to form 3.978 g of a black copper oxide. What is the empirical formula for this copper oxide?Given that the molar mass of the compound is about 80 g, name this compound.
2.404 g of a compound were burned in oxygen and found to produce only 3.520 g CO2 (g), 2.564 g SO2 (g) and 1.440 g H2O (l). Determine the empirical formula of the compound.A) C2SH4B) C2SH2C) CSHD) C4SH2 E) C2S2H4
There are two binary compounds of mercury and oxygen. Heating either of them results in the decomposition of the compound, with oxygen gas escaping into the atmosphere while leaving a residue of pure mercury. Heating 0.6498 g of one of the compounds leaves a residue of 0.6018 g. Heating 0.4172 g of the other compound results in a mass loss of 0.016 g. Determine the empirical formula of each compound.
A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the compound yields 16.01 mg CO2 and 4.37 mg H2O. The molar mass of the compound is 176.1 g/mol. What are the empirical and molecular formulas of the compound?
Combustion analysis of 63.8 mg of a C, H and O containing compound produced 145.0 mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound?A) C5H2OB) CHOC) C3H6OD) C3H7OE) C6HO3
On combustion analysis, a 0.450 g sample of a chemical compound gives 0.418 g of water and 1.023 g of carbon dioxide. Assuming that the empirical formula of the compound is CxHyOz, find the values of x, y and z.
A hydrocarbon  with general formula CxHy was burned completely in air, yielding 0.18 g of water and 0.44 g of carbon dioxide. Which formula could give such data?A. C2H2B. C2H4C. C2H6D. C6H6
Determine the empirical formula for a hydrocarbon if the complete combustion of a sample produces 5.28 g of CO2 and 1.62 g of H2O. 
The combustion of ethane (C2H6) produces carbon dioxide and steam: 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l) How many moles of CO2 are produced when 5.85 mol of ethane are burned in an excess of oxygen?
In the combustion of hydrogen gas, hydrogen reacts with oxygen from the air to form water vapor. If you burn 33.5 g of hydrogen and produce 299 g of water, how much oxygen reacted?