CHY 123 Lecture Notes - Lecture 7: Chemical Formula, Molar Mass, Empirical Formula
Document Summary
Chy chapter 3 mass relationships and chemical. Using the atomic mass of elements and the over all molar mass when in a compound, you can determine the mass percentage of each element in the compound. Do it everytime for each element in compound mass of a in whole x. The simplest whole number ratio b/w numbers of different elements in a compound. Glucose has a molecular formula of c6h12o6 so the empirical formula is. Example: vitamin c has 40. 92% carbon, 4. 58% hydrogen, and 54. 50% oxygen. Combustion analysis - a technique requiring you to burn a sample of the unknown substance in a large excess of oxygen gas. The combustion products will be trapped separately from each other and the weight of each combustion product will be determined. From this, you will be able to calculate the empirical formula of the substance. Example: we have a 0. 2000g sample made up of c, h, and o.