CHY 103 Lecture Notes - Lecture 4: Combustion Analysis, Chemical Formula, Elemental Analysis
18 Jul 2016
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Things not covered but you really need to know: Determining a chemical formula from experimental data including table 3. 3 (polyatomic anions). Review: the empirical formula is the simplest whole number ratio between numbers of different elements making up a compound, e. g. glucose, has molecular formula is c6h12o6 ,the empirical formula is_____________ Elemental analysis techniques report composition of compounds in terms of percentages. Procedure for converting mass % to empirical formula: From mass percent assume a 100 g sample to obtain mass of each element: use atomic weights to obtain moles of each element, calculate mole ratio by dividing by lowest number of moles. If necessary, multiply to get the whole number mole ratio. Example: vitamin c has 40. 92 % c, 4. 58 % h and 54. 50 % o. Since the mole ratio of h is not close to a whole number we need to multiply by ____in order to make it whole.
