TheSynthesisofMagnesiumOxideLabReport (1).docx - AudreyAnna...

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AudreyAnna Aragon CHEM 121L Section 04 , Determination of Magnesium Oxide’s Empirical Formula Abstract This procedure’s main purpose was to synthesize Magnesium Oxide through a roasting process to determine the ratios of each element. We roasted pure Magnesium of known mass to create Magnesium Oxide, and weighed this to measure how much oxygen was absorbed, and therefore the ratios of each element in the resulting compound. We found that the empirical formula of Magnesium Oxide is Mg1O1. Introduction Joseph Proust, a highly successful French chemist of the 19th century, discovered the Law of Definite Proportions. He found that for a given compound, the proportions of each element will always be constant. Proportions are the defining numbers in an empirical formula. Though molecular formulas are more complicated to derive, empirical formulas can be fairly simple to derive through experimentation by measurement of the mass of each element in a compound. In this experiment, we derive the empirical formula of Magnesium Oxide by synthesizing it with a known amount of Magnesium and a measured amount of oxygen to find it’s proportions. Experimental Data First, to explore the combustion of Magnesium, we burned a small strip of it. We noticed that it burned extremely bright, too bright to observe directly. When it was finished burning, it left a white powder residue. We then set up our bunsen burner to roast a crucible with a small amount of Magnesium. First, we set the flame on the empty crucible to dry out all the water contained within the ceramic.

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