mag lab student example (EX5)

mag lab student example (EX5) - Burning Magnesium Lab...

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Burning Magnesium Lab Introduction When magnesium is heated within the presence of oxygen it forms magnesium oxide. This same experiment was conducted in a Crescent Valley science lab using a crucible to heat the magnesium in and a Bunsen burner to heat the crucible. This lab was conducted to prove that a compound’s empirical formula can be determined experimentally. The empirical formula of a compound is the lowest whole number ratio of atoms of elements in the compound. The product made within this lab, magnesium oxide, should theoretically have the empirical formula MgO. We have learned about empirical formulas in class, as well as percent composition. Percent composition is the percent by mass of each element in a compound. Within this lab, we worked with magnesium oxide and its empirical formula and percent composition. Theoretically, we determined these to be MgO and 60.3% Mg, 39.7% O, respectively. Also, theoretically (with use of a periodic table), we determined the reaction within this lab to be represented by this chemical formula: 2Mg + O 2 2MgO. The product was created though a mix of combustion and combination of reactant atoms. Combustion reactions create light and heat, as seen as a bright flare of yellow light when the magnesium in the crucible was exposed to oxygen. Solid combination products (in this case magnesium oxide) will have a greater mass than their reactant counterpart (magnesium). The empirical formula of a compound can be discovered experimentally through a process of conversion factors. In the case of this lab you must use the initial mass of magnesium and the calculated mass of oxygen in the product to find the percent composition of the product. Once those numbers are found, use them to convert from grams (since percent composition is the percent by mass
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mag lab student example (EX5) - Burning Magnesium Lab...

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