The Magnesium Metal Of Magnesium Oxide

1206 WordsFeb 24, 20165 Pages
In this experiment, we burned magnesium metal to produce magnesium oxide. To calculate the empirical formula of magnesium oxide, the purpose of our experiment, we weighed the magnesium metal prior to the burning and the resulting magnesium oxide at the end of the burning period. However, since our magnesium was coiled too tightly within the crucible, it did not burn for the entire 45 minutes of the lab, even when we added hydrochloric acid to speed up the reaction. Consequently, our results were erroneous, and we were unable to calculate the actual empirical formula, which is MgO. Therefore, we borrowed the data of another group, and understood that roughly 0.89 moles of oxygen were available per mole of magnesium, yielding the calculated empirical formula as MgO. Introduction The burning of magnesium produces light and carbon dioxide. This occurs because it is a combustion reaction. If we burn the magnesium out in the open, the oxygen would combine with the magnesium and the reaction would occur faster. The whole purpose of this investigation is to figure out the chemical equation by burning the magnesium in a slow and orderly fashion. To figure this balanced chemical equation out, we require the mass of the product that is created. Theory/Background When heated in air, magnesium reacts spontaneously with oxygen, producing a bright white light. This combustion creates magnesium oxide. The empirical formula, the lowest whole number ratio of all atoms in a compound or
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