The Empirical Formula Of Magnesium Oxide

1359 WordsOct 27, 20156 Pages
bstract * TERMS* The objective of this lab was to find the empirical formula of magnesium oxide. In order to produce magnesium oxide. In this experiment, magnesium reacted in an oxygen-rich environment while inside of a crucible. The masses before and after the oxidation were both measured. The masses that were resulted were then used to calculate the empirical formula of magnesium oxide. The simplest whole-number in the form of a ratio in which atoms join and form a compound is known as the empirical formula. By finding the percent composition of each element in the compound you are able to determine the empirical formula. When finding the empirical formula it is important to know how to find things such as the limiting reagent, percent yield along with the theoretical yield. The limiting reagent is a substance that will not let the reaction proceed because of its presence. The percent yield and the theoretical yield are both found by comparing the reaction and the experimental yield and recording those results. Introduction When it comes to chemistry, compounds will always more than one elements. These elements will always have a mixture of a certain proportion by mass for a given compound. When dealing with compounds it is important to find the empirical formula because it helps to show all the known elements of that compound and they display the smallest whole number of moles and the number of atoms each element contains. Empirical formulas are helpful for finding an
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