Empirical Formula Of Magnesium And Oxygen

The purpose of our experiment is to figure out the empirical formula of magnesium and oxygen once they are reacted together. Putting the piece of magnesium in the crucible with the lid somewhat open, we induce heat to have the oxygen and magnesium chemically react. The Independent Variable is the elements used, Magnesium and Oxygen. The Dependent Variable is the mass of the elements.
For one thing, matter is anything that takes up space, and it is composed of miniscule particles called atoms. Different types of matter can be categorized in two sections: composition and properties. The physical properties can be observed or measured without changing the composition of matter, and in physical change, there are two properties, extensive and

Molecular formula is based on the actual numbers of atoms of each type in the compound. An empirical formula is often calculated from elemental composition data. You can determine the empirical formula of a compound from percent composition information or by knowing the mass of each element present in the compound. The weight percentage in each of the elements present in the compound is given by the elemental composition. An empirical formula rhyme: Percent to Mass, Mass to Mole, Define by small, Multiply until

The ending result was an average amount of 0.162(g) Magnesium in the crucible, and 0.043(g) Magnesium and Oxygen in the crucible. The ending empirical formula was MgO2. We were not able to get a correct answer for our experiment, because it messed up during the process. Our magnesium was coiled too much in the bottom of the crucible, so it wasn’t able to combust correctly. So instead, we used a total of 9 groups experiments to find an average mass and empirical