Empirical Formula Lab Report

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Determining the Empirical Formula of Magnesium Oxide Lab Report

Observation and Results

Mass (g)
Mass of clean, empty crucible and lid
54.3464 g
Mass of crucible, lid and magnesium
54.3919 g
Mass of crucible, lid and magnesium oxide
54.4093 g
Table 1: Experimental Masses of Equipment, Reactants and Products
Masses of relevant equipment, reactants and products were recorded to be used later in calculations to determine the percent composition and empirical formula of magnesium oxide.
Mass of magnesium
0.04550g
Mass of oxygen
0.01740g
Mass of Magnesium Oxide
0.06290g
Experimental - Percent Composition of Magnesium
72.3370%
Experimental - Percent Composition of Oxygen
27.6630%
Moles of Magnesium
0.001871657 moles
Moles of Oxygen
0.0010875 moles
Experimental Empirical Formula Subscript of Magnesium
3.00000
Experimental Empirical Formula
…show more content…
The law of conservation of mass is when the total mass of the products must equal to the total mass of the reactants. Plus, it illustrates the product when magnesium is oxidized with oxygen gas with energy as a form of a heat source. The findings from the experiment are that there was 0.04550g of magnesium, 0.01740g of oxygen and 0.06290g of magnesium oxide. These are the weights of the reactants and products in this chemical reaction which is used to find percent composition and percent error. The amount of magnesium used in the chemical experiment was determined by subtracting the mass of the crucible and lid from the mass of the crucible, lid and magnesium strip. A similar math was used to determine the mass of oxygen by subtracting the mass of the crucible, lid and magnesium strip from the mass of the crucible, lid and magnesium oxide. Then to find the weight of magnesium oxide, the mass of the crucible and lid was subtracted from the mass of the crucible, lid and magnesium

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