Exploring Empirical Formulas- Final HA

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1 Abell Chemical Analysis: Exploring Empirical Formulas Hailey Abell Aakariti Aakariti CHM 1100- 06H Michelle Newsome 15 November 2023

2 Abell Purpose This experiment was performed to better understand the makeup of an empirical formula and how to form it. Specifically, the goal of the experiment was to determine the empirical formula for magnesium chloride. Introduction An empirical formula can be described as the simplest ratio of elements in the compound (Helmenstine, 2020). The empirical formula represents whole numbers in their lowest condition, while the molecular formula represents the true ratio of elements in the compound (“Empirical versus Molecular Formulas,” 200 C.E.) . The experiment involved a chemical reaction, specifically a redox reaction. The products of the reaction were Mg 2 Cl 7 , , which was a solid, and H 2 , which was a gas. The empirical formula of the compound was calculated using the moles of magnesium and the moles of chlorine in the sample. To do this the given amount of each substance was divided by the molar mass of the substance and was then divided by the smallest amount. The whole compound was then multiplied by a whole number to remove the decimal point for the moles in chlorine. The amount of chlorine was determined by dividing the mass of chlorine in the product by the molar mass of chlorine. It is imperative to ensure that all the water is removed from the final product; if this is not done, the weight value will not be accurate. This was done by repeating the heating and weighing process of the beaker until the weights were close. The data from the lab allows the participant to determine the empirical formula of the compound by using the mass and moles

3 Abell of the substances. The experiment was carried out to better understand how empirical formulas are configured. Methods The instructions for the experiment came from the student handout on Pilot. The experiment began by weighing an empty 150 mL beaker on the scale. A piece of magnesium was then placed into the beaker and weighed. The mass of magnesium was determined through subtraction. Three mL of 6 M HCl solution was then added to the beaker. Once this happened, the magnesium dissolved, creating a colorless solution. The beaker was then heated on a hotplate at 100 degrees Celsius until the liquid was dissolved. The weight was then taken and the mass and recorded. The heating process was then repeated and weighed once again. The process would be repeated if the values were not within 0.05 grams. The beaker was then cleaned out, and the other calculations were made. Results Table 1 shows the original mass of the beaker along with the mass of the substances along with the difference between the weighings. The calculations for the moles of the product and the empirical formula of the product are also shown below. TABLE 1- Empirical Data Mass (g) Mass of empty 150 mL beaker 78.125 Mass of beaker and magnesium 78.150

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