Copper, H2o and Its Empirical Formula

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g

Mass of Dehydrated Sample (g)

0.71 g

Mass of Water evolved (g)

0.31 g

Mass of Empty Watch Glass (g)

37.03 g

Mass of Watch Glass and Copper (g)

37.72 g

Mass of Copper (g)

0.69 g

Results

This data had to be very precise in calculating mass because one wrong number would throw everything off. Each mass calculated had two versions of itself; the empty version and the filled version. Often enough one of those number was subtracted from the other in order to get the isolated mass of one element or compound needed for the empirical formula. Little to no errors were made because checking over the numbers was simple considering calculations were vital in this lab. In the end, 0.69 g of copper was isolated,0.31 g of water was evaporated and the empirical formula was Fe3O4.

Discussion of Theory

Empirical formulas are used as a simpler way of expressing how much of an element is in a compound. While doing empirical formulas, calculations have to be firmly correct or the formula will be expressing a different compound. Doing empirical calculations is one of the more easier things in chemistry to check because it is all about numbers. Of course measuring the correct masses are important also. Empirical formulas are also known as the whole number mole ratio because figuring out how many moles are present is what it is all about. It is possible to have more than one correct mole ratios according to John Dalton, a chemist who wrote the modern atomic theory, but he figured that if the exact masses of the elements are known then the exact formula can be achieved. Water is a natural solvent for ionic compounds because they latch onto solid substances which turns them into water of hydration. However, with the use of heat, this water can quickly be evaporated, thus leaving the compound only composed of said elements. The water that was evaporated is important also because it is a necessary calculation to have in order to figure out the percent water composition also. Elements are easier to separate in a substance than compounds considering compounds are chemically combined and elements are not. If compounds are present in the substance them other chemicals, such as acids, will have to be used in order to separate the elements. Once every element is separated, all that is left to do is use the data to find the empirical formula. Finding the empirical formula requires just a few quick steps. First, find the moles of each element. Next, find the mole ratio by dividing all the mole values by the lowest mole value. Lastly, write out the empirical formula using the new ratio numbers. In chemistry, empirical formulas are seen everywhere and Dalton’s atomic theory is the reason.

Conclusion

In conclusion, this experiment explained how heat and chemicals can be used to separate elements in a substance in order to figure out how much of each was present. Without empirical formulas, dealing with substances and solutions could be dangerous considering the knowledge pertaining to the contents in the mixture would be low. Dalton’s atomic theory plays a huge part in the background when it comes to figuring out why empirical formulas make sense. Empirical formulas are everywhere and now it is easier trying to figure them out considering the steps have been laid out to follow.