Experiment#2

Experiment#2 - Determining an Empirical Formula TITLE:...

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Determining an Empirical Formula
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 Determining an Empirical Formula PURPOSE:   This lab was an exercise in teaching the students how to determine the empirical  formula through the observance of a chemical reaction. The purpose of this lab is to use  the original concentration of copper chloride (aqueous) and the mass of the product  created through a chemical reaction and apply the principles of law conservation of  mass and the law of definite proportions, to calculate the percentage composition of  copper chloride compound and empirical formulas of copper chloride and zinc chloride.  PROCEDURE:  The procedure was followed as indicated in the handout for experiment  two.  DATA AND OBSERVATIONS: Copper chloride with a concentration of 2.02g 2.02 g of copper chloride per 25.0 mL of  solution was obtained. It was clear blue in appearance. After the reaction finished taking  place the solution was murky grey in appearance. While the zinc still had some copper  on it. In the process of decanting zinc chloride from the copper and rinsing the copper, a  negligible amount of copper was lost in solution. An average mass for the empty  crucible and the zinc after reaction was obtained, as well as the mass of the zinc before  reaction and of the crucible with copper (see Table 1).  Table 1. Data for the Masses Obtained  Tria l Mass of  Empty  Crucible  (g) Mass of  Crucible 
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This note was uploaded on 06/10/2008 for the course CHEM 01 taught by Professor Kryatov during the Spring '07 term at Tufts.

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Experiment#2 - Determining an Empirical Formula TITLE:...

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