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Finding the Empirical Formula of a Compound

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Lab - Finding the Empirical Formula Aim: To investigate a compound and determine its empirical formula. In this assessment, we find x in the formula: CuS04.xH20 by removing the water of crystallization from hydrated copper(II) sulphate by heating it, and then using the empirical formula method of calculation to work out the formula. Apparatus: Crucible, Bunsen Burner, Tripod, Pipe clay triangle, and a sample of the compound (I took CuSO4 . xH2O, where x is an unknown constant we need to find to determine the empirical formula. Method: 1. The apparatus was set up as shown in the diagram below. 2. ...read more.


Trial Number Original Mass of compound � 0.01 g Final Mass � 0.01 g Mass of Copper Sulphate � 0.01 g Mass of Water lost � 0.01 g 1 2.00 1.24 1.24 0.76 2 0.46 0.26 0.26 0.20 The data from Trial 1 was then used to calculate the empirical formula CuSO4 H2O Calculations for CuSO4 Calculations for H2O Masses of Compounds 1.24 0.76 Molar Mass 160 18 64 + 32 + (4 x 16) 2 x 1 + 16 No. of Moles 0.00775 0.042222 1.24 / 160 0.76 / 18 Ratio of Moles 1 : 5.448029 CuSO4 : H2O :: 1 : (0.04222 / 0.00775) ...read more.


7H2O Conclusion: From the results obtained, it seems like the empirical formula of the compound is CuSO4 . 5H2O or CuSO4 . 7H2O . However, the theoretical result we should have obtained is CuSO4 . 5H2O . Hence, there have been some large errors in the second trial. The results wasn't taken as an average of the two results obtained, as the second results was erroneous due to mistakes made during the experiment. Evaluation: Evidently, the first experiment was quite accurate, as the theoretically expected results were achieved. However, the second experiment was grossly inconsistent, which indicates that there have been some random errors. The second set of results is faultier, but this is because some of the Copper Sulphate fell out of the crucible while measuring its mass. ...read more.

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