AP CHEM - 4 x 6H 2 O The moles of the experimental value...

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Samuel Castrejon Period 1 9/20/11 Empirical Formula of Hydrate Conclusion: After the completion of the lab, the purpose of the lab was able to be accomplished. The purpose of the lab was to determine the empirical formula of an unknown hydrate using primary and secondary data. The secondary data was the mass of the crucible which was 15.9 grams and with the hydrate inserted the mass came out to be 19.5 grams. Following the second heating the final mass of the crucible with the hydrate came out to be 18.1 grams. After calculations the mass of the hydrate was found to be 2.2 grams. With the secondary data the empirical formula was found which CuSO
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Unformatted text preview: 4 x 6H 2 O. The moles of the experimental value was precisely 5.5 moles of H 2 O after dividing the moles of water by the moles of copper (II) sulfate the ration was 1:6 while the theoretical value was 5 moles of H 2 O because the empirical formula of the anhydrate copper (II) sulfate should have been CuSO4 x 5 H 2 O, a ratio of 1:5. with these values the percent error was found to be 10 percent. A source of error could have come from the heating of the crucible. Accurate heating of the crucible could have caused error, if more time and trials when heating the crucible had been taken then the percent error may have decreased...
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