The Law of Definite Proportions and Empirical Formula

The Law of Definite Proportions and Empirical Formula -...

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The Law of Definite Proportions and   Empirical Formula            Fatima Elzin SJU Chemistry 1111L 73139 September 30, 2009 Pedro Bastos, Anne Okafor
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Fatima Elzin SJU Chemistry  111L 9/30/09 Dr. Bastos The Law of Definite Proportions and Empirical Formula 1. Will your weighings give a mass that is too high or too low if the crucible is still  warm when you weigh it? Explain why.   It will give a value that is too low,  because when the crucible is hot all the particles are not compact yet therefore  the mass will be lower. 2. Does this experiment successfully demonstrate the law of definite composition?  Justify your answer.  Yes this experiment demonstrates the law of definite  composition stating that a compound always contains two or more elements  combined in a definite proportion by mass 3. Why are you certain that the amount of copper in your crucible remains 
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Unformatted text preview: constant? Because in the experiment the only change is in the amount of sulfur, the amount of copper is unaffected by the heat. 4. Are your results for the two heating steps identical? Why? No they are not identical because of the fractional uncertainties. There may have been errors in measurement. 5. What would be the effect if all of the copper reacted but enough oxygen was present to form copper (II) oxide? There would not be much of an effect. 6. What would be the effect on your results if some of the copper remained unreacted? The mass would not be the same and therefore the copper and sulfur would not be in proportion. 7. Using your results, calculate the empirical formula of copper sulfur compound. Cu2S...
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This note was uploaded on 04/24/2010 for the course CHE 1111L-0 taught by Professor Jain during the Spring '08 term at St. John's.

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