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Finding thr Percentage Composition of Magnesium Oxide

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Introduction

Lab Report Percentage Composition of Magnesium Oxide Student: Salma Youssef Partner: Madison Easton Professor: Mr. D. Fontaine Due: Wednesday, November 23 Course code: SCH3U Introduction According to Encyclopedia Britannica, the law of definite proportions is a ?statement that every chemical compound contains fixed and constant proportions (by weight) of its constituent elements.? Using experimental data in this investigation, it will determine the percentage composition of magnesium oxide. Chemists believe that the energy released by the synthesis combustion reaction is sufficient to allow magnesium to also react with nitrogen in the air. This reaction produces magnesium nitride. What remains unclear is whether enough magnesium nitride forms to noticeably alter the percentage composition of magnesium oxide. This report presents the experiments procedures, results, analysis, and questions. Purpose To find the percentage composition by mass of magnesium oxide. Testable Question What effect, if any, does the formation of magnesium nitride have on the percentage composition of magnesium oxide determined in this experiment? Hypothesis The percentage composition by mass of magnesium oxide will be about 60.31% magnesium and 39.69% oxygen. Experimental Design You will burn two identical strips of magnesium in ceramic crucibles. ...read more.

Middle

Observations Mass of crucible and lid Mass of crucible, lid and Mg After heating (first time) After adding H2O After heating (final time) 32.13g 32.34g 32.47g 32.47g 32.47g Analysis This lab was conducted in order to confirm the chemical formula of magnesium oxide. In this investigation, one strip of magnesium was coiled and put into a ceramic crucible and cooked over a Bunsen burner with an intense flame. The magnesium nitride that may have formed was chemically converted to magnesium oxide and the mass and percentage composition of the product was determined. Source(s) of Error This investigation required extreme caution as there were many possibilities for error. In order to prevent magnesium oxide escaping from the crucible during heating, the lid was left slightly ajar. The size of the slot (too large) could have greatly altered the final mass of the product. Magnesium may not have reacted completely with oxygen. The water may not have evaporated completely. Any leftover compounds in the crucible from previous experiments may have varied or contaminated the reaction. Leftover compounds could also have added extra mass to the total mass. The water could have been contaminated. ...read more.

Conclusion

1. The testable question that asked: what effect, if any, does the formation of magnesium nitride have on the percentage composition of magnesium oxide determined in this experiment? The formation of magnesium nitride has a significant impact on the percentage composition of magnesium oxide. There is only 60.31% of magnesium in magnesium oxide. If there is more magnesium nitride in the mixture, then the percentage of magnesium will also be higher. 1. A student observes unreacted magnesium remaining in the crucible. What effect would this have on the percentage composition calculation? Why? 1. The unreacted magnesium remaining in the crucible would affect the percentage composition calculation by making it lower, because not all of the magnesium was used up in the reaction. 1. Suggest a modification of this experiment that would prevent magnesium from reacting with nitrogen. 1. By lifting the lid of the crucible regularly, it could have prevented the magnesium from reacting with nitrogen, and instead it will allow adequate supplies of oxygen from the air to react. The magnesium will react preferentially with oxygen, but if all the oxygen is used up, the magnesium will react with the nitrogen. 1. Research and write the chemical reactions involved in converting magnesium nitride to magnesium oxide during Part A of this experiment. 1. Mg3N2 + 6 H2O ï 3 Mg(OH)2 + 2 NH3 ...read more.

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