Empirical Formula Lab Report

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Recommended: Magnesium oxide formula

Conclusion :

Theoretically, the empirical formula for magnesium oxide was MgO, only one of each element, and the percent composition of 60% magnesium and 40% oxygen. However, from the data collected during the lab, the empirical formula was found to be Mg2O, and the percent composition was calculated to be 75% magnesium and only 25% oxygen. These results point towards a more magnesium-heavy product being synthesized, with a practical magnesium percent composition rise of 15%. These discrepancies could have been caused by unyielding chemical reactions that took place. The magnesium had to be heated in the presence of air for approximately 2 minutes to ensure it bonded with nitrogen. Throughout the lab, heating the contents was a problem due to the wind and having the Bunsen burner turned down too low causing the crucible to turn black from the weak flame charring it. Because of this, the magnesium most likely did not have enough time and heat to react with the nitrogen …show more content…

The Bunsen burner should have been turned up higher from the beginning to ensure the heat was reaching its contents directly, not just the crucible. The window should be closed and the intensity should be turned up to prevent the wavering flame. By doing this, the reactions would have been more likely to take place and lead to the desired and expected results. Not allowing the water to evaporate completely could have affected the resulting mass and composition of the product. Having the heat turned up would also have saved time, which a big portion of was spent simply gathering supplies. This should have been done quicker so the lab could have been started sooner, preventing the rush towards the end when we barely had enough time to evaporate the water from the contents. By doing these things, the results of the lab could have been more accurate and discrepancies in the results could be

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