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determining the empirical of magnesium oxide

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Introduction

MAGNESIUM OXIDE-EMPIRICAL FORMULA CHEMISTRY HL JAIME CASTRO A. 10-2 PRESENTED TO: KEITH RIGBY ANGLO COLOMBIAN SCHOOL EXPERIMENTAL SCIENCES DEPARTMENT RESULTS: The following table shows the mass recorded for the crucible, the magnesium and the magnesium oxide. Table1. Showing the masses recorded during the practical Crucible /g �0.01g Crucible and magnesium /g �0.01 g Crucible and magnesium oxide /g �0.01g 25.50 25.67 25.80 If we subtract the mass of the crucible from the masses recorded in table 1 we can get the values of the masses of the magnesium and the magnesium oxide, the next table shows the exact masses of both magnesium and magnesium oxide. Table2. Showing the mass of Magnesium and the mass of magnesium oxide Magnesium /g �0.01 g Magnesium oxide /g �0.01g 0.17 0.30 ANALYSIS OF RESULTS: Taking in count the data recorded in table 2 we can calculate the mass of the oxygen from the air that reacted with the ...read more.

Middle

(i)Magnesium (ii)Oxygen From the process developed above we can say that the ratio there is between magnesium atoms and oxygen atoms in magnesium oxide is of 1:1, and therefore the empirical formula is MgO, which means there is one oxygen atom for every magnesium atom. Now to evaluate how reliable our results are we must calculate the percentage error of the practical and the total percentage of uncertainty. Percentage error This percentage is calculated by adding up the percentage error of the ratio between magnesium and oxygen. a) (for magnesium) b) (for magnesium) The total percentage error of this practical was of 15% Total percentage uncertainty This percentage is calculated by the addition of the percentage uncertainty of the masses of magnesium and of oxygen. Percentage uncertainty of the mass of Magnesium Uncertainty: �0.01g Mass of magnesium: 0.17g Percentage uncertainty = 5.9% Percentage uncertainty = 5.9% Percentage uncertainty of the mass of Oxygen Uncertainty: �0.01g ...read more.

Conclusion

The presence of the previously mentioned random errors can be easily explained by understanding the method used to develop the practical, since the oxygen was allowed to go into the crucible by taking the lid off, so when this occurred some of the newly formed magnesium oxide escaped out of the crucible and therefore some of it wasn't registered in the mass of magnesium oxide. To avoid the presence of the random errors I can suggest to improvements for this practical, first of all the use of better or more specialized equipment that allows us to have a more controlled way of introducing oxygen into the crucible where the magnesium is being heated. And secondly I suggest repeating the practical at least 2 times in order to calculate an average of the results so the possibility of random errors is reduced to its minimum. ?? ?? ?? ?? ...read more.

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