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Chemistry Investigation to find the Empirical Formula of Magnesium Oxide

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Introduction

Empirical Formula of Magnesium Oxide 24/14/2012 Empirical Formula of Magnesium Oxide ________________ Data Collection and Processing Diagram Set-up Quantitative observation: During the experiment the crucible used was slightly damaged however did not continue to break or cause any inconvenience to the investigation. For approximately ten minutes, no reaction was visible. The substance contained no odour. After approximately fifteen minutes the piece of magnesium commenced to burn with an overall duration of twenty minutes. When burnt, the magnesium converted to bright orange colour. During the reaction the lid of the crucible was lifted to see any changes or if the magnesium had combusted, and whilst doing this white smoke escaped the crucible which may perhaps be magnesium oxide. By the completion of the reaction, it was noticed that not all of the magnesium was combusted and left some silvery remnants. Raw Data Table 1 – Raw data of the total weight of the crucible including magnesium Trial 1 Group Weight of crucible ± 0.001 (g) Total weight before ± 0.001 (g) Total weight after ± 0.001 (g) 1 37.140 37.250 37.238 2 37.841 37.924 38.038 3 33.405 33.520 33.613 4 33.834 33.979 33.971 5 39.133 39.264 39.322 6 32.784 32.823 32.844 Trial 2 Group* Weight of crucible ± 0.001 (g) ...read more.

Middle

Difference in mass (gained)(± 0.001g) 31.806 - 31.773 = 0.03300 *Data has been removed in the following tables due to lack of validity Table 5 - Mass and number of moles in Mg, O and MgO Mass of mg (± 0.001g) Moles of Mg (± 0.001 mol dm-3) Mass of O (± 0.001g) Moles of O (± 0.001 mol dm-3) Mass of MgO (± 0.001g) 0.083 0.00341 0.114 0.00713 0.197 0.115 0.00473 0.093 0.00581 0.208 0.131 0.00539 0.058 0.00363 0.189 0.039 0.00160 0.021 0.00131 0.060 0.164 0.00675 0.039 0.00244 0.203 0.135 0.00553 0.056 0.00350 0.191 0.150 0.00617 0.043 0.00269 0.193 0.086 0.00354 0.113 0.00706 0.119 *Some data has been removed in the following tables due to lack of validity Graph 1 – The comparison of the moles of magnesium and oxygen Table 6 – Finding the Empirical Formula for Mg and O Empirical formulae Calculations (±0.001 mol dm-3) Empirical formulae 1 : 2.087 ≈1 : 2 1 : 1.223 ≈ 1 : 1 1.487 : 1 ≈ 2 : 1 1.222 : 1 ≈ 1 : 1 2.767: 1 ≈ 3 : 1 1.587 : 1 ≈ 2 : 1 2.295 : 1 ≈ 2 : 1 1 : 1.997 ≈ 1 : 2 Average of Empirical Formula Ratio 1 : 1 Table 7 – The uncertainty of Mg and O Moles of Mg Uncertainty percentage (%) ...read more.

Conclusion

Because these errors came from having too many researchers doing each trial, perhaps having a smaller group of researcher will able to generate reliable results by reducing the random errors. The method required the lid to be lifted up quickly .However, due to infor a while the lifted was lifted up and not placed down until after a few moments and the heat or magnesium oxide could have escaped from therefore affecting the results. And so, if this repeated the lifting of the lid should be constantly and quickly. Or, utilise a transparent crucible that allows the observation of the Mg but still containing the MgO. The window was open during the experiment which caused the loss of MgO due to the strength of the wind. To minimise the loss of MgO it would be recommended for the experiment to be conducted within a fume cupboard so that no wind could increase the loss of MgO when opening the lid or as stated before a transparent crucible would allow the observation of the Mg without the need to open the lid of the crucible. Turnit in Receipt Paper ID 263331967 Paper title Chem IA Term 3 Assignment title Magnesium oxide IA - DCP/CE Author Teresa Nguyen E-mail tnguy32@eq.edu.au Submission time 24-Aug-2012 02:08PM Total words 1364 ________________ | Page ...read more.

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