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EmpiricalFormula_LabReport

Now that the crucible was cooled down the students

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temperature. Now that the crucible was cooled down the students added a few drops of distilled water to the now white/gray powder magnesium. When the water was added to the crucible it released a slight ammonia smell and so the cover was placed slightly open so that any water or ammonia could escape. The crucible once again was heated gently until the contents within had dried and then it was heated strongly for 10 minutes. After the 10 minutes were over the crucible was cooled to room temperature and the mass once again was recorded on the analytical balance. The student then heated the crucible one last time for 3 minutes and allowed it to cool. They again measured the mass on the analytical balance making sure that the consecutive masses were within the 5 mg tolerance. The two masses were then averaged and the average value was recorded as the “gross weight of oxide”. To finish the students cleaned the crucible they had used and returned all the equipment back to its appropriate place. Having collected all the data needed
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the students converted the number of grams of magnesium into moles and calculate the amount of oxygen in the oxide and also converted that number into moles. Lastly using the number of moles for both magnesium and oxygen they determined the empirical formula for oxide to the nearest whole number. Analysis: The crucible was heated numerous times at the beginning of the experiment to obtain a constant mass but also to burn off any excess volatile material that had been left behind in it from previous experiments. The experiment was performed in the crucible rather than burning the
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Now that the crucible was cooled down the students added a...

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