Chemistry Lab Report Synthesize magnesium oxide and determine its empirical formula

Chemistry Lab Report
Synthesize magnesium oxide and determine its empirical formula.

Terri williams
12/07/17

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Purpose:
The empirical formula of a compound is defined as the formula that shows the ratio of element present in the compound, but not the actual numbers of atoms found in the molecule. The ratios are denoted by subscripts next to the element symbols.
Since formulas are written in mole amounts, the masses of the individual elements that make up the compound must be converted to moles. Then the ratio of moles is adjusted to small, whole numbers.
Materials:
Magnesium ribbon
Distilled Water
Dropper pipets
Balance
Crucible and cover
Crucible tongs
Bunsen burner and matches or lighter
Ring stand, ring, and clay triangle
Wire gauze
Beaker
Procedure:
One clean crucible and its lid were set in a clay triangle and ring support to be heated for 3 mins with a bunsen burner to make sure the crucible was dry. It was then removed by tongs to the wire gauze for cooling. After the empty crucible cooled, its mass was recorded using a balance. 0.4 g of coiled magnesium ribbon was placed in the crucible so it sits in the bottom. The crucible, magnesium and cover was weighed and the mass was also recorded. The crucible and its cover askew was heated, magnesium begun to smoke and flare, but the cover was not removed. After 10 mins in the bunsen burner, the crucible was cooled. The mixture in the crucible appeared to be gray-white ash which was identified as magnesium oxide and magnesium nitride. 2 drops of distilled water was added to the residue to convert any magnesium nitride to magnesium oxide. The crucible was heated once more for 5 mins, removed and placed on the wire glaze for cooling. The crucible, cover, and magnesium oxide mass was recorded one last time with a balance.
Data and results:

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