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Determining the formula of magnesium oxide Free essay! Download now

Home > A Level > Chemistry > Determining the formula of magnesium oxide

Determining the formula of magnesium oxide

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Downloads to date: N/A | Words: 354 | Submitted: 07-Feb-2012
Spelling accuracy: 96.0% | Number of pages: 3 | Filetype: Word .doc


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magnesium oxide

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Determining the empirical formula of magnesium oxide
Method
The apparatus and chemical includes Bunsen burner, Crucible with lid, Tongs, Pipe clay triangle, Ceramic mat, Tripod, Emery paper and Magnesium ribbon
For health and safety reason wear lab coat and eye protection throughout the experiment.
If the magnesium ribbon looks a bit tarnished clean it using the emery paper and coil it tight that it fits in the crucible.
Weigh the empty crucible with lid on for three times and record the result in grams.
Bunsen burner should be set up on the ceramic mat using the tripod.
Pipe clay triangle should be placed over the tripod
Place the crucible containing magnesium on the pipe clay triangle and put the lid on.

Turn the Bunsen burner on and set it to blue flame. When the crucible starts getting hot lift the lid up using the tongs to let oxygen in without letting any of the magnesium oxide escape.
This process should be continued until there is no glow visible in the crucible
Reweigh the crucible with lid containing the product when the apparatus is cooled down.

Results
Items
Mass(g)
Mass crucible+lid
35.012g
Mass crucible+lid+magnesium
35.489g
Mass crucible+lid+magnesium oxide residue
35.765g
Calculations
* Mass of magnesium used =mass crucible+lid+magnesium mass crucible+lid
35.489-35.012 = 0.477g
* Mass of oxygen that combines with magnesium = Mass crucible+lid+magnesium oxide residue -Mass crucible+lid+magnesium
35.765-35.489 = 0.276g
* Mass of the magnesium oxide residue = Mass of magnesium used + Mass of oxygen that combines with magnesium
0.477+0.276 = 0.753g


Mass(g)
Magnesium used
0.477
Reacted oxygen with magnesium
0.276
Magnesium oxide residue
0.753

Masses of these two elements and their relative atomic mass is used to work out the amount in moles of magnesium and oxygen to form magnesium oxide
RAM of 1 mole of magnesium = 24.3 g
RAM of 1 mole of oxygen = 16.0 g
Magnesium = 0.477/24.3 = 0.020 mol
Oxygen = 0.276/16 =0.017 mol

Element
Moles
Magnesium
0.020
Oxygen
0.017

Empirical formula of magnesium oxide shows the amount of atoms in ratio in each element in a compound, by calculating in moles.
Magnesium = 0.020/0.017 = 1.2 =1
Oxygen =0.017/0.017 = 1
Ratio = 1:1
Therefore the empirical formula of magnesium oxide is MgO
Mg(s) + O2(g) ? MgO(s)

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