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
You can download this essay for free. All you need to do is register and submit at least one of your essays to us.
Or you can purchase this essay for just $2 instantly without registering
Downloads to date:
| Words: 354 | Submitted: 07-Feb-2012
96.0% | Number of pages: 3 | Filetype: Word .doc
This is what the first 3 pages of the essay look like
Determining the empirical formula of magnesium oxide
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.
Mass crucible+lid+magnesium oxide residue
* 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
Reacted oxygen with magnesium
Magnesium oxide residue
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
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)
Download this essay in full now!
Just upload at one of your essays to our database and instantly download your selection! Registration takes seconds
Comments and reviews
Reviews are written by members who have downloaded the essay
No comments yet. If you download the essay you can review it afterwards.