determining the empirical of magnesium oxide

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MAGNESIUM OXIDE-EMPIRICAL FORMULA

CHEMISTRY HL

JAIME CASTRO A.

10-2

PRESENTED TO:

 KEITH RIGBY

ANGLO COLOMBIAN SCHOOL

EXPERIMENTAL SCIENCES DEPARTMENT

RESULTS:

The following table shows the mass recorded for the crucible, the magnesium and the magnesium oxide.

Table1. Showing the masses recorded during the practical

 

If we subtract the mass of the crucible from the masses recorded in table 1 we can get the values of the masses of the magnesium and the magnesium oxide, the next table shows the exact masses of both magnesium and magnesium oxide.

Table2. Showing the mass of Magnesium and the mass of magnesium oxide

ANALYSIS OF RESULTS:

Taking in count the data recorded in table 2 we can calculate the mass of the oxygen from the air that reacted with the magnesium in order to form magnesium oxide, this can be done by just finding the difference between the values of the two masses, like shown below.

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Mass of Magnesium:  0.17g(±0.01 g)                     Mass of Magnesium oxide:  0.30g(±0.01 g)

Mass of oxygen = (Mass of Magnesium oxide — Mass of Magnesium) = (0.30 — 0.17) = 0.13g

Mass of oxygen = 0.13g

Now that we know that the mass of the oxygen involved in the reaction we can calculate the empirical formula of magnesium oxide, by doing the following procedure.

First of all divide the masses of both Magnesium and Oxygen by their specific Relative atomic mass, as shown below.

(i)Magnesium

Mass involved in the reaction=0.17g

RAM=24.31 ...

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