Experimental Perseverance of the Mixture of Magnesium Oxide.
Magnesium is a mental, it is recognized to react with oxygen. Magnesium (mg) reacts strongly when heated up in the presence of atmosphere, which is why we have chosen high heat in our solution to facilitate burning. This oxidation process reaction creates magnesium oxide gaining oxygen from the air flow. When showing of electrons occur a chemical relationship is made and the atoms combine to form a molecule.
So , the predicted molecular method:
Mg & O2---------> MgO2
Since the Magnesium combines with 2 atoms of fresh air we need to equilibrium the formula:
2Mg & O2--------> 2MgO
This tells use that 2 moles of magnesium gives a couple of moles of MgO. Proportion of 1: you conversion.
So theoretically, the number of skin moles calculated for magnesium ought to give the same number of moles of MgO.
Using the same balance for a lot of weighing from this experiment.
Recorded the mass of a dried out porcelain crucible and cover via an analytical balanced.
Obtained a length of pre-cut magnesium and cleaned with emery daily news. Then coiled the bows around a pencil to ensure not necessarily wrapped too tightly, in that case placed into the bottom of the crucible.
Record the mass with the magnesium ribbon and crucible with lid via the same analytical equilibrium.
Putting the crucible firmly on the clay-based triangle. The lid collection slightly off-centre on the crucible to allow surroundings to enter but to prevent the magnesium (mg) oxide from escaping.
Heated the crucible at a high 'blue' flame through the Bunsen burner.
Checked the magnesium occasionally, until all the magnesium changed into a gray-white powder.
In order to cool and record the mass from the end product, crucible plus sport bike helmet with the same analytical weighing scales as earlier.
Mass of crucible + lid
Mass of crucible + lid + Mg
Mass of Mg
Mass of crucible + sport bike helmet + MgO
Mass of MgO deposits
Mass of oxygen that combined with Mg