the oxygen consumed was .19 18.71-18.52=.19
3. The number of moles used for magnesium is .015 Moles of Mg: .38g/1 x 1 mol Mg/24.3g=.015 mol The number of moles of oxygen is .011 Moles of O: .19g/1 x 1mol O/16.0 g= .011 mol
4. The empirical formula of this oxide is MgO.
Discussion:
Magnesium is an alkaline earth metal, which reacts vigorously when heated in the presence of oxygen to produce magnesium oxide and magnesium nitride. The addition of water to the product causes a second reaction which leaves magnesium oxide as a solid product. An empirical formula gives the simplest whole-
number ratio of the different atoms in a compound.
In any lab, there are bound to be uncontrollable errors. In this specific lab, a loss of matter via particle dispersion into the atmosphere may have occurred while lifting the crucible lid, allowing substance to escape while heating. Another error would be that the magnesium may not have been fully reacted before being weighed, or the crucible and contents might not have cooled off completely/dissolved the water droplets entirely before weighing.the oxygen consumed was .19 18.71-18.52=.19
3. The number of moles used for magnesium is .015 Moles of Mg: .38g/1 x 1 mol Mg/24.3g=.015 mol The number of moles of oxygen is .011 Moles of O: .19g/1 x 1mol O/16.0 g= .011 mol
4. The empirical formula of this oxide is MgO.
Discussion:
Magnesium is an alkaline earth metal, which reacts vigorously when heated in the presence of oxygen to produce magnesium oxide and magnesium nitride. The addition of water to the product causes a second reaction which leaves magnesium oxide as a solid product. An empirical formula gives the simplest whole-
number ratio of the different atoms in a compound.
In any lab, there are bound to be uncontrollable errors. In this specific lab, a loss...