- Labeled Sketch of the Apparatus:
- Data Processing and Presentation:
- Calculation of the Mass of Magnesium Ribbon:
m (Mg) = m (crucible + lid + Mg) – m (crucible + lid)
= 15.336 – 15.313 =
= 0.023 ± 0.002 g
- Calculation of the Mass of Magnesium Oxide:
m (MgxOy) = m (crucible + lid + combustion product) – m (crucible + lid)
= 15.351 – 15.313
= 0.038 ± 0.002 g
- Calculation of the Mass of Oxygen In the Magnesium Oxide:
m (O) = m (MgxOy) – m (Mg)
= 0.038 – 0.023
= 0.015 ± 0.004 g
- Calculation of the Moles of Oxygen and Magnesium:
n (Mg) = m (Mg) ÷ M(Mg)
= 0.023 g ÷ 24.31 g.mol-1
= 0.00095 mol (uncertainty to be found in the next question)
n (O) = m (O) ÷ M (O)
= 0.015 g ÷ 16.00 g.mol-1
= 0.0009 mol (uncertainty to be found in the next question)
- Determination of Uncertainties In Moles:
Since the molar mass is a definitional quantity, its uncertainty is zero, thus:
Δn (Mg) = 1/24.31 (± 0.002) = ± 0.00008 mol
Δn (O) = 1/16.00 (± 0.004) = ± 0.0003 mol
Table 2: Quantities of the oxide and its constituting elements
- Calculation of the Empirical Formula:
Table 3: Calculation of the empirical formula
Thus the empirical formula is MgO.
- Conclusion and Evaluation:
- Conclusion:
- Researching the Empirical Formula of Magnesium Oxide:
Consulting , the empirical formula of magnesium oxide is MgO which is identical to the one I got.
- Differences and Roundings I Made:
When subtracting the masses, I didn’t round any results. However, when calculating the moles of Mg and O, I rounded my results to the corresponding number of decimal places in order to match their uncertainties.
- Evaluating the Procedure:
- The Percentage of Purity of Initial Mg:
The initial reactant is not 100% pure Mg, otherwise the number of moles of both Mg and O would have been exactly equal, which is not the case.
- Side Reactions That Might Have Occurred:
After heating the crucible, its lid and the magnesium for almost 10-13 minutes, I noticed that gray powder was no longer forming so I decided that the reaction was over.
- Improving the Investigation:
- The Bunsen Burner was not well functioning so it took us a lot of time to get to the perfect flame.
- When the magnesium began to bum, we didn’t remove the burner; we kept it until the end of the experiment which we shouldn’t have done.