DRAFT: This module has unpublished changes.

Data Analysis:


Determined mass of magnesium oxide by subtracting the mass of the crucible and lid, from the mass of the crucible, lid, and magnesium oxide: 0.2893g

Determined mass of oxygen by subtracting the mass of the magnesium from the magnesium oxide: 0.1013g

Determined amount of magnesium in the compound, by dividing the mass of the magnesium in the compound, by the number of grams per mole in 1 mole of magnesium: 0.0077mol

Determined amount of oxygen in the compound, by dividing the mass of the oxygen in the compound, by the number of grams per mole in 1 mole of oxygen: 0.0063mol

Used the molar ratio to determine the experimental empirical formula of the compound:

Taken to the nearest whole molecule, this experiment finds the empirical formula of MgO to be 1:1

 

Conclusion:

The goal of this experiment is to determine the Empirical Formula of a Compound. (The Empirical Formula of a Compound is the simplest whole number ratio between the elements of a compound) If one can synthesize a compound from elements, then it is possible to determine an experimental empirical formula for the compound, from its molar and stoichiometric ratios. By reacting Mg with pure O, (or air, and then using water and heat to remove any magnesium nitride formed upon exposure to the air), and then calculating the ratio between the moles of Mg and O, it is possible to determine experimentally the empirical formula of MgO.

 

Taken to the nearest whole molecule, this experiment finds the empirical formula of MgO to be 1:1

 

The accepted empirical formula of MgO: 1:1

The experimental empirical formula of MgO: 1:1.221

Percent error: 22.1%

 

Possible sources of error include:

  • Failure to properly react all of the Magnesium with Oxygen, and/or failure to react all of the Magnesium Nitride with water. (Disrupting subsequent measurements due to differences in mass)
  • Failure to properly clean the paperclip used for mixing. (Thus removing from the contents of the crucible, and disrupting subsequent measurements)
  • Human error is always in effect, given that the laboratory does not function under ideal conditions. As such, there is always the possibility of inaccuracies with measurement, perception of measurement, inaccuracies of equipment, and other such errors. (However, this is not likely to be the sole cause of the inaccuracies within this experiment, though it may contribute to it.)

 

Possible improvements that could be made for subsequent experiments include using more precise instruments, reacting the Magnesium in a pure Oxygen environment (removing the possibility of Magnesium Nitride forming, and possibly not reacting fully with water), and repeating the test multiple times, to minimize the possibility of an anomalous result skewing the final measurement.

DRAFT: This module has unpublished changes.