To install StudyMoose App tap and then “Add to Home Screen”
Save to my list
Remove from my list
To determine the empirical formula of magnesium oxide by conducting a reaction between magnesium and oxygen.
c. Continue heating until the magnesium burns completely, leaving magnesium oxide.
The empirical formula is determined by the ratio of moles of magnesium to moles of oxygen.
Conclusion:
Based on the experimental data, determine the empirical formula of magnesium oxide.
Remember, the molar mass of magnesium (Mg) is approximately 24.31 g/mol, and the molar mass of oxygen (O) is approximately 16.00 g/mol.
Make sure to follow all safety protocols and guidelines while conducting the experiment.
PROCEDURE
Verified writer
Proficient in: Chemistry
5 (339)
“ KarrieWrites did such a phenomenal job on this assignment! He completed it prior to its deadline and was thorough and informative. ”
If the magnesium does not seem to be burning, increase the heat. Minimize the escape of white smoke, which represents magnesium oxide, to retain it for subsequent weighing.
Table 1: Qualitative data – experimental observations
| Observations | |
| Reactant Magnesium metal | Thin, silver, shiny solid |
| During the reaction | White smoke and white light was produced |
| Product Magnesium oxide | Grey, powdery solid |
Table 2: Quantitative data – experimental data
| Mass (g) | Absolute Uncertainty (±g) | |
| Mass of crucible and lid | 20.2029 | ±0.0005 |
| Mass of crucible, lid and magnesium | 20.3993 | ±0.0005 |
| Mass of crucible, lid and magnesium oxide | 20.5090 | ±0.0005 |
| Mass of magnesium | 0.1964 | ±0.0010 |
| Mass of magnesium oxide | 0.3061 | ±0.0010 |
Mass calculations:
Mass of Mg = (mass of crucible, lid and Mg) – (mass of crucible and lid) = (20.3993) – (20.2029) = 0.1964
Mass of Magnesium oxide = (mass of crucible, lid and magnesium oxide) – (mass of crucible and lid)
= (20.5090 – 20.2029)
= 0.3061
Mass of O in Magnesium oxide = (mass of crucible, lid and magnesium oxide) – (mass of crucible, lid and Mg) = (20.5090) – (20.3993) = 0.1097
Absolute uncertainty calculations:
Uncertainty in Mg = uncertainty in (mass of crucible, lid and Mg) + uncertainty in (mass of crucible and lid) = 0.0005 + 0.0005 = 0.0010
Uncertainty in Magnesium oxide = uncertainty in (mass of crucible, lid and magnesium oxide) + uncertainty in (mass of crucible and lid) = 0.0005 + 0.0005 = 0.0010
Uncertainty in O = uncertainty in (mass of crucible, lid and magnesium oxide) + uncertainty in (mass of crucible, lid and Mg) = 0.0005 + 0.0005 = 0.0010
DATA PROCESSING
Empirical formula calculations:
|
Mg |
O |
|
|
Masses (g) |
0.19640.0010 |
0.10970.0010 |
|
Moles (mol) |
0.0010 |
0.0010 |
|
Divide by smallest |
||
|
Simplest whole number ratio |
However, there is an absence of uncertainty in molar masses, leading to no percentage error in this regard. Consequently, the percentage error in moles is equivalent to the percentage error in masses.
Therefore, the Mg:O ratio is determined as 1.178 ± 0.01673 : 1.
Conclusion:
Following the experiment and the subsequent data analysis, the derived empirical formula is Mg₁.₁₇₈ ± 0.₀₀₁₆₇₃O. However, the expected empirical formula for magnesium oxide is MgO, indicating a 1:1 ratio. The experimentally determined ratio deviates from this, suggesting systematic errors unaccounted for in the error analysis.
Evaluation:
In summary, there were significant shortcomings in the experimental design, with improvements suggested to address identified limitations and enhance the reliability of results.
Empirical Formula Determination of Magnesium Oxide: Analysis, Errors, and Improvements. (2024, Feb 29). Retrieved from https://studymoose.com/document/empirical-formula-determination-of-magnesium-oxide-analysis-errors-and-improvements
👋 Hi! I’m your smart assistant Amy!
Don’t know where to start? Type your requirements and I’ll connect you to an academic expert within 3 minutes.
get help with your assignment
