Empirical Formula For Magnesium Oxide Essay
The purpose of this lab was to find the empirical formula for magnesium oxide.
To find this formula, a strip of Magnesium ribbon was burned in a crucible over a flame from a bunson burner. After the strip caught fire multiple times with the cover on, and 10 drops of distilled water were added, and the crucible was lightly heated. The crucible was then weighed and the mass recorded. Calculations were performed and the mole ratio of Mg to O was recorded. The results of other lab groups performing the same experiment were also recorded.
The results did not match the actual empirical formula for magnesium oxide. Our empirical formula of magnesium oxide was Mg4O3 instead of MgO which is the actual empirical formula. In performing the calculations, there was a 32% error.
There were several uncertainties which may have led to the results not being closer to the actual empirical formula for magnesium oxide. First, as noted in the Observations, the burner that was being used was not able to be adjusted which caused the magnesium ribbon to not burn quickly. The flame was not strong enough to reach the magnesium or turn the crucible red hot, so that the magnesium could have begun to burn. This may have caused a later reaction to not occur properly or fully. The mass of magnesium oxide may be impacted if some of the magnesium does not fully …show more content…
Although the data did not match the actual empirical formula of a 1:1 ratio for Mg to O, the experiment established a process to determine the empirical formula. The experiment calculated a relatively high percentage error. Errors may have occurred in the process including the use of the inadequate bunson burner and not allow sufficient time to warm the crucible after distilled water was added. However, the process did allow for calculations to be made regarding the empirical formula for magnesium oxide, percentage error, and standard
To find this formula, a strip of Magnesium ribbon was burned in a crucible over a flame from a bunson burner. After the strip caught fire multiple times with the cover on, and 10 drops of distilled water were added, and the crucible was lightly heated. The crucible was then weighed and the mass recorded. Calculations were performed and the mole ratio of Mg to O was recorded. The results of other lab groups performing the same experiment were also recorded.
The results did not match the actual empirical formula for magnesium oxide. Our empirical formula of magnesium oxide was Mg4O3 instead of MgO which is the actual empirical formula. In performing the calculations, there was a 32% error.
There were several uncertainties which may have led to the results not being closer to the actual empirical formula for magnesium oxide. First, as noted in the Observations, the burner that was being used was not able to be adjusted which caused the magnesium ribbon to not burn quickly. The flame was not strong enough to reach the magnesium or turn the crucible red hot, so that the magnesium could have begun to burn. This may have caused a later reaction to not occur properly or fully. The mass of magnesium oxide may be impacted if some of the magnesium does not fully …show more content…
Although the data did not match the actual empirical formula of a 1:1 ratio for Mg to O, the experiment established a process to determine the empirical formula. The experiment calculated a relatively high percentage error. Errors may have occurred in the process including the use of the inadequate bunson burner and not allow sufficient time to warm the crucible after distilled water was added. However, the process did allow for calculations to be made regarding the empirical formula for magnesium oxide, percentage error, and standard