Determine the Empirical Formula of Magnesium Oxide by reacting a known mass of Magnesium with Oxygen Essay Example for Free

Determine the Empirical Formula of atomic number 12 Oxide by reacting a known mass of Magnesium with Oxygen EssaySafetyRisk judgment Properly follow lab safety guidelines by wearing lab coats, gloves, and goggles and clear any personal belongings off the experiment ambit or the apparatus table. Gently handle glassware. Be careful when dealing with Bunsen burners. Make sure the crucible does not break while passion it as it might break callable to the immense air pressure inside.ConclusionMg10O3 is the empirical formula we found through our experiment. Theoretically, the empirical formula is MgO. This is because Magnesium is a group 2 element so it would lose two electrons to form Mg2+ ion. Oxygen is a group 6 element so it would larn two electrons to form a O2- ion. So in theory, the empirical formula is MgO. Therefore we see were nowhere close obtaining a empirical formula to the divinatory answer though according to our uncertainty for Oxygen which is 3 it could be the o xygen we had weighed 5g and so therefore giving us a much dead-on(prenominal) result of Mg10O2 which would go to a simplest ratio of Mg2O which would be closer to the theoretical answer. In addition to this according to our huge uncertainty the ratio could have besides been 11 if the ratio would have led to 66. Though we see that the reason behind getting such an inaccurate answer is due to the incomplete combustion and due to not using a much more precise and accurate balance to weigh the apparatus and chemicals used.