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 Magnesium Oxide by reacting a known down of Magnesium with type O EssaySafetyRisk Assessment Properly follow lab sentry duty guidelines by wearing lab coats, gloves, and goggles and clear any personal belongings off the experimentation area or the apparatus table. Gently handle glassware. Be careful when dealing with Bunsen burners. invent sure the crucible does non break while heating it as it might break callable to the immense air pressure inside.ConclusionMg10O3 is the empirical law we found through our experiment. Theoretically, the empirical dominion 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 gain 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 theoretical answer though according to our uncertainty for Oxygen which is 3 it could be the oxygen we had weighed 5g and so therefore giving us a much accurate result of Mg10O2 which would go to a simplest balance of Mg2O which would be closer to the theoretical answer. In addition to this according to our huge uncertainty the ratio could confound also been 11 if the ratio would have led to 66. Though we see that the causation 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.