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Empirical Formula of Magnesium Oxide

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Introduction

Empirical Formula of Magnesium Oxide Name: Suleman Esam Date: 16/10-07 Purpose: The purpose of this lab was to experimentally determine the empirical formula of magnesium oxide. Background: Metal oxide is formed when a metal reacts with oxygen. Magnesium is an alkaline earth metal. When magnesium is heated, it reacts vigorously in the preset of oxygen. It is easy to ignite it when it is shred or powdered, but difficult when it is bulk. Once the metal is ignited, it is hard to extinguish it. Equipments: - Magnesium ribbon - Crucible & lid - Bunsen burner - Steel wool - Pipe clay triangle - Tripod - Crucible tongs - Balance - Goggles Procedure: 1. We took on our goggles and stated the experiment. 2. First we placed a tripod over a Bunsen burner. On the tripod, we placed a pipe clay triangle and over it the crucible & lid. 3. ...read more.

Middle

7. Finally, when the magnesium that finished reacting, we let it cool. When it had cooled, we recorded the mass of crucible with magnesium oxide and its lid. COMBINED MASS OF THE OBJECTS AFTER = 33.450g �0.002g Result Now I have every mass that I need to find the empirical formula for magnesium oxide, except the mass of oxygen. By subtracting the mass that the object before the reaction from what it had after magnesium was burned, we find the mass of oxygen. COMBINED MASS OF THE OBJECTS BEFORE - COMBINED MASS OF THE OBJECTS AFTER = MASS OF OXYGEN (33.450g - 33.279g) � (0.002g + 0.002g) = 0.171g �0.004g A summary of all the mass is listed in the chart below. OBJECT MASS (g) UNCERTAINTY (g) Objects before 33.279 �0.002 Objects after 33.450 �0.002 Mg 0.324 �0.002 Oxygen 0.171 �0.004 Magnesium oxide 0.495 �0.006 By finding the amount of moles of these two atoms, we can determine the empirical formula for magnesium oxide. ...read more.

Conclusion

Errors The mole of magnesium and oxygen was not the same. I found out that the mass of oxygen was smaller then it was supposed to be. This error can have occurred by three things: 1. We did not found out the empirical formula for magnesium oxide properly; because magnesium also reacted with nitrogen. It takes three magnesium atoms, while it takes only two nitrogen atoms to form a compound. Nitrogen is also lighter then oxygen; thus our combined mass after the reaction became smaller then if the magnesium had totally reacted with oxygen. 2. When we lifted the lit while magnesium ribbon was reacting, we let out smoke. That was magnesium oxide in vapour. 3. There is a possibility that maybe not all of the magnesium reacted. Improvements: If we had carried the experiment a little more, we could have removed the magnesium nitride. By adding some drops of water and then heating it up, we will get this formula: Mg3N2 + 6H2O � 3Mg(OH)2 + 2NH3 The result will be ammonia gas, which will depart when heated. ?? ?? ?? ?? ...read more.

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