Empirical Formula Lab Report Essay

INTRODUCTIONJohn Daltons atomic theory states that elements merge in simple numerical symmetrys to grade multiforms. A compound, no yield how it is formed, always contains the same elements in the same proportion by weight. The right of mass conservation states that mass can neither be created nor destroyed. In this experiment, the mass of the metallic element was non destroyed or created the metals mass was simply changed into a compound form once the shove along reacted to it.The net mass of the reactant array of the comparability and the product side of the equation should be equal if the experiment is done correctly. The molecular formula represents the fare of all elements in a compound. The empirical is the simplest whole number ratio of the elements in that compound.Combustion reactions always involve oxygen and are roughly always exothermic. Exothermic reactions give off energy in heat energy form. The purpose of this experiment is to find the empirical formula o f a compound apply whole numbers. To investigate this experiment, the masses of the metal and gas were metrical to obtain the empirical formula of the compound.PROCEDUREBefore starting the experiment, the materials needed were gathered melting pot and chapeau, bunsen burner burner, deionized or distilled water, striker, magnesium ribbon, sandpaper (if needed), form triangle, wire pad, crucible tongs, electronic scale, ring clamp, experiment stand, paper to study data. Two of each necessary material was gathered in revision to conduct two trials at once.To prepare for the experiment, the ring clamp was habituated to the stand at about 2/3s the way up the stand. The crucible and lid were rinsed with water, dried, and then placed on a clay triangle. The Bunsen burner was hooked up to the gas line and the gas was turned on. The ack-ack gun was started with the striker and the flame was adjusted to the height of the ring clamp. The crucible and lid were heated light for 4-6 minutes until the bottom of the crucible became red. The flame was increase and the crucible and lid were heated for another 10-12 minutes. The crucible and lid were allowed to imperturbable on the wire pad. The mass of the cooled crucible and lid was recorded using the electronic scale.This procedure was repeated once more for each trial. In each trial, the ribbon was placed into the crucible and the lid was placed over it. The mass of the crucible, lid and magnesium was recorded. The crucible containing the magnesium was heated gently for 2-3 minutes. The heat was gradually intensified and heated for another 2-3 minutes. One side of the lid was lifted with the crucible tongs to allow the oxygen inner. The metal started glowing. The crucible, lid and compound were heated for another 3 minutes.The metal was canvass periodically until no more glowing was observed. The crucible was then take away from heat and then cooled on the wire pad. 3 drops of deionized water was added to t he cooled compound. The crucible was reheated with the lid partially off, allowing the water vapor to escape. The sample was heated easily and then the heat was intensified for 15-17 minutes. The crucible, lid and compound were allowed to cool on the wire pad. The mass of the crucible, lid and compound was recorded. The sample was reheated for an extra 5 minutes, then the combined mass of the crucible, lid and metal oxide was measured. The metal oxide was habituated of in the proper marked contained and the crucible was cleaned of any residue and rinsed with deionized water.RESULTSUnits effort 1Trial 2Before Heatingg23.860 afterward 1st Heatingg21.38323.859After 2nd Heatingg21.385 mountain of Crucible, Lid and surfaceg21.57524.054Mass of metalg0.1900.195Mass of Crucible, Lid and Metal Oxide after 1st heatingg21.64624.1742nd Heating Mass Measurementg21.64824.174Mass of Metal Oxideg0.2630.315Number of Moles of Metal in the risemol0.007820.00802Mass of Oxygen in Compoundg0.07300.1 20Number of Moles of Oxygen in the Compoundmol0.004560.00750Simplest Whole Number Ratio of Oxygen to Metal351415Empirical Formula for the Compound using Whole NumbersMg5O3Mg14O13DISCUSSIONIn order to hire magnesium oxide, MgO, the magnesium strip had to be heated. Under normal circumstances, manner temperature, magnesium metal, Mg, reacts very slowly with the oxygen, O, in the production line. However, as magnesium is heated, it reacts fast with the oxygen and burns with a white light to produce MgO.To cheer others from the smoke, containing Magnesium Oxide, the crucible had to remain covered. Some magnesium oxide escaped, when the crucible was not covered. The crucible had to be slightly ajar when heating up the magnesium, so that oxygen could get to the reaction. Without oxygen, a fire cannot exist. The shininess of the metal Mg turned to a dull appearance as it changed to MgO. As the magnesium reacted to the oxygen, it also reacted with the nitrogen in the air to form magnes ium nitride, Mg3N2.To resign the nitrogen from the crucible, we added water to the mixture and heated it up. This would cause the Mg3N2, to react with the water, H2O, to form ammonia water, NH3, and magnesium hydroxide, Mg(OH)2. The NH3 was driven off during the heating. One sign of this reaction was the ammonia smell given off. This is because upon heating, the Mg(OH)2 would break into MgO and H2O, which would be driven off by the heat. The second reheating was so that any remnants of the Mg(OH)2 of the crucible had been converted to MgO. This was also to deplete an accurate final mass of our product MgO.After the lab, the inside of the crucible was black. This is because the magnesium not only reacted with the oxygen and the nitrogen in the air but also with the porcelain of the crucible. The reason for waiting for the crucible to cool onward weighing it was because at higher temperatures, the molecules inside are still active, make the weight to be off. During Trial 2, the ma gnesium was not properly burn down off and caused the calculations to be off. The magnesium looked as if it had stopped glowing, but the inside coil was not completely burned.REFERENCESwww.iun.eduwww.chemistry.about.comwww.universetoday.com/john-daltons-atomic-theoryLab Experimentwww.purdue.edu