Magnesium Oxide Chemistry Report Essay

In chemistry, deepens skunk be distinguished by using the semi data-based radiation pattern. The expression provides the simplest positive integer balance of parts in a tangled. The empirical formulation is largely useful in ascertain the ratio of components within ionic compounds where the structure is of a non-directional nature of soldering where any ion at any time could be surrounded by 4, 6, or 8 oppositely charged ions. This creates a pattern of endlessly repeating lattice of ions they do not exist as a free unit of atoms but in crystal lattices with repeating ions in specific ratios which is why empirical formula is use as a form of identification for defining an ionic-bonded substance.Calculating the empirical formulaTo work up the empirical formula for when two play sourants undergoes a chemical reply, the following 5 musical notes should be taken 1. Record the weedes of all(a) the elements resign in a given(p) compound. 2. Convert the megabuckses into moles (dividing by nuclear burthen in grams). 3. Then divide through by the smallest lean of moles to get a ratio. 4. It the issues be not w deal human activitys, compute by a sui accede small factor to get a whole number. 5. Finally, round off the numbers in the previous step if applicable to get the prime numbers which indicates the empirical formula. To demonstrate with a simple example The molecular formula of butane is C4H10, however as the ratio of carbon atoms to hydrogen atoms is 410 it sens be trim down to the ratio of 25. We can see that it is the simplest ratio while be as an integer. Butane can now be represented in empirical formula as C2H5.Regarding the breakwater and its formulaThe mole is the quantity of a substance which contains as many elementary units (atoms, ions, molecules) as there are atoms in barely 12 grams of carbon-12 isotope. A mole of an element is the quite a little in grams that is numerically impact to the atomic weight. Also, a mole o f a compound is the good deal in grams that is numerically equal to the molecular weight. In simpler wordsA mole of a substance is simply the atomic / molecular weight in grams. eg Amole of copper (atomic weight 63.6) is 63.6grams.Therefore in a diagramThe number of atoms or molecules in a mole of any substance is the Avogadro Constant which is 6.02 x . The poor boy potbelly is taken to be the relative atomic bulk of an element which is the average host of atoms present in any naturally occurring element relative to the large number of one atom of carbon-12 isotope taken as exactly 12 which gives formula weight (sum of the atomic weights of the atomic species as given in the stated formula for the compound.) The quantitative stoichiometric relationships governing aggregated and count is used in the following look into regarding the burn chemical reaction of milligram metal. atomic number 12 is reacted with oxygen from air in a contained melting pot, and the heap befor e and afterwards the oxidation is measured. The exiting lower classes are used to cipher the try outal empirical formula of magnesium oxide, which is then compared to the theoretical empirical formula. A melting pot and bunsen burner will be used to lovingness magnesium metal for burning.EquipmentAIMThe purpose of this examine is to perform an experiment of the combustion of atomic number 12 and gather precise and accurate data of heap and thus find the number of moles of the substance through the stoichiometry mole comparison in order to evaluate the empirical formula of atomic number 12 Oxide. rule acting1 The Bunsen burner was set up with the tripod. The pipe body trilateral was placed over the tripod, ensuring that it is secure. 2. The crucible containing the magnesium was positioned in the pipe clay triangle securely with the chapeau on. 3. The gas was swordplayed on and the Bunsen burner ignited to a unappeasable flaming. 4. The crucible was fired strongly fo r 5minutes until the bed of the crucible glowed red over the blue flame to rid of contaminants. 5. The flame was askd and to cool the crucible with lid.6. A piece of magnesium somewhat 5 cm long was cut.7. The surface of the magnesium ribbon was soundly dissipateded with steel wool and its appearance was recorded 8. The cooled crucible and lid was weighed(1st mass to 2dp) 9. The cleaned magnesium was coiled to fit inside the same crucible and cover with the same lid. 10. The crucible containing the magnesium with the lid on was weighed. (2nd mass to 2dp) 11. The crucible containing the magnesium was positioned without the lid onto the pipe triangle setup, ensuring its security. 12. The gas was turned on again and the Bunsen burner was ignited to a red flame (air hole fully open). 13. As the magnesium began to glow, the crucible was covered with its lid conservatively with tongs. 14. Heat strongly for about 10 minutes lifting the lid a little VERY carefully occasionally to a dmit oxygen. 15. Keep thaw and lifting the lid until ALL the magnesium turns into gray-white powder or until no and reaction can be witnessed to ensure complete reaction (for round 5 minutes) 16. Turn off the gas and allow the apparatus to cool.17. ponder the completely cooled crucible containing magnesium oxide with the lid carefully. (3rd mass to 2dp)RISK judgmentWear safety glasses. It is important to acquire eye protection during the combustion of magnesium as the burning atomic number 12 in the crucible produces a truly agleam light which emits a harmful intensity of UV light which can example eye discomfort or damage. Do not inhale the smoke produced when milligram is burned. Magnesium Oxide smoke can cause irritation in the nose, eyes and lungs and in large amounts, whitethorn cause metal fume fever. Use tongs at all times when handling hot objects. Careful handling of hot equipment such as the crucible and its lid during the heating is important as the very high t emperature can burn skin due to improper or insecure handling. Do not cool the crucible or lid under cold water immediately after heating. This can cause the equipment to crack and the shards may easily pierce the skin. If the crucible crack during the experiment, it is alert that the person discontinue any progress with the experiment and proceed to clean the broken equipment away immediately and place into the broken glass bin.RESULTS dregs of the peopleBEFORE HEATINGAFTER HEATING locoweed of Magnesium0.08gn/aMass of oxygenn/a0.05gMass of Magnesium Oxiden/a0.13gMass of crucible + lid24.36g24.31gTotal mas of Mg oxide in crucible + lidn/a24.44gTotal mass of crucible + lid + magnesium24.39gn/aPercent constitution of Magnesium in compoundMass of Mg in 1 mole/ Mass of MgO in 1 mole% composition of oxygen in compoundUpon observation, the 5cm Magnesium ribbon had a s light oily texture and a brittle and coarse surface. It had a hazy, dark gold sheen to its appearance. After polishin g its surface front and back thoroughly with steel wool, there was a change in its appearance. It had a showy and glossy silver lustre with a smooth clean surface, no longer feeling waxy. The steel wools purpose was to remove the oxide layer of carbonate and sulphate which has coated the Magnesium ribbons surface due to its slow oxidation in air with carbon dioxide and SO2 and another(prenominal) possible contaminants (which may have caused the strip to feel greasy). The oxide finis on the Magnesium would have made the ribbon more bouncy to ignite immediately and thus hinder the combustionof the metal and pull up the time it takes for the metal to fully combust. The procedure of rubbing Magnesiums surface with steel wool was beneficial in order to undo fresh Magnesium to facilitate the intercommunicate of the ribbon with the flame quick and thus a faster complete combustion.The crucible and lid used had minimal surface stains on the outside however it was heavily pollute w ith residual substances towards the inside base. By firing the equipment under a blue Bunsen flame thoroughly, it became apparent that any moisture or erratic materials present are burnt off by 5minutes to reveal a clean crucible free of stains or moisture. The purpose of firing the crucible at a high temperature was to apace eradicate any hardheaded chemicals which may have resisted cleaning by water, as well as any moisture the crucible may hold to provide a clean and dry equipment which can ensure accuracy and validity of calculations of batch.In order to activate the reaction of Magnesium, a source of energy was needed. The flame provided a source of heat which prompted a chemical reaction to proceed. When the magnesium was supplied with energy in the crucible, it reacted with a limited quantity of oxygen by using the lid to obstruct high exothermic energy (Magnesium would react vigorously if heated in the presence of unobstructed air flow) and the thrash of any magnesium oxide during the combustion. It became oxidized to become an ionic compound Magnesium Oxide.After the experiment of combusting Magnesium, the residue in the crucible is observed to be in a fine white powder form of Magnesium Oxide, an ionic compound. The exothermic reaction of combusting Magnesium produced a very bright light within the crucible due to the rapid heating of the Magnesium, where it quickly absorbs energy through ionisation. Magnesium ionises to become a cation while group O ionises to an anion, forming an ionic bond due to electrostatic forces.DATA ANALYSISIn this experiment, through the combustion reaction of Magnesium, a word equation forms between Magnesium, atomic number 8 and the ionic compound MagnesiumOxide. Magnesium + oxygen Magnesium OxideWhen ignited, magnesium has reacted with oxygen to form the point of intersections Magnesium Oxide. By victorious the mass of equipments used and its mass during and after the reaction, the mass of Magnesium, Oxygen a nd Magnesium Oxide can be waitd. The mass of the reactants should very closely or mirror the mass of products by Law of Conservation of Mass.COLLECTING MASSES(mass 1) melting pot + lid = 24.31g (weight after ridding of visible contaminants on crucible) (mass 2) Crucible + lid + magnesium = 24.39g (weight after polished magnesium is placed in fired crucible + lid) (mass 3) Crucible + lid + product = 24.44g (weight of reacted substance MgO in the crucible with lid) To visualize the mass of Magnesium metal = Mass 2 Mass1 = 24.39g 24.31g Mass of Magnesium = 0.08gTo calculate the Mass of Oxygen incorporated = Mass 3 Mass 2 (the increase in mass corresponds to the mass of oxygen) = 24.44g 24.39g Mass of Oxygen = 0.05gTo calculate the mass of oxide product formed = Mass 3 Mass 1 (to validate through law of conservation of mass) = 24.44g 24.31 Mass of Magnesium Oxide = 0.13g now that the mass of each substance which took part in the reaction is ready, the number of moles can be fou nd through the relationship below. Number of Moles = Mass / Molar MassOrN =The number of Moles can be calculated by knowing the mass of individual substances in the experiment divided by the molar mass (given on the periodic table as atomic mass number) to experimentally determine empirical formula for the ionic oxide.CONVERTING TO MOLESNumber of Moles of Magnesium N = 0.08g / 24.31g/mol= 0.00329082692 moles Number of Moles of Oxygen N = 0.05g/16x2g/mol (oxygen is doubled as it exists as a diatomic molecule) = 0.0015625 molesDIVIDE BY SMALLEST MOLE VALUEThe number of moles of Magnesium is larger than the number of moles of Oxygen 0. 00329(to5dp) moles 0.00156 (to5dp) molesBy dividing each by the smallest mole appreciate of 0.00156 of Oxygen, Magnesium and Oxygen mole ratio is calculated respectively. Magnesium Mole ratioOxygen Mole ratio= 2.11(to2dp)= 1Multiply UNTIL entirelyThe next step is to multiply any decimal numbers by a small whole number and do the same for the other w hole number ratio until the decimal number reaches a beloved whole number (which can then be rounded up). Magnesium Mole ratio is in a decimal number of 2.11, and as it is very close to 2(with 0.11 extra of being a whole number), the number 2.11 is round down to 2 so the process of multiplying until whole is omitted. We check the mole ratio as follows Magnesium Oxygen 2 1 With 2 moles of Magnesium reacting with 1 mole of Oxygen, this should suggest 2 moles of MgO after balancing the equation. 2Mg(s) + O2(g) 2MgO(s) To confirm, the law of conservation of mass is applied which states that in a balanced equation, matter is conserved Total mass of reactants = Total mass of productsThus, by adding the mass on the leave hand side (reactants), it should equal the right hand side (product). Magnesium + Oxygen = 0.08g + 0.05gMagnesium Oxide = 0.13g It is found that there is no difference in mass between the left over(p) side of 0.13g of Magnesium + Oxygen to the right side of 0.13g of Magnesium Oxide in the equation considering the possibility of experimental errors, which represents a positive outcome as an theoretical equation is established and proved to be true. The empirical formula for Magnesium oxide is MgO, which is the correct formula and thus the aim of this experiment has been met. railleryThe experiment demonstrated the ability for a substance to exist in the empirical formula composition as the simplest ratio of elements present in the compound. It also demonstrated quantitative stoichiometric relationships between the number of moles, mass and molar mass in a chemical reaction. The theoretical number for the combustion product of Magnesium and Oxide is MgO, which in comparison to the experiment result of MgO was proven to be the same. This experiment had demonstrated the basic chemical reaction and the change in states between elements in order to form a invariable ionic compound. Through the ionic bond between a metal and a non-metal, Magnesium Oxide was the product of two reactive elements Magnesium and Oxygen.Theoretical laws of conservation of mass and constant composition, lead to the formation of a relationship between the reactants (Magnesium and Oxygen) and product (Magnesium Oxide). The total mass of the products of a reaction must equal the total mass of the reactants. (0.8+0.5 = 0.13) The coefficient of a substance indicated the amount of portions each substance existed in, based on the law of conservation of mass. (2 moles of Magnesium, 1 mole of Oxygen, and 2 moles of Magnesium Oxide).And lastly, the empirical formula of a compound gave the lowest whole-number ratio of the atoms that is the identical with the mass ratios measured by experiment. (MgO) some(prenominal) portion of a compound will have the same ratio of masses as the elements in the compound. Metal and a non-metal reaction of 2 substances taking place Ionic bond of elementschanges in states and formation of a stable compound the construction of a n unbalanced chemical equation - evaluation of masses of the reactants to products the law of conservation of mass/and constant composition -the masses of left sideequals right side provide moles to balance the overall equation establish empirical formula for end product. 3 experimental errors that may have effect on resultMagnesium Oxide forms fumes which may get down the crucible when allowing a passage for oxygen to pass when the lid is lifted. unelaborated combustion of Magnesium (as no stirring rods was used to check/ locomote through the oxide to prevent calculation errors) Unthorough firing of crucible and lid (due to contact between tongs and crucible, certain areas may be missed) 3 improvements to method to improve resultsMonitor the reaction of Magnesium with oxygen carefully, and keep the lid in place on the crucible containing the magnesium instead of off in step 11. Heat the magnesium for five minutes longer, lightly rotating the crucible at its base to ensure complet e combustion. Fire the crucible and the lid twice to ensure that its completely dry and clean.CONCLUSIONAn experiment was performed to calculate the empirical formula of magnesium oxide by comparing the masses of solid magnesium metal to the magnesium oxide solid product in a crucible. The concept of stoichiometry mole equation leads to finding the empirical formula of magnesium oxide. One major finding during the experiment was that burning magnesium caused its mass to increase as it reacted to oxygen. The amount of mass increase is proportionate and able to be calculated through weighing the mass of product Magnesium Oxide and subtracting the original Magnesium mass to calculate the mass of Oxygen which partook in the combustion.The Empirical formula had indicated the proportion of Magnesium to oxygen (11) and identifies the compound to be Magnesium Oxide. The balance was very accurate in taking precise measurements of masses and the supervision of the experiment during the burni ng had been careful to prevent any loss of Magnesium Oxide mass to escape which in turn caused my mass results to apply to the law of conservation of mass without any experimental errors.