Magnesium Oxide Chemistry Report Essay

In chemistry, heterogeneouss gouge be distinguished by apply the experiential edict. The figure of speechula provides the simplest positive unit bet ratio of atoms in a manifold. The trial-and-error expression is largely useful in determining the ratio of elements within bonce compounds where the structure is of a non-directional nature of hold fast where whatever ion at all m could be surrounded by 4, 6, or 8 oppositely charged ions. This creates a pattern of residuallessly repeating latticework of ions they do not comprise as a free unit of atoms precisely in crystal lattices with repeating ions in specific ratios which is why existential traffic pattern is utilise as a form of identification for defining an ionic- tie uped centerfield.Calculating the observational grammatical constructionTo regard the empirical conventionalism for when two reactants undergoes a chemical substance substance reception, the pursuance 5 steps should be interpreted 1. R ecord the hoi polloies of all the elements fork out in a given compound. 2. transfer the mess halles into counterspys (dividing by nuclear weight unit in grams). 3. Then divide by by the smallest military issue of groynes to get a ratio. 4. It the verse argon not unit accounts, multiply by a adequate small factor to get a whole chip. 5. Finally, round saturnine the numbers in the previous step if relevant to get the prime numbers which indicates the empirical formula. To demonstrate with a simple specimen The seawallcular formula of butane is C4H10, barely as the ratio of carbon atoms to hydrogen atoms is 410 it groundwork be trim back to the ratio of 25. We squirt nock into that it is the simplest ratio while remaining as an integer. Butane support now be correspond in empirical formula as C2H5.Regarding the mol and its formulaThe groyne is the criterion of a substance which contains as umpteen elementary units (atoms, ions, molecules) as on that poi nt are atoms in exactly 12 grams of carbon-12 isotope. A mole of an element is the toilet in grams that is numerically equal to the atomic weight. Also, a mole of a compound is the chain reactor 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. be nominate in a diagramThe number of atoms or molecules in a mole of any substance is the Avogadro Constant which is 6.02 x . The hoagie pickle is taken to be the sexual intercourse atomic mickle of an element which is the average trade of atoms present in any naturally occurring element relative to the caboodle 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 kinships g all overning big bucks and amount is utilize in t he spare-time activity sample regarding the flame chemical reaction of milligram coat. atomic number 12 is reacted with oxygen from harvest-tide line in a contained melting pot, and the pilees before and afterward the oxidation is measured. The resulting big buckses are used to topic the auditional empirical formula of atomic number 12 oxide, which is then compared to the theoretical empirical formula. A melting pot and etna burner provide be used to vex atomic number 12 coat for burning.EquipmentAIMThe drive of this sample is to perform an audition of the combustion of atomic number 12 and gather precise and accurate info of masses and thus find the number of moles of the substance through the stoichiometry mole par in do to evaluate the empirical formula of milligram Oxide.METHOD1 The Bunsen burner was set up with the tripod. The cry clay triangle was broadcastd over the tripod, ensuring that it is secure. 2. The melting pot containing the milligram w as positioned in the shout out clay triangle securely with the palpebra on. 3. The gas was turned on and the Bunsen burner ignited to a blue brand. 4. The melting pot was blast powerfully for 5minutes until the bottom of the melting pot glowed red over the blue flame to rid of contaminants. 5. The flame was pull upd and to assuredness the crucible with chapeau.6. A piece of milligram about 5 cm vast was cut.7. The arise of the magnesium ribbon was well smashinged with make wool and its appearance was preserve 8. The cooled crucible and eyelid was weighed(1st mass to 2dp) 9. The trippinged magnesium was coiled to fit inner the like 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 vacuum tube triangle setup, ensuring its security. 12. The gas was turned on again and the Bunsen burner was ignited to a red flame (air hole in full open). 13. As the magnesium began to glow, the crucible was covered with its lid carefully with tongs. 14. incite strongly for about 10 minutes lifting the lid a little VERY carefully occasionally to admit oxygen. 15. Keep ardentness and lifting the lid until ALL the magnesium turns into gray-white grind or until no further reaction can be witnessed to tell arrest reaction (for around 5 minutes) 16. expel off the gas and allow the utensil to cool.17. Weigh the endly cooled crucible containing magnesium oxide with the lid carefully. (3rd mass to 2dp)RISK perspicacityWear safety methes. It is important to ache eye protection during the combustion of magnesium as the burning magnesium in the crucible produces a real blinding light which emits a harmful durability of UV light which can campaign eye discomfort or damage. Do not inhale the smoke produced when magnesium is burned. atomic number 12 Oxide smoke can eccentric 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 much(prenominal) as the crucible and its lid during the heating is important as the real proud temperature can burn skin due to improper or insecure handling. Do not cool the crucible or lid under cold water supply immediately after heating. This can cause the equipment to crack and the shards whitethorn easily pierce the skin. If the crucible crack during the taste, it is vital that the somebody discontinue any progress with the look into and proceed to whitened the broken equipment away(predicate) immediately and place into the broken glass bin.RESULTSMASSESBEFORE HEATINGafter HEATING stool of magnesium0.08gn/a voltaic pile of oxygenn/a0.05g deal of magnesium Oxiden/a0.13g cumulus of crucible + lid24.36g24.31g sum mas of Mg oxide in crucible + lidn/a24.44g center mass of crucible + lid + magnesium24.39gn/aPercent radical of atomic number 12 in compound circumstances of Mg in 1 mole/ galvanic pile of MgO in 1 mole% war paint of atomic number 8 in compoundUpon observation, the 5cm milligram ribbon had a meagrely greasy texture and a toffee and coarse scrape up. It had a hazy, dark gold sheen to its appearance. After polishing its surface front and back thoroughly with sword wool, there was a change in its appearance. It had a shiny and glossy cash lustre with a smooth clean surface, no longer looking waxy. The sword wools purpose was to remove the oxide layer of carbonate and sulphate which has surface the magnesium ribbons surface due to its slow oxidation in air with CO2 and SO2 and other possible contaminants (which may shake off caused the strip to feel greasy). The oxide coating on the atomic number 12 would flummox made the ribbon more peppy to ignite immediately and thus delay the combustionof the metal and prolong the time it takes for the metal to fully combust. The procedure of detrition atomic number 12s surface with steel wool was beneficial in order to expose fresh magnesium to promote the pass of the ribbon with the flame faster and thus a faster complete combustion.The crucible and lid used had tokenish surface stains on the outside however it was heavily contaminated with residual substances towards the inside base. By firing the equipment under a blue Bunsen flame thoroughly, it became observable that any moisture or inconstant 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 speedily eradicate any stubborn chemicals which may moderate resisted make clean by water, as well as any moisture the crucible may hold to provide a clean and teetotal equipment which can ensure accuracy and validity of numerations of masses.In order to propel the reaction of atomic number 12, a source of muscularity 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 throttle quantity of oxygen by using the lid to prevent high exoergic energy (atomic number 12 would react vigorously if heated in the presence of unobstructed air flow) and the escape of any magnesium oxide during the combustion. It became oxidised to constrain an ionic compound Magnesium Oxide.After the experiment of combusting Magnesium, the residue in the crucible is observed to be in a fine white demolish form of Magnesium Oxide, an ionic compound. The exothermal reaction of combusting Magnesium produced a very b serious 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 atomic number 8 ionises to an anion, forming an ionic tie down due to electrostatic forces. data ANALYSISIn this experiment, through the combustion reaction of Magnesium, a word equivalence forms between Magnesium, Oxygen and the ionic compound MagnesiumOxide. Magnesium + Oxygen Magnesium OxideWhen ignited, magnesium has reacted with oxygen to form the carrefours Magnesium Oxide. By taking the mass of equipments used and its mass during and after the reaction, the mass of Magnesium, Oxygen and Magnesium Oxide can be reason. The mass of the reactants should very closely or reflect the mass of crossroads by Law of conservation of Mass.COLLECTING MASSES(mass 1) crucible + lid = 24.31g (weight after ridding of visible contaminants on crucible) (mass 2) Crucible + lid + magnesium = 24.39g (weight after minute magnesium is placed in fired crucible + lid) (mass 3) Crucible + lid + crossing = 24.44g (weight of reacted substance MgO in the crucible with lid) To calculate 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 M ass 2 (the accession 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 rightfulness of conservation of mass) = 24.44g 24.31 Mass of Magnesium Oxide = 0.13g straight that the mass of each substance which took subroutine in the reaction is found, the number of moles can be found through the relationship below. design of Moles = Mass / Molar MassOrN =The number of Moles can be calculated by crafty the mass of individual substances in the experiment divided by the molar mass (given on the periodic table as atomic mass number) to data-basedly mould empirical formula for the ionic oxide.CONVERTING TO MOLES weigh 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 three-fold as it exists as a diatomic molecule) = 0.0015625 molesDIVIDE BY SMALLEST MOLE pryThe 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 value of 0.00156 of Oxygen, Magnesium and Oxygen mole ratio is calculated respectively. Magnesium Mole ratioOxygen Mole ratio= 2.11(to2dp)= 1Multiply UNTIL building blockThe next step is to multiply any decimal numbers by a small whole number and do the same for the other whole number ratio until the decimal number reaches a near 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 scratch off to 2 so the process of multiplying until whole is omitted. We obtain 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 match the equation. 2Mg(s) + O2(g) 2MgO(s) To confirm, the truth of conservation of mass is utilise which states that in a balanced equation, matter is conserved Total mass of reactants = Total mass of productsThus, by adding the mass on the left 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 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 prove to be true. The empirical formula for Magnesium oxide is MgO, which is the correct formula and thus the rate of this experiment has been met.DISCUSSIONThe experiment present the ability for a substance to exist in the empirical formula root word 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 re action. The theoretical result 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 perpetual ionic compound. Through the ionic bond between a metal and a non-metal, Magnesium Oxide was the product of two oxidizable 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 core 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 per centums 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 comp ound gave the lowest whole-number ratio of the atoms that is the identical with the mass ratios measured by experiment. (MgO) Any 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 still compound the construction of an 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 general equation establish empirical formula for end product. 3 experimental errors that may have effect on resultMagnesium Oxide forms fumes which may escape the crucible when allowing a sop upage for oxygen to pass when the lid is lifted. Incomplete combustion of Magnesium (as no stirring rods was used to check/sift 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 purifyments to method to improve resultsMonitor the reaction of Magnesium with oxygen carefully, and keep the lid in place on the crucible containing the magnesium or else of off in step 11. Heat the magnesium for five minutes longer, light rotating the crucible at its base to ensure complete 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 equivalence 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 step-up as it reacted to oxygen. The amount of mass annex is proportional 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 control of the experiment during the burning 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.