Heat of Formation of Magnesium Oxide

ObjetiveTo finalize the light up formation of MgO ( milligram Oxide) using Hesss Law, which states the heat within a chemical reaction is independent of the pathway amidst the initial and final states.IntroductionChemical reactions require heat expertness to complete, called an endothermic reaction, or produce heat energy, and thus called an exothermic reaction. The heat energy produced by such(prenominal) reactions can be measured using a calorimeter, a piece of equipment that can isolate the reaction in an insulated container. Using the calorimeter one can indeed determine the rise and fall in temperature of the reaction. When this temperature change is multiplied by the heat ability, the amount of heat needed to raise the temperature of a body by one degree, we can measure the change in converting our initial components (reactants) to their respective products.In this experiment we will measure the amount of heat released from 3 reactions (HA HB HC) and picture the sum of a ll 3 reactions to determine HT, which will give us the heat formation of MgO. If Hesss law holds true and barring minimum experimental error, the pathway we use to determine HT should have no bearing on our calculation matching the accepted calculation of MgO.MethodsAs per lab manual we use a calibrated calorimeter (using a rounded end thermometer so as to not puncture a hole in the calorimeter) to determine the heats of reaction for Magnesium (Mg) with Hydrochloric Acid (HCl) and Hydrochloric Acid with Magnesium Oxide (MgO). Then using mathematical formulas we were able to calculate the heat formation of MgO, which is measured in kJ/Mol. Since both reactions are in dilute water supply solutions ofHCl it was necessary to know the heat capacity of water, but because some heat would be transferred to the calorimeter whose heat capacity was unknown, we had to record a subject area factor (x) based upon the specific heat of water using the equation m(h2o)+XCwater+water=-1(m( nut wate r)Cwatertice water).We then recorded the mass (m) of live temperature water and ice water each in a respective cup and then poured the ice water into the room temperature water and recorded the temperature change. By knowing (x) we could then calculate the heat of reaction for Mg with HCl (HA kJ/mol) and for HCl with MgO (HB kJ/mol) using the equation q=m(HCl+X)C T where m is the mass of the reactant used with Mg + X, C is the heat capacity of water (4.184 J/gC), and T is the total temperature change in each reaction. Using the results of these calculations and Hesss law we can then determine the heat formation for MgO.DataAll mass readings are given in units of grams (g), and all temperature readings are given in degrees Celsius (C).Part AMass of the Calorimeter + RoomTemp Water (g)48.08Mass of room temp water (g)46.29Mass of Cal + room temp water + icewater (g)115.40Mass of ice water (g)67.32Temp of room temp water (C)42.4Temp of the ice water (C)0.1Final temp. of room temp water (C)17.3Change in temp of ice water (C)17.2Change of temp of room temp water (C)-25.1Mass of the calorimeter (g)1.79Part 2AMass of Calorimeter (g)1.79Mass of Cal + HCl (g)103.55Mass of HCL (g)101.76Mass of Mg (g)0.5Temperature of HCl (C)20.3Final temperature of HCl + Mg (C)42.0Change in Temperature (C)21.7Part BMass of Calorimeter (g)1.79Mass of Cal + HCl (g)101.76Mass of HCl (g)99.88Mass of MgO (g)0.8Temperature of HCl (C)20.3Final temperature of HCl + MgO (C)25.8Change in Temperature (C)5.50Results and DiscussionTo calculate X using the equation m(h2o)+XCwater+water=-1(m(ice water)Cwatertice water) the variable star X must be isolated and doing so we were than able to calculate the correction factorBased on the calculations of the calorimeter correction factor, X was determined to be 0.158 g. Then using the equation q=m(HCl+X)C *T, where q is equal to the amount of energy given off, and than calculating the value in -kJ/Mol (because these are exothermic reactions) we were able to determine HA and HB.qA=m(HCl+X)C xTqA=(101.76 g + 0.158 g) x 4.184 J/gC x 21.7CqA= 9250 J = 9.250 kJ 9.253602176qB= m(HCl+X)C xTqB=(101.76 g + 0.158 g) x 4.184 J/gC x 5.50CqB=2350 J = 2.350 kJTo then calculate the heat formation of MgO HT, the sum of all the reactions must be determined including HC, the heat formation of water, which is already predetermined to be -285.8 kJ/mol. However to determine the proper equation for HT, the stoichiometric equations must first be balancedTherefore the heat formation of MgO was determined to be -618.35 kJ/mol. According to the textbook, the accepted value for HT=-601.8 kJ/mol. To determine the accuracy of the calculation we can determine the % errorAs far as accuracy goes a portion error of 2.75% is very acceptable. Because the methods of the experiment were conducted using a crude calorimeter I would have expected the percent error to be higher, assuming that because of its formula it would not have very high efficiency.I would expect that any error that might have occurred happened during the transference from one cup to another. Because the substances were transferred so quickly and pickings into account the number of seconds that it took to replace the thermometer to begin recording data again it is possible that energy was either lost in the transfer or energy was lost before the recording was actually able to begin.ConclusionIn this lab we were able to determine the heat of formation of MgO using a simply constructed calorimeter, which was found to be -618.35 kJ/mol.