Chemistry IA design format Essay

1.0.0- Introduction1.0.1- instruction Question- If the host of atomic number 12 reacted with hydrochloric bitter is smor catalystbordd entrust the temperature of the consequence increase and the aggregate batch decrease.1.0.2- Hypothesis- If the set of milligram that is reacted with hydrochloric acid is transportd the temperature of the resolvent will increase and the total mass will decrease.1.0.3- Theory- The reply between milligram and hydrochloric response is written as follows, Mg(s)+ 2HCL (aq) (MgCl2(aq)+H2 (g) (Ng, 2008, pg 1). This response goes done two distinct qualifys that both have an exertion on the cipher shift in the reaction. total heat refers to changes in vital force in a deepen (Assut, 2008, pg 1). Two distinct changes can occur. An endothermic change occurs when the zero universe listless is grater then the vigour being released whereas and exoergic change is when the elan vital being released is greater than the energy being absorb ed. Energy is absorbed when perplexs are broken and energy is released when they are recoil (Newton, 2008, pg1). Energy change cannot be directly careful. still energy change affects the physical force of heat. hence a heat change is indicative of an energy change. If the heat increase in the solution the change will be exothermic and if the heat decreases the reaction will be endothermic. In respects to the reflexion Magnesium configurations an ionic bond with chlorine to form the salt magnesium chloride. When this bond is formed energy is released in the form of an endothermic change, this energy draw would be quite small however because the bond is ionic and does not take much energy to create since magnesium and chorine bond easily. that the second change is that hydrogen irrupts off from chlorine in the hydrochloric acid and hydrogen is released as a gas.The breaking of bonds would absorb energy in that respectfore forming an exothermic reaction. Hydrogen and chorine however form a very strong covalent bond. Covalent bonds form between atoms with similar electronegative forces and are at that place for take a lot of energy to break ( Anissimov, 2008, pg 1) Since the endothermic change is weak and the exothermic change is strong it can be predicted that the overall change will be exothermic and therefore the solution will heat up. Temperature change in a chemical reaction can be measured with a device known as a calorimeter. A calorimeter measures the heat of the solution before the reaction has occurred and then again after the reactant has been added (Whel, 2008, pg 1). These two value can be mathematically manipulated to find the comparative change in temperature.If two of the same message have different masses it heart and soul there is to a greater extent of the one cognitive content. In a mass of a substance there is a certain(prenominal) follow of material that can be reacted. By increasing mass the amount of substance that may be reacted increases. Therefore if mass increased the amount that of substance reacted will increase as headspring providing there is enough of the reactant. This will in squirm increase the energy change. Also if much of the substance reacts with the reactant more of the reactant will be used up. This means that if the magnesium is increased there will be more reaction with hydrochloric acid this means that more hydrogen will be released as gas and the total mass of the solution will decrease. henceforward the change in heat should be greater if their entire solution is lighter as more of the hydrochloric acid has been reacted and hydrogen lost as a gas.How the reaction works (Figure 1)Mg(s)+ 2HCL (aq) (MgCl2(aq)+H2 (g)1.1.0- chairling variables1.1.1- Variables (Table 1)Variable caseful of variableMethod for controlMass of magnesiumIndependentMass will change for individually sample, sample range will be 2g, 4g, 6g, 8g and 10g high temperature change unfreeThis will be calcula te by subtracting the final heat of the solution by the initial heat of the solution. The data will be gathered by using a calorimeter flip in mass in solutionDependentThis will be calculated by mensuration the weight of the solution and subtracting the weight of the calorimeter and the magnesium. The original mass not including calorimeter and the magnesium will then be subtracted by this value to mind the change of mass in the solution.Initial temperatureControlledThe temperature of the solution will be heated to 25c and the reaction skip overed immediately.External temperatureControlledThe room temperature will be controlled at 24cVolume of hydrochloric acidControlledThe flashiness of hydrochloric acid will be 40mls per sample.Measuring frame-upControlledA 50ml calorimeter with electronic thermometer and a scale with milligram accuracy.Time of experimentControlledThe experiment will be ended when reaction is fully complete and reaction will be given 10 seconds to adjust befor e results are takenReplicationsControlledStandard 5 replications of each sample will be performed.1.1.2- Control used in comparison- The reacted samples will be compared against hydrochloric acid with no magnesium that is also 25 degrees Celsius. Since the temperature trunk constant there should be no energy or mass change, this would mean that on a graph this would represent a straight patronage which others samples with energy changes (heat changes) could be compared to.BibliographyNg, H.N, 2008, Acid reactions, Vat.Gov.Un, Accessed 21/08/09, http//vat.maharashtra.gov.in/communicationcenter/QueryAnswerSubjectwise.php?start=3090&subId=0000000007.Asset, M.A, 2008, Chemical Enthalpy, Nasa.gov, Accessed 21/08/09, http//www.grc.nasa.gov/WWW/K-12/airplane/enthalpy.htmlNewton, R.N, 2008, Energetics and bonding, little-known sponsor, Accessed 21/08/09, http//www.webchem.net/notes/how_far/enthalpy/enthalpy_diagrams.htmAnissimov, T.A, 2007 Chemical bonding, Simon Frasier University, Acce ssed 21/08/09, http//www.chem1.com/acad/webtext/chembond/Whel, L.W, 2006, Calorimeters, Stanford University, Accessed 21/08/09, http//www2.slac.stanford.edu/vvc/detectors/calorimeters.htmlAcknowledgmentsThe procedure of this experiment is a adaption of a old class experiment. The source of the procedure is unknown, so thank to Miss Crook for the inspirations for this design.