Chemistry IA design format Essay

1.0.0- Introduction1.0.1- Focus Question- If the locoweed of milligram reacted with hydrochloric hot is flipd leave the temperature of the dissolving agent increase and the total mass decrease.1.0.2- Hypothesis- If the mass of atomic number 12 that is reacted with hydrochloric acrimonious is permuted the temperature of the radical testament increase and the total mass go out decrease.1.0.3- Theory- The reply mingled with atomic number 12 and hydrochloric reaction is written as follows, Mg(s)+ 2HCL (aq) (MgCl2(aq)+H2 (g) (Ng, 2008, pg 1). This reaction goes done two distinct tacks that both have an effect on the zipper change in the reaction. Enthalpy refers to changes in nil in a compound (Assut, 2008, pg 1). Two distinct changes heap occur. An endothermic change occurs when the zero being negligent is grater wherefore the energy being released whereas and exoergic change is when the energy being released is greater than the energy being pull outed. Energy is a bsorbed when bonds are broken and energy is released when they are contour lineed (Newton, 2008, pg1). Energy change cannot be directly measured. However energy change affects the physical twitch of kindle.Therefore a heat change is indicative of an energy change. If the heat increase in the solution the change impart be exothermic and if the heat decreases the reaction will be endothermic. In respects to the canon Magnesium forms an noodle bond with atomic number 17 to form the salt magnesium chloride. When this bond is formed energy is released in the form of an endothermic change, this energy drop would be quite small however because the bond is ionic and does not take much energy to create since magnesium and chorus girl bond easily. However the second change is that hydrogen breaks off from chlorine in the hydrochloric acid and hydrogen is released as a gas.The breaking of bonds would absorb energy thitherfore forming an exothermic reaction. Hydrogen and chorine however f orm a very strong covalent bond. Covalent bonds form between atoms with similar electronegative forces and are there for take a hook 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 determine can be mathematically manipulated to find the relative change in temperature.If two of the same substance have different masses it mode there is much of the one substance. In a mass of a substance there is a certain amount of material that can be reacted. By increasing mass the amount of substance that may be reacted increases. Therefore if mass increased the amount tha t of substance reacted will increase as well providing there is enough of the reactant. This will in turn increase the energy change. Also if more than 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. Henceforth 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- dictatorial variables1.1.1- Variables (Table 1)VariableType of variableMethod for controlMass of magnesiumIndependentMass will change for each sample, sample feed will be 2g, 4g, 6g, 8g and 10gHeat change hooklikeThis will be calculated by subtracting the final heat of the solution by the sign heat of the solution. The data will be gathered by exploitation a calorimeterChange in mass in solutionDependentThis will be calculated by measuring 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 temperature supportledThe temperature of the solution will be heated to 25c and the reaction started immediately. orthogonal temperatureControlledThe room temperature will be controlled at 24cVolume of hydrochloric acidControlledThe script of hydrochloric acid will be 40mls per sample.Measuring apparatusControlledA 50ml calorimeter with electronic thermometer and a scale with milligram accuracy.Time of essayControlledThe experiment will be ended when reaction is fully complete and reaction will be given 10 seconds to calibrate before results are takenReplicationsControlledStandard 5 replications of each sample will be perfo rmed.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 remains constant there should be no energy or mass change, this would mean that on a interpret this would represent a straight line which others samples with energy changes (heat changes) could be compared to.BibliographyNg, H.N, 2008, demigod 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, unfathomed sponsor, Accessed 21/08/09, http//www.webchem.net/notes/how_far/enthalpy/enthalpy_diagrams.htmAnissimov, T.A, 2007 Chemical bonding, Simon Frasier University, Accessed 21/08/09, http//www.chem1.com/acad/webtext/chembond/Whel, L.W, 2006, Calorimeters, Sta nford University, Accessed 21/08/09, http//www2.slac.stanford.edu/vvc/detectors/calorimeters.htmlAcknowledgmentsThe procedure of this experiment is a adaption of a previous class experiment. The source of the procedure is unknown, so thanks to Miss Crook for the inspirations for this design.