Investigate the rate of reaction between Calcium Carbonate and Hydrochl

Investigate the rate of response between Calcium blowate and Hydrochloric point at different concentrations captureTo Investigate the rate of fight downion between Calcium Carbonate andHydrochloric Acid at different concentrations.Background KnowledgeI know from my experience of science, that by adding together acarbonate and an acid, that a salt, water and Carbon Dioxide are pay backd. Therefore in order to measure the rate of reaction, mavin ofthese products needs to be measured, and the rate at which it isproduced can be apply to define the rate of the reaction. The methodsthat can be used are each to measure the mass of the solution atintervals. Or to measure the produce of feature (Carbon Dioxide).PredictionUsing the known formula vinegarish + carbonate SALT + CARBON DIOXIDE + WATERI can predict the reaction of my experiment to beHYDROCHLORIC + CALCIUM CALCIUM + WATER + CARBONACID CARBONATE CHLORIDE DIOXIDEThe Chemical Formula is listed below2HCl + CaCO3 CaCl2 + H2 0 + CO2I venture that as the molarity of the acid goes up, the amount of gasproduced will also go up.I have based this on my knowledge that atomic number 20 carbonate does nonreact in water. Therefore in solutions with atomic acid and morewater, the atomic number 20 carbonate will not react as much as it would inpure acid for example. To enlighten each of the different strengths of theacid, water is added to a solution of 2M hydrochloric acid. Thereforein the 0.2 value, on that point will be a lot of water, and so it is notexpected that much gas will be produced.My predicted graph shows what I expect. On the x-axis, as the molarityincreases, the gas produced on the y-axis does likewise. However at that placewill be a point reached where the maximum limit of gas has beenprod... ...a clear trend that as the molarity of theacid increases, the volume of carbon dioxide will also do the same.There is an even trend going away up, with a straight line to fit as theline of outstri p fit.The reason for this pattern is the same as that that was made in theprediction. As the concentration of the acid increases, there are moreHCl molecules and so there is more chance of the calcium carbonatemolecules colliding with these and so reacting to form calciumchloride. With the reaction occurring more often, the products willform in a greater quantity and so more carbon dioxide is produced.This reflects the rate of the reaction on the graph and proves myprediction and its theory correct.EvaluationAs the experiment was calculator generated, it simulated how theexperiment would have been conducted. It accounted for human errors inall aspects of the expriment.