Investigate the rate of reaction between Calcium Carbonate and Hydrochl

Investigate the rate of reaction between Calcium Carbonate and Hydrochloric Acid at different concentrationsAimTo Investigate the rate of reaction between Calcium Carbonate andHydrochloric Acid at different concentrations.Background KnowledgeI kip down from my knowledge of science, that by adding together acarbonate and an acid, that a salt, water and Carbon Dioxide areproduced. consequently in order to taproom the rate of reaction, single ofthese products needs to be measured, and the rate at which it isproduced can be used to define the rate of the reaction. The methodsthat can be used are either to measure the mass of the solution atintervals. Or to measure the produce of gas (Carbon Dioxide).PredictionUsing the known pee-peeulaACID + carbonATE SALT + CARBON DIOXIDE + WATERI can predict the reaction of my experiment to beHYDROCHLORIC + CALCIUM CALCIUM + WATER + CARBONACID CARBONATE CHLORIDE DIOXIDEThe Chemical code is listed below2HCl + CaCO3 CaCl2 + H20 + CO2I think tha t as the molarity of the acid goes up, the amount of gasproduced give also go up.I have ground this on my knowledge that calcium carbonate does notreact in water. Therefore in solutions with little acid and morewater, the calcium carbonate will not react as much as it would inpure acid for example. To make each of the different strengths of theacid, water is added to a solution of 2M hydrochloric acid. Thereforein the 0.2 value, there 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 therewill be a point reached where the maximum limit of gas has beenprod... ...a devolve trend that as the molarity of theacid increases, the volume of carbon dioxide will also do the same.There is an even trend going up, with a great line to fit as theline of best fit.The reason for this pattern is the same as that that was made in th eprediction. 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 computer generated, it simulated how theexperiment would have been conducted. It accounted for human errors inall aspects of the expriment.