Rates of Reaction :: GCSE Chemistry Coursework Investigation

An Experiment to show the reaction mingled with Hydrochloric acid and atomic number 20 CarbonateIntroductionHydrochloric acid + Calcium Carbonate Calcium Chloride + CarbonDioxide + Water2HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H20(l)In this experiment we forget be investigating the variables that thunder mugaffect the speed of reaction between hydrochloric acid and calciumcarbonate. During this experiment carbon dioxide is produced. This iswhat we are going to use to record the speed of reaction, for thefaster the reaction the faster carbon dioxide is produced.Variables=========A variable affects the rate of reaction between a number of chemicals.For a reaction to occur the particles have to collide with sufficientenergy to break the bonds between them. This amount of energy neededis called energizing energy. In a reaction, only the particles withenergies above the Activation Energy will cause a reaction.The different variables that could be used areText buffet Surface Area Wh en a warm reacts with a liquid or gas, the bulge out area of the solid particles makes a difference to the speed of the reaction. From the diagram you can see that the three smaller particles have a larger surface area all together (shown as blue) than the larger particle and so will react faster. There are to a greater extent calcium carbonate particles on the the concentration of the hydrochloric acidText Box surface for the acid to react with. Powders of a Calcium carbonate react even faster as the of calcium carbonate particles showing to react with the acid particles is even greater. Crushing up the solid in an experiment can make a long experiment a lot faster and more violent. The reason that, with a larger surface area a solid reacts faster is that there are more particles showing for the liquid or gas to react with. Temperature===========This is one of the most impressive ways of speeding up the rate of areaction. From disturbing the chemical you are transferring energy intothe particles. When particles do collide, they are more likely toreact, rather than middling bounce off each other, if they are movingfaster. When the particles have more energy they collide more oftenand with more force with the other chemical. With more collisions andwith a larger force it is more likely that the collisions will besuccessful. This means that the rate of reaction will be greater.change in heat can change the rate of the reaction. The first curve onthe graph shows a reaction when the chemicals involved are of a low