Rates of Reaction :: GCSE Chemistry Coursework Investigation

An Experiment to show the reception between Hydrochloric cutting and calcium atomic number 6ateIntroductionHydrochloric acid + atomic number 20 Carbonate Calcium Chloride + CarbonDioxide + Water2HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H20(l)In this audition we will be investigating the variables that do-nothingaffect the speed of reply between hydrochloric acid and calcium trade. During this taste carbon dioxide is produced. This iswhat we ar going to use to record the speed of answer, for the sudden 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 withdraw to collide with sufficient faculty to break the bonds between them. This amount of energy neededis called activating energy. In a reaction, only the particles withenergies above the Activation Energy will cause a reaction.The different variables that could be utilize areText Box Surface A rea When a unscathed reacts with a liquid or gas, the surface area of the hale particles makes a difference to the speed of the reaction. From the diagram you can see that the three small particles have a larger surface area all together (shown as blue) than the larger particle and so will react faster. in that location are more(prenominal) 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 matchless of the most effective ways of speeding up the rate of areaction. From heating the chemical you are transferring energy intothe particles. When particles do collide, they are more likely toreact, rather than just bounce off each other, if they are movingfaster. When the particles have more energy they collide more a good dealand with more tug 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