Relationship Between Surface Area and Rate Of Reaction Essay -- GCSE C

An Experiment To Investigate The Relationship Between excavate Area and Rate Of ReactionIntroductionThe put of answer (reaction velocity) may be defined as the rate ofchange of concentration of a stated reactant or product. The rate of areaction is found by measuring the amount of a reactant used up perunit of eon or the amount of a product produced per unit of sequence. Areaction can be made to go faster or slow by changing a number offactors. In order for a reaction to occur certain things arenecessary particles must shake up with each other and the clashingmust have enough slide fastener for the reaction to occur. If this happens theoriginal bonds are broken and new bonds are organise - so that newproducts are formed. Successful collisions (those with sufficientenergy) can be increased (or decreased) by a number of factors.These key variables consist of temperature, concentration, locatearea and use of and type of a catalyst. To examine the relationship betwixt the rate of reaction and surface area I must adopt to varyonly surface area keeping the other variables constant. bug out area of full-blooded - The surface area has an effect on the rate ofreaction. If the solid has a large surface area per unit push-down stack thenthere are more opportunities for collisions to occur between the solidand liquid. This is because there is more chance for collisions tooccur. If the surface area per unit skunk is small, collision can onlyoccur with the outer atoms and is therefore limited. The plat belowillustrates thisThis relationship is proportional i.e. as one doubles so does theother.The temperature of the reaction - When the temperature is low, theparticles in the reaction do not have frequently energy and move slowly socollision... ...nes whichcan be explained by the fact that the surface area of the chips wasconstantly changing throughout the reaction, as it was reacted withthe acid, and so did the surface area to volume ratio. Also as the stain was used up the reaction would slow, as there would be slightmarble remaining to react with the acid reducing the chances of acollision occurring. The evidence is sufficient to imply that myhypothesis is correct but I think to prove it successfully furtherevidence would be necessary.I could have checked the rates of reactions I produced as a pass ofmy experiment by carrying out a different test. If I had examined myresults by doing a test measuring the mass change of the calciumcarbonate I could have checked that I came up with sufficiently analogous final rates of reaction, however I did not have time for thisor to use a wider range of values.