Factors Affecting Rates of Chemical Reactions Type 2.Doc Uploaded Successfully

Factors alter Rates of Chemical Reactions Prepared By Kelly Gunter For Ms. Brohman Course SCH-4U Introduction The master(prenominal) purpose of this lab was to investigate how temperature, concentration, the addition of catalysts, and the substitution of a more than reactive reactant, can affect the reaction. The shock theory explains that in coiffure for a reaction to occur, reacting bureauicles moldiness collide with one another. An effective clash makes reactants result in a reaction and for to be successful ii things must happen, the correct orientation of reactants, and the sufficient hit energy.The orientation of reactants explains that reacting particles must collide with the proper orientation relative to one another, for sufficient collision energy, it explains that the reactants must collide with energy that is sufficient to break the bonds in the reactants and to arrest to form the bonds on the products. In part 1 the heat of the collision = the increase of effec tive collisions resulting in the product, and that the increase of temperature = sufficient energy or the Ea increases. cancel 2 the increase of concentration = the rate increase of the reaction.In part 3 the increase of bonds = decrease of reaction rate. Procedure Refer to handout. Observations take time off 1 Hot water Bath Ice water bathe Room temperature Temperature of Solution 77C 11C 22C Time for sulphur to come in 6 seconds 140 seconds 79 seconds Part 2 HCl Acid Solution Time (s) for Magnesium typewriter palm tree to disappear 6. 0 mol/L 33 s 3. 0 mol/L 49 s 1. 0 mol/L 158 s 0. mol/L 1486 s Part 3 8. It took 1 drop for the violet colour to disappear. 9. It was 30 drops 10. It took 1 drop for the colour colour to disappear, but the colour lingered longer than it did in step 8. countersign In part 1, its shown that the higher the temperature was the faster it took for the sulphur to appear in the solution.In Part 2, it shows that the increase of the concentrat ion of the HCl the faster the Magnesium ribbon takes to disappear, and the lower the concentration of the HCl the slower it takes for the Magnesium Ribbon to disappear. In Part 3 the solution for Iron2sulfate it only took one drop for the colour purple to disappear, for the oxalic demigod it took 30 drops for the colour purple to disappear and in the oxalic acid with the manganese sulphate as a catalyst it took only 1 drop for the colour purple to disappear but the colour had lingered for cunt more than it did in step 3.