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

Factors Affecting Rates of Chemical Reactions Prepared By: Kelly Gunter For: Ms. Brohman Course: SCH-4U Introduction The main purpose of this lab was to investigate how temperature, concentration, the addition of catalysts, and the substitution of a more reactive reactant, can affect the reaction.
The collision theory explains that in order for a reaction to occur, reacting particles must collide with one another. An effective collision makes reactants result in a reaction and for to be successful two things must happen, the correct orientation of reactants, and the sufficient collision 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 begin to form the bonds on the products. In part 1 the heat of the collision = the increase of effective collisions resulting in the product, and that the increase of temperature = sufficient energy; or the Ea increases. Part 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 Part 1 | |Hot water Bath |Ice water bath |Room temperature | |Temperature of Solution |77°C |11°C |22°C | |Time for sulphur to appear |6 seconds |140 seconds |79 seconds | Part 2 [HCl] Acid Solution |Time (s) for Magnesium Ribbon 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 purple colour to disappear. 9.

It was 30 drops 10. It took 1 drop for the purple colour to disappear, but the colour lingered longer than it did in step 8. Discussion In part 1, it’s 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 concentration 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 acid 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 bit more than it did in step 3.

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