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Investigating the Factors That Affect the Rate of a Chemical Reaction

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Introduction

Investigating the Factors That Affect the Rate of a Chemical Reaction Introductory information In a chemical reaction more than two reactants are put together which makes a new product. For successful reactions to take place particles of different elements or compounds need to collide, and react together. A successful reaction happens when successful collisions take place. For successful collisions, particles must collide with enough energy to give a sufficient amount of force when colliding. From this you can see that in order for a reaction to take place, collisions between reacting particles need to happen. Activation energy represents the minimum energy needed to break bonds with reactants, with this they can react forming a new product's'. Two reactions colliding with enough energy new product The reaction that I will be investigating is the reaction between hydrochloric acid and magnesium ribbon. I will use different concentrations of hydrochloric acid to see the affects, outcomes and the time taken. As the reaction proceeds I will time how long it takes for the magnesium ribbon to fully dissolve, this happens because the magnesium reacts with the hydrochloric acid. Magnesium + hydrochloric Acid ==>?Magnesium Chloride + H2O Mg(s) + 2Hcl(aq) ==>?MgCl + H2(g) I will decide when my reaction has stopped by observing the magnesium ribbon and when it is out of sight and there are no more bubbles I will stop the timer. ...read more.

Middle

I did this by watching when the magnesium ribbon had stopped reacting and disappeared. Although I was just using this method to find out how long a particular concentration took to finish reacting I attached a glass syringe to my conical flask to observe how much hydrogen was being produced, so that I could be prepared when it came to doing my actual experiment. The table below shows the amount of hydrochloric acid and water I used for a certain percent and the time taken for the magnesium ribbon to fully stop reacting. Volume of HCL (ml) Volume of H2O % of concentration Time taken for the mg ribbon to disappear (in seconds) 10 0 100 62 9 1 90 114 8 2 80 192 7 3 70 370 6 4 60 497 5 5 50 640 4 6 40 900+ 3 7 30 1080 2 8 20 1205+ 1 9 10 - From looking at the information from my preliminary I have decided to use the following concentrations for my actual experiment: 20%, 40%, 60%, 80%, 100%. The reason why I have decided to use these percentages of concentrations is because even though it shows a variety it will not be as time consuming as 10% concentration of hydrochloric acid took 1205 seconds which was approximately 20 minutes. ...read more.

Conclusion

36 39 37 160 36 37 39 37 170 38 38 39 38 180 39 38 40 39 190 39 39 40 39 200 39 39 40 39 210 39 40 40 40 40% Time (sec) Volume 1 Volume 2 volume 3 Average 10 5 6 4 5 20 8 7 7 7 30 8 8 9 8 40 9 11 10 10 50 13 11 12 12 60 15 13 14 14 70 17 16 16 16 80 19 18 17 18 90 20 18 19 19 100 22 20 21 21 110 23 22 22 22 120 24 23 23 23 130 25 24 24 24 140 26 25 24 25 150 26 25 25 25 160 27 26 25 26 170 28 27 26 27 180 29 28 27 28 190 30 29 28 28 200 31 29 28 29 210 32 30 29 30 220 32 30 30 30 230 33 31 30 31 240 33 31 31 31 250 34 32 31 32 260 35 32 32 33 270 35 33 32 33 280 35 33 33 33 290 35 33 34 34 300 35 33 34 34 310 35 33 34 34 320 35 33 34 34 To find my average number of hydrogen produced I added the 3 volumes together then divided by 3. The answer most close I decided was my average. ...read more.

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