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Rates of Reaction

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Rates of Reaction Introduction For this investigation I will be carrying out experiments to see what kind of factors affect rate of reactions. Reactions happen inside and outside our body every single second. Reactions also occur all over the world in natural and man-made products. I will be investigating rate of reactions and what factors affect these. Aim My investigation is to investigate the rate of reaction when magnesium is put into Hydrochloric acid. I shall be keeping and changing different variables and make it as fair as possible. The main factor that I shall be investigating is how the concentration of the hydrochloric acid changes the rate of reaction to the magnesium. Prediction I predict that the higher the concentration of the acid, the faster the rate of reaction will be. I predict this because I believe that the higher the concentration of the acid, the greater the number of acid molecules (hydrogen ions) present in that volume. This means that there are more acid molecules colliding with the particles on the surface of the reactant (magnesium) thus increasing the rate of reaction. When the reaction between hydrochloric acid and magnesium occur, the hydrochloric acid will dissolve the magnesium and produce hydrogen gas. ...read more.


54 40 60 0.8 112 130 121 30 70 0.6 196 223 209.5 20 80 0.4 556 613 584.5 * Time taken for the magnesium to dissolve in seconds Analysis On the graph it shows a nice clean curve that passes through most points. Some though are just slightly off but I don't think any are so off that it could be called an anomalous result. The curve sweeps across the page very rapidly and then begins to straighten off. In the first part of the graph (0-60 seconds), it shows a rapid drop. At the beginning, it is almost vertical (15-30secsonds) but as you go along it begins to turn more and more to the right. This again backs up my prediction. Where it is near vertical, this is the part where the acid is most concentrated. This shows that the more concentrated the acid is the faster the magnesium will dissolve. Round about 30-60 seconds though, it begins to get more horizontal and starts the flat out. I think this happened because as the concentration went down, the rate of reaction slowed down as well. Even though it is still eroding the magnesium away, it is taking a longer time than when it is most concentrated. ...read more.


When mixing the water and acid, whichever you poured in last could have stayed at the top more and the solution might not have properly mixed. When the magnesium was put in it either floated or sunk, or sunk half way through the experiment or even floated back up. This sometimes happened and the times were completely off from what it was. The magnesium sometimes and often did float and fizz to the side of the beaker. I thought that if it were stuck at the side the acid could no have got to it more freely than if it was in the middle which could have changed the results as well. For every concentration of acid solution used we kept the same beaker over and over again. We just poured the used solution out with some acid/water left clinging to the glass. We then poured the new solution in and the both could have mixed. Even though this might not affect it so mush it could have altered the entire percentage ration of acid/water. If I were to do this experiment over again I would probably eliminate some of the notes above, this would make the test a lot fairer. I would definitely repeat it at least 3 times or even more to make the results more reliable. I don't think I would change much else as most of the other factors I was happy with. ?? ?? ?? ?? ...read more.

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