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Rate of Reaction Between, Hydrochloric Acid and Magnesium

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Introduction

Rate of Reaction Between, Hydrochloric Acid and Magnesium Aim I aim the find out whether the concentration of acid effects the amount of gas given off in a set amount of time between hydrochloric acid magnesium ribbon. Prediction I predict that the higher the concentration, the quicker the gas will be given off. The atomic collision theory describes how the reaction quickens. I looked up the collision theory in a textbook "Science in Action", and found the following information. The collision theory explains how a reaction can only take place when reactive particles meet, under certain conditions. It stands to reason that if you have more reactive acid particles (a higher concentration of particles) in the same place, they are more likely to collide with another particle, and react. However, other aspects also affect the reaction, but are all made more likely if there are more molecules. For the molecules to react they have to have * Enough energy to achieve an activated complex. This energy that they need is activation energy. * The right orientation for the reaction to take place. ] Also, when these reactions take place quickly, the produce a lot of heat, so if the reactions do happen more quickly with the stronger acid, they will be quickened still be the increase in heat. This increase in energy makes the particles vibrate quicker, and therefore collide with other particles, again increasing there chance of reaction. ...read more.

Middle

40 17 19 22 19.33333333 50 19 23 22 21.33333333 60 19 23 22 21.33333333 70 19 23 22 21.33333333 5 7 12 13 10.66666667 10 13 18 19 16.66666667 15 16 19 19 18 2 20 19 19 19 19 25 19 19 19 19 30 19 19 19 19 35 19 19 19 19 2 10 8 7 8.333333333 4 15 15 15 15 6 19 21 21 20.33333333 8 21 21 21 21 2.5 10 21 21 21 21 12 21 21 21 21 14 21 21 21 21 16 21 21 21 21 It is difficult to see any trend using only a table so I have produced a graph that held all the data: As you can see from the graph, the time at which the reaction stopped is more or less the same ml3. This is because I used the same amount of magnesium, and the same amount of acid, so I will get the same amount of hydrogen, no matter how strong the acid is. You can also see from the graph the speed at which the reactions took place. 0.5 moles being the slowest and 2.5 being the quickest. This proves my prediction that the stronger the acid, the quicker the reaction The collision theory explains how a reaction can only take place when reactive particles meet, under certain conditions. It stands to reason that if you have more reactive acid particles (a higher concentration of particles) ...read more.

Conclusion

gas is given off, between hydrochloric acid magnesium ribbon" and because the results are what I expected, and I carried out the experiment with care, also the fact that I repeated the experiment many times, it is reasonable to presume that I can draw a simple conclusion like, "the higher the concentration, the quicker the gas will be given off " If I were to do the experiment again I would change the way I inserted the magnesium into the flask. I think I would have a double chambered flask that would be able to have the wall removed. See diagram. I could combine this idea with the alternative way I could do the experiment, as described in my planning. The method would be to: Place magnesium and the acid in a flask, which is then plugged with cotton wool, to prevent any liquid splashing out, during the reaction. Next, the flask is weighed, then tipped up to let the reactants mix and a clock is started. The mass is noted at regular intervals, until the reaction is complete. I would use the same volumes for all the chemicals in the new experiment, as I see no good reason changing them. I would expect the graph for the result to be much the same, but obviously with different axis labels and values. For example In conclusion, the experiment did prove my prediction that the rate of reaction doubles with when the acid strength doubles. Daniel Hill 10S Rate of Reaction Between.doc Page 1 of 8 ...read more.

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