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An experiment to show the rate of reaction between Magnesium ribbon & Hydrochloric acid.

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Introduction

An experiment to show the rate of reaction between Magnesium ribbon & Hydrochloric acid. Aim: To find out the rate in which magnesium ribbon dissolves in different molars of hydrochloric acid, and which factors affect the rate of reaction. Prediction: The 'Collision Theory' says that particles can only react if they collide with enough energy for the reaction to take place. As well as the collision theory there are also other factors that will effect how quickly and effectively the reactions take place. The four factors that effect the rate of a chemical reaction are: TEMPERATURE, CONCENTRATION OF ACID, SURFACE AREA OF THE REACTANT and USE OF A CATALYST. Temperature The higher the temperature of the solution, the faster the rate of reaction, and vice versa. This is because as the solution heats up the particles gain energy and begin to move faster and with more energy. This causes more successful collisions per minute and consequently a faster rate of reaction. We carried out an experiment in lesson, which involved placing marble pieces in hydrochloric acid. We altered the temperature of the acid and recorded the speed in which the marble dissolved in the different temperatures. ...read more.

Middle

I put on my goggles before collecting the acid and continued to wear the goggles until I had stopped handling the acid at the end of the experiments. * I placed all of the boiling tubes in the rack and stuck labels around them so I could identify each tube accurately, for example 10:0, 9:1, 8:2 etc which represents the ratio of acid to water. * Then, using two separate measuring cylinders, one for acid and one for the water, I measured out accurately the solutions of acid:water. * When I had done this I cut the magnesium ribbon to lengths of 2 cm trying to maintain a high level of accuracy. * Next, I placed a piece of the ribbon inside the boiling tubes one by one, timing how long it took for the ribbon to dissolve and recording my findings for each tube before moving to the next consecutive tube. * I repeated the experiments three times for each tube, replacing the acid after each test to ensure the acid was at its most reactive throughout. * I then used the results to get a list of average times and I plotted a graph of the results. ...read more.

Conclusion

This again may have been inaccurate, as I couldn't check that I used exactly the right amount each time. As I repeated the results it also not certain that I used the same amount for the same tubes in each repeat. Other factors, although I tried to prevent this, could have maybe affected my experiments. If the temperature in the room was higher in one lesson than in the other, the particles in the acid would have had more energy and so caused the reaction to take place faster. If the magnesium ribbon pieces were not exactly the same some would have had a smaller/ larger surface area causing the rate of reaction to be faster/slower which would nave had an effect on my results. Although I did get some anomalous results it is clear that I have proved my prediction to be correct. The results were sufficient to prove my theory, but if I were to do the experiments again I would repeat them more than three times to get a higher level of accuracy. Along with access to more skilled equipment and more repeats, I feel that my results would or could be flawless and highly accurate. Overall my experiments went well and I feel I achieved the results I set out to obtain. 7 1 Rachele Peat 11J1 10/01/2002 Chemistry Cwk 1 ...read more.

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