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Magnesium and Hydrochloric Acid Investigation

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Chemistry Coursework Planning Aim In this experiment, I am trying to find out if changing a factor involved in reacting magnesium with hydrochloric acid. Prediction There are several factors that could effect this experiment, these are: Temperature Surface area Size Concentration Amount of solution These could all affect the result of the experiment in different ways. All the above could speed up or slow down the rate of reaction or change the total amount of gas produced. This is because there will be more or less particles in the reaction or the energy in the particles would be changed, for example, if the temperature were increased, the reaction would occur faster because the particles would be moving faster and have a higher chance of colliding with something. I am only going to investigate the effect of concentration on the rate of reaction. The concentration should affect the speed at which the reaction takes place. The higher the concentration of acid the faster the reaction should occur. This happens because the higher concentration means there are more acid particles in the solution and therefore there is a greater chance that one will collide with the magnesium ribbon and react with it. I think that if I double the concentration of the acid the speed of the reaction should also double. [image002.gif] This is what I think the graph will look like. ...read more.


I will do a trial experiment of concentration 2.0 and 1.0 to make sure there is a difference in results. This is the table I will use: Results Table Experiment No. Water (cm�) Acid at 2.0m (cm�) Concentration (m) Time 10 20 30 40 50 60 70 80 1 0 20 2.0 0 20 2.0 0 20 2.0 2 5 15 1.5 5 15 1.5 5 15 1.5 3 10 10 1.0 10 10 1.0 10 10 1.0 4 15 5 0.5 15 5 0.5 15 5 0.5 5 20 0 0.0 20 0 0.0 20 0 0.0 Obtaining I only made a one change to my plan. This was to use 4 cm of magnesium ribbon instead of 5 cm because it was easier to coil up and put in the conical flask. The experiment was carried out safely and fairly. The results were accurate as they were checked by a second person, as they were taken. This is the table of results: Results Table Experiment No. Water (cm�) Acid at 2.0m (cm�) Concentration (m) Time 10 20 30 40 50 60 70 80 Average Amount of gas produced Average for experiment Average rate of reaction 1 0 20 2.0 40.00 47.00 48.50 48.50 48.50 48.50 48.50 48.50 47.25 0 20 2.0 45.00 47.50 47.50 49.50 49.50 50.00 50.00 50.00 48.625 0.10 0 20 2.0 40.00 50.00 50.00 50.00 50.00 50.00 50.00 50.00 48.75 45.46 2 5 15 1.5 19.00 36.00 44.00 ...read more.


The 2.0m and 0.5m lines have a lot less prominent curves and areas where the reaction has stopped. The 1.0m graph shows a relatively steep curve and only a short point at which the reaction stopped where as the 1.5m graph contains a larger level section and less of a curve. Evaluating There are no noticeable readings that do not fit the patterns in the graphs that I have drawn. I think the reading for the experiments where sufficient but I think I could have done the readings at 5-second intervals instead of 10 seconds. This would have allowed the 2.0m graph to contain more of a curve. I think the results that I have taken are accurate and reflect the experiment. I think the experiment was a fair test however there my have been slight variances in the water temperature and pH that I was unable to control, the acid my have also had a slight temperature variance. This could be over come by using distilled water kept in the fridge/heater with the water. I did three repeat readings of each experiment and I think doing any more would not change the results. If I had more time I would have been able to measure the full length of time for the 0.5m experiment to see how long it really takes and if a curved graph is formed. I would have also done a few experiments in-between the ones I did to find out if there is a less radical drop between 1.0m and 0.5m. ...read more.

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