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Investigation into the rates of reaction of magnesium with hydrochloric acid.

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Investigation into the rates of reaction of magnesium with hydrochloric acid Aim: To discover how the rate of reaction of magnesium with hydrochloric acid varies when the concentration of the hydrochloric acid is changed. Prediction: After doing previous experiments, I have decided that an investigation to see if concentration changes the rate of reaction will be the best to work with. I could have investigated other factors that affect the rate of reaction such as: Surface area, pressure, surface area, temperature of acid and light. Working in a classroom environment, the concentration will be easiest to test, as it doesn't require lots of sophisticated equipment and will give me sufficient results to be able to plot a graph. I predict that the highest concentration of acid will react the quickest. I think this because according to the collision theory, if the concentration is higher, the chance of collisions is more likely. E.g. ...read more.


* Set up 6 test tubes containing the following acids (15ml) in a test tube rack: 1, 1.5, 2, 2.5, 3, 3.5 and 4 molar. * Add magnesium ribbon to each concentration of acid and start the stopwatch * When the reaction stops, stop the stopwatch * Record results in a table Diagram: Results: Concentration (molar) 1st Attempt (seconds) 2nd Attempt (seconds) 3rd Attempt (seconds) Average (seconds) 1.5 32 32 29 31 2.0 12 16 24 17 2.5 20 10 13 14 3.0 7 11 8 8 3.5 5 26 7 12 4.0 9 5 9 7 Conclusion: From the results table and the line of best-fit graph, you can see that the results did match my prediction in the form of a curved graph line. However, there were two anomalous results in the form of the 3.0 and 3.5 concentrations. After a repetition of these two (below) I deduced that something must have been wrong with the original test Concentration (molar) 1st Attempt (seconds) 2nd Attempt (seconds) 3rd Attempt (seconds) Average (seconds) ...read more.


Another factor that I could investigate in future, is the fact that when the reaction takes place, carbon dioxide is given off, there for the mass will get lighter. If I used a mass balance and put on it a flask of HCL and CaCO3, the flask would get lighter. Furthermore, if I were to connect the mass balance to a computer, I could record the changes and program the computer to produce a graph automatically. The problem with doing the experiment in classroom environment is that there are many ways in which the experiment can be tampered with so that it is not accurate. Ideally all experiments would be done in a controlled laboratory using computers that can be programmed to do the same things exactly the same over and over again. Also computers can measure time into fractions of a second. Taking all of this into account I cannot say that my conclusion can be scientifically proved. The conditions were not the same each time and, although I tried hard, experiments in a classroom can never be repeated exactly the same each time. GCSE Chemistry/ Mg + HCL Joe Smith ...read more.

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