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Investigating rates of reactions. The reaction I am going to be looking at is between magnesium and hydrochloric acid.

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N kbistry Coursework - Rates of reaction Introduction I am going to be investigating rates of reactions. The reaction I am going to be looking at is between magnesium and hydrochloric acid. Key Variables 1. Temperature of solution) 2. Concentration of reactant 3. Surface area of a solid 4. Use of catalyst 5. Light Key variable for investigation Concentration of reactant Factors to be controlled * Temperature - This cannot be completely controlled because it depends on the room temperature at the time * Surface area of magnesium strip - This can be made very accurate by cutting the magnesium strips the same length, but this cannot be 100% accurate. * Volume of reactant - I can also make this very accurate but it would be very difficult to get the volume of each concentration perfectly accurate. Prediction I think that if I half the concentration of the reactant then the reaction will take twice as long. Reason The reason I have made my prediction the way I have is because I have recently done an experiment using calcium carbonate which gives off carbon dioxide. I found that the more concentrated the solution was with hydrochloric acid the faster the reaction was. Another reason for making my prediction is because of the collision theory. ...read more.


I thought the first 5 concentrations worked well and I am going to use these in my real experiment. Obtaining precise results In my real experiment I am going to try obtain precise and reliable results. To make my readings as precise as possible I am going to start the stop watch 10 seconds before I drop the magnesium into the concentrations of hydrochloric acid so that I do not have to worry about starting the stopwatch.. I am also going to be very careful in pouring the right volumes and concentrations I am using. I will also be very precise with measuring the surface area of each strip of magnesium. To make my results even more accurate I will repeat the experiment. Concentrations 7. 50ml of hydrochloric acid. (2mol/l) 8. 40ml of Hydrochloric acid and 10ml of distilled water. (1.6mol/l) 9. 30ml of hydrochloric acid and 20ml of distilled water. (1.2mol/l) 10. 20ml of Hydrochloric acid and 30ml of distilled water. (0.8mol/l) 11. 10ml of Hydrochloric acid and 40ml of distilled water. (0.4mol/l) 12. 50ml of distilled water. (0mol/l) Results Below is a table to show the results of my experiment with concentration 1. (2moler) Time Run 1 Hydrogen given off in cm3 Run 2 Hydrogen given off in cm3 Average Hydrogen given off in cm3 0 - - - 10 40 42 41 ...read more.


I believe this is because I carried out m experiment carefully and made sure I did not make any mistakes which could of lead to and odd results. The only problem that I came across in my experiment was the amount of time I had to do it in. I overcame this by doing some of the experiment in my lunch hour. The only problem that arose in my method was reading the amount of hydrogen being given off from the syringe. This was a weakness to the accuracy of my results. I believe that the strengths in my method were the organisation of my equipment and the measuring of my solutions. My results seem very reliable but there is some ways in which I could of made them more reliable. I could of got somebody else to take the stopwatch and tell me when to read the measurements from the gas syringe. This would have been much more efficient. I could of also done more repeats to make my results more reliable. I think that my results are sufficient to form a firm conclusion because they show clear trends in my tables and in my graphs. I believe I have sufficient evidence to form a firm conclusion but to be sure I should do more repeats. Further work I could do is to try more concentrations of hydrochloric acid. Chemistry coursework - Rates of reactions Jamie Hannath 11JWT ...read more.

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