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Factors affecting the rate of a reaction

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Factors affecting the rate of a reaction by Jason Phelan AIM: My aim is to study the rate of the concentration of a chemical called Sodium Thiosulphate (Na25203) and investigate which certain factors/variables I may change and which factors I do not change during my experiment. In my investigation I will plan my experiment explaining how to obtain your results using a method that I will provide, and I will also mention what chemicals and apparatus I will use for the experiment. PREDICTION I predict that when I add 5cm3 of hydrochloric acid each time to my solution, and change the amount of Na25203 (Sodium Thiosulphate), remembering to balance my solution with water (keeping the solution a 55cm3), then you will find that when you double the amount of Na25203, then the rate of how fast the reaction takes place will also double. This is because the Sodium Thiosulphate and the rate of the reaction are both proportional to each other, meaning that they both go up in steady intervals. I know this will happen because in my science lesson I found out that when you increase Sodium Thiosulphate, (thus meaning there is more particles in the solution), the Hydrochloric acid particles collide more often with the Thiosulphate particles meaning the reaction (the rate) ...read more.


Here are the 3 series of my results. 1. Amount of Na25203 Amount of H20 Amount of 2HCL Time taken for X to disappear (Seconds) Rate 100 time 10cm3 40cm3 5cm3 251 0.39 15cm3 35cm3 5cm3 127 0.78 20cm3 30cm3 5cm3 80 1.25 25cm3 25cm3 5cm3 73 1.36 30cm3 20cm3 5cm3 54 1.85 35cm3 40cm3 15cm3 10cm3 5cm3 5cm3 42 35 2.38 2.85 2. Amount of Na25203 Amount of H20 Amount of 2HCL Time taken for X to disappear (Seconds) Rate 100 time 10cm3 40cm3 5cm3 260 0.38 15cm3 35cm3 5cm3 135 0.74 20cm3 30cm3 5cm3 80 1.25 25cm3 25cm3 5cm3 66 1.51 30cm3 20cm3 5cm3 51 1.96 35cm3 40cm3 15cm3 10cm3 5cm3 5cm3 42 34 2.38 2.94 3. Amount of Na25203 Amount of H20 Amount of 2HCL Time taken for X to disappear (Seconds) Rate 100 time 10cm3 40cm3 5cm3 193 0.51 15cm3 35cm3 5cm3 114 0.87 20cm3 30cm3 5cm3 83 1.10 25cm3 25cm3 5cm3 68 1.47 30cm3 20cm3 5cm3 56 1.78 35cm3 40cm3 15cm3 10cm3 5cm3 5cm3 45 35 2.22 2.87 Here is a table to show the mean time and the mean rate. ...read more.


They are basically to watch the X underneath the conical flask until you are sure it has gone, using the same person for checking the X to disappear would help because people's eyesight can differ and it would help for more accurate results. Washing the apparatus after each test would also help because remains of chemicals used previously could still be lingering somewhere on a test tube, etc. when you are measuring amounts of certain chemicals, you should use a measuring cylinder to get accurate measurements. Instead of using a measuring cylinder, you could weigh the chemicals on electronic scales because you can get much more detailed measurements. In the future if you wanted or needed to carry out this experiment again, you could perhaps change the amount of hydrochloric acid and keep the sodium thiosulphate the same through out remembering to dilute the solution with water. If you still wanted to prove that when adding more of one chemical, the particles collide more often and cause a faster reaction, you could use different chemicals instead. I couldn't recommend any but it could prove the theory to a greater extent. "Factors which effect the rate of a reaction", by Jason Phelan ...read more.

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