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Stuart Patterson

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Stuart Patterson. Chemistry Coursework. Mr. Mitchell Page 1 Investigation to show the rate of reaction between Sodium Thiosulphate and Hydrochloric Acid. In this experiment, I will be investigating, the rate in which Sodium Thiosulphate reacts with Hydrochloric Acid when added together at different concentrations. In order for the Sodium Thiosulphate to react with the Hydrochloric Acid, * Collide with each other * The collision must have enough energy to react. For particles to react, they need to have more energy than the activation energy barrier (Ea). The rate of reaction is determined by the amount of particles above the Ea barrier, therefore the more that have enough energy to react, the quicker the reaction. In my investigation, I could increase the temperature of the solutions. This would increase the speed of the particles and the amount of energy they have, so there would be more collisions and more would have an increased energy than the activation energy barrier, so more will react and the quicker the reaction would occur. I could increase the concentration of sodium thiosulphate, to increase the amount of particles, and consequently the amount of collisions would rise and more particles would have more energy than the activation energy barrier, making the reaction would be quicker. If I was to add a catalyst, it would increase the rate of reaction. This would occur, because the catalyst would lower the Ea barrier. ...read more.


When the concentration of the sulphuric acid doubles so does the rate of the reaction, as shown on the graph. As the concentration doubles, (0.5M to 1M), the rate of the reaction doubles (0.01sec-1 to 0.02 sec-1 ), and I predict the similar results from this investigation. Page 2 The Method. List of equipment; 1 beaker 1 pepet 1 pair of safety goggles 1 stop clock 1 square piece of card with a distinct X marked on. The technique to use for my investigation is as follows: 1. Firstly put your safety goggles on! Add Sodium Thiosulphate to Hydrochloric Acid, regarding to the dilutions table on PAGE 1, in turn. I.e. Do one row of dilutions at a time. Start the clock once the solution is created in the beaker. 2. Place the 'X' card underneath the beaker. (So you can see it.) 3. Start the clock once the solution is created into the beaker. 4. Monitor the solution from above. Be wary of toxic gases which are released from the investigation. 5. When you cannot see the X through the base of the beaker, the reaction is complete. Stop the clock and note down the time to two decimal places, on a table the same as the results table attached. 6. Empty the solution into the sink, rinse the beaker and instruments you have used thoroughly, ready to use again. ...read more.


I predicted this, and when the concentration doubles so does the rate due to twice as many particles with more energy than the activation energy barrier, which I also predicted. Results. A line of best has been added to my graph. I noticed that there is a pattern to the average results I gained. The line of best fit on the graph, goes up in a regular curve. There are no anomalous results. My hypothesis is accurate to the results I gained. I predicted that the more Sodium Thiosulphate there was in the solution, the speedier the reaction would be. Evaluation. I think, the way I carried out this investigation was extremely fair and accurate. The variables were maintained to a high standard. My evidence should be valid for this investigation. I believe the results I have gained from this experiment, where found accurately and fairly. The results, could have been more accurate, if I repeated the experiment a further two times. My results are reliable enough to place them onto a graph with a line of best fit, which enabled me to come to the conclusion that if you double the concentration of the solution, the rate of the reaction is also doubled. The method used to conduct this experiment, was effective. There were no anomalous results, which is what I expected, but did not predict. I found keeping the output variables constant difficult because I had to keep checking the amount of solution used was correct to the units necessary. ...read more.

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