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Factors affecting the rate of reaction between Sodium Thiosulphate and Hydrochloric acid.

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Introduction

Factors affecting the rate of reaction between Sodium Thiosulphate and Hydrochloric acid. Aim: In this experiment I aim to measure the affect of concentration on the rate of reaction between Sodium Thiosulphate and Hydrochloric acid. HCl + Sodium ThiosulphateSodium Chloride + Sulphur Dioxide + sulphur + water HCl + Na2S2O3 NaCl + SO2 + S + H2O Prediction: I predict that with increasing concentration, of Hydrochloric acid, the rate of reaction will increase. I think this because increasing the concentration of a substance in solution means that there will be more particles of that substance. When there are more particles in a reaction, the rate of reaction is increased because there are more particles to collide and so the reaction takes place quicker. (In this case the formation of Sulphur which turns the colourless substance cloudy.) I also predict that the rate of reaction and the concentration will be proportional. i.e if you double the concentration then the rate of reaction will increase by half. I think this because if you double the number of particles then the reaction should be twice as quick, and so half the time. ...read more.

Middle

This can be clearly seen in the results table and the graph, which both show that with increasing concentration the time taken for the solution to become opaque decreases. However, according to these results, I was not correct in saying that the concentration and rate of reaction are proportional. If you look at concentrations 2 and 4 in the results table, 10cm� and 20cm�, the time taken for concentration 4 to turn the solution opaque is not half the time taken for concentration 2. If my prediction was correct then it should be half the time. The reason that the rate of reaction increases as the concentration increases is Kinetic theory. Kinetic theory states that as you increase the concentration the number of particles of that substance increases. A chemical reaction can only occur between particles when they collide with a certain amount of force (Activation energy). As there are more particles to collide in a higher concentration the chance of them colliding is increased and so the reaction takes place quicker. In this reaction one of the products is Sulphur. ...read more.

Conclusion

Another possibility is that my eyesight was not that great at times and I may have missed the 'X', when I should have seen it, and stopped the timer. Or if I just didn't check to see the 'X' accurately. I believe that if I were to do this experiment again with more accurate equipment (such as a light meter rather than a cardboard marked with a 'X' or more accurate measuring equipment), or if I spent more time being accurate, then the results would be different. I think that they would all be closer to the line of best fit. I also think that the results would show that the rate of reaction and concentration are proportional like I originally predicted. If I were to do this again then I would like to investigate the rate of formation of Sulphur in a similar way to the rate of reaction of this solution. However, despite the imperfections of this experiment, I believe that my results were clear enough to support at least part of my conclusion, namely the relation between rate of reaction and concentration. It was not good enough though, to prove that the rate of reaction and concentration are proportional as I predicted. Stephen Rooney 10s - 2 - ...read more.

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