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Investigation of the rate of reaction with Sodium Thiosulphate and Hydrochloric Acid.

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Introduction

Investigation of the rate of reaction with Sodium Thiosulphate and Hydrochloric Acid Introduction: We must produce a piece of coursework investigating the rates of reaction, and the effect different concentrations have on them. The rate of reaction is the rate of loss of a reactant or the rate of formation of a product during a chemical reaction. It is measured by dividing one by the time taken for the reaction to take place. There are five factors which can affect the rate of a reaction, according to the collision theory of reacting particles. These factors are temperature, concentration (of solution), pressure (in gases), surface area (of solid reactants), and catalysts. We will be investigating only the affect that concentration has on the rate of reaction due to the fact that this is the most practical factor to investigate. Aim: We aim to see the effects of a change in concentration on the rate of a reaction between the two following substances: Sodium Thiosulphate + Hydrochloric Acid Na?S?O? ...read more.

Middle

Fortunately, this did not happen due to cautious organisation. Prediction: I predict that as the concentration of Sodium Thiosulphate increases, the rate of reaction will increase. This means that the graph drawn as part of my results will have positive correlation, and will probably be curved as the increase in rate of reaction will not be exactly the same as the concentration is increased. This can be justified by relating to the collision theory. If solutions of reacting particles are made more concentrated there are more particles per unit volume. Collisions between reacting particles are therefore more likely to occur. Results: The time taken for the reaction to happen was recorded and can be seen on the table below. Conc. of HCl | Run1 | Run 2 | Run3 | Run4 | 1M | 7.5s | 7.15s | 8.1s | 7.3s | 0.5M | 11.5s | 10.5s | 11.4s | 10.6s | 0.25M | 21.5s | 21.1s | 21.3s | 21.3s | 0.01M | 69.5s | 75.2s | 73.5s | 73.7s | 0.025M | 495.2s | 556.7s | 560.4s | 537.9s | 0.001M | * | * | * | * | Conc. ...read more.

Conclusion

The graph shows a positive correlation with a curved line as I predicted and shows that my referral to the collision theory is also correct. This means that, as the concentration of Sodium Thiosulphate increases, the rate of reaction does increase. Fair Test: In order for my findings to be valid, the experiment obviously needed to be a fair one. The reactions were carried out as fairly as we could have made them at that time. To make sure this was the case, we used the same types of beaker for the experiment so that the depth did not vary; we used the same substances in each of the reactions; we did not agitate, heat, or in any other way encourage the rate of reaction to increase; we made sure that the measuring cylinders and beakers for the Hydrochloric Acid and Sodium Thiosulphate were not mixed up - all reactions were done at room temperature. We could have made the results more accurate by doing the experiment more times than we did, though we had already done them 8 times which should be sufficient. Another way of increasing the accuracy of the results would be to use a pipette for maximum accuracy. Ross Saunders Science Coursework ...read more.

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