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Testing the Rate of the Reaction between Na2S2O4 and HCl.

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Introduction

2. October. 2002 Testing the Rate of the Reaction between Na2S2O4 and HCl Introduction This experiment is test the theory that the higher the concentration of a substance the faster the rate of its reaction with another substance. In this experiment the two substances being used are sodium thiosulphate and hydrochloric acid. The equation for this reaction is: Preliminary My preliminary experiment helped me get a grasp of the overall experiment. In the preliminary I changed the concentration of the hydrochloric acid instead of the concentration of the sodium thiosulphate. The measurements I used were fifty cm cubed of sodium thiosulphate, which remained constant throughout the experiment, and then, starting at ten cm cubed of hydrochloric acid changed the volume of the hydrochloric acid. The apparatus I used was the same as list in the planning section. The experiment was done at room temperature and pressure. Here is a table of my results: Experiment Na2S2O4 HCl H2O Time Reaction rate 1 50 cm cubed 10 cm cubed 0 cm cubed 16.83 s 0.059 2 50 cm cubed 7.5 cm cubed 2.5 cm cubed 23.74 s 0.042 3 50 cm cubed 5 cm cubed 5 cm cubed 27.41 s 0.036 As you can see, the results show a ...read more.

Middle

Having looked at this theory I predict that the lower the concentration of the sodium thiosulphate solution will affect the rate of reaction. I also predict that lower the concentration the longer the change in time taken. Apparatus= * Three burettes and burette stands, * One conical flask, * Three beakers, * A thermometer, * Paper with a cross on it, * A large supply of sodium thiosulphate, * Hydrochloric acid and distilled water. The table I collect my evidence in will look like this: Number HCl Na2So4 H2O Time taken 1 10 cm cubed 50 cm cubed 0 cm cubed 2 10 cm cubed 45 cm cubed 5 cm cubed 3 10 cm cubed 40 cm cubed 10 cm cubed 4 10 cm cubed 35 cm cubed 15 cm cubed 5 10 cm cubed 30 cm cubed 20 cm cubed 6 10 cm cubed 25 cm cubed 25 cm cubed 7 10 cm cubed 20 cm cubed 30 cm cubed 8 10 cm cubed 15 cm cubed 35 cm cubed 9 10 cm cubed 10 cm cubed 40 cm cubed 10 10 cm cubed 5 cm cubed 45 cm cubed The Collision Theory The collision theory is an idea that explains the rates of the reaction. ...read more.

Conclusion

However, my results do show one anomaly. This is in the first result I took. This is most likely due to incorrect measuring, a human error. Analyzing My evidence shows very clearly that the rate of reaction is positively affected by the concentration of the substances. My graphs clearly show that the rate of reaction is affected by the concentration of the substances involved in the reaction. On the graph there is a clear curve, excluding one result, an anomaly, which I account for due to human error in measuring. This shows that the lower the concentration the loner it takes, and the lower the concentration goes the longer amount of time it takes (shown by the presence of the a curve on the graph). On the graphs you can clearly my inaccuracies particularly at the beginning resulting in the graphs not appears as symmetrical as they should. Evaluating In this experiment there is large evidence to support the statement that my results aren't accurate due to either human failure or the speed of the equipment available. If better, faster equipment had been available for the experiment my results would be more reliable. Improvements could include using a computer to time and say when the solution has gone cloudy, leaving less room for human error. ...read more.

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