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Factors which affect the rate of reaction between dilute hydrochloric acid and sodium thiopsulphate

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Introduction

KS4 GCSE Science Coursework I am going to investigate the factors, which affect the rate of reaction between dilute hydrochloric acid and sodium thiopsulphate. The factors that could affect the rate of reaction between dilute hydrochloric acid and sodium thiosulphate are: * Temperature * Concentration I am going to investigate concentration of the sodium thiosulphate solution, as temperature is a lot harder to control than concentration. I predict that the more concentrated the sodium thiosulphate is the quicker the reaction, and the more dilute the sodium thiosulphate is the slower the reaction this is based on the collision theory (below). The dilute hydrochloric acid solution will have the same volume (10ml) of dilute hydrochloric acid each time but the water will go up 2.5ml and the sodium thiosulphate solution will go down 2.5ml. The more water that goes into the solution the longer a fine deposit of sulphur (precipitate) takes to form. The formula is below: Na2 S2 O3 + 2HCL = 2NaCL + H2O + S02 +S The rate of reaction in the solution depends on the amount of particles in the solution for instance A concentrated solution (i.e.: more particles of sodium thiosulphate) ...read more.

Middle

and pour both dilute hydrochloric acid and sodium thiosulphate (and water later on) into the beaker at the same time. Start the stopwatch and start stirring. * When the solution has gone cloudy and the cross is no longer visible stop the stopwatch and record the time. * Repeat these steps until a full set of results is finished. To help me with my investigation I carried out a preliminary experiment the results are as follows: Concentration (ml) Time (minutes/sec) Sodium thiosulphate Dilute hydrochloric acid Water 25 10 0 30:04 sec 20 10 5 43:50 sec 15 10 10 57:04 sec 10 10 15 1m:34 sec 5 10 20 4m:21sec From this preliminary experiment I found out that the higher the volume of water is the longer the reaction takes to happen. This is because it is "diluting" the solution. This helped me as knew that the results of my final experiment would also follow this trend. When I do the experiment properly I will use more concentrations and I will repeat each concentration so that I can get an accurate average and plot a graph. ...read more.

Conclusion

As the concentration of the solution decreases the rate of reaction increases. This is because when the solution is more concentrated it has more molecules of the reactants in it and the frequency of successful collisions is greater therefore the rate of reaction is quicker. This is also show in my preliminary experiment. This shows that my prediction using the collision theory: "The more molecules there are the frequency of succesful collisions is greater and therefore the reaction rate is speeded up" Is correct and that it applies to the experiment My results were accurate but I could have repeated them more often to get more accurate averages. There were no great anomalous results (fluctuations) in the line of best fit but at 80% there was a slight change in the line. This could be due to human error as I collected enough results for a definite conclusion. If I had the chance to do the experiment again take more care ion getting the results so that there were not any errors also I could use a Data logger as this would be computerised and would be able to give more accurate answers, as it is better and no "human errors" could be made ...read more.

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