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# Investigating how Temperature affects Rate of Reaction

Extracts from this document...

Introduction

SC1 Investigation Plan In this investigation I am going to see how temperature affects the rate of reaction. To do this I will change the temperature at which a reaction between Sodium Thiosulphate and Hydrochloric acid is conducted. Here is a chemical equation for this reaction: Hydrochloric acid +Sodium Thiosulphate� Sodium chloride + sulphur dioxide + sulphur + water. 2HCl(aq) + Na2S2O3(aq) � 2NaCl(aq) + SO2(g) + S(s) + H2O(l). The precipitate of sulphur is what causes the solution to go cloudy. I will mix the reactants in a flask and then place the flask on a piece of paper with a black X drawn on it. I will time how long it takes for the X to disappear totally. This is how I will measure the rate of the reaction. I plan to take twelve readings, using twelve different temperatures. The range I will use will between 10 and 50 degrees. This is because under 10� and the reaction takes too long and over 50� the reaction is too quick and so reaction time plays a major part in the result and the percentage error will be greater. To carry out the investigation my dependant variable will be the temperature of the reactants as this is the one I will change. ...read more.

Middle

Also I should not go lower then 10�C because if the rule applied then the time would be approximately be 140�C, which is almost too long. This is because if the experiment takes less than ten seconds, reaction time makes a difference to the result, and if I am out in my reactions by 1 second, then that is a 10% error, which is far to large to draw an accurate conclusion. Also if the experiment takes longer than 150s then it is hard to tell when X has fully disappeared and a few seconds out can also create a large percentage error. Obtaining Here are the results I obtained: Starting temperature (�C) Finishing temperature (�C) Time taken for X to disappear (seconds) Rate of reaction (s-�)(to 2 significant figures) 12 13 104 0.0096 15 15 85 0.011 17 17 70 0.014 21 21 55 0.018 24 24 51 0.020 27 27 46 0.022 31 30 41 0.024 33 33 28 0.036 35 35 33 0.031 41 41 15 0.067 45 45 12 0.083 49 50 11 0.091 I did not make any changes to my plan while doing the experiment. I collected an even number of results from all areas of the range I was working in. ...read more.

Conclusion

Again this was probably due to an error in the experiment. I think that my final conclusion was an accurate one, even though it did not fit exactly with my prediction. I think this because I conducted the experiment carefully, and nearly all my results fitted neatly onto the trend line on the graph. Also the pattern that is shown makes sense using scientific theory. If I were to carry out this experiment again, I would probably do more readings for the values of temperature. I could also try higher temperatures of solution and just really try to make sure reaction time was good enough. I would also try to improve the accuracy of the procedure by more thoroughly washing the apparatus after each experiment as some chemicals may have been left in the flasks and may have affected the results. If I were to do further experiments to see if the 10�C rule applied, I would probably use different concentrations and see if the 10� rule applied with that. To do this I would use a different concentration for the two reactants used, and use a similar range of temperatures to ascertain whether or not the theory applies. I would predict from my results that the outcome will be no different with a larger concentration or a smaller concentration. 1 ...read more.

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