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Sodium thiosulphate solution Investigation

Extracts from this document...

Introduction

Aim. Sodium thiosulphate solution of concentration 40g/litre is poured into a conical flask. When a small volume of dilute hydrochloric acid is produced the mixture goes cloudy. I wish to find out what alters the rates of reactions in this solution. I am going to find out the reaction rate using temperature. Prediction. If the temperature in the solution is high then the molecules which are in the solution gain energy and move at high speed, therefore the chance of the particles colliding is increased which will make the reaction take place a lot quicker. If the temperature is low the particles have less energy and are less likely to collide. Reasons & Explanations. Chemical reactions take place when the particles of the reactant collide. They first have an activation energy which is very low. I have studied that if the temperature in a reactant is high then the particles will collide more often due to energy increase, and if the temperature is low then the reaction will take place at a much lower rate. The collisions have to have enough energy to break the bonds between particles. After looking at more revised experiments and doing a test of my own as a little insight into what may happen. ...read more.

Middle

I will measure out 10ml of the hydrochloric acid in the 10ml measuring cylinder. I will start the timer at this point whilst adding the hydrochloric acid to the sodium thiosulphate in the conical flask. I will watch over the conical flask with the contents until the 'X' I will make a recording of the time it takes for the reaction to happen. I will repeat the process but place the conical flask containing the sodium thiosulphate in a hot water bath and complete the experiment and redord the reacion time again. I will do the experiment again but instead of using hot water I will use ice to make the temperature drop dramatically and follow the same procedure. Then I will revise all of my experiments and carry them out again to see if I can make an average out of the entire of my experiment for the rate of reaction. Fairness. I will keep this experiment fair by being as accurate as possible in all experiments with the recordings of temperatures and also the measuring of solutions. Also making sure I start the stop watch as soon as I add the hydrochloric acid to the sodium thiosulphate to make even more accurate recordings of time. ...read more.

Conclusion

My prediction was wrong about if the temperature rising by ten Celsius that the time for the reaction to take place would divide by two, although some higher temperature did this. My results show that they are no where near dividing by two at all instead the reaction time has around 10 seconds taken off for the lower temperatures. Evaluation. This investigation could be made more accurate by using time more efficiently, by not rushing the results and taking measurements more slowly to enable more accurate measures of solution etc. All equipment could be rinsed more thoroughly to employ less contamination is the experiment as I think that most of the inaccurate measures and reaction times were caused by. The investigation to me was not fair as I did not keep to all the points I made about keeping free from any contamination, I can only prove if there was any contamination by repeating the entire experiment again and using more time to complete each recording. To enhance my experiment recording I could use more detailed information on reactions to see whether my recordings are close to experiments that are the same as what I am doing. More revision on the experiment could be used to see where other people have gone wrong and how they have corrected the anomilie. Rates Of A Reaction. Sean O'Garra 10x 10K1 ...read more.

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