The reaction between sodium thiosulphate and HCL :: GCSE Chemistry Coursework Investigation

The reaction between sodium thiosulphate and HCL Aim - The aim of this experiment was to find out the rate of a reaction at different temperatures. - We also wanted to find out the rate of the reaction at a different temperature in bigger or smaller surface areas. Prediction - My prediction is, by increasing the temperature a reaction will happen more quickly. The more heat - The Faster reaction and more collision. The lower the temperature - The slower the reaction and less collision. GRAPH My Understanding Reactions occur at different speeds in different temperatures. I’ve learnt that if the temperature is high reactions will take place much more quickly and the particles will collide more often. The table and graphs prove my theory. The Calculator was used for calculating the average of the times that was recorded for the reactions to happen. The Beaker was used to mix the chemicals for the reaction to take place. The Stop watch was used for timing how long it took for the reaction to happen. Method - For this experiment I first set up the apparatus with the apparatus that is shown above. - I then poured 5lm of HCL into a conical flask. - I then measured 10 ml of sodium thiosulphate, - I then I added it to the 5 ml of HCL. - I recorded how long it took for the reaction to take place, which was how long it took for the X to disappear. - With the times that I recorded from the experiment, I calculated an average. - I then repeated the experiment at 3 different temperatures. Factors and Fair Test To make this a fair test I: - Kept the amount and concentration of the chemicals the same. - Varied the temperatures to find out how long it would take for a reaction to happen at different temperatures - Did each experiment at each temperature three times to make the experiment more fair. I also calculated an average, this reduces any anomalous data. Conclusion - My results show that the hotter the reactants the faster the reaction. - This happened because the particles move more quickely and collide more often as stated in the collision theory. - The experiment proved my prediction correct which was based upon the