Chemistry Concentration effects rate of reaction Essay

I chose to spend hydrochloric pane at 100% for the principal(prenominal) experiment. Main Experiment For the of import experiment I chose to change the soaking up of the sodium Thiosulphate. I bequeath be testing the immersions 100%, 90%, 80%, 70%, 60%, 50%, 40%, 30%, 20% and 10% and recording the results. I will then plot 2 graphs, a term graph, and a rate of answer graph. Results HCL (cm) Na2S2O3 (cm) Water (cm) premiere Experiment (s) Final Experiment (s) Increase in Time.On the adjacent page I have drawn a graph to scan the time taken for the response. By looking at my graph I can enamor that some points be slightly off of the logical argument of best fit. To start out sure that my line of best fit wasnt wrong, I decided to plot a chemical reaction graph. To plot the reaction graph I had to work out 1/time for apiece result and then plot it on a graph. Instead of the time on the y axis of the graph, I had to do a case for my 1/time and so the numbers were non too belittled I had to time the 1/time by 100, so on the axis I had to label it, 1/time x 10. The reaction graph is on the next page.By looking at the reaction graph I could see that the results for the sodium thiosulphate at 70%, 50%, 30% and 20% were quite away from the line of best fit. I retested these and worked out the 1/time for them, I then plotted them in blue on the reaction graph and found they fitted much better. These are the retest results HCL (cm) Na2S2O3 (cm) Water (cm) Time Taken (Seconds) 5 35 15 60 5 25 25 80 5 15 35 167 5 10 40 251 Some results were significantly different. The original results whitethorn have not been as accurate as thither may have been contamination, imprecise measurements or different excitement making the render seem to disappear quicker.Analysis By looking at my results I can see that my prediction was patch up The more concentrated the Sodium Thiosulphate, the faster it will react. This is because there are more molecules of Sodium Thiosulphate, so they are more plausibly to collide making the reaction faster. When the assiduity is lower, the reaction takes limit slower. The following diagram, used in my prediction, seems to be correct. In the low concentration, 50% concentration on the Sodium Thiosulphate, you can see that although there are the same amount of molecules, there is water which the Hydrochloric acid will overly bump into.This means that the Hydrochloric acid is less likely to bump the Sodium Thiosulphate molecules and thus, make the reaction slower. I have also found out that the higher the temperature, the faster the reaction takes place, this proves my theory correct in which the higher the temperature, the faster the reaction. However, this does not prove that the particles are mournful faster as I would need an electron microscope to see if this was correct. However, when the concentration of the Sodium Thiosulphate and Hydrochloric acid is changed it also has an effect on the reaction rate.This is because there are more molecules of the Sodium Thiosulphate and Hydrochloric acid and thus, they bump into each opposite more often. Evaluation Overall this reaction was successful, but I destine it could have been made more fair. I carried out the experiments over several(prenominal) days, and this may have made it unfair as the temperature and weather was different. I could have had more accuracy by carrying out the experiments in a temperature controlled environment. I also looking at that the reaction was unfair due to inaccurate measurement, all measurements relied on the in the raw eye and may have not been the measurement we wanted, but appeared to be.I think that a way to make them fairer would be to use scales and weigh the chemicals, or use a pipette. both of these methods are more accurate, but are much slower. In the main experiment I found some odd results, but retested them and they fitted in. The original results may have not been as accurate as there may have been contamination, inaccurate measurements or different lighting making the image seem to disappear quicker. I also feel that the reaction is an unfair one to test as it relies on the naked eye to tell when the image has been obscured completely.This can be difficult as different lighting levels can make it easier to see and sometimes the merciful brain may fool you into thinking the image is still there. I could change my method to make it more fair I could use lasers instead of the eye to see when the image has gone. I would place lasers on each side of the beaker, when the laser beam path gets fully obscured by the build up of sulphur, the beams would get cut and the computer will accurately record when this has happened.