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To investigate what affects the rate of reaction between Sodium Thiosulphate and Hydrochloric Acid.

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Sean Robinson Chemistry Investigation Introduction: The aim of this experiment is to investigate what affects the rate of reaction between Sodium Thiosulphate and Hydrochloric Acid. This is the Formula; Sodium Hydrochloric Sodium Sulphur Thiosulphate + Acid = Chloride + Sulphur + Dioxide + Water Planning: My experiment could go wrong in several ways if I didn't have safety in perspective. These include * Wearing safety goggles as chemicals are being heated as they could spit or splash out of the test tubes and go into your eyes and possibly blind you. * Have ties/hair hidden as Bunsen burners are being used and hair could be singed etc. * Have bags under bench as glass, and hot chemicals are being transported around and chemicals could be spilt on someone or glass could break and someone could fall on to it. * Wiping spills up as someone can slip on the chemical and hurt himself or herself or anyone who is near. * The acids are corrosive and so you need to take care when handling and be careful so no acid goes onto your skin. * Breakages must be notified as someone unaware of the breakage may hurt himself or herself on it. * Using tongs when holding hot glass/chemicals as you may burn yourself or drop a container containing acid. ...read more.


I chose this because this has a decent time of reaction at room temperature and when it is heated up it will still be measurable. I think that this wont get too fast or too slow and it will give a good set of results. Obtaining Evidence Results: Temperature (*c) Time(s) Rate (S-1) 20*c 223 4.48 40*c 52 19.23 60*c 20 50.00 80*c 16 62.53 100*c 12 83.33 Back Up Results: These were taken off a computer. When the light shines through the conical flask, which has Sodium Thiosulphate and Hydrochloric Acid inside it. The light that passes through the substance is picked up by the light sensor. We stopped the experiment when the sensor picked up 70% of the light. You can see this on this diagram. You can see the light sensor underneath the conical flask and the lamp above the flask. The light sensor picks up the light coming through the reacting substance. This acts just the same as my original experiment. Backup Results: Temperature (c) Light Intensity Time(s) Rate (S-1) 10 70.0 132 7.58 20 70.0 86 11.63 30 70.0 65 15.38 40 69.8 60 16.67 50 70.0 41 24.39 60 69.8 31 32.26 70 70.0 28 35.71 80 69.8 22 45.45 To work out rate, we took 1000 and divided it by the time leaving me with the rate. ...read more.


Also when there is more water added then the time it takes to react is much slower. My original prediction was that when the temperature increased then the rate of reaction would decrease. I know this because, when the temperature decreased the time it takes for the reaction to take place increased and when the temperature increased the time it takes to react decreased. e.g. Temperature (*c) Time(s) Rate (S-1) 10*c 134 7.46 100*c 12 83.33 My results also prove my scientific explanation as when the temperature increased, the time decreased and the rate increased. This shows that when the temperature increased the time it took for the reaction to take place also decreased. This shows that more reactions took place in a shorter time so my theory of 'temperature increase time decrease' was correct. Evaluating Evidence On my graphs on the backup results there seems to be an anonymous result on both graphs. I took repeat readings in-case I didn't rinse my apparatus as well, and remaining particles were still in the flask I was using, which would have affected my results. I think my experiment went quite well overall. My range of values were very satisfying as I took a number of readings which show the rule of when the temperature is increased then the rate of reaction is also increased. If I did this experiment again I would change the amount of time I took for getting my temperatures more accurate. ...read more.

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