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Investigating the Effect of Heat on the Rate of Reaction Between Sodium Thiosulphate Solution and Hydrochloric Acid.

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Investigating the Effect of Heat on the Rate of Reaction Between Sodium Thiosulphate Solution and Hydrochloric Acid. Planning In this experiment I shall investigate the effect of temperature on the rate of reaction. I shall do this by placing the Sodium Thiosulphate solution and the Hydrochloric acid together inside test tubes kept at different temperatures and measuring their rates of reaction. The equation of this reaction is: Sodium + Hydrochloric � Sodium + Sulphur + Sulphur + Water Thiosulphate Acid Chloride Dioxide Na2S2O2(aq) + 2HCl(aq) � NaCl(aq) + S(s) + SO2 + H2O The Formula for rate of reaction is: Rate of Reaction = Amount of Sulphur Produced Time The colourless solutions will react to become cloudy over a period of time and will eventually become opaque due to sulphur being produced. In this reaction the rate of reaction will be measured by timing how long it takes for the solution to become opaque. As the amount of sulphur put into the reaction at the beginning is constant, the amount of sulphur that has been produced at the stage of the reaction when the solutions become opaque will also remain constant. Rate of reaction is proportional to As the amount of sulphur put into the reaction is always the same, it acts as the constant of proportionality therefore we can take as ...read more.


In all reactions there is an energy barrier, which needs to be broken in order for the reaction to occur; this is known as the activation energy. Normally only a small percentage of collisions result in a reaction but if temperature is increased then more of the particles will have enough energy to break the activation energy barrier therefore more of the collisions between particles will be successful so the rate of reaction will increase. Obtaining How I Obtained My Results I obtained my results by putting Sodium Thiosulphate solution and Hydrochloric Acid together in a conical flask and then heating the water bath around the reaction vessel to certain temperatures and measuring how long it took for the solution to become opaque using a stop clock. 1st Set of Results Temperature Time Taken for Solution to Become Opaque (Seconds) 30�C 44.87 40�C 51.33 50�C 40.39 60�C 37.40 70�C 28.86 80�C 29.07 Repeat Set of Results Temperature Time Taken for Solution to Become Opaque (Seconds) 30�C 54.24 40�C 43.62 50�C 39.99 60�C 34.13 70�C 35.04 80�C 27.76 Observations When conducting the experiment I noticed that at a higher temperature the solutions became colourless more quickly. I also noticed that the solutions seemed to become cloudy very rapidly at the start of the reaction yet as the reaction progressed they become more cloudy at ...read more.


This would reduce errors and could even eliminate any anomalous results. My results could have been made more reliable by taking another repeat set of results. Unfortunately, due to constraints regarding time, I was unable to do this so my results may not be as reliable as they should be. I could also have made my results more accurate by using more appropriate ways of measuring the substances for example I could have used a burette instead of a measuring cylinder. If I did the experiment again I could narrow the range of my readings by taking readings every 5�C instead of every 10�C. This would enable me to draw a more accurate graph. I could also try to investigate the effects of reactants with larger surface areas or more concentrated solutions. If I was correct in this investigation then these variables should affect the rate of reaction. If magnesium chips were placed in acid, the chips with larger surface areas should react more quickly as more of the particles are able to collide with other particles, causing the rate of reaction to be faster. Higher concentrations of the reactants in solution should also cause an increase in the rate of reaction because there would be more of the particles of the reactant available for colliding; therefore more successful collisions should occur in any period of time. GCSE Chemistry Coursework Gemma Hillidge ...read more.

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