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We are studying the rate of reaction between Hydrochloric acid and Sodium Thiosulphate. We are going to change the concentration of the Hydrochloric acid.

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Introduction

Science Coursework Preliminary Experiment Aim We are studying the rate of reaction between Hydrochloric acid and Sodium Thiosulphate. We are going to change the concentration of the Hydrochloric acid. Theory The Collision theory is when particles store up enough activation energy, they collide and react with each other Hydrochloric Acid + Sodium Thiosulphate --> Sulphur + Sulphur Dioxide + Sodium Chloride + Water 2HCl + Na2S2O3 --> S + SO2 + 2NaCl + H2O The factors that could affect the rate of reaction are: * Temperature * Concentration * Catalysts * Surface area Temperature affects the reaction by changing the speed of the reaction depending on the temperature of the Thiosulphate. If it is hot, then the reaction is quicker than if it was cold. Concentration affects the reaction depending on how concentrated the reaction is. If it is highly concentrated, the reaction is quicker than if it was not highly concentrated. Catalysts speed up reactions if they are compatible and surface area affects differently in different situations. ...read more.

Middle

Actual Experiment Aim We are studying the rate of reaction between Hydrochloric acid and Sodium Thiosulphate. We are going to change the concentration of the Hydrochloric acid. Theory The Collision theory is when particles store up enough activation energy, they collide and react with each other Hydrochloric Acid + Sodium Thiosulphate --> Sulphur + Sulphur Dioxide + Sodium Chloride + Water 2HCl + Na2S2O3 --> S + SO2 + 2NaCl + H2O The factors that could affect the rate of reaction are: * Temperature * Concentration * Catalysts * Surface area Temperature affects the reaction by changing the speed of the reaction depending on the temperature of the Thiosulphate. If it is hot, then the reaction is quicker than if it was cold. Concentration affects the reaction depending on how concentrated the reaction is. If it is highly concentrated, the reaction is quicker than if it was not highly concentrated. Catalysts speed up reactions if they are compatible and surface area affects differently in different situations. If it is large it reacts quickly and if smaller it reacts slower. ...read more.

Conclusion

2M 50cm3 0cm3 24.38 2M 40cm3 10cm3 37.38 2M 30cm3 20cm3 48.53 2M 20cm3 30cm3 1.06.94 2M 10cm3 40cm3 2.29.97 EXPERIMENT 3 HCL Na2S2O3 Water Time (s) 2M 50cm3 0cm3 23.77 2M 40cm3 10cm3 29.07 2M 30cm3 20cm3 42.59 2M 20cm3 30cm3 1.07.26 2M 10cm3 40cm3 2.35.54 AVERAGES HCL Na2S2O3 Water Time (s) 2M 50cm3 0cm3 24.32 2M 40cm3 10cm3 33.26 2M 30cm3 20cm3 44.77 2M 20cm3 30cm3 1.07.29 2M 10cm3 40cm3 2.34.83 (GRAPH OF ANALYSIS ON SEPARATE SHEET) Conclusion We have found out that the higher the concentration, the slower the acid takes to react with the Thiosulphate solution. Meaning that the less diluted the Thiosulphate is, the faster reaction time will be produced when mixed with the Acid. Analysis If I were to do this experiment again, Instead of using a cross, I would use a light sensor to give a more accurate reading. This is because the cross method depends on one person's sight and analysis of weither the cross is gone or not. Light sensors will change their value until it stops, when the reaction is over. The reaction may still be going on, even when the person tells the timer that the reaction is finished. ...read more.

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