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# The Effect of Temperature on Rate of Reaction.

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Introduction

The Effect of Temperature on Rate of Reaction The outcome variable for this experiment is to conclude what changes are made to the temperature, when Hydrochloric Acid is reacted with Sodium Thiosulphate. Diagram: Sulphur + Sulphur dioxide + Water 2Hcl + Na S O S + SO + H O + 2Na u 2 2 4 2 2 (aq) (aq) (s) (g) (l) For this experiment the apparatus I will use is as follows: * Thermometer to measure the temperature of the solutions (0-100�c) * Acid to complete the solution (5cm3) * Conical Flask to hold the solutions * Measuring Cylinders for each solution to be put in: - Acid (0-10cm) - Water (0-50cm) - Thio (0-100cm) * Water is used to dilute the solutions * Stopwatch to time the rate of reaction * Bunsen Burner to heat the mixture and carry out the experiment * Pipette to allow accurate measurements of solutions In my preliminary experiment, I am going to measure and observe the effect that temperature has on the rate of a reaction. First of all I am going to put in 50cm3 of Thio into a conical flask, then heat it up using the Bunsen burner. Then I will add 5cm3 of Hydrochloric Acid into the solution and measure the amount of time it takes to go cloudy. I will repeat this experiment numerous times changing the amount of Thio in groups of 10cm to see if there is a large change in the time the solution takes to react. ...read more.

Middle

We did this to see if the level of concentration had any effect on the rate of reaction, and the solution reacted reasonably faster. The third time round the reaction took place a lot faster, so we decided to use this one as our repeat. But we would be measuring the temperature this time also. I predict the higher the concentration of acid; the faster the reaction will take place. This may also mean that a higher temperature is reached. I am going to use The Collision Theory as evidence to back up my decision. The more energy the particles have to collide the more likely they are to react, and the higher the temperature is the harder the particles will collide. This causes more chance of a successful collision, just like Activation Energy! The Activation Energy graph below is an example of an exothermic reaction, where heat is lost. If it was endothermic the graph would look opposite to what it does now. Activation Energy: Reactants Products I think that the graph I produce will have a smooth curve like this: I say this because I assume the higher the temperature is, the faster the reaction will take place. Temp Time Here are the results that I came up with when I repeated the experiment: Temperature: Acid: Thio: Water: Time Taken: 35�c 5cm3 40 cm3 10 cm3 18 secs 40�c 5 cm3 40 cm3 10 cm3 12 secs 45�c 5 cm3 40 cm3 10 cm3 3 secs 49�c 5 ...read more.

Conclusion

This was down to the timer being set late meaning we missed out on a few seconds while the reactions had already started happening. It could have also been down to the different room temperatures each time the experiment was done and the heat of the flasks and Bunsen burner from the previous experiment. I know that my evidence is sufficient to support my conclusion, as the line of best of fit on my graph was a smooth curve and quite close to each point. This shows my results are accurate and reliable. I didn't really have any difficulties whilst doing the experiment, but at first I didn't really understand why we had to keep on repeating the experiments. But, then I started to understand and realise it was so we could get an accurate line of best fit on our graphs and to test the solutions at different temperatures to compare them. If I were to repeat this experiment I would: * Maybe do it in hot and cold conditions to see what the results would be like, so maybe getting rid of the Bunsen Burner would help me to do this. * Do my graph on the computer using MS Excel, to give me more accurate results * Possibly repeating the experiment more than twice to get a bigger variety of results so I could compare the differences between them. * I could have controlled the temperature of the solution by insulating the test tube, so all solutions would remain at the same temperature. (i.e. like a flask or vacuum) Roschelle Alexander-Greenaway 11R Physical Science Ms. Gregory ...read more.

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