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Investigating the effect of temperature on the rate of reaction between hydrochloric acid and calcium carbonate.

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Introduction

Investigating the effect of temperature on the rate of reaction between hydrochloric acid and calcium carbonate. Hydrochloric Acid + Calcium Carbonate --> Calcium Chloride + Carbon Dioxide + Water 2HCl + CaCO3 --> CaCl3 + CO2 + H2O Aim. To find out how the temperature of acid effects the rate of the reaction between Hydrochloric Acid and Calcium Carbonate. I will do this by changing the temperature of the Hydrochoric acid and keeping the Calcuim Carbonate the same. Theory. By starting at a low temperature, the particles do not collide with much energy giving a slow reaction. As you increase the temperature, the particles should collide with more energy giving a faster reaction. The concentration of the acid, the time given inbetween each measurement, the surface area of marble chips, the number of marble chips, the volume of acid and the catalyst all affect the rate of reaction. The higher the concentration of acid, the more chance the particles have of colliding. The longer the time between each measurement, the longer time the particles have to collide. The bigger the surface area of marble chips, the more calcium carbonate exposed to collisions. The more marble chips, the more calcium carbonate the acid has to react with. ...read more.

Middle

Results. 10� Time (seconds) Experiment 1 (cm cubed) Average (cm cubed) 10 20 20 20 30 30 30 40 40 40 50 50 50 55 55 60 60 60 70 65 65 80 75 75 90 80 80 30� Time (seconds) Experiment 1 (cm cubed) Experiment 2 (cm cubed) Average (cm cubed) 10 30 20 25 20 40 40 40 30 50 52 51 40 62 63 63 50 70 68 69 60 75 72 74 70 80 75 78 80 80 80 80 90 82 90 86 40� Time (seconds) Experiment 1 (cm cubed) Experiment 2 (cm cubed) Average (cm cubed) 10 30 30 30 20 40 40 40 30 50 55 52 40 60 60 60 50 70 70 70 60 80 80 80 70 85 80 83 80 85 83 84 90 85 83 84 50� Time (seconds) Experiment 1 (cm cubed) Experiment 2 (cm cubed) Average (cm cubed) 10 30 20 30 20 40 40 40 30 45 45 45 40 50 45 40 50 60 50 60 60 70 60 70 70 75 72 75 80 80 75 80 90 85 75 85 70� Time (seconds) Experiment 1 (cm cubed) Experiment 2 (cm cubed) Experiment 3 (cm cubed) Average (cm cubed) 10 50 40 45 48 20 60 50 60 60 30 65 55 65 65 40 70 58 69 70 50 ...read more.

Conclusion

- The readings of volume of water off the large measuring cylinder were not accurate because it is difficult to take an accurate reading at exactly every 10 seconds. Also there are not many measurements on the side of the measuring cylinder. To overcome this problem I could use a friction free syringe. This would be easier to read off and could be brought to eye level. My results do not completely support my prediction. The graph looks a lot different to how it would with the correct results and how my prediction explains. I could do extra work to try to get more accurate results such as: - - Investigating more temperatures (5�, 15�, 20�, 60�, 80�, 85� and 90�) as well as the original temperatures. I would do the experiments by making a water bath of the correct temperature and place the acid in it. I would set up the original apparatus the same but this time once the acid had reached the correct temperature I would leave it in the water bath and do the reaction while the acid was still in the water bath. I could also repeat my experiments 4 times instead of twice therefore being able to spot anomalous easier and making sure my experiment was fair each time I did it. By Emma Cromarty. ...read more.

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