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Rate of Reaction Between Marble Chips and the Varying Concentrations of Hydrochloric Acid

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Rate of Reaction Between Marble Chips and the Varying Concentrations of Hydrochloric Acid Planning Before starting the experiment I had to work out how much marble chips would be needed and how much HCl would be needed. I decided that 20 grams of marble chips would be needed and I measured this on a pan balance. The chips would have to be of medium size as from a previous experiment done in class I realize that changing the surface area of the marble chips would change the rate of reaction. I then used 100 cm3 of HCl and this would be the only variable that I will change. I decided to use the concentrations of 0.5M, 1.0M, 1.5M and 2.0M (1mole/dm). To make these different concentrations I added different proportions of distilled water to the 2 molar HCl. For the 2M solution I left the HCl alone, for the 1.5M solution I put 75 cm3 of HCl and 25 cm3 of distilled water. ...read more.


The results we achieved was as follows: Volume of Sodium Thiosulphate Volume of Water Concentration of Sodium Thiosulphate Time in seconds 1000 Time 50 0 0.15 22.70 44.05 40 10 0.12 29.26 34.18 30 20 0.09 40.58 24.64 20 30 0.06 66.25 15.09 10 40 0.03 139.45 7.17 I think that the results of the marble chips and HCl experiment will show the same results as this Sodium Thiosulphate experiment. As the higher the concentration the increased amount of ions per cm3 and therefore more frequent collisions between them, which then makes the experiment react faster. Another reason I think that the rate of reaction will increase is that the experiment is exothermic, this means that it will give itself more energy and therefore more collisions and faster collisions. Also in the 2.0M solution compared with the 0.5M solution there are much more HCl particles in the same volume so the are going to collide with each other more often. ...read more.


65.23 74.82 72.72 70.92 14.23 Analyzing Evidence and Drawing Conclusions From looking at my results and graph I am able to conclude that the more concentrated the acid the quicker the reaction happened and the faster the gas was produced. This is as I predicted and I think they match quite well as the rate of reaction graph is basically a straight line and the average time graph has an increasing gradient. Evaluating Evidence Overall this was a very successful experiment and everything went very smoothly, and that was why my results were very good, and I am able to make the conclusion that the higher the concentration the faster the rate of reaction. From looking at my results I can see that there were no poor results, which was a good thing, and it proves that everything went very well. There was no real source of error in the equipment. The only possibility was if the temperature of the acid had changed from when we did the first reading to the finish. ...read more.

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