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Plan on Reaction of Calcium Carbonate and Hydrochloric Acid.

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Introduction

Plan on Reaction of Calcium Carbonate and Hydrochloric Acid The factor I am going to investigate when reacting Calcium Carbonate and Hydrochloric Acid is the surface area. How will the surface area of Calcium Carbonate affect the rate of the reaction? I will do this by having different surface areas of Calcium Carbonate, mix it with hydrochloric acid, and measure the amount of gas produced and compare results. The gas given off is CO2, this is because the high density charge of the cation causes polarisation of the anion (CO32-) this makes it easier for the carbonate ion to decompose into carbon dioxide and O2-. The O2- can readily react with two H+ ions from the hydrochloric acid thus making H2O and CO2. I will do this by collecting the amount of gas from each experiment into a gas syringe. The three experiments will consist of: ground up Calcium Carbonate, chips of Calcium Carbonate and a cube of Calcium Carbonate. I will do the experiment three times to make an average. To make this a fair test I will keep other factors the same, temperature of water and the concentration of the acid the same (2 molar acid). If I change the temperature or concentration of the acid it could affect the rate of the reaction because of the collision theory. ...read more.

Middle

Here is a table for my results I collect: Time/seconds Volume of Gas/ cm3 Marble Cube Marble Chips Ground Up Marble 1 2 3 1 2 3 1 2 3 10 20 30 40 50 60 Hypothesis Using my knowledge of the collision theory I predict that the smaller surface area the rate of reaction will increase. If you increase the surface area there are more chances that the reagents will collide with each causing a reaction. Relating this to my experiment the largest surface area is ground up Calcium Carbonate. This means I predict that this will have the fastest rate of reaction and the marble cube will have the slowest rate of reaction because it has the smallest rate of reaction to its volume. Analysis From my experiment I found out that changing the surface area of the marble pieces does affect the rate of reaction because of the collision theory. It states that if you increase the surface area the rate of reaction will increase also because there is a larger chance that the reagents will collide and react. This proves that my prediction was correct. Each experiment reacted faster. It changes because each time I increased the surface area the rate of reaction increased. It took less time for the reaction to finish. ...read more.

Conclusion

Due to school equipment my results had some anomalies in it, in the marble cube experiment at 100 seconds the result was just above the line of best fit. With more accurate equipment this would be corrected. One problem I had was with the ground up pieces of marble it was too reactive for the experiment, when I tried to time the experiment it was all over within ten seconds. It was a problem because I couldn't take down the gradual increase of gas being produced the experiment was over to quick. I could improve the experiment if I lubricated the gas syringe to reduce even more friction, which would affect the amount of gas being collected and if had a more accurate gas syringe, which gave more detailed measurements. My experiment is reliable if I repeat it again I would get the same results because each experiment I repeated three times and got very similar results each time. If I repeated it I would not use random sized marble chips as they would each have a different surface area preventing my results to be as accurate as they can be. My results prove that surface area does make a difference, but it doesn't prove how much surface area does make a difference because I only used three very different amounts. It does not make accurate enough results to state exactly how much will make a difference to the rate of each test. Matthew Broomfield 121 Stowe School ...read more.

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