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Rates of Reaction Practial

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Introduction

Rates of Reaction Practical Aim: The aim of this investigation is to investigate how the rate of reaction of Calcium Carbonate (CaCO3) with Hydrochloric acid (HCl) could be affected by surface area. Equation: HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H2O(l) Hypothesis: I predict that the more the surface area the faster the rate of reaction because it increases the chances of collision. This is because more calcium carbonate is exposed to the acid molecules so they are more likely to collide. When measured in the same mass the smaller chips have a larger surface area altogether. Here is a diagram to show this: (if cut into 8 equal pieces) ==> Apparatus: - Two beakers (400ml) - Large Calcium Carbonate Chips (5g) - Small Calcium Carbonate Chips (5g) - Calcium Carbonate Powder (5g) - Hydrochloric Acid 1M (100ml) - Spatula - Accurate Scale - Stopwatch Method: 1. ...read more.

Middle

0.011g 0.073g 0.291g 90 0.025g 0.087g 0.298g Results Graph: Conclusion: From observing my results I have found out that powder has the quickest rate of reaction, then comes small marble chips and lastly large marble chips have the slowest rate. This is because when the size of particles is reduced it increases the surface area available for collisions to occur. When the chip is larger the acid particles can only collide with the edge of the chip. If the chip is cut into several smaller pieces, the acid particles (in the second diagram) can now reach the centre part of the original larger chip. This is why the powder had the quickest rate of reaction. In conclusion my prediction was right. I predicted that the smaller the chips the faster the rate. Evaluation: When I started the experiment my original plan was to react zinc with hydrochloric acid. ...read more.

Conclusion

This means that I could only compare and assume that the powder had more surface area than the large calcium carbonate chips. I then figured out a way to solve this problem, which is to purchase calcium carbonate chips cut into cube form in different sizes. This way I would be able to measure and calculate the surface area of each size of calcium carbonate cube therefore I would actually know the surface area. This way not only would I have more surface areas to confirm the trend, my results would be much more accurate and clear. If I could do this experiment again I would repeat my method but record every 30 seconds instead so that the change is more visible, and record until 3 minutes so that the calcium carbonate would dissolve more thoroughly. I would also repeat it several times to make sure my results are accurate and reliable and that my prediction was right and experiment on more surface areas to confirm the trend. ?? ?? ?? ?? ...read more.

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Here's what a teacher thought of this essay

3 star(s)

The report is fairly straight forward. The experiment is of limited complexity and requires a limited degree of precision. The data collected is of a reasonable quality. However the lack of repeats limits the reliability. There are improvements suggested throughout.

Marked by teacher Cornelia Bruce 18/04/2013

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