Experiment: Testing Rates of Reactions

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[pic 1]

[pic 2]

The results shows that:

The first state of calcium carbonate slowly reacted causing the balloon to grow very slowly.

The second state of calcium carbonate quickly reacted causing the balloon to grow quickly.

The third state of calcium carbonate quickly reacted causing the balloon to grow quickly but then the balloon slowly deflated.

The Heated calcium carbonate (concentration 1 and 2) was quicker than the non-heated calcium carbonate.

The first concentration was the base of all testing and it mainly showed how each state of calcium carbonate reacted.

The second concentration increased the rate of reaction for all the states of calcium carbonate.

Discussion:

The calcium carbonate dissolved into the acid causing a chemical reaction and producing gas e.g. HCl (aq) + CaCO3(s) = CaCl2 (aq) + CO2 (g) + H2O (l). The element that was measured was the CO2.

Each state reacted differently due to its size and volume. For example the larger rock had a larger surface area causing it to react slower and produce less gas which fuelled the balloon slower.

The smaller rock had a quicker burst due to its surface area causing it to react quickly but not too fast that the rock dissolved completely. The reaction was so fast that it made the balloon size increase the largest but due to this the balloon deflated because there was no more gas left to fill up the balloon.

The powder dissolved as soon as it was exposed to the acid due to its small size, this caused the gas to escape quickly which had the quickest burst of them all and had some of the higher recordings but due to it dissolving very quickly the balloon started to deflate quicker.

The states showed the larger the calcium carbonate surface area the longer the rate of reaction.

The first concentration was the basic testing for the 3 states of calcium carbonate. The concentration was 1 mole and had the simplest reaction and was used to have a basic level of results.

The first heated concentration caused the 3 states to react faster. This was because the particles vibrated faster causing the reaction to take place a lot quicker than the first reaction.

The second concentration was 2 mol compared to 1 mol (which was the amount of mol placed in the first concentration) increased the concentration which made the calcium carbonate react quicker and caused the 3 states to have a higher rate of reaction compared to the first concentration (both normal and heated).

The second heated concentration made the calcium carbonate react the fastest which showed that the heated concentration and increased concentration caused the calcium carbonate to react the fastest.

Conclusion:

The hypothesis was proven to be correct and showed that the increase in temperature and concentration caused the reaction to occur faster proving that heat and concentration affect rate of reaction. The experiment also shows that the large the surface area the longer the rate of reaction is. Each variable was followed correctly so the experiment wasn’t tampered with which could of affected the results drastically and each experiment was followed correctly and without error.