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Experiment to study the Effect of a catalyst on the rate of reaction.

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Experiment to study the Effect of a catalyst on the rate of reaction Hypothesis The Collision Theory says that the role of a catalyst is to provide the reaction with an extra, alternative pathway for the reaction to occur; the activation energy for this alternative pathway is less than the activation energy for the reaction without the catalyst. As a result, more of the particles have energy greater than the new activation energy, so when they collide, the particles don't just bounce off each other, but the collision leads to reaction and so the rate of reaction increases. In other words, with the catalyst present, the collisions don't have to be energetic, so more of them will have sufficient energy to lead to reaction. It isn't possible, using simple collision theory to predict quantitatively the exact effect of the catalyst on the rate of reaction, but we can try and predict the effect if changing the total amount of a catalyst used. Because of this, we know that the more catalyst we use, the faster the reaction rate will be, but we need to make a quantitive prediction. ...read more.


Clean the side arm flask with tap water and then distilled water, and push the syringe back to 0cm�. Do this experiment using one spatula, then 3/4s of a spatula, then half a spatula, then a quarter of a spatula and finally 1 and a half spatulas of Manganese (IV) oxide. In each, use a level spatula, not a heaped one. Observations Table to show Volume of oxygen formed in each experiment Time (s) Expt.1-full spatula[vol o2 (cm�)] Expt. 2-3/4 spatula[vol o2 (cm�)] Expt. 3-1/2 spatula[vol o2 (cm�)] Expt. 4 -1/4 spatula[vol o2 (cm�)] Expt. 5-1.5 spatulas[vol o2 (cm�)] 0 0 0 0 0 5 20 10 10 60 10 35 20 15 70 15 45 26 22 80 20 55 33 27 88 25 58 38 30 95 30 60 41 35 97 35 60 45 36 100 40 47 40 100 45 49 42 50 50 45 55 51 46 60 52 47 65 53 48 70 54 50 75 54 51 80 51 From my graphs, with the Time (s) on the x-axis and the Volume of o2 formed (cm�) on the y-axis, I found the rates by dividing volume over time and by drawing a tangent at the beginning, and I displayed them in the table below: Amount of catalyst (spatulas) ...read more.


of o2 because we had to look at the stop clock very quickly as well as the measurements of the gas in the syringe, and write them down quickly before it changed, so the Vol. of o2 is probably inaccurate as well. My results do not give a definite answer to whether my hypothesis is correct or not. It was hard to put the bung in the flask quickly so no oxygen escaped out before it could be measured. It was also very hard to measure the Vol. of o2 produced because you had to look at the stop clock syringe and write down the results very quickly. This also meant that we didn't get very many points as we could only measure the volume every 5 seconds. An improvement would be to not worry about writing results down as they happened, as just mark the amount of oxygen onto the syringe with a board pen. This would also mean that I'd be able to get more results because I'd be able to get them down at smaller intervals, e.g. every 2 seconds instead of every 5. A solution for the bung problem would be to use a delivery tube. To get a more accurate measure of catalyst, I would weigh it. I would also repeat the experiment to get averages. ...read more.

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