Coursework Rates of reaction Essay Example for Free

Coursework evaluate of reaction EssayInvestigating the effect of ingress on the set out of reaction Skill(s) assessed Topic C10 Experiment 9 (in S4) Investigating the factors affecting the rate of reaction IGCSE Coursework Skills C2, C3, C4 Some of the factors affecting the rate of a reaction that you hire studied are Temperature Concentration Surface area Aim Investigating the effect of changing the concentration on the reaction between calcium carbonate and hydrochloric acid, by collecting the carbon dioxide gas inclined off.CaCO3(s) + 2HCl(aq) CaCl2(aq) + H2O(l) + CO2(g) Hypothesis My hypothesis is that as we increase the concentration of the HCl, the rate of the reaction allow be faster this is because more collisions will be present Materials Small calcium carbonate chips Dilute hydrochloric acid (1 counterspydm-3) Distilled water supply Delivery tube Bowl Conical flask ( nose candyml) Beaker Measuring cylinder (100 cm3) Stop watch equaliser Clamp Clam p holder Safety Glasses. Method 1. Collect all materials 2. Fill the bowl and the 100 cm3 cylinder with water 3. Holding the end so that the water doesnt go out, turn the cylinder spinning top down and place it down the bowl, keeping it still with the clamp, put the delivery tube at the jam of the cylinder 4. Weight 3g of small size calcium carbonate chips 5. Put on your safety specs 6. Add the 3g of small carbonate chips into the conical flask 7. Add the HCl acid in the conical flask 8.Quickly afterwards put a cork so that you shut all air entries in the conical flask 9. At the same quantify as you place the cork, start timing how a great deal it takes to get 50cm3 of gas 10. Repeat this experiment using different concentrations of HCl acid by diluting the acid with distilled water, to take in it a sensible test use always the same amount of chips and always reach 25cm3 in the measuring cylinder so that only concentration and not amount will affect the rate of reaction.1 1. Record your results in a neat and tidy table Results Table Volume of 1. 0 mol dm-3 HCl (cm3) Volume of H2O (cm3) Concentration of HCl (mol dm-3) Time (s) to reach 50ml Time to reach 100ml graph Anomalous Results In this experiment we were lucky to find no anomalous results at all, everything went on as we planned it was going to go like. ConclusionAs you can see in the graph, our hypothesis was right, as we increased the concentration of the HCl acid in out experiment, more collision were happening and therefore the time for it to reach 50ml was becoming smaller and smaller, meaning that the reaction was becoming faster. So we end up with the expiration more concentration of acid = faster rate of reactions = more collision. We could also see in the drift/pattern that at first, when we started increasing by only 0. 2 in concentration, the time for it to reach 50ml lessen from 38 to 17 seconds, almost half of what it was before.After a while, as we increased the concentration, the variation between the two concentrations began to get smaller and smaller, it first started at decreasing from 38s to 17s, then from 17s to 9s, 9s to 7s and from 7 to five-spot seconds. At this last 2 differences, at the change from 0. 6 to 0. 8, and 0. 8 to 1 in mol dm-3 of concentration of HCl, the difference was in both only of 2s, showing off that if the acid was moreover too concentrated, and almost getting to being fully concentrated, the difference in time to reach the 50ml will become smaller and smaller.Evaluation/Improvement The experiment was carried out really well, there was no evidentiary anomalous result which indicated that we were doing the right thing, the experiment fulfilled our hypothesis decision, it went on as we planned it would. We should be in possession of repeated the experiment, repeating the experiment would get to given us much more accurate results, and we have used the same balance for each measuring of calcium carbonate, so that we make it a fair test.