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Investigate the effect of concentration on the rate of reaction.

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Chemistry Coursework I have been given the task for my coursework to investigate the effect of concentration on the rate of reaction. Equipment * 10g marble chips (calcium carbonate) * Measuring cylinder * Conical flask * Delivery tube * Goggles * Bowl * Stop watch * Hydrochloric acid * Water Method I will have 10g of marble chips in a conical flask and then put in 50ml of hydrochloric acid first and I will observe the reaction. With a stopwatch I will record every 20 seconds up to 3 minutes, I will measure the volume of gas given off by reading of the measuring cylinder. The second experiment I will do the same but this time I will have 45ml of acid and 5ml of water each time marble chips will remain 10g): Hydrochloric Acid (ml) Water (ml) 1st Experiment 50 0 2nd Experiment 45 5 3rd Experiment 40 10 3rd Experiment 35 15 4th Experiment 30 20 6th Experiment 25 25 The rates of the chemical reactions can be speeded up by: * Temperature -if temperature increases the particles to move quicker therefore collide into each other * Concentration (pressure) ...read more.


I think that the higher the concentration the more energy the marble chips get, the more they collide with each other to increase the reaction, the rate of it simply depends on how hard and often the reacting particles collide with each other. If the acid is diluted with water it would make it weaker and also slower to react with the chips of calcium carbonate and because there are less particles of the reactant between the water molecules, which would have enabled it to make collisions and therefore react quicker. Whereas if the solution has a stronger concentration with less water or none at all it would react at a faster rate, this is because there will be more of the particles reacting and colliding at a more faster rate than a solution with a weaker concentration and large surface area. The Equation. Calcium + Hydrochloric Calcium + Water + Carbon Dioxide. Carbonate Acid Chloride The Chemical Equation CaCo (s) + 2HCl (aq) Ca Cl (aq) + H O +Co (g). ...read more.


On my graph, the lines do not fit exactly. I presented my graph by putting in a best fit. In doing this I could see if any points were anywhere near to the line or far off the line. Evaluation Throughout this investigation I was quite happy because to be honest I knew very well what I was supposed to do (not that I never do) and I carried out the investigation quite well apart from a couple of anomalies. My results are quite reliable and I was able to draw a graph and make conclusions from them (fastest reaction). Only one experiment didn't fit in the pattern, which I have circled on the graph. I would do the experiment again to avoid the error I did in this investigation. The error that I made was to speed the reaction up at times I shook the conical flask around which I shouldn't really have done because it changed the result. In future I will not shake the conical flask and I will use a magnetic stirrer to keep the same the velocity of speed. I would definitely do this experiment again because the results I have obtained ...read more.

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