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# An Experiment to investigate whether the concentration of HCl affects the rate of reaction with CaCO3

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Introduction

An Experiment to investigate whether the concentration of HCl affects the rate of reaction with CaCO3 PLANNING Aim: My aim for this experiment is to find out if the concentration affects the rate of reaction between CaCO3 & HCl. Prediction: I predict that the high molarity concentration solution will have a much faster rate of reaction than the weaker solution. I have predicted this from my knowledge of a previous experiment and scientific knowledge. Recently I did a similar experiment involving a sodium thiosolphate cross instead of the calcium carbonate, from this I found that the higher concentration solutions, faster the reaction, therefore I believe the same results may occur. The speed of the reaction was proportional to the concentration of the reactant, which I predict, will also happen in our experiment. I think that this happened because the more HCl in the solution the greater the concentration and there will be more particles colliding and more energy and therefore a faster rate of reaction. The reason I think that the rate of reaction will increase is that the experiment is exothermic, this means that it will give itself more energy and therefore more collisions and faster collisions. Also in the 2.0M solution compared with the 0.5M solution there are much more HCl particles in the same volume so the are going to collide with each other more often. ...read more.

Middle

Concentration Concentration is a very important factor in rates of reaction. The concentration of a solution can greatly effect a reaction this is because there will be more particles of the reactant to react with, which will increase the time taken for the reaction. If the concentration of an acid is increased, the rate of reaction will increase because the collision rate would be higher and the amount of CO2 would be given out more quickly. Below is an example graph as you can see that the high concentration will react: Temperature The higher the temperature the more energy each particle will have which means it will vibrate more, causing the amount of collisions to increase. As the particles collide more than usual at a high temperature then it will have a high chance of reacting, this will increase the rate of reaction. Below is a graph of how temperature and the rate of the reaction are related: Activation Energy Activation Energy is an amount of Energy needed for a reaction to occur, this amount varies from different elements and type of reaction. This may save energy for industrial use, as they will only supply the amount of energy needed exactly and not more. The Collision Theory From the kinetic theory of gases, the collision theory of bimolecular reactions in a gas phase was developed. ...read more.

Conclusion

In addition, I will use a clock to measure the rate of reaction from as soon as the reactants are put together. The measurements will all be taken to 2d.p. to ensure they are all fair. Risk Assessment I will wear safety glasses to protect my eyes from any accidents that may occur. Lab coats will be worn to ensure clothes stay free from unwanted stains. I will also have to check the apparatus for any broken pieces, that way; I can avoid injury to myself or avoid a mistake in my experiment through a leak. The most important thing is safety. Also, with the stronger molarity solutions, they may be corrosive, so I must take care not to spill any onto bare skin. Fair Test We must make sure that we use the same size and roughly the same mass of chips, this is because we want to keep the chips roughly the same all the way through the experiment so that it will be a fair test and the results we be in relation to each other, otherwise the results will be completely different to what we will expect and it will ruin the experiment. We must also take our readings at the same intervals throughout the experiment i.e. I will take a reading every thirty seconds for all of my experiments. Empty Results Table Distilled Water Time taken (seconds) Volume of CO2 collected in beaker(cm3) 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0 ...read more.

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