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Look at two variables that affect at the speed of the reactions between Marble Chips (CaCO3) and Hydrochloric Acid (HCl).

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In this piece of coursework I am going to look at two variables that affect at the speed of the reactions between Marble Chips (CaCO3) and Hydrochloric Acid (HCl). I will use four different states of division of the marble chips. These will be: * Large chips * Medium chips * Small chips * Powder I will also vary the concentration of my Hydrochloric acid. * 2.5 Molar * 2.0 Molar * 1.5 Molar * 1.0 Molar * 0.5 Molar In any reaction a solid is needed, our solid is Marble Chips. EQUIPTMENT: * Beakers (250ml) * Measuring cylinder (50cm3) * Bungs * Thermometer (00C-110oC) * Electronic Scales (0.00g) * Weighing boats * Boiling tubes (50cm3) * Marble chips (Small, Medium and Large) * Hydrochloric acid (2.5 - 0.5 Molar) From this reaction, Carbon Dioxide is produced, and it is the collection of this gas that will measure the reaction for us. I predict that, " the more concentrated the acid, the quicker the reaction will be." Also " the larger the chips, the longer the reaction will take." I think this because a reaction occurs when particles collide. This process is based on random particle movement. ...read more.


Because of the fact that the marble chips come with a thin layer of powder on the outside, we have decided to leave the reaction for thirty seconds at the beginning before we start collecting the Carbon Dioxide. After the thirty seconds, we placed a boiling tube (50cm3) on top of the glass tube coming from the conical flask and timed to see how long it takes to fill the tube completely with the Carbon Dioxide. We will also measure the temperature of the room, because it may be carried out on different days so the temperature could have changed. This temperature change could affect our results by many seconds. I believe that my prediction that " the more concentrated the acid, the quicker the reaction will be,'' will be proven correct because stronger acids come with more severe warnings on them, thus must be more corrosive. The more corrosive an acid is the faster it should make this reaction happen. The equation is CaCO3 + 2HCl CaCl2 + H2O + CO2 Firstly we tested the different chip sizes and came up with these results. Time in Second Size of Chips Time 1 Time 2 Average Rate 1/time in seconds S 14 13 13.5 0.74 M 23 22 22.5 0.04 L 26 ...read more.


All my readings were repeated and an average was taken. If there were an anomalous result they were re-tested and changed accordingly. My equipment was kept the same the whole way thought the experiment so the only things that were changing were my variables. This means that my experiment was a fair test thus the results are as reliable as they could be. After doing my experiment and analysing my findings I can now say that there are two clear conclusions The more concentrated an acid is the faster it will react The larger the surface area of a reactant the faster the reaction will be Because of the fact that my experiment met my expectations and the exportations of basic science, I would say that my experiment has nothing that needs changing. I am very happy with the way my experiment went and with my method. However it would have been nice to get all the results done in the one day, because there could have been different factors that could potentially have affected my work, e.g. using different apparatus, the apparatus I am using may have other chemicals left in it, or there could have been a small temperature rise, that was not noticed on the thermometer, these are all small things that could affect my results in a big way. ...read more.

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