Rates of Reaction - Magnesium Strips and Hydrochloric Acid.
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Rates of Reaction: Magnesium Strips and Hydrochloric Acid Introduction Rates of reaction occur when two chemicals bond. The chemical bonds can be either very strong or very weak. I expect that when I add magnesium to the hydrochloric acid that depending on the amount of hydrochloric acid that the acid will eventually dissolve the magnesium and consequently produce hydrogen gas. All chemical reactions involve reactants. When these reactants are mixed together they cause a chemical reaction to occur which will make products. The reactants that I will use are hydrochloric acid and magnesium. I predict that the chemical reaction will take place as soon as the magnesium is dropped into the hydrochloric acid. Magnesium chloride and hydrogen gas are the products formed during this reaction. The formula equation for this experiment is: Magnesium + Hydrochloric acid = Magnesium Chloride + Hydrogen Mg + 2HCl = MgCl2 + H2 The reason that the magnesium reacts with hydrochloric acid is because the magnesium is rather a reactive substance as it is high in the reactivity series. When the chemicals react a displacement reaction takes place. The magnesium displaces the hydrogen in the hydrochloric acid forming magnesium chloride and hydrogen gas. Whether the rate of this reaction increases or decreases, depends on these factors: * The surface area of the magnesium ribbon used * The temperature of the Hydrochloric
The volume of hydrochloric acid that I am going to use is 25ml. I am going to measure the rate of the reaction by collecting the hydrogen gas that is produced during the experiment in an upside down measuring cylinder, which is full of water and also placed in a container of water. The gas that is produced will pass through a delivery tube which is stuck into a rubber bung in a conical flask where the initial reaction will begin to take place. I will quickly drop the length of magnesium into the flask and put the delivery tube under the upside down measuring cylinder. I will then start the stop watch, then I will record the volume of gas produced every 20 seconds until I can see that the reaction is no longer continuing. Fair Testing In order to keep my investigation fair I will have to ensure that I keep the following the same: * Length of magnesium * Surface area of the magnesium * Volume of acid used * Starting temperature of the acid I think that it would also be a good idea if I made sure that all the equipment is in use properly. For example the bung is in the flask correctly, as this would affect the results.
This pattern suggests that the reaction rate increase when the concentration of the acid increases because if you increase the concentration of the acid you are introducing more particles into the reaction which will in turn produce a faster reaction because there will be more collisions between the particles which is what increases the reaction rate. The evidence I have been able to gather from this investigation seems to lead to a quite firm conclusion. I might not have been able to find the exact speed of the reactions but the pattern seems to be correct as I have repeated readings four times and seem to have a similar result for each of the repeated readings. I used the variable of concentration, which seemed to be of a good choice as it would show the results of how more acid molecules reacting with magnesium, would result in a faster reaction. Evaluation There will always be ways in which you can improve your investigations and the same thing goes for the investigation which I carried out. The problems that occurred throughout the investigation for me were; * Pouring the exact amount of hydrochloric acid * Time scale in which we was on If I was to repeat this investigation I would try to ensure that I do it as accurately and thoroughly as possible. Chemistry Coursework: Rates of Reactions 1 Lauren Skeldon
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