A reaction between Hydrochloric Acid and Magnesium ribbon.
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Introduction In a reaction between Hydrochloric Acid and Magnesium ribbon, the Hydrochloric Acid will dissolve the Magnesium ribbon and produce Hydrogen gas. All chemical reactions involve reactants which when mixed may cause a chemical reaction which will make products. In case the reactants are hydrochloric acid and magnesium ribbon. The chemical reaction takes place when the magnesium ribbon is dropped into the hydrochloric acid. The products that are formed during this reaction are hydrogen gas and magnesium chloride. The formula equation for this experiment is: Mg + 2HCl MgCl2 + H2 The word Equation for this experiment is: Magnesium + Hydrochloric acid Magnesium Chloride + Hydrogen (s) (aq) (aq) (g) Magnesium will react with hydrochloric acid, because it is higher in the reactivity series that hydrogen. When the two chemicals react a displacement reaction will take place and the magnesium will displace the hydrogen in the hydrochloric acid forming magnesium chloride and hydrogen gas. Depending on certain factors the rate that this reaction will take place will either increase or decrease. The factors that may affect the rate of reaction are as follows: * Temperature of the Hydrochloric Acid * Mass of the magnesium ribbon used * Concentration of the Hydrochloric acid * Surface area of the magnesium ribbon used All of these factors will change the rate of reaction because of the Collision Theory.
I predict that the more concentrated the acid the faster the reaction will take place because the more concentrated the acid is the faster the magnesium will react and more hydrogen gas will be given off in a quicker time. The basis for my prediction is pretty understandable, because as my scientific knowledge shows, in higher concentration of Hydrochloric acid there is more possibility of particles with Activation energy colliding and starting a reaction as compared to Lower concentration of Hydrochloric acid. Apparatus Measuring Cylinder: Conical Flask: Cork and a Bent Tube: Stand: Clamp: Ground Glass Syringe: Hydrochloric acid (Hcl) starting from 0.25, 0.50, 0.75. 1.00 And 1.50: Magnesium (Mg) ribbon, each one 4cm in length: Stop Watch: Fair test We have to make sure that we use the similar size, amount and roughly the same mass of magnesium, this is because we want to keep the ribbon roughly the same all the way through out the experiment so that it will be a fair test and the results will be related to each other, otherwise the results will be completely different to what we expect and it will be, and it will ruin the experiment.
Even though the experiment went very well, we could have still improved the method, by the time we close the lid (cork) we have loss of hydrogen gas, due to a reflex reaction. One Method which would have given us more accurate results is as follows: Conclusion My results table and graph show me that when I increase the concentration of the hydrochloric acid, the initial rate of reaction also increases. Altogether I tested 5 different concentrations of hydrochloric acid. 0.25M, which was the lowest concentration of acid that I used. And increase by 0.25 each time until I reach 1.50M hydrochloric acid, which was the highest concentration that I used, produced the fastest rate of reaction. I repeated all 5 concentrations three times to make sure that they were reliable results and in all cases the higher the concentration the higher the rate of reaction. I have already stated this in my prediction had stated this in my prediction. As we look at the graph we can clearly see that in all five results at the beginning the reaction happened more quickly than at the end where we can see that it started to tail off. The graph clearly shows how reaction rate of reaction increases when the concentration level is increased. ?? ?? ?? ?? Kartik Ganeshan Science Coursework Yr - 11 Rates of Reaction
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