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Investigate the reaction between Magnesium (Mg) and Hydrochloric Acid (HCl)

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Introduction

Mario Creatura Rates of Reaction: Investigate the reaction between Magnesium (Mg) and Hydrochloric Acid (HCl) Planning Prediction I predict that as the concentration of the hydrochloric acid increases, the average rate of the reaction will decrease until it will be almost un-noticeable when the concentration reaches 0.0. I have made this prediction due to the informative work that I have executed previously to this experiment; involving rates of reaction of different solutions and substances. Through doing similar experiments and theory work I have discovered that the Collision theory plays a major part in understanding what elements affect the speed (rate) of the reaction. The Collision theory describes perfectly reaction rates. The theory states that the rate of a reaction depends on how often and how hard the reacting particles collide with each other. This therefore means that depending on the amount of collisions and the force that is put behind them depends on the speed of the reaction. There are several ways of increasing the rate of collisions (temperature etc.), the one that I am planning to use is by decreasing the concentration of the hydrochloric acid and water (Hydrogen Oxide) solution. If the solution is more concentrated it means that there are more particles of hydrochloric acid between the water molecules, which makes collisions between the particles on the magnesium more likely due to the increase of reactant's (hydrochloric acid) particles. Method Equipment to be used Hydrochloric Acid (HCl) 1.0 cm strips of Magnesium (Mg) ...read more.

Middle

Volume of H2O (cm3) Concentration (m) 1 Time (s) 2 Average 25 0 2.0 25.81 24.00 24.905 20 5 1.6 44.22 32.28 38.30 15 10 1.2 74.28 71.03 72.655 12.5 12.5 1.0 130.53 142.38 136.455 10 15 0.8 149.50 162.56 156.03 5 20 0.4 1140.25 1095.32 1117.785 0 25 0.0 - - - I now plan to interpret this information into two graphs, Concentration vs. Average Time and Concentration vs. Average Rate. To do this I will have to find out what the rate of the reaction is. I will do this by using another equation, this time it is: - Average Rate = 1 Average Time (s) By using this equation I will have to alter the table of results by adding two more columns (rounded to 4d.p): - Average Rate (1/t) Average Rate (1/t)-3 0.0406 40.1526 0.0261 26.1097 0.0138 13.7637 0.0073 07.3284 0.0064 06.4090 0.0001 00.8946 The test has been made fair by using the method stated in the Plan. I have used the same length of magnesium for every result and I have also used the amount of acid and water as accurately as possible. The graphs clearly show that as the concentration of the acid in the solution increased, the average rate decreased. This shows that my prediction was correct, I stated that as the 'concentration of the hydrochloric acid increases, the average rate of the reaction will decrease until it will be almost unnoticeable when the concentration reaches 0.0.' The first graph (concentration vs. ...read more.

Conclusion

From the evidence that I have gathered by doing this experiment I believe that I can draw up a valid conclusion. I have discovered that the Collision theory plays a major part in understanding what elements affect the speed (rate) of the reaction. The Collision theory describes perfectly reaction rates. The theory states that the rate of a reaction depends on how often and how hard the reacting particles collide with each other. This therefore means that depending on the amount of collisions and the force that is put behind them depends on the speed of the reaction. There are several ways of increasing the rate of collisions (temperature etc.); the one that I planned to use was to decrease the concentration of the hydrochloric acid and water (Hydrogen Oxide) solution. If the solution was more concentrated it means that there are more particles of hydrochloric acid between the water molecules, which makes collisions between the particles on the magnesium more likely due to the increase of reactant's (hydrochloric acid) particles. Using this theory I have proven that my experiment has worked and that my prediction was accurate. I feel that if I had gathered some more results from the experiment then I would have got a wider and more accurate set of results. But even with these extra sets of results I am sure that the graphs would not have changed their trends or shapes to a great extent. On the whole I feel that the experiment went well, with accurate readings and correct results, giving me good results for an accurate and clear conclusion. ...read more.

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