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effect of concentration on the rate of reaction

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Introduction

In this piece of coursework I am going to investigate the effect of concentration of sulphuric acid on the rate of reaction on magnesium. Magnesium+ Sulphuric Acid � Magnesium+ Hydrogen Mg (s) + H�SO4 � Mg SO4 +H2 Scientific Knowledge The Collision Theory For particles to react they must collide with each other with sufficient energy to cause a successful reaction. In the case of Magnesium and sulphuric acid, the magnesium atom must collide with the hydrogen Ions from the sulphuric acid. The collision must have enough energy for the reaction to be successful. Step 1 The Hydrogen Ions are continually moving around in the solution. In doing this they will to collide with Magnesium. Step 2 If the reaction is enough energy from the collision the reaction will happen. Hydrogen gas and Magnesium Ions are produced. If there is a successful reaction the word equation will be; Magnesium+ Sulphuric Acid � Magnesium+ Hydrogen Mg (s) + H�SO4 � Mg SO4 +H2 In a given amount of time if there are a lot of successful collisions, a lot of hydrogen gas will be produced. The rate of a reaction depends on how many successful collisions there are in a given amount of time. If there are not many collisions, then the rate of reaction is slow. ...read more.

Middle

Magnesium ribbon (10cm) Distilled water Method 1) Set up the apparatus as shown above. 2) Clean the magnesium ribbon with sandpaper to remove the oxide layer. 3) Then cut a 1cm length of magnesium using the scissors. 4) Measure 25cm3 of sulphuric acid using the burette in to the conical flask. N.E read the burette at the eye level from the bottom of the meniscus. 5) Then add 1cm of magnesium and start the stop clock. 6) Swirl conical flask once and watch for the reaction to be completed. I.e. the effervesce has stop. 7) Record the time in seconds in the results table. 8) Repeats steps 3-7 with same concentration of acid to ensure the result are reliable. 9) Repeat steps 2-8 with the different concentration shown in the results table. Safety * Make sure you are wearing goggles because sulphuric acid is corrosive and if any off it got into your eyes it would be dangerous. * A corrosive substance has the chemical hazard of visibly destroying or irreversibly damaging living tissue by chemical action. * If any acid spills on your hands wash them immediately. * Make sure you wear goggles at all times. ...read more.

Conclusion

No reaction Takes place. The concentration of sulphuric acid. There will be more hydrogen Ions per unit volume if the concentration of sulphuric acid is increased. This means that there is more chance of a collision between the Magnesium Atoms and the Hydrogen Ions. The more successful collisions that take place with the magnesium atoms per unit of time, the faster the rate of reaction. See the diagram on the next page Evaluating Points which do not fall on the curve of best fit are anomalous results Above the line. to fast H2SO4 may have been more concentrated than . should have been of Mg . . to slow Below the line to slow Mg to big H2SO4 to dilute How ever there is a clear general trend in the graph showing that as concentration increase so does the rate of reaction. I can conclude my results. Burettes Stop clock Ruler Scissors X scalpel more accurate Conical flask prevents acid spray Swirling X use a magnetic stirrer Sanding Mg X may not have been evenly removed . affected the amount of Mg present. Any changes or improvements that I would do would be; repeat each experiment for a third time, take a class set of results and process to ensure the result were more reliable and use a magnetic stirrer instead of swirling. ?? ?? ?? ?? 1 Candidate Centre No. 71321 ...read more.

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