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# How concentration Affects The Rate of Reaction of Hydrochloric Acid and Magnesium Ribbons.

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Introduction

10th February raheem hussain 11w1 How CONCENTRATION Affects The Rate of Reaction of Hydrochloric Acid and Magnesium Ribbons Aim:I am going to investigate the effects of concentration on the rates of reaction Introduction: Factors affecting the rates of reaction are * Surface area * Concentration * Pressure * Temperature * Adding Catalyst The reaction that I am going to be looking at is between a metal, magnesium strips and an acid, hydrochloric acid. The result of these two reacting would leave me with a salt, which would be magnesium chloride and a gas, which will always be hydrogen. The word equation for this reaction is: Magnesium+Hydrochloric---- Magnesium+Hydrogen Acid Chloride The symbol equation for this is: Mg+2hcl----- MgCl2+h2 Concentration: If the concentration of any reactant in a solution is increased, the rate of reaction is increased o Increasing the concentration, increases the probability of a collision between reactant particles because there are more of them in the same volume. ? * Increasing the concentration of reactant A or B will increase the chance or frequency of collision between them and increase the speed of product formation (slower to faster). ...read more.

Middle

There is also kinetic energy present so this means when collisions occur, they do not always result in a reaction. If the two colliding molecules have sufficient energy they will react. Method: The steps I will take to do this experiment successfully are as follows: 1. Put on safety goggles 2. Collect clamp stand, clamp and boss 3. Collect conical flask and measuring cylinder 4. Collect stop clock 5. I will measure solution of 20ml of 0.2molar hydrochloric acid out in a measuring cylinder accurately. 6. Pour hydrochloric acid into the conical flask 7. Measure the starting temperature of the hydrochloric acid 9. Measure 4cm of magnesium ribbon 10. Drop the magnesium into the conical flask 11. Quickly place the rubber bung into the conical flask 13. Start timing with the stop clock 14. Record the amount of gas evolved every 20 seconds for 120 seconds 15. I will repeat this experiment three times so my results are reliable. 16. I will then do the same for 0.4, 0.6, 0.8 and 1 molar. Fair test: In order to keep my experiment a fair test I will have to make sure that I keep the following factors the same: � Starting temperature of the acid � Volume of acid used (cubic centimeters) ...read more.

Conclusion

Conclusion: My results prove beyond doubt that as the concentration of the acid increases, the time taken for the reaction decreases. This supports the prediction to a high extent because the results follow the trend that was predicted. Their were no anomalous results as I expected and altogether I tested 5 different concentrations of hydrochloric acid 0.2M, which was the lowest concentration of acid that I used, there was no reaction. 1M hydrochloric acid, which was the highest concentration that I used, produced the fastest rate of reaction. I repeated all 5 concentrations three times. Evaluation: In my graph it does not show any incorrect results this is due to the fact that the results that where repeated were similar to each other so the averages obtained when plotted on the graph did not leave me with any anomalous results. I believe there was a set pattern all through my results showing that as the concentration of acid is increased, the rate of reaction also increased. If I was to this experiment again I would change the place where we do the reaction because the temperature of the class room was not always constant. I would use a syringe instead of just tubing and a cylinder to measure the gas given out to make it more accurate. ...read more.

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