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Using different concentrations To speed up the rate of reaction.

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Introduction

Using different concentrations To speed up the rate of reaction Introduction In this investigation I am going to look at the different factors that affect the rate of reaction. The factor that I am going to investigate is the concentration of the acid used, which in this case is Hydrochloric acid (HCL). The different factors that affect the rate of reaction are: > Temperature > Concentration of acid > Surface area of magnesium > Catalyst > Pressure Rates of reaction means how fast a chemical reaction takes place. During a chemical reaction many changes may take place, some of these changes are obvious: e.g. the solution may change colour. The less obvious changes are: > Change in mass > Volume of gas made > PH > Temperature "Bob McDuell GCSE chemistry" Temperature Temperature can affect how fast a reaction takes place. When the temperature is increased the particles move faster as they have more KINETIC ENERGY. The faster the particles move the are more successful collisions, there are E.g. if you increase the temperature by 10`C the rate of reaction will double "Bob McDuell, GCSE Chemistry" Concentration If the acid has a high concentration the more likely it is that there will be more collisions. There will be more collisions, as there are more particles of the reactant in the solution. ...read more.

Middle

used I am going to change the following things in my experiment: > Concentration of acid I am going to repeat this experiment four times so that I can obtain accurate results. I am going to use five different concentrations of acid in my experiment. Fair test To make this experiment a fair test I will: > Amount of magnesium ribbon used > Collect the same amount of gas > Use the same volume of acid all the time Apparatus/ diagram For this experiment you will need: > Magnesium ribbon 0.15 grams each time > Hydrochloric acid up to 2 moles > Water (to dilute acid) > Pipette > Measuring cylinder - 35CM3 > Gas syringe > Stop watch > Clamp > Conical flask > Safety goggles Method > Collect apparatus > Set up as shown above > Collect magnesium ribbon 0.15g > Measure out 25 cm3 of HCL acid using a measuring cylinder (change concentration as appropriate) The concentrations that I am going to use are: > 2 molar > 1.66 molar > 1.34 molar > 1 molar > 0.66 molar (you have to change the concentration of the acid by diluting the acid with water) > Make sure that you are wearing safety goggles > Place acid into flask > Place magnesium ribbon in to flask > Quickly place bung onto flask > Check that the bung is securely on, and there are no gaps > Start timer quickly ...read more.

Conclusion

My graph doesn't prove this theory correct, but there were fairly accurate compared to the equipment I had available. I still some anomalous results, this may be due to change in environment or inaccurate readings. Evaluation I think that my method was correct, as my experiments did run smoothly. If I could do the experiment again I would do all the experiments in one day, so that there wouldn't be a change in environment. The accuracy of my experiment was good in comparison to the equipment we had available. One thing that should be improved on was the time period it took for us to place the bung on the flask, this would have effected the time taken to produce 50cm3 of hydrogen gas. Another reason for these anomalous results is that the concentration of the acid could have been wrong. Another possible reason is that when the flask was washed it may have been washed with too hot or too cold water, which would have changed one of the variables I was keeping the same in my experiment. As you can see from my results table my results were constant throughout the repeats of the experiment. If I could do the experiment again I would have repeated it again to get a more accurate average. Overall I think that my experiment went well, and that I obtained accurate results. Diagram Komal Patel 11GS Chemistry C/W ...read more.

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