Rate of reaction
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Investigate the effect of concentration on the rate of reaction between magnesium with hydrochloric acid.
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Introduction
To investigate the effect of concentration the rate of reaction of magnesium with hydrochloric acid I am going to perform this experiment in order to discover how the concentration of an acid affects the rate of the reaction. I am going to perform this test using the following apparatus: A cylinder, Beakers, Stop Clock, Thermometer, goggles, and scissors. I am going to keep all my apparatus at the same room temperature and I am going to do this experiment 3 times in order to maintain a certain level of accuracy. After doing this experiment 3 times, I will average all of the results. The acid in which I am going to use in this experiment is 1M in strength. What I will do is I will use 50cm3 of acid for the first lot of magnesium. I will then take away 5cm3 of the acid and replace it with water so it makes a complete beaker full of 5cm3 water and 45cm3 of acid. I will then continue doing this until I have reached 25cm3 of acid and 25cm3 of water. ...read more.
Middle
1. Measure 50 cm3 of water into a 50cm3 measuring cylinder. 2. Transfer the Acid from the measuring cylinder to the beaker. 3. Then add the 2.5 cm of magnesium ribbon. 4. Stir once and start the clock as soon as the magnesium is dropped in the acid timing how long this takes to dissolve using the stop clock. 5. Repeat this using the measurements as stated in the results table. 6. Make sure that the experiment was repeated 3 times for more accuracy. 7. Average all the results up to get a final set. It is important that the beakers and all apparatus are being supervised at all times so that the most possible accuracy is maintained. If it is required, then ensure to repeat any odd looking results. Try and ensure that all measurements are as accurate as possible, to ensure fairness amongst all of the solution. Analysis I found out that the higher the concentration of the acid, the quicker the magnesium is able to react and dissolve into the solution. Result Table Exp No Volume of Acid Volume of Water Time in Seconds (1) ...read more.
Conclusion
I do believe that there was a couple of anomalous result, and I will highlight these on a second results table below. Exp No Volume of Acid Volume of Water Time in Seconds (1) Time in Seconds (2) Time in Seconds (3) Average 1 50 0 147 134 138 139 2 45 5 191 190 192 191 3 40 10 216 210 211 212 4 35 15 367 334 340 349 5 30 20 474 443 461 459 6 25 25 540 539 541 540 I do believe that I would have been able to make the experiment ever so slightly better by improving a couple of things. 1. I would have tried to keep the surrounding temperature at the same temperature if possible. 2. I would make sure that all of the magnesium ribbon is cut at exactly the same length. 3. I would have tried to make sure that we were using the same taps. 4. I would have possibly redone a few more of the results which I believe to be anomalous. 5. I think the experiment would be even more accurate if I had done the experiment more then 3 times. 6. I would use brand new magnesium ribbon, due to the fact that the old magnesium ribbon had formed an magnesium oxide layer. 1 ...read more.
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