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whether the strength of Hydrochloric acid will affect the speed of the rate of reaction when reacting with Magnesium Ribbon.

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Introduction

I want to find out whether the strength of Hydrochloric acid will affect the speed of the rate of reaction when reacting with Magnesium Ribbon. Variables There are two important independent variables in my investigation the first of which is the concentration of the Hydrochloric Acid used during the investigation. The concentration of the acid will partly determine how fast the reaction takes place, if we put some of the magnesium ribbon into the HCL at 2molar then it might have simply dissolved within a few seconds and then I would not have had time to record down any decent enough results to plot a graph with. The other important independent variable that will affect the speed of the rate of reaction is the length of magnesium ribbon. We need to put enough Mg Ribbon into the HCL so that it doesn't run out straight away but also so that the experiment stops by itself once the gas syringe has filled up. The reasons for choosing these two independent variables are that it would be too hard to try and find a catalyst for this experiment; a catalyst is a substance that increases the rate of a chemical reaction without being consumed in the reaction. Finding a catalyst for this particular experiment could take months never mind the amount of time we have been given for our experiment. The independent variable that I will change is going to be the hydrochloric acid, we will use 50ml of HCL at the following molarity concentrations; 2molar, 1.6molar, 1.2molar, 0.8 molar and 0.4 molar. I have decided to experiment with these different strengths of molar because I think it will give a wide set of results to put into a graph. The dependant variable I shall be measuring will be the time it takes for the magnesium to completely react with the hydrochloric acid, I shall record the times for each concentration of hydrochloric acid three times so that it makes it a fair test. ...read more.

Middle

I will take measurements ranging from 1ml� to 100ml�, as this is the largest amount of gas that the gas syringe will hold. I will check that my results are reliable by firstly checking that everything went as predicted in which the weakest solution took the longest time in order to give off all the gas and that the strongest solution would finish reacting the quickest. Another way which we will check that the results are reliable will be to check the results against the preliminary experiment. I shall make sure that my results are accurate by keeping some aspects of the experiment the same. The things that are going to be kept the same are the amount of hydrochloric acid and water, there will always be 50ml no matter what the concentration, The length of the magnesium ribbon will not change either; there will always be 10cm of that and the temperature at which the experiment will take place will always be near enough the same because we shall carry it out at room temperature and although we cannot always control this we will always do the experiment in the same room as to try to lessen this possible change. We will change however the concentration of the hydrochloric acid. Results 2.0 Molar Results Volume of Gas (cm�) Set 1 Set 2 Set 3 Time (Seconds) Set 1 Set 2 Set 3 R of R (cm�/second) R of R (cm�/second) R of R (cm�/second) 0 0 0 0 0 cm�/sec 0 cm�/sec 0 cm�/sec 5 64 55 70 12.8cm�/sec 11cm�/sec 14cm�/sec 10 88 77 86 4.8 cm�/sec 4.4 cm�/sec 3.2 cm�/sec 15 89 78 86 0.6 cm�/sec 0.2 cm�/sec 0 cm�/sec 20 89 78 86 0 cm�/sec 0 cm�/sec 0 cm�/sec 1.6 Molar Results Volume of Gas (cm�) Set 1 Set 2 Set 3 Time (Seconds) Set 1 Set 2 Set 3 R of R (cm�/second) ...read more.

Conclusion

This result was 7cm�/second over the other 2 sets of results. One explanation for this odd result could possibly be that we put the bung into the top of the conical flask too late and didn't start the stop clock at the same time. My results I think are very accurate because the volume of gas measured from the gas syringe and taken down were accurate to the nearest cm� and the rates of reaction was accurate down to the nearest tenth of a cm�/second. I think that my results are good enough and accurate enough to give a firm conclusion that the stronger the molarity of the hydrochloric acid is then the faster the magnesium ribbon is going to dissolve. I think this because my results show it, the starting strength which was 2molar took less than half a minute whereas the finishing strength which was 0.4molar took 5 and a half minutes, this was the longest results set out of all strengths of hydrochloric acid. There are a few ways in which I could make my reaction more accurate and reliable and the most obvious would be that I would have to find a way to hang the magnesium above the hydrochloric acid so that as soon s the bung goes in the acid drops and the stop clock starts, this would therefore eliminate any possible abnormalities. I think a way in which I could make this experiment last longer and to give extra evidence would be to do the same experiment only using smaller gaps in strengths of the hydrochloric acid, in other words do the experiment again only use hydrochloric acid of 2molar, 1.8molar, 1.6molar, 1.4molar...and so on until you got down to 0.2molar. This would give you a much more wider set of results especially if you did all of those strengths 3 times as we have done in this experiment. That is another way of making the experiment more accurate, by repeating it more than 3 times to so that we had enough sets of results for each strength to rule out any abnormalities. By Joey ...read more.

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