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# An Investigation Into The Effect Of Varying The Acid Concentration On The Rate Of Reaction Between Hydrochloric Acid And Marble Chips.

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Introduction

An Investigation Into The Effect Of Varying The Acid Concentration On The Rate Of Reaction Between Hydrochloric Acid And Marble Chips I am investigating how the concentration of hydrochloric acid will effect the rate of reaction when calcium carbonate (marble chips) are added to the acid. Hydrochloric acid + calcium carbonate � Calcium chloride + Water + Carbon Dioxide To measure the rate of reaction I could * Time how long it takes for the Ca CO3 to dissolve * Time how long it takes for the fizzing in the system to finish * Time how long it takes to collect a specific volume of CO2 * Time how long it takes for a loss of a specific mass to take place. The factors that could affect the rate of this reaction are, temperature in which the reaction takes place, concentration of the acid, surface area of calcium carbonate, using a catalyst. The variables are all of the factors affecting the rate of reaction. I will keep all of the variables the same apart from the concentration of the acid. Reactions happen when particles collide together with enough energy to form a bond, therefore the more collisions the more chances of bonds being made. This is the collision theory. As the concentration of the acid increases there are more particles for the calcium carbonate to react with in the same amount of ...read more.

Middle

As soon as this is done I shall start the timer. Once the measuring cylinder has collected 100cm� of carbon dioxide I shall stop the timer. I will record my time to the nearest second. I shall repeat this once more with each concentration, with 6 different concentrations. Results Amount of CO2 collected (cm�) Time into reaction (minutes) 0.25m Test 1 0.25m Test 2 0.25m Av 0.5m Test 1 0.5m Test 2 0.5m Av 0.75m Test 1 0.75m Test 2 0.75m Av 1 6 4 5 18 14 16 27 19 23 2 19 15 17 29 23 26 46 34 40 3 24 22 23 36 34 35 58 48 53 4 32 28 30 41 47 44 70 62 66 5 34 36 35 59 51 55 77 71 74 6 37 41 39 62 64 63 86 80 83 7 42 46 44 65 69 67 93 89 91 8 43 47 45 72 74 73 98 94 96 9 49 49 49 79 81 80 100 100 100 10 51 53 52 80 82 81 11 53 55 54 83 85 84 12 54 56 55 85 87 86 13 56 58 57 86 88 87 14 57 59 58 88 88 88 15 58 60 59 88 88 88 Amount of CO2 collected (cm�) ...read more.

Conclusion

This is an alternate way of measuring the reaction, without having to upturn the cylinder. I am happy with the consistency of the temperature of the HCl. My results are accurate; however I do appear to have results that are anomalous, which are prominent in my graph. For example the results for 0.25m at 7 minutes, and 0.5m at 7 and 8 minutes are inconsistent and stand out on the graph. These could have occurred if the conical flask was shaken during the experiment. I repeated all of my results a second time none of my results were drastically out of place however there were some which perhaps more inconsistent than others. If I were to repeat the experiment I would make sure that I repeated the experiment three times instead of just 2. Although this would take up much more time, I feel it more important to obtain the most accurate results possible. In addition, out of pure interest I would like to find what happens when the temperature of the HCl increases. To do this I would heat the acid to different temperatures at regular intervals and add the same amount of Ca CO3. I expect to see that as the temperature increases so does the reaction time. My precise results enable me to come to strong conclusion that the higher the concentration of HCl the less time was taken to collect 100cm� of CO2 when reacted with Ca CO3. ...read more.

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