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To investigate the factors affecting the rate of reaction of calcium carbonate (limestone) with hydrochloric acid

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Introduction

SHURREEN MILES 10.G REACTION OF CALCIUM CARBONATE GCSE COURSEWORK AIM: To investigate the factors affecting the rate of reaction of calcium carbonate (limestone) with hydrochloric acid. SCIENTIFIC KNOWLEDGE: When you add hydrochloric acid to limestone it reacts giving off gases which is carbon dioxide, the concentration of the acid will also affect the rate of reaction like the surface of the limestone also if the water in the experiment is warm or cold. The scientific equation is CaCO3 (S) + 2HCl (aq) - CaCl2 (aq) + H2O (1) + CO2 (g). Example of the concentration is that when the concentration is in creased the particles will be closer together and when the solution is made warmer the particles move faster. PREDICTION: I predict that as the temperature of the acid increases, the rate of reaction will increase. ...read more.

Middle

2) Fill up beaker with 100mls of water, put the beaker on top of the gauze. 3) Heat the water up until it reaches 30C. 4) Pour 25mls of the 1.5 molar hydrochloric acid into the boiling tube. 5) Place the boiling tube in the beaker and put the thermometer in the boiling tube to make sure the acid is at 30C. 6) Fill the measuring cylinder up with water. 7) Turn the water bath, upside down over the cylinder and hold the bath down firmly. 8) Tip the bath and cylinder upside down, still holding them together firmly so that the bath is placed firmly on a flat surface with the cylinder inside it. Hold the cylinder tightly in the bath to make sure no water escapes. ...read more.

Conclusion

RESULTS: Temperature Test 1 Test 2 Test 3 Average rate of reaction 30 C 57ml/30secs 50ml/30secs 40ml/30secs 49ml/30secs 40 C 65ml/30secs 65ml/30secs 50ml/30secs 60ml/30secs 50 C 80ml/30secs 70ml/30secs 69ml/30secs 73ml/30secs 60C 100ml/30secs 97ml/30secs 91ml/30secs 96ml/30secs 70 C 130ml/30secs 127ml/30secs 99ml/30secs 119ml/30secs CONCLUSION: Like I said in my prediction as the temperature increased, so did the rate of reaction also as it says in my scientific knowledge the collision statement did take place. As the temperature became more the particles began to move faster which resulted in more collisions. EVALUATION: After evaluating my results they were not very useful, I repeated the method three times then I could find the difference between the results to work out the average, if I did this experiment again I think the equipment would have to be different. I could also change the amount of acid and limestone or even the temperature. ?? ?? ?? ?? ...read more.

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