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# Coursework: rates of reaction, strength of acid

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Introduction

Coursework: rates of reaction, strength of acid I have been asked to investigate the speed of reaction of acid acting on marble chips. Aim To find out what factors effect the rate of a reaction - the reaction between marble chips and hydrochloric acid. Key factors The Quantity of marble chips used , This could increase or decrease the surface area of the marble chips. Speeding up or slowing down the reaction because with a larger surface area more of the marble is reacting with the acid. The amount of acid used, more or less acid could change the amount of time that the reaction takes. Varying the amount of acid used would alter the time for the reaction because there are more or less acid particles to react with the marble chips. More acid longer time, less acid quicker time. The strength (concentration) of the acid used, alters the amount of particles of acid in cm3, this means that as the strength increases the amount of particles increase, giving more acid particles to react with the marble chips. Increasing the acid strength will speed up the reaction but taking longer to finish because there are more acid particles to react with the marble chips. The size of the marble chips, as marble chips increase their size there is less surface area for the acid to react with. ...read more.

Middle

This is because there are more particles in the same volume so more collisions are possible every second." Preliminary work When I first set up my preliminary experiment I started with 50 ml of hydrochloric acid and one 2 g piece of calcium carbonate, measuring the amount of carbon dioxide produced. The results were to difficult to record with the equipment and to time consuming. I then decided to half the amount of hydrochloric acid and have 2g of smaller calcium carbonate to increase the surface area. I did this to speed up the reaction so that it was also easily measurable in 1 minute intervals. The method that I used for the preliminary work was almost the same system but I only used a 1000 cm3 measuring cylinder. The problem with this was that with the lower concentration acid results were hard to read. So for the real experiment I decided to use smaller measuring cylinders. Preliminary results 0.5 mol cm3 15 29 40 55 73 92 109 125 129 136 141 141 as you can se the results took to long to collect and they would not produce great graphs. Plan To test my prediction and my hypothesis I am going to put Hydrochloric acid and marble chips together and measure the amount of gas given off every minute. ...read more.

Conclusion

These results nearly support my prediction, that the higher the concentration the faster the reaction will take place. The later 3 sets of results support this but the first two do not this may be because the are less particles to react with the calcium carbonate . The results also support my graph shape prediction that was that the line is steeper at the start and levels of towards the end. Evaluation Looking at my graph their is one anomalous result from my 1mol results. As there is only one wrong point I have decided that it was an error in the recording of this result. I do not think that the equipment used for this experiment was accurate because the gas that we were measuring was carbon dioxide. I know that carbon dioxide is soluble with water so as it passed through the water it would have mixed and the product that was in the measuring would not be all the carbon dioxide that was given off. Taking results was not hard but a times could be confusing recording at 30 second intervals. I feel that the evidence that I collected reliable , because of the close readings and few inaccuracies. Also that the results were what the BBC Bitesize agreed with. Also when I repeated the experiment the results were similar to each other and usually only 10 difference between each other. ...read more.

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