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Measuring the rate of reaction between hydrochloric acid and magnesium.

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Introduction

Measuring the Rate of Reaction between Hydrochloric Acid and Magnesium Aim To investigate the rate of reaction between Magnesium and varying concentrations of Hydrochloric acid. Prediction As the concentration of Hydrochloric acid increases so therefore the rate of reaction should also increase Reasons I have chosen to change the concentration of Hydrochloric acid this is my independent variable This graph shows us that there are more collisions because there are more particles therefore the rate of reaction increases too. The rate of reaction increases because the number of collisions with enough energy to cause also increases. Other Factors to Control Temperature - When the temperature in a reaction increases the rate of reaction also increases. This is because the number of collisions between particles increases as they change thermal energy into kinetic energy (particles move around more).The particles collide more often with enough energy to break bonds and make new bonds. Pressure - When pressure is increased in a reaction the rate of reaction also increases. ...read more.

Middle

The diagram below shows how the apparatus should be set up so that I can perform the experiment. I will explain a step by step procedure which I followed to carry out this investigation 1. Collect all the right apparatus and set up the apparatus like shown on the above diagram 2. Measure 10 cm3 of Hydrochloric acid of chosen mol(0.5 mol) using a measuring cylinder and pour into the round bottomed flask 3. Add the magnesium to the flask and replace the rubber tubing quickly as possible and start the stopwatch 4. Record the time it took to reach the target of 40 cm3 of Hydrogen gas 5. Repeat the above 2 more times keeping everything the same each time. 6. Now repeat all the above for mol of 1m 2m, 2.5m ,4m and 5m 7. Clear up at the apparatus and put back all apparatus in their appropriate place Results Concentration of Hydrochloric Acid Trial Time Taken to collect 40 cm3 (seconds) Average Time Taken (seconds) ...read more.

Conclusion

Secondly when we washed the contents after each trial water may have been present instead we could dry the beaker very well. Lastly we missed out many different mol of Hydrochloric Acid. If I was to repeat this investigation I would investigate all the intermediate concentrations e.g. 0.5,1,1.5,2,2.5,3,3.5,4,4.5 and 5 . This wider range of values would improve the reliability of results and the ability to draw to a conclusion. We could have extended our investigation by investigating other factors concerning Rate of Reaction. These could have been the following * Temperature * Surface Area * Pressure We could of investigated what the relationship is between each of these factors and see if the results produced this. We could have investigated the rate of reaction on other substances like sulphuric acid. Conclusion From my results I conclude that my prediction is correct. My prediction was that if the concentration of Hydrochloric Acid increases therefore the rate of reaction should also increases this is because the number of collisions between the Magnesium and Hydrochloric acid increases so the time taken for 40cm3 of Hydrogen gas to be collected decreased therefore the rate of reaction increases. ...read more.

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