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Metal Reactivity Coursework

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Introduction

Metal Reactivity Coursework Aim: To put the following metals into a reactivity series: Magnesium (Mg) Zinc (Zn) Iron (Fe) Calcium (Ca) Copper (Cu) Aluminium (Al) Method Plans: 1) Secondary Source: "Chemistry Counts" by Graham Hill. Record visual reactions, i.e. how bright the reaction is, how violently it reacts, and how fast the reaction is completed. This, however would be impossible with the metals concerned as, not only is it highly inaccurate but also slow: Iron takes a long time to react. The other reason is that you would then need a scale of violence for comparison of the various metals. 2) Record the amount of hydrogen produced upon reacting each metal with hydrochloric acid over a constant period of time. The higher the rate of hydrogen produced, the more reactive metal. Unfortunately the amount of hydrogen produced in each case is negligible. To get enough hydrogen produced to give meaningful results, large amounts of acid and metal are required. According to another secondary source, 30g of hydrochloric acid reacting with 0.54g of Aluminium gives of 0.067% of that- 0.02g as hydrogen. You would need at least ten times that much to be able to obtain a recording, therefore the experiment is not possible. 3) Measure the enthalpy change of reaction by measuring the heat produced at set intervals, thereby building a graph to extrapolate a curve giving us a maximum temperature rise. ...read more.

Middle

hydrochloric acid at a concentration of 2mol/dm3 mercury thermometer graduated to 1�c electronic timer plastic lid Two lots of 0.1 mol of each metal: Table of amount of each metal needed: Metal Mass of 0.1 mol (in g) Calcium 4 Magnesium 2.4 Aluminium 2.7 Zinc 6.54 Iron 5.6 Copper 6.35 A degree of accuracy is important, which is why everything used in this experiment should be constant except for the metal involved. Testing each metal twice makes sure an accurate reading is taken, without fear of using a 'bad' result. Diagram of apparatus: Key factors: Room temperature. Room pressure. Key Variables: Concentration of acid- must be constant. Amount of acid- a constant volume (0.1 moles).( The reason for only 0.1 mol is that you need two moles of HCl to react with one mole of a metal. So as I want to have an excess of metal I am only going to use half of the acid needed to react with the metal) Mass of metal- 0.1 mol Time readings are taken every 30 seconds for nine and a half minutes Having the above as constants adds to the accuracy of the experiments. Amount of acid needed. I want to use double the amount of metal than acid needed to react with the metal. The chemical equations are the following: (I am using M as the symbol for metal, and assuming M forms M�+ ions we can write a general equation as) ...read more.

Conclusion

If I was to do the experiment again and I wanted as accreat results as i possibly could and the experiment to be as fair as it could, I would have to use an more accreat way of measuring the temperature rise such as an sensor to a computer, as when I did it I only had an thermometer in if I wanted it to go down to the decimal placing had to be gess work as it was in this experiment. I would also change the way I insulated the experiment, not that mine was not effective but there are even better ways of insulating it. I would also use metals that had not been exposed to the air as the air reacts with them and on some metals such as iron it forms an less reactive coat on the metals. That is what I believe happen to all of my meals apart from Magnesium, as there paths should have followed that of Magnesium in the sense that it goes up then down, but in my experiment they did not, this I believe is because the had all ready reacted with the air forming an coat on the metals and that is why I took longer for them to react as the acid had to react with these coat first. Rhys Beddoe i ...read more.

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