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An Investigation Into The Factors That Affect The Enthalpy Change During A Displacement Reaction.

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Introduction

zinc and cuso4 reaction An Investigation Into The Factors That Affect The Enthalpy Change During A Displacement Reaction. Background Knowledge The reactivity series is an order that places metals in that series depending how vigorously that metal reacts with water, air or acid. A more reactive metal could displace a less reactive metal from its' compound. Zinc (Zn) is a more reactive metal than Copper (Cu); it is higher in the reactivity than copper and thus when some zinc is placed in a solution of copper sulphate a displacement reaction takes place. The zinc goes into solution while the copper is "forced" out of solution. The situation can be described as follows: The full equation is: Zinc + Copper Sulphate = Copper + Zinc Sulphate Zn(s) + CuSo4 (aq) = Cu(s) + ZnSo4 (aq) The Ionic equation is: Zinc + Copper = Copper + Zinc Zn(s) + Cu 2+(aq) = Cu(s) + Zn 2+(aq) The experiment will be exothermic; this means during the reaction, energy will be given off, mainly heat energy. ...read more.

Middle

will apply including the wearing of safety goggles, no running, the washing of hands after undertaking the experiment and no eating in the laboratory. Preliminary work During the undertaking of preliminary work, prior to doing the experiments that the final results would be taken from, a few interesting and relevant points were taken. Such as the quantities of Zinc and Copper sulphate solution used, I found during the preliminary work that 30cm3 of CuSo4 wasn't enough and that 70 was too much, which is why I kept the volume of CuSo4 at 50 ml3 as a constant. Similarly I found that any more than 5g of Zinc used would produce varied results and hinder the accuracy of the experiment. This is why I kept the constants at 50ml for the CuSo4 and only a maximum of 5g for the zinc. I also found that using a plastic lid over the cup aided the insulation, thus giving more accurate results. Experimental prediction I predict that the greater the mass of zinc, the greater the heat produced within the experiment. ...read more.

Conclusion

For example I would make sure that the correct apparatus was used each time, and that the apparatus was used correctly. In calculating the average results the figures would be given to 2 decimal places instead of one to ensure a higher accuracy in the final answers. When I think that the temperature has stopped rising I will time 30 seconds, if the solution doesn't get any hotter I will record this temperature as it will be the peak temperature, counting the thirty seconds makes sure that the solution is at the hottest it is going to get. Experimental procedure - Collect, prepare and set up all the apparatus correctly, including the weighing of zinc and the measuring of copper sulphate solution. - Pour the copper sulphate solution into the polystyrene cup, read the initial temperature of the solution and note it. - Into the solution add the Zinc and stir. - Watch the thermometer, when the solution stops rising in temperature, time out 30 seconds. If the temperature doesn't get any hotter record this temperature as this will be the peak temperature. - Note this temperature in a pre-prepared table. - Repeat this four times for each mass of zinc (1-5g). ...read more.

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