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What are some of the General Features of Redox Reactions?

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What are some of the General Features of Redox Reactions? This experiment is designed to establish whether a Redox reaction takes place when zinc is added to copper (II) sulphate solution and whether copper, magnesium or aluminium reacts with zinc (II) sulphate solution. COSSH/Risk Assessment. Copper (II) sulphate solution (1.0 mol dm-3 (20cm3)) Harmful Zinc (II) sulphate solution (1.0 mol dm-3 (20cm3)) Harmful Zinc Powder (1g) Flammable Magnesium Powder (1g) Flammable Aluminium Powder (1g) Laboratory coats must be worn at all times Eye protection must be worn at all times In case of spillage, absorb and wash to drain with copious water. Wash area with copious water. Method. 1. A small beaker (25cm3) was half filled with copper (II) sulphate solution and a note of its temperature taken using a glass thermometer ranging from 0-110oC. ...read more.


sulphate solution and a copper strip instead of the zinc strip the experiment was repeated between steps 1 and 2 and the results recorded as before. 6. Magnesium and Aluminium powders were individually placed into beakers of Zinc (II) sulphate solution stirred and the maximum temperature was recorded. Experimental Observations. Product Tested Copper (II) Sulphate solution at 19oC Product Tested Zinc (II) Sulphate solution at 18.8oC Zinc Strip 20.4oC, Copper deposited on surface but surface turned blacker as time went on. Copper Strip No reaction was recorded Zinc Powder 25oC, The solution appeared blackened. Magnesium powder 19.3oC Filtrate A shade lighter in comparison than the original solution. Aluminium Powder 18.9oC Conclusions. In order for a deposit to form on the zinc strip and a rise in temperature a reaction must have taken place and this can be shown as; Zn (s) ...read more.


The reverse reaction did not take place between the copper strip and the zinc (II) sulphate solution. The very small temperature change recorded when the magnesium was added to the zinc (II) sulphate solution shows that a Redox reaction has taken place, but not as vigoroursly as the zinc in copper (II) sulphate solution, and this reaction can be show as; Mg (s) ? Mg2+ + 2e- Oxidation and Zn2+ (aq) + 2e- ? Zn (s) Reduction Al (s) ? Al2+ + 2e- Oxidation and Zn2+ (aq) + 2e- ? Zn (s) Reduction Questions. Repeating the experiment ensuring that all the steps of the method are taken with care, accuracy and using thermal insulated test tubes instead of beakers, giving a greater concentration of the solution, would have yielded greater temperature changes in a shorter time, which would ensure as accurate a result as possible. ...read more.

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