{"id":1404,"date":"2017-02-27T19:40:49","date_gmt":"2017-02-27T19:40:49","guid":{"rendered":"http:\/\/www.experimentoscientificos.es\/?p=1404"},"modified":"2021-03-05T12:10:00","modified_gmt":"2021-03-05T12:10:00","slug":"reaccion-redox-sulfato-cobre-hierro","status":"publish","type":"post","link":"https:\/\/www.experimentoscientificos.es\/en\/reaccion-redox-sulfato-cobre-hierro\/","title":{"rendered":"REDOX Reaction Copper Iron Sulphate"},"content":{"rendered":"
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COPPER ALUMINIUM SULPHATE REDOX EXPERIMENT SHEET<\/h2>\n\n\n\n\n\n\n
Theme<\/strong><\/td>\nRedox Reaction<\/a>, Atoms<\/a><\/td>\n<\/tr>\n
Category<\/strong><\/td>\nScientific Experiments<\/a>, Chemistry Experiments<\/a><\/td>\n<\/tr>\n
Main products<\/strong><\/td>\nCopper sulphate<\/td>\n<\/tr>\n
Short description<\/strong><\/td>\nIn this experiment we are going to look at the oxidation-reduction (Redox) reaction between Copper Sulphate (CuSO4) and Iron Metal (Fe). This experiment is very important for 3 fundamental reasons: 1. It is one of the most important reactions in chemistry (oxidation-reduction (Redox) reaction). 2. Through this reaction we are going to achieve the circulation of electrons (the principle of electricity in batteries and cells) and 3. we are going to obtain copper metal from other substances. It is the reaction between copper sulphate in solution and iron metal.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

We first look at the oxidation potentials<\/a> of the components:<\/p>\n

Fe2+(aq) + 2e- \u2192 Fe(s) 0.440V
\nSO42-(aq) + 4H+(aq) + 2e- \u2192 2H2O(l) + SO2(g) -0.17V
\nCu2+(aq) + 2e- \u2192 Cu(s) - 0.340V<\/p>\n

We see that the materials with the greatest potential to enter into oxidation-reduction would be the atom<\/a> from Iron<\/a> (which is oxidised) and copper (which is reduced). On the other hand, the reaction will take place in an aqueous solution of copper sulphate, which would be sufficient to conduct the electrons that are going to be transferred. To increase the conductivity of the solution we are going to add sodium chloride (common salt), in this way our reaction will be accelerated and we will be able to see the effects more quickly.<\/p>\n

The reaction that will therefore take place is:<\/p>\n

CuSO4 + Fe -> FeSO4 + Cu<\/strong><\/p>\n

As soon as the iron metal is introduced into the copper sulphate solution, a reddish layer starts to form on the iron in a few minutes, this is already the reduced copper (copper metal) that is being deposited on the iron. Furthermore, the solution changes from the bluish colour of the copper sulphate to the green colour of the iron sulphate that is being generated. If we maintain the reaction over time, the copper will continue to deposit until all the copper in the solution is consumed (or until all the iron is consumed, which in this case would not be the case because there is more iron than copper sulphate).<\/p>\n

COPPER IRON SULPHATE REACTION EXPERIMENT STEP-BY-STEP<\/h2>\n