Helpf Essay

529 words - 2 pages

Redox ReactionObjective:To perform a single replacement Redox reaction between Aluminum metal and Copper sulfate to yield Copper metal and Aluminum sulfate. Calculation of percentage.Discussion:Oxidation is the loss of electrons and reduction is the gain of electrons. In the present case, Aluminum is converted to the cation Al3+ and hence has been oxidized. Copper cation Cu2+ has been reduced to metallic copper. The molecular and net ionic equations along with the oxidation and reduction half reaction are given below.2Al(s) + 3Cu(SO4)(aq) Al2(SO4)3(aq) + 3Cu(s)2Al(s) + 3Cu2+(aq) 2Al3+(aq) + 3Cu(s)Al(s)Al3+(aq) + 3e-Cu2+(aq) + 2e-Cu(s)Percentage yield is given by actual yield divided by theoretical yield and expressed as a percentageMaterials:Aluminum foil, Copper sulfate.5H2O, 6M HCl(aq), stirring rod, beaker, measuring cylindersProcedures:A clean dry 125ml beaker was weighed and then recorded. Copper Sulfate was then carefully added until 2g had been added. Then the beaker was weighed again with the copper sulfate and then recorded. 10ml of deionized water was poured in a small graduated cylinder and then placed into the beaker to dissolve the copper salt. Once the copper dissolved completely the color of the substance was recorded. 2 ml of 6M HCl solution was measured in a graduated cylinder, and then added to the solution and mixed well. Then .25g of aluminum foil was weighed in small pieces and then added slowly while using a stirring rod to mix the solution during the reaction. The color of the solution was noted as the pieces of aluminum were added and they no longer darkened the surface. Then an additional 5 ml of 6M HCl was added to facilitate the reaction of any excess metal with the acid....

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