OXIDATION-REDUCTION REACTION OF MAGNESIUM

INTRODUCTION For this experiment we studied an oxidation-reduction counterbalanceion of milligram and hydrochloric acid solution. We compared the experimental measured amount of a product and the amount predicted by the theoretical calculation of a tick off equation: Mg (s) + 2HCl (aq) ? MgCl2 (aq) + H2 (g) PROCEDURE First we obtained a disrobe of pre-cut milligram ribbon, cleaned it with steel wool to remove any signs of oxidation from the s misstep (which would alter our results), and then weighed it (individual masses of the magnesium strips for all(prenominal) trial can be found in plug-in I below). We filled a large beaker more than half(a) right smart full with warm tap weewee. We allowed the water to bait for a while to bring it to get on temperature. While the water equalized, we obtained a 100ml- receive cylinder and filled it with tap water (also at room temperature), and created with a hat of plastic wrap. It was important when creating this li d that no air bubbles formed low the lid. Then we change the graduated cylinder in the beaker full of water and guardedly withdraw the lid. We folded up our magnesium ribbon and wrapped it with a hapless objet dart of copper wire so the magnesium would react and not break off during the reaction. We put this magnesium piece at the bottom of the beaker underneath the graduated cylinder. using a thistle tube we gently propped the end of the tube up under the inverted graduated cylinder and then poured 10ml HCl into it. As the magnesium began to react, we slowly pulled the tube out and waited as the be directionless bubbles began to displace the water in the cylinder. After all the magnesium was consumed, we moved the graduated cylinder up and down in the water to equalize the water levels. Once we had accomplished... If you want to trip up a full essay, order it on our website: OrderCustomPa per.com

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