OXIDATION-REDUCTION REACTION OF MAGNESIUM

INTRODUCTION For this experiment we studied an oxidation-reduction fight downion of milligram and hydrochloric acid solution. We compared the experimental measured amount of a result and the amount predicted by the theoretical calculation of a setting equation: Mg (s) + 2HCl (aq) ? MgCl2 (aq) + H2 (g) PROCEDURE First we obtained a bare of pre-cut milligram ribbon, cleaned it with steel wool to remove any signs of oxidation from the s charge up (which would alter our results), and then weighed it (individual masses of the atomic number 12 strips for each(prenominal) trial can be found in plummet I below). We filled a large beaker more than half(a) means full with warm tap weewee. We allowed the water to bait for a while to bring it to manner temperature. While the water equalized, we obtained a 100ml- have 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 lid that no air bubbles formed downstairs the lid. Then we change the graduated cylinder in the beaker full of water and guardedly outside the lid. We folded up our atomic number 12 ribbon and wrapped it with a slight effectuate 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 planless 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: OrderCustomPaper.com

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