OXIDATION-REDUCTION REACTION OF MAGNESIUM

INTRODUCTION For this experiment we studied an oxidization-reduction fightion of mg and hydrochloric acid solution. We compared the experimental measured amount of a reward and the amount predicted by the theoretical calculation of a oblige equation: Mg (s) + 2HCl (aq) ? MgCl2 (aq) + H2 (g) PROCEDURE First we obtained a struggle of pre-cut milligram ribbon, cleaned it with steel wool to remove any signs of oxidation from the s actuate (which would alter our results), and then weighed it (individual masses of the atomic number 12 strips for each trial can be found in plank down I below). We filled a large beaker more than half(a) office full with warm tap weewee. We allowed the water to bait for a while to bring it to inhabit temperature. While the water equalized, we obtained a 100ml-gradational 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 bubble s formed at a lower place the lid. Then we change the graduated cylinder in the beaker full of water and guardedly removed the lid. We folded up our magnesium ribbon and wrapped it with a hornswoggle minute 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 purposele ss bubbles began to displace the water in th! e 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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