The Element Magnesium

Abstract: An ice calorimeter was used to study the reaction of magnesium metal and 1.00M

Sandpaper was used to remove impurities from the magnesium strips, resulting in a grey strip, with a bit of metallic lustre. The strip of magnesium received was extremely malleable and was easily cut into 1 cm strips and folded into a tiny ball.

The most noticeable of them was oxygen, nitrogen and hydrogen. It was also known then that when a metal was heated in the air it became and oxide, this change was accompanied by an increase in mass. An example of an oxide is magnesium oxide. This happens when magnesium, a metal, reacts with the oxygen when it burns. An example calculation is when the mass of the reactant, magnesium, is 2.39 grams and the product, magnesium oxide (MgO) is 3.78 grams. (LearnChemistry) We can see a noticeable change in the mass. It must therefore mean that oxygen from the air must have been absorbed. The total amount of oxygen absorbed is 1.39 grams. This reaction can be reversed by heating the magnesium which releases the oxygen and returning the metal, magnesium, into a pure metal.

As for metal, it has many uses. In fact, modern civilization has thrived off of things where iron is used like: buildings, car frames, bridges, and much more.

Materials:Magnesium stripCrucibleCrucible coverClay triangleIron ringRetort standTongsBalanceBunsen burnerProcedure:1.obtained a strip of magnesium between 30-40 cm long2.coiled magnesium strip into a tight roll3.measured the mass of the crucible and cover4.Added the magnesium strip to the crucible and measured the

The masses before and after the oxidation are measured. The calculated masses are then used to find out the experimental empirical formula of magnesium oxide. A Bunsen burner will be used to heat magnesium metal. The experiment relates because we are determine the formula for magnesium oxide. Procedures

The aim of the lab was to determine the molar enthalpy of the combustion of magnesium using values from reactions between magnesium and magnesium oxide in hydrochloric acid solution using Hess’s Law and Calorimetry. The calculated molar enthalpy of the combustion of magnesium from this experiment was -633.6KJ/mol. This result was found by putting a known mass of magnesium metal as well as magnesium oxide powder into a concentration of HCl. Firstly, a styrofoam calorimeter was used to determine the standard reaction temperature of magnesium metal and hydrochloric acid. Next, calorimetry was again used to determine the reaction temperature of magnesium oxide and hydrochloric acid. Lastly, the thermochemical equations for the two

| After ignition of magnesium light and toxic fumes are made, and white powder (2MgO or Magnesium Oxide) is left over.

Because it is dangerous to burn magnesium, it is not possible to directly record heat change. Our lab team suggests an indirect way of determining the heat of combustion for magnesium. To accomplish this, we need to perform two separate trials. One uses a solid (powder) version of MgO, while the other uses Mg ribbon. With the results from these, we can use Hess’ Law to determine q=∆H. This provides both a safe and successful way of indirectly determining the heat of combustion for magnesium.

To begin Lab 7 of Chem 115, a clean and dry porcelain crucible and its cover were obtained. Next, an iron ring was attached to a ring stand. A clay triangle was placed on top to the ring and a Bunsen burner was placed under the ring. Following the setup for the experiment, the crucible and its cover were placed on the clay triangle and were heated for about five minutes. After, the burner was turned off and the crucible and cover were left to cool to room temperature. Once the crucible and its cover had reached room temperature, tongs were used to move them to a wire gauze. Using the wire guaze, the crucible and its cover were transported to an analytical scale to weigh and record the mass of it. Next, a strip of magnesium was obtained and

How empirical formula of Magnesium Oxide is obtained by heating Magnesium in the presence of air?

This is in follow up to our telephone conversation on 08/22/17 regarding the above-referenced matter. I received your email and have reviewed the file.

Iron can be used for a wide range of resources in the contemporary world. It is the most abundant, least expensive, and most used of all metals. It is vital to human and animal life, and humans use it in a variety of devices to make life convenient. It is combined with other elements to make steel or other compounds for many commercial uses, the most common of which include making fuels, lubricants, automobiles, machine tools, hulls of large ships, building parts, machine parts, cooking pots and pans, cutlery, surgical equipment, and aircraft. Iron (III) “is used in the treatment of sewage, as a dye for cloth, as a coloring agent for paint, an additive in animal feed, and in the manufacture of printed

Mercury is a transition metal that is also known as “quicksilver.” No one is sure who discovered this element. Mercury has been used since ancient times; the Chinese, Egyptians, and the Hindus have been known to use mercury. In 1500 B.C. mercury was found in ancient Egyptian tombs. There also has been writings found that have said “liquid-silver” and “water-silver” written by Aristotle in the fourth century B.C.

Using chemical principles that you have learned this year, explain why you used copper wire to make the basket that held the magnesium in place.