Empirical Investigation Of An Empirical Formula For Magnesium Oxide

2. The second source of error in the lab is when opening the lid of the crucible which allowed smoke of magnesium oxide to escape. During the lab, we removed the lid a couple of times to allow oxygen to enter the crucible so the magnesium reacts with the air to form magnesium oxide. However, the smoke could have easily escaped from the crucible because of the strong force of heat from the laboratory burner. This could have affected the lab results by decreasing the final mass when some of the product have escaped.

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

Although we know that Magnesium was discovered in 1755, the scientist that discovered it is still disputed today. One source reveals, the first person to recognize that magnesium was an element was Joseph Black at Edinburgh (Magnesium). But others accredit Sir Humphry Davy an English chemist, through the electrolysis of a mixture (The Element Magnesium). While the chemist may not be decided on, magnesium has become a very effective substance through history. Magnesium is the lightest metal that can be used to build things, although its use as a structural material is limited since it burns at relatively low temperatures (The Element Magnesium). This became a large benefit to the Germans in WWII. Magnesium-aluminum alloys are used where strong, lightweight materials are required, such as in airplanes, missiles, and rockets (The Element Magnesium). Magnesium can be located on the far left side of the periodic table. It classified under the Alakine Earth Metal family and it is also grouped as a metal (The Element Magnesium).

In this experiment, the empirical formula of magnesium oxide was determined by converting a sample of magnesium into magnesium oxide and then determining the molar ratio of magnesium to oxygen. This ratio was found by placing a sample of magnesium into a crucible then heating it in the presence of air. To ensure that the reaction was complete the crucibles were fired multiple times and also massed between each firing. This reaction then formed magnesium hydroxide (Mg(OH)2) and magnesium nitride (Mg3N2). Water (H2O) was added to these two products in order to create magnesium oxide. By subtracting the mass of the magnesium sample from the mass of the magnesium oxide the mass of oxygen that formed the oxide was determined. The number

This was calculated by taking the mass of 4-tert¬-butylcyclohaxanol, dividing it by the theoretical yield determined by mass of the limiting reagent, 4-tert¬-butylcyclohaxanone, and multiplying by 100. This percent yield is respectable, but a higher one could have been obtained. A source of error resulting in a lower percent yield was the filtering to remove the magnesium sulfate out of the dried organic solution. When filtering, some of the liquid was absorbed into the filter paper, prohibiting some of the product from being recovered. To prevent this loss, one should use a pipet to recover the product from the magnesium sulfate. The product that was recovered during this experiment, was spectroscopically analyzed, and a ratio of cis-trans product was found.

In this lab, we will create a chemical reaction between the reactants oxygen (O2) and magnesium (Mg) using combustion. The product will be magnesium oxide (MgO). In this lab we will record the masses of reactants and products to perform stoichiometry of the chemical equation Mg + O2 -> MgO. The actual yield of product will differ from the theoretical yield based on how the experiment is performed. The independent variable is the product amounts and the dependent variable is the percent yield.

In this experiment, we burned magnesium metal to produce magnesium oxide. To calculate the empirical formula of magnesium oxide, the purpose of our experiment, we weighed the magnesium metal prior to the burning and the resulting magnesium oxide at the end of the burning period. However, since our magnesium was coiled too tightly within the crucible, it did not burn for the entire 45 minutes of the lab, even when we added hydrochloric acid to speed up the reaction. Consequently, our results were erroneous, and we were unable to calculate the actual empirical formula, which is MgO. Therefore, we borrowed the data of another group, and understood that roughly 0.89 moles of oxygen were available per mole of magnesium, yielding the calculated empirical formula as MgO.

The surface area of the magnesium is measured in a simple and acceptably accurate way. One piece of magnesium will be cut up into multiple pieces (2, 4 and 8) as accurately as possible. The Dependent variable in this experiment is the temperature of the chemical reaction produced when magnesium and hydrochloric acid, overtime. This will be measured through probes that are connected to data loggers.

I found your discussion about magnesium highly informative and interesting. You included so many facts about magnesium that I didn’t know. For instance, I didn’t even know the main function of magnesium. Also, I didn’t know that ATP requires magnesium to function. Also I find your “primary deficiency and toxicity conditions” section was very interesting. I also find the different deficiencies very interesting. I also felt better after reading your discussion because I feel as if I am deficient in a lot of vitamins, but you stated that magnesium is present in many different foods. I didn’t know this prior to reading your discussion post, so it relieves some anxieties I have about receiving all of my minerals and vitamins. I also didn’t know

The purpose of this experiment is to determine the mass of a piece of the magnesium, without weighing the magnesium on a balance. To determine the mass of the magnesium, without weighing is to use stoichiometry of a chemical reaction to be able to determine the mass of the magnesium. If the volume of hydrogen gas produced can be determined by using the combined gas law equation, then the mass of magnesium being used can be determined using

Magnesium is a shiny grey solid that assembles to five other elements. Magnesium’s atomic number is 12 and it has 12 neutrons, 12 electrons and 12 protons. Magnesium’s symbol is known as Mg. It is the ninth abundant element in the universe. Magnesium was discovered by Joseph Black in 1775. It was isolated by Sir Humphry Davy in 1808. The name magnesium originates from the greek word for a district in Thessaly called Magnesia. It is related to magnetite and manganese, which too was originated from the area, and used differentiation as separate substances. Magnesium can be found both on Earth and other places in the universe. On Earth, it can be found in the crust as a compound with oxygen. A compound is when two or more elements chemically

In this today’s lab, Percent Yield of Hydrogen Gas from Magnesium and Hydrochloric Acid, the purpose is to study the stoichiometry of H2 produced from the reaction between magnesium (Mg) and hydrochloric acid (HCl). The chemical equation for this reaction is Mg +2HCl -> MgCl2 + H2. It was predicted that 0.0029 moles of hydrogen gas would be formed from 0.07g of magnesium metal and 10 mL of hydrochloric acid. The hypothesis was proven correct based on an actual yield of 0.00299 moles of hydrogen gas. We know this because after measuring the volume and pressure of our results, we used the Ideal Gas Law Equation to calculate the number of moles. We also calculated the percent yield by dividing the experimental number of moles of hydrogen gas

The atomic number of Magnesium is 12. The condensed electron configuration is Ne 3s2. The complete configuration is 1s2 2s2 2p6 3s2. The atomic number of Magnesium is 12. The condensed electron configuration is Ne 3s2. The complete configuration is 1s2 2s2 2p6 3s2. The atomic number of Magnesium is 12. The condensed electron configuration is Ne 3s2. The complete configuration is 1s2 2s2 2p6 3s2. The atomic number of Magnesium is 12. The condensed electron configuration is Ne 3s2. The complete configuration is 1s2 2s2 2p6 3s2. The atomic number of Magnesium is 12. The condensed electron configuration is Ne 3s2. The complete configuration is 1s2 2s2 2p6 3s2. The atomic number of Magnesium is 12. The condensed electron configuration

Water vapor and magnesium oxide on the surface of the magnesium ribbon can cause error in this experiment.

Magnesium is 30% lighter than aluminum and possesses excellent mechanical properties. It has higher weight to strength ratio, damping capacity, dimensional stability, impact and dent resistance when compared to aluminum alloys or steel alloys. These properties have increased the usage of magnesium alloys in the automotive and aerospace industry for weight reduction. But magnesium alloys are often associated with some limitations such as low ductility, lower strength, poor workability (due to hexagonal lattice structure), lower creep resistance and lower corrosion resistance. Alloying with rare earth metals like Gadolinium, neodymium and cerium have