Magnesium oxide

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    Magnesium Oxide Lab Report

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    The burning of magnesium in open air causes a chemical reaction that forms the compound, magnesium oxide. This reaction occurs due to the heat that provides energy to activate the reaction. A blinding white flame will burn as the reaction occurs. In this lab, magnesium is burned in an open crucible over a Bunsen burner several times until the magnesium ceases to burn. This process allows for the magnesium to completely react with the oxygen found in the open air, forming the chemical compound magnesium oxide. However, our lab did not provide us with the hypothesized results, as no reaction occurred when the magnesium was burned, potentially due to an error in the process. The purpose of this lab is to identify and examine the oxidation-reduction…

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    Abstract: In this lab our main objective is to find the empirical formula of MgO, magnesium oxide. To do this first we have to make sure when we burn Mg in the crucible and it reacts to with O. This lab experiment Mg is complicated by another factor. Mg is so reactive that it reacts with N in the air so some of the Mg which is suppose to react with O will react will N instead. This obstacle can be overcome by simply adding water to the Mg3N2 to yield MgOH2 and NH3. This will undo the reaction so…

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    Title Determining the Empirical Formula of Magnesium Oxide Introduction Chemical formulas imply the arrangement of compounds. Empirical formulas are the simplest whole number ratio of the elements present in a compound (Owen, 2014). However, the actual amount of each type of atom that a compound is consisted of is called the molecular formula. For that reason, the deduction of the empirical formula and the molar mass of a compound is required to determine the molecular formula of the compound.…

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    In part C, the enthalpy of formation of magnesium oxide was found by adding together three reactions, as shown in the table below. Experiments were performed to obtain the ΔHrxn value of the first two reactions in the table, which were reactions 4 and 5 respectively in the experimental section, while the ΔHrxn for the third reaction in the table was provided. Using the ΔT obtained experimentally, heat energy (q) was determined using the equation q = mCΔT + CΔT where q was the heat, m was the…

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    percentage composition of magnesium and oxygen in magnesium oxide and evaluate if the composition varies or remains constant. To test this, magnesium was heated and made to react with the oxygen gas in the atmosphere. This reaction formed the ionic compound, magnesium oxide. The percentage composition was later calculated based on the results of the experiment as shown in the above calculations, Figure 4. These results were compared to the expected percentage composition also calculated in…

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    (Maximum length 1 page including chemicals equations) The hypothesis of this experiment is that empirical formula is going to be close to a ratio as 1:1, because that is the theoretical empirical formula for the compound magnesium oxide. Empirical formula is simplest formula for a compound, it is the smallest possible whole- number ratio of subscripts of the elements in the formula. Generally, this the same thing as its simplest molecular formula, this is generally the actual number…

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    If heating magnesium in the presence of oxygen and they react completely, then the ionic compound’s empirical formula can be found using this equation by calculating the masses of magnesium and oxygen in this equation: Mg + O2 → MgxOy Since an ionic compound is the hopeful result of this lab, an ionic compound is a chemical compound comprising ions, which ions are an atom or molecule with a net electric charge due to the loss or gain of an electron. Ions can be negatively charged and called…

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    In this lab, students learned that in a combination reaction, two or more substances react to form one substance. This can be seen in reaction #2. In reaction #2, magnesium reacts with oxygen to produce magnesium oxide. Although the students can only see magnesium and magnesium oxide, the students were informed on the lab sheet that oxygen was also one of the reactants. This reaction allowed students to see how two substances, magnesium and oxygen, react to produce one product, magnesium oxide.…

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    There are five common ways to predict the product of chemical changes. They are synthesis (composition), decomposition, single replacement, double replacement, and combustion. Each can be used for different types of problems based on the equation of experiment presented to you. They can also be found using observations throughout the experiment. You use these base guidelines to write a well balanced equation with physical states and all of the reactants and products that are produced. Our…

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    The powder do not affect the chemical structure of the magnesium in the fire extinguishing process. However, a protective coat of magnesium oxide is formed on all the surface of the magnesium as it reacts very fast with air. This layer makes it hard for it continue burning. However, in case water is used when removing the residues even after several days, the fire may reignite. The water will firstly expose the surface of the magnesium residues to reaction and react with it (magnesium) to…

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