Oxide Essays

This investigation is about proving the formula of magnesium oxide by making magnesium oxide. The first reactant of the experiment is magnesium metal (Mg) and oxygen (O2), the oxygen will be in the air and provide oxygen atoms for the formation of magnesium oxide (MgO), which is the product of this experiment (In association with Nuffield Foundation). We are performing this experiment to improve our critical thinking skills as we will have to analyse the data and results to form conclusions, and

Calculations: how did we calculate and determine the mass of magnesium oxide? we Determined the mass of MgO (magnesium oxide) by subtracting the mass of the crucible with lid on from the mass, weight of the crucible with lid, and magnesium oxide. then in order to determine the oxygen mass, we will subtract the mass of the magnesium from the mg oxide to find out the amount of magnesium in the compound, divide the mass of Magnesium ( numbers of grams in one mole of magnesium we did the same way to

Steel wool Magnesium oxide powder 10 to 15cm strip of magnesium ribbon 100mL graduated cylinder 1.00 mol/L hydrochloric acid 3 Styrofoam cups (calorimeter) Eye dropper Mass scale GLX temperature probe Fume hood Procedure A length of a 0.5g magnesium strip was polished using steel wool 1.00 mol/L hydrochloric acid was obtained from the fume hood 1.00 mol/L hydrochloric acid was added to the graduated cylinder to measure at 100

independently discovered oxygen, They were both able to produce oxygen by heating mercuric oxide (Hg0) . Oxygen is a highly reactive element and is capable of combining with other elements . It is required by most living organisms and for most forms of combustion . Oxygen and Magnesium combine in a chemical reaction to form this compound. When the magnesium metal burns it react with oxygen found in the air to form Magnesium Oxide. Mg loses the electrons to have an octet , Oxygen gains two electrons to have an

atomic number is12. Also, magnesium is a very reactive metal, and in the free state does not exist in nature. It has a very slow reaction rate with cold water, and a very fast speed with hot water. Magnesium oxide process is very fast, if left it open, it would forming a layer of magnesium oxide on the surface of the metal. Magnesium also burns very rapidly when it's at room temperature. The combustion process is very intense, and

The labs purpose is to determine magnesium oxides percent yield. In this lab we will create a chemical reaction when two solutions are mixed. Those two solutions are magnesium and oxygen in the reaction Mg + O2 MgO. After these two solutions are mixed, magnesium oxide is produced. The percent yield of magnesium oxide is calculated and reported in this activity. The percent yield is dependent variable and the product amounts is the independent variable in this experiment. Stoichiometry is a method

table. It has an atomic mass of 24.305g and is the 8th most abundant element in the Earth’s crust. When metal magnesium is heated and in the presence of oxygen, a combustion reaction occurs and the product of this exothermic reaction is magnesium oxide. It can also be observed that while this reaction is in progress, a bright, white light is emitted (Ophardt, 2001). Oxygen, O, is a Group 16 element with an atomic number of

Titanium Dioxide (TiO2) is known as the ultimate white pigment because of its high refractive index and also its brightness. This dust is naturally occurring from the oxides of titanium. This compound has many application uses. These include Paint manufacturing, food coloring, sunscreen products and the Pharmaceutical industry to name a few. According to the IARC (International Agency for Research on Cancer), it is classified as a Group 2B Carcinogen, basically it states that it is potentially cancerous

In order to create 5 grams of MgSO4 from MgO (Magnesium Oxide) and H2SO4 (Sulfuric acid), we needed to create a balanced equation to find the amount of other chemicals we would need. The balanced equation was MgO + H2SO4 --> MgSO4 + H2O. After creating a balanced equation, we found the amounts of MgO and H2SO4 using stoichiometry. The amount of Magnesium Oxide was 1.674 grams and the amount of Sulfuric acid was 6.923 milliliters. In order to create as close to 5 grams of MgSO4 as possible, we decided

chemical reactions to create solid magnesium oxide with the aim being identifying the percent composition and empirical formula of the compound. Background Information : To determine magnesium oxide’s percent composition and empirical formula, the masses of magnesium and oxygen separately must be found and then divided by the total mass and multiplied by 100 to find the percent makeup of each element within the compound. However, to obtain magnesium oxide, it had been synthesized from magnesium and

Magnesium Oxide: Percent Composition and Empirical Formula Lab Report Andjela Mandic 10/28/14 Period 1  Purpose The purpose of this lab was to find the percent composition as well as the empirical formula of magnesium oxide. Data Mass Description Trial 1 (Emily’s Group) Trial 2 (Tom’s Group) Trial 3 (Sara’s Group) Mass of crucible, cover, & magnesium 38.8g 38.80g 37.446g Mass of crucible & cover 38.4g 33.52g 37.156g Mass of magnesium 0.34g 0.289g 0.29g Mass of crucible, cover, & magnesium oxide 37

started to use. I quickly paused the experiment once I noticed the rubber tongs were gluing together. This minor mistake is avoidable and easy to fix. Our first conclusion was that magnesium burns to form new compounds. It reacts with oxygen to form oxides of each metal. This was an example of combustion and combination/synthesis reactions. Next, was the CuCO3 reaction, where we used a wood splint to discover that CO2 gas was present. After we

Calorimetry 1 The purpose of this experiment is to identify the mystery metal given to us (metal A). We are going to identify the mystery metal by looking at both its physical properties as well as its heat capacity. The heat capacity of the metal will be calculated using a setup/method described below. We will also look at the physical properties of the metal such as its magnetic properties, density, whether it is lustrous or dull, etc. by observation. Our mystery metal is not very lustrous and

Conclusion: Every compound has a uniquely identifying molar mass as well as individual properties. In this lab, the purpose was to use the properties that three unknown alkali metal carbonate powers have, to identify the molar mass. For the three unknown substances, they all were white powders of about the same texture, and they all reacted when added to hydrochloric acid. Based on these properties, it is impossible to distinguish which one is which due to the similarities, so it is necessary to

Question. How can nitric oxide production from perfused organs be determined? Problem. It is thought that Nitric Oxide is important in signalling between neurons as well as in the vascular endothelium. NO plays a key role as the endothelium-derived relaxing factor (EDRF), which regulates vascular constriction and relaxation and is thus highly correlated with perfused organs (1). Since nitric oxide is so important in the vascular system, a sensitive and specific method is needed to detect it in

Name: Avishak Deb Roy Partners: Leevell Penn, Varugh, Butler Bio 101 Lab Report #1 02.22.2018 Swimming speed of paramecium tetraurelia in different levels of treatment. Introduction Paramecia is a unicellular Protista which are naturally found in aquatic habitats. It is easily cultured in the laboratory. It is oblong shaped and covered with short hairy structure called cilia. Paramecia does not pose any health or ethical concerns and the population can be maintained if there is a

Fig shows 3.13 powder diffarction pattern (it shows diffraction lines and holes for incident and transmitted beam) If a powdered specimen is used,instead of a single crystal,then there is no need to rotate the specimen,because there will always besome crystal at an orientation for which diffraction is legitimate.Here a monochromatic X ray beam is incident on a powdered or polycrystalline sample.This method is use ful for samples that are difficult to obtain in single crystal form. The powder method

The central purpose of this experiment was to determine the experimental empirical formula of an oxide of magnesium by performing a synthesis reaction. It was hypothesized that the formula that was derived from the recorded data would be identical to the theoretical empirical formula. After performing calculations with the data that had been collected within the duration of the experiment, it was deduced that the empirical formula of the product generated by the synthesis reaction was Mg5O6. Since

. Experimental 2.1 Catalyst preparation In this paper we have to use different types of nitrate precursors to preparation of the catalysts. The precursors we used to preparation of the catalysts are cobalt nitrate, cerium nitrate, copper nitrate and manganese nitrate. All the chemicals are used for manufacturing of the catalyst are A.R. grade and they are purchased from Otto Chemie Company. The different types of nitrate precursors was used to preparation of the catalyst and they are dried at 120°C

Determination of the molar mass of magnesium Aim To determine the molar mass of magnesium with the ideal gas equations and Dalton’s law about partial pressures. Materials and chemicals gas measuring tube 50.0cm3 graduated cylinder 1000.0 cm graduated cylinder 10.0cm3 cork with a hole copper wire thermometer barometer magnesium ribbon HCL 35% (concentrated) Background theory Dalton’s Law of Partial states that the total pressure of a gas is equal to the sum of pressure of each individual