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Magnesium Burning Lab Report

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The magnesium burned did not leave significant odor like matches or candles do because it reacts with the oxygen, which is present within the air. This means that it's not necessarily reacting with the fire as the candles or matches do. Thus, magnesium and oxygen reacting together makes the compound, magnesium oxide as a result. The only reason why is looks likes it's burning is due to the fire is because the reaction between magnesium and oxygen, as they create the heat. This results the bright lighting like that of fire. This relates back to the chemical equation because there is a combustion reaction between oxygen and magnesium. This combustion reaction is the whole entire reason as to why energy is given off and then the magnesium metal
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Chemical compounds that are available to determine are CaCO3, CaCl2, Ca(NO3)2, mgCl2, MgSO4, KCl, HCl, HC2H3O2, KNO3, K2SO4, NaC2H3O2, Na2CO3, NaCl, Na2SO4, HNO3, H2SO4, HNO3, H2SO4, NH4Cl, (NH4)2SO4, K2CO3, 0.1 M AgNO3, 0.2 M BaCl, Mg(s), NaOH, and KOH. To start this experiment, start with the flame test by gathering a Bunsen burner and a Nichrome wire. Connect the Bunsen burner with a rubber tube to a laboratory gas. To prepare solutions for the flame test, weigh out 0.205 gram of Unknown Compound using an analytical balance and mixed it into a 140 mL beaker filled with 20 mL ionized water. Ensure that solid is completely dissolved using a stirring rod.

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I, myself, can think of many possibilities of what caused the fire. One possibilities could have been that he was making something on the stove and didn’t notice and/or didn’t smell something weird. Another possibility is that the smoke detector

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This was displayed in table 1, where the final temperatures of the water are lower compared to the initial temperatures, showing that the potassium chloride took heat energy away from the 20 mL of water. Endothermic deicers work slower than exothermic deicers, because endothermic deicers require warmer temperatures to dissolve, which makes them inferior when environmental temperatures are very low. Additionally, exothermic deicers will release energy as heat when the compounds dissociate, consequently, melting snow and ice faster.4 Furthermore, when comparing the enthalpy of dissolution of potassium chloride to magnesium chlorides value of -270, the most exothermic value in table 2, potassium chloride is shown to be a significantly worse deicer. Magnesium chloride being notably exothermic means that the compound can dissolve at low temperatures and releases copious amounts of heat

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647 Words | 3 Pages

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 37.518g 33.92g 37.640g Mass of magnesium oxide 0.441g 0.44g 0.484g Mass of combined oxygen 0.156g 0.16g 0.194g *Ignition failed, so all data was taken from groups for which ignition occured. Observations:

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In addition, properties such as color and magnetism provide additional identification. Keywords: combustion, steel wool, iron, magnetite, ferric oxide When a candle burns, the wax disappears. When wood burns, the wood is reduced to ash to about ten percent of its

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This occurs since the heat is transferred to the surroundings, not all of the energy released from the reaction would have been transferred to the solution. The calculated enthalpies of reaction would be smaller than the accepted value. MgO on the surface of the magnesium ribbon would result in lower ∆H and ∆T values. The calculated enthalpies of reaction would be inaccurate since the excess MgO would render the Mg impure and yield false results. The enthalpy of combustion for Mg would not be accurate since the MgO coating would also contribute to the mass of the magnesium ribbon.

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It was found that the reaction was limited to taking place to only the mouth of the test tube, as it is the only place where a mostly yellow and orange flame burned, which was opening downwards. The part of the flame that is furthest from the mouth glowed blue. During the reaction, very little sound was produced to the extent that one can only hear it in a quiet room. In addition, very large amounts of black soot was produced continuously throughout the entire reaction, which congregated towards the mouth of the test tube so that the amount of soot decreased as the distance between it and the mouth of the test tube

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The purpose of this lab was to determine the percent water in magnesium sulfate heptahydrate, or Epsom salt. The experimental percent water is determined to be 42.06% in both trials, making the average also 42.06%. To determine this percent water a heating and cooling procedure was used. First, the vials were cleaned of impurities using the lab oven and were not touched after this point.

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Since less energy is produced from the reaction, a yellow flame (often called a “safety flame”) is produced. . The yellow flame is also brighter than the blue flame because the specks of carbon glow when heated (BBC

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My knowledge of heat transfer in a lava lamp before instruction was that waves of electricity was sent through the power cord and heated the lamp. This would then heat the wax in the lamp causing it to bounce around the lamp. I did not know the amount of wax a lava lamp contained, but after seeing a lamp that has not been plugged I was quite surprised. I had believed there had only been a couple of tablespoons within the lamp, but that is because a lot of the wax sits at the bottom. Also, I did not know lava lamps contained wax I believed it was a gummy substance that was not very dense, which allowed it to more around easily.

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This measurement is accurate to Dr. Wile’s description of the outcome. He said, “Metals have small specific heats, so it [the answer] should be less than 1 J/g˚C.” Calorimetry is the science of determining the changes in energy of a system by measuring the heat exchanged with the surroundings. Calorimetry experiments are performed in order to determine the heat flow between two substances and a calorimeter is used. A calorimeter is a device that is used to measure the amount of heat transferred to or from an object. The science of calorimetry is that the energy gained or lost by the water is equal to the energy lost or gained by the object.

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Valenzuela et. al. (1995) [100] has proposed a hydrometallurgical procedure for the separation of molybdenum from Chilean molybdenite concentrate. The molybdenite concentrate was first leached with nitric acid originated from the reaction of NaNO3 and H2SO4, which provided a solid phase, composed of MoO3 and residual solution. Molybdenum was separated with alkylphosphonic acid PC-88A by solvent extraction method, from the leach liquor containing copper, rhenium and iron among other impurities.

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