reaction of sulfuric acid in a reaction with magnesium to produce magnesium sulfate. Through the use of an ice calorimeter‚ the rxn H° D for this reaction is determined to be 1 360kJ mol − − × . Introduction: This report details an experiment in thermochemistry. Included are the methods‚ results‚ and interpretation of results of an experimental determination of an enthalpy of reaction. The reaction being studied is between sulfuric acid‚ and magnesium metal. ( ) ( H2SO4 aq +Mg s)®H2 ( g )+MgSO4
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This technique is known in the mining industry as solution mining. The soluble copper is then filtered to remove unreacted ore (the residue) from the filtrate containing the copper+2 ion. The copper in the filtrate is then treated with metallic magnesium to precipitate the copper as the familiar orange-brown metal. This copper is dried and weighed. From these data the percent copper in the original ore can be determined. In this experiment you will use many of the concepts and techniques you have
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Lenny Parisi March 2‚ 2015 Mrs. Miller S period The plane crash‚ the storm‚ the heat‚ the unmanageable fear of the beast‚ and the lack of food and water. These are the conditions these boys were living in during their time on the island. Ladies and gentlemen of the jury‚ these boys have killed. Do you really think these seven to twelve year old children intentionally committed murder? The horrible conditions drove them to an unstable state of mind and greatly affected the decisions they made. Prosecutors
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by measuring the differences in the mass of the hydrous and anhydrous salt. By using this mass‚ the percentage of water‚ the number of moles and the complete formula of the salt were derived. HYPOTHESIS- If the water is driven off of hydrated magnesium sulfate‚ then it would be colorless because it is made of Group 2 metals‚ which do not form colors. OBJECTIVES- a) To use the method of “weight by difference” to determine mass quantities. b) To determine the mass of an anhydrous salt by heating
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reactions formed between various acids and bases with the aid of indicators. Equipment: 1. Safety goggles. 2. Droppers. 3. Red Litmus paper. 4. Blue Litmus paper. 5. pH paper. 6. Well plate. 7. Micro spatula. Materials: 1. Zinc. 2. Magnesium. 3. Iron. 4. Copper. 5. HCL. 6. HC₂H₃O₂. 7. NaOH. 8. Phenolphthalein. Procedure: Part A: 1. Add five drops of HCL‚ HC₂H₃O₂‚ and NaOH to different depressions in the well plate. 2. Place a drop of each solution onto a piece of red litmus
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various metals by observing their reaction with hydrochloric acid. Materials: 2 M hydrochloric acid Detergent Test tubes and test tube rack 0.5 pieces of magnesium‚ aluminium‚ iron‚ zinc and cooper Sand paper Ruler Timer Bench mat Method: 1. The surface of the magnesium was cleaned with a piece of sandpaper 2. The Magnesium was placed into a test tube 3. Three Drops of detergent were added to the test tube 4. 2cm of hydrochloric acid was added to the test tube 5. The timer was set
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wetlands that had outflowing streams. Finally‚ mean ammonium and phosphate availability was generally higher in groundwater-dominated systems‚ whereas all precipitation dominated wetlands had low nutrient availability. In respects to the dissolved magnesium used in the study‚ Thobaben and Hamilton believe that Mg2+ is useful for the hydrogeomorphic classification of wetlands in glacial landscapes where carbonate minerals impart high Mg2+ concentrations to groundwater. Therefore‚ Thobaben and Hamilton
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CO2(s) C(s) + 2MgO(s) Magnesium is a stable element and reacted violently with the liberation of much heat through combustion. The magnesium ribbon burned inside the dry ice (CO2(s)) mainly because it combined with oxygen in CO2 thus leaving elemental carbon behind. The Mg ribbon burned in air resulted to the formation of the white product (MgO) while the rest of the Magnesium ribbon that burned between the two slabs of dry ice resulted to a black product (C(s)). The Magnesium had been oxidized and
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Introduction The objective of this experiment is to combine Magnesium (Mg) with hydrochloric acid (HCl) to determine the molar volume of hydrogen gas (H2) (converted to the molar volume at STP) and then‚ to compare obtained results with the molar volume of an ideal gas. To determine the measured molar volume of hydrogen gas‚ we are going to use this equation: The molar volume of the ideal gas will be determined by the equation ‚ where T = 237 K‚ P = 101.3 kPa. The hydrogen gas will be collected
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Aim: To examine a number of different chemical reactions and determine if they are exothermic or endothermic. Apparatus: • Test tubes {Around 10-12 in number} • Test-tube rack • Spatula • Digital thermometer { ± 0.1° C} • Digital balance {± 0.01 g} • Measuring cylinder {± 0.5cm³} • Different chemicals Introduction/Theory: Exothermic reactions are those reactions that release energy in the form of heat. Endothermic reactions need to absorb energy in the form
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