energy than the reactants Enthalpy changes are normally quoted at standard conditions. Standard conditions are : • 1 atm pressure • 298 K (room temperature or 25oC) • Solutions at 1mol dm-3 • all substances should have their normal state at 298K Standard enthalpy change of formation In an exothermic reaction the ∆H is negative In an endothermic reaction the ∆H is positive When an enthalpy change is measured at standard conditions the symbol is used Eg ∆H The enthalpy of formation of an element
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this laboratory was to use two different techniques to attempt to identify the melting point and the mole ratio of hydrated water to anhydrous aluminum‚ potassium‚ and sulfate of AlKSO4. The hypotheses were: if the alum was put in a capillary tube the melting point of alum will be able to be determined; and the water of hydration in alum crystals will be possible to determine if the alum is heated with a Bunsen burner. Results: Part 1: Data Table | Trial 1 | Trial 2 | Measured Melting
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anode | Glucose (C6H12O6) | No | Nothing changes | Nothing changes | Dilute Sulfuric Acid (H2So4) | Yes | Bubbles | Bigger bubbles | Sucrose (C12H22O11) | Yes | Light bubbles | Light but more visible bubbles and light brown liquid | Copper Sulfate (CuSo4) | Yes | Light bubbles | Changes color to brown and oxidation is observed | Ethanol (c2H5OH) | No | Nothing changes | Nothing changes | Calcium Hydroxide (Ca(OH)2) | Yes | Light bubbles | Light bubbles but more than in anode |
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(l) Water is added to make a pumpable slurry. Flotation (separation of valuable content) Cu2S(s) + H20 (l) CaCO3(s) (added to give a basic PH level) pine oil or C2H5OH (liquid called a frother) C3H5KOS2 (potassium amyl xanthate to make the copper particles cling to the bubbles as they rise to the surface) O2 (pumped into bottom of tank‚ agitates soloution and starts to froth‚ bringing bubbles to the surface) Cu2S particles adhere to the bubbles‚ which is separated from the liquid‚ tailings
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REPORT OF INDUSTRIAL VISIT Letter of Transmittal 31-Oct-2013 To The Head of the Discipline Chemistry Discipline Khulna university‚ KHULNA Dear Sir‚ Sub: Report of the One – Day industrial visit On receiving the letter of permission from Bashunddhara Cement Industries Ltd. Mongla‚ students of Chemistry Discipline with five faculty members went on an industrial visit Bashunddhara Cement Industries Ltd. Mongla on 05-010-13. We all assembled at the university at 8 a.m. and left the university
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Copper (II) Sulfate Purpose: The purpose of this lab is to find out how many moles of water there are in one mole of Copper Sulfate (CuSO x HO) and the percent by mass of water in the hydrate. This will be accomplished by heating a determined mass of the hydrate to remove the water‚ and by measuring the salt left over. Introduction: This laboratory experiment will be done to find out how many moles of HO are present per one mole in the hydrate CuSO. A hydrate is a compound that has a fixed number
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Introduction : Copper(II) sulphate‚ is a type of salt which it is formed by combining both copper ion and sulphate ion through the experiment of double displacement between dilute sulphuric acid ‚ and copper(II) carbonate ‚ . Through this process‚ the copper ion will displace the hydrogen ion as it is more electropositive and sulphate ion will displace carbonate ion as it is more electronegative. The resulting copper (II) sulphate solution when cooled can easily crystalize
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6. (2) By Dehydrogenation of 2-proponal The hydration of propene [115-07-1] gives 2-propanol [67-63-0]‚ which is then dehydrogenated to acetone. In the United States a C3 stream containing 40 – 60 % propene is used for the manufacture of 2-propanol. A large number of catalysts for 2-propanol dehydrogenation have been studied‚ including copper‚ zinc‚ and lead metals‚ as well as metal oxides‚ e.g.‚ zinc oxide‚ copper oxide‚ chromium-activated copper oxide‚ manganese oxide‚ and magnesium oxide. Inert
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The purpose of this lab was to find out the reaction of iron nails and CuSO4‚ copper sulfate solution. Before starting the experiment‚ there were two possible outcomes of the reactions. CuSO4 + Fe → FeSO4 + Cu or 3CuSo4 + 2Fe → Fe2(SO4)3 + 3Cu. The ion chart showed that iron can only make two charges‚ +2 and +3. As the liquid evaporated‚ the weight changed because the liquid added to the nail’s weight. In a real world situation‚ scientists can use ratios to determine how much of a substance that
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with the dried sample‚ which will produce elemental copper. By measuring the mass of copper that forms‚ you will have the necessary information to determine the moles of copper and chlorine in your sample‚ and you will be able to establish the proper chemical formula. OBJECTIVES • • • In this experiment‚ you will Ev al Determine the water of hydration in a copper chloride hydrate sample. Conduct a reaction between a solution of copper chloride and solid aluminum. Use the results of the
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