exo-norborneol was produced by a hydration of alkenes by using an acid and excess water. Hydration of alkenes is the acid-catalyzed addition of water to a carbon-carbon pi bond that leads to the formation of an alcohol. Norbornene is a bridged cyclic hydrocarbon‚ this molecule contains a double bond that induces significant ring strain‚ and therefore‚ it is highly reactive. In order for this reaction to occur‚ equilibrium must be established between the hydration and dehydration processes. To drive
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Many nurses are weak with drug calculations of all sorts. This article will help to review the major concepts related to drug calculations‚ help walk you through a few exercises‚ and provide a few exercises you can perform on your own to check your skills. There are many reference books available to review basic math skills‚ if you find that you have difficulty with even the basic conversion exercises. Common Conversions: 1 Liter = 1000 Milliliters 1 Gram = 1000 Milligrams 1 Milligram = 1000
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Copper is an element that occurs in minor amounts in the earth’s crust. Estimates of average crustal prevalence are on the order of 0.0058 percent by weight. Deposits considered to be economically recoverable at current market prices may contain as little as 0.5 percent of copper or less‚ depending on the mining method‚ total reserves‚ and the geologic setting of the deposit. Here is the flow sheet on how to process copper from Zenith. Copper Process Flow Sheet: Copper ore is first quarried from
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Chemistry Internal Assessment: Determining the Enthalpy Change of a Displacement Reaction AIM: To determine the enthalpy change for the reaction between copper(II) sulfate and zinc. BACKGROUND THEORY: Bond breaking is endothermic while bond forming is exothermic. The reaction between copper(ll) sulfate and zinc is exothermic as the energy required to form the bonds of the products is greater than the energy required to break the bonds of the reactants. In an exothermic reaction‚ heat is
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of MgO‚ using a calorimeter and determining the enthalpy of two reactions. Applying Hess’ law we were able to determine the standard heat formation of MgO. Introduction Energy exchanged in a chemical reaction can either be in the form of heat or light. If light is involved a glow is seen‚ if heat is involved the temperature of the system will change(lab manual page 35). The amount of heat exchanged under constant pressure is called the enthalpy change‚ this can either be endothermic or exothermic
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Yr: 2014 Yr: 2013 Remarks 1.1 Profitibality Ratio 1.1.1 ROE= x 100 = 10.71% x100 = 10.30% Higher the better 1.1.2 ROTA= x100 = 18.27% x100 = 19.45% Higher the better 1.1.3 GPM= x100 = 71.67% x100 =70.35% Higher the better 1.1.4 OPM= x100 =28.72% x100 =29.79% Higher the better 1.1.5 NPM= x100 =43.48% x100 =39.46% Higher the better 1.1.6 NPM= x100 =38.74% x100 =35.04% Higher the better 1.2 Asset Utilisation 1.2.1 TA TURN= x100 =18.27% x100 =19.45% Higher the better 1.2.2
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Sample Calculations I-Beam (S8x18.4) Dimensions: D= 8 in; h= 7.148 in; bf= 4.001 in; tw= 0.271in; tf= 0.426in; L (length of the beam) =18.4 in I= (bf*D3 – h3 (bf – tw))/12= 57.6 in4; E (Referenced value of Young’s modulus) = 29X106 psi Theoretical Strain: ε= σ/E= (M*y)/(E*I) P = load a = distance from support to the applied load (48 in) y = distance from neutral axis to the extreme element in y-direction The sing in the theoretical strain (±) determines if the strain is in compression
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CALCULATIONS Determining the amount Limiting Reagent used. nlimiting reagent = Molarity x Volume or Mass / Molar Mass Example: Limiting reagent is 5mL of 1.0 M HCl nlimiting reagent = Molarity x Volume nlimiting reagent = (1.0 [mol/L]) x 0.005 [L]) = 0.005 mol Determining the qrxn and qcal. qrxn + qcal = 0 -qrxn = qcal qrxn = ΔHrxn x nlimiting reagent qcal = Ccal ΔT qrxn = - Ccal ΔT + mcsolid ΔT (note: only if there is a precipitate formed in the reaction)
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3rd‚ 2009 Lab Report #3: Copper Cycle Abstract: The purpose of the experiment is to cycle solid copper through a series of five reactions. At different stages of the cycle‚ copper was present in different forms. First reaction involves reaction between the copper and nitric acid‚ and copper changed from elemental state to an aqueous. The second reaction converted the aqueous Cu2+ into the solid copper (2) hydroxide. In the third reaction Cu(OH)2 decomposed into copper 2 oxide and water when heated
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Capacity for a Calorimeter and of the Enthalpy of an Acid-Base Reaction Abstract The purpose of this lab was to first‚ determine the specific heat capacity of a homemade calorimeter‚ and second‚ to calculate the enthalpy of reaction for an acid-base reaction between 6M KOH and 6M HNO3. To determine the specific heat capacity of the calorimeter‚ two differing temperatures of water were measured and volume was measured and mixed within the calorimeter. The enthalpy of reaction for an acid-base reaction
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