common alternate form of thermite. List of different ‘thermites’: Iron (III) oxide (Red): Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(l); ΔH = -847.6 kJ/mol The ratio of Iron (III) oxide to Aluminum powder by mass is about 3:1. This is the reaction I chose to do. Iron (II‚ III) oxide (Black): 3Fe3O4(s) + 8Al(s) → 4Al2O3(s) + 9Fe(l); ΔH = -3347.6 kJ/mol The reaction using Fe3O4 (-3347.6kJ/mol) produces a substantially larger amount of energy than the reaction using Fe2O3 (-847.6kJ/mol). the
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Entropy Spontaneous Reactions: reactions that given the necessary Ea‚ proceed to completion without continuous assistance Enthalpy and Spontaneity * exothermic reactions tend to be spontaneous * Endothermic reactions can be either * Electrolysis of water is non-spontaneous it will stop if you stop the supply of energy * DD reaction between ammonium nitrate and barium hydroxide is spontaneous‚ even through the Entropy * Measure of disorder or randomness * Can apply to
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H2O2(l) H2O(l) + 1/2 O2(g) The equations are: 1 H2(g) + O2(g) H2O2(l) 2 H2(g) + 1/2 O2(g) H2O(l) Hf = 188 kJ Hf = 286 kJ Solution: Sample Problem 2: Use the following equations: 1 1/2 N2(g) + 3/2 H2(g) NH3(g) 2 1/2 N2(g) + O2(g) NO2(g) 3 H2(g) + 1/2 O2(g) H2O(g) Hf = 46.0 kJ Hf = +34.0 kJ Hf = 242.0 kJ to calculate the enthalpy of reaction
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during‚ and after a reaction of Sulfuric acid and Magnesium ribbon takes place in the calorimeter reaction test tube. Two trial experiments were preformed. The average of both trials was calculated to be -363.67 kJ/mol‚ which is compared to the theoretical yield of enthalpy change; -464.2 kJ/mol. Lab partner was John Grek. Results: Table 1 Change in volume in calorimeter after adding magnesium ribbon to Sulfuric acid
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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 = 0 kJ mol-1 Standard enthalpy change of combustion The standard enthalpy of combustion of a substance is defined as the enthalpy change that occurs when one mole of a substance is combusted completely under standard conditions. (298K and 1 atm)‚ all reactants
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Tara Keller Finding the Ratio of Moles of Reactants in a Chemical Reaction 9/6/13 Introduction The purposes of this lab are to measure the temperature change of the reaction between solutions of sodium hydroxide and phosphoric acid‚ calculate the enthalpy‚ H‚ of neutralization of phosphoric acid‚ and compare the calculated enthalpy neutralization with the accepted value. Theory Calorimetry is the measurement of change of heat in a reaction. A calorimeter is a tool to measure the amount of
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16-1 Solutions Manual for Thermodynamics: An Engineering Approach Seventh Edition Yunus A. Cengel‚ Michael A. Boles McGraw-Hill‚ 2011 Chapter 16 CHEMICAL AND PHASE EQUILIBRIUM PROPRIETARY AND CONFIDENTIAL This Manual is the proprietary property of The McGraw-Hill Companies‚ Inc. (“McGraw-Hill”) and protected by copyright and other state and federal laws. By opening and using this Manual the user agrees to the following restrictions‚ and if the recipient does not agree to these restrictions‚ the
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the equation. T = H°S°. Calculation Plug in the values of the class average from Table 2. T = 65.750 kJ/mol196.735 J/molK T = 0.334 kJ/K Convert kJ to J T 334K or 61°C Above this temperature‚ the dissolution of borax in water will no longer be spontaneous. Theoretical H° and
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CHAPTER 1 PRODUCTION 236250 TONNES PER YEAR OF ACETONE 1.0 INTRODUCTION Acetone is a clear‚ colorless‚ volatile liquid with sweer odor. It is both the simples aliphatic ketone and the most commercially important. It has a distinctive fruity or mint-like odor and a pungent taste. It is also found naturally in plants‚ tress‚ volcanic gases‚ and forest fires and as a by product of the breakdown of body fat. Nearly all world production of acetone is via cumene peroxidation‚ as a coproduct with
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Dr. Bolaños CHEM 110 - Exam #3 Fall 2010 Student Number _____________________ Name:________KEY_____________________________ There are 11 questions totaling 104 points (8 pages). PLEASE look over the entire examination BEFORE you begin to ensure your packet is complete. REMEMBER: The best place to start your exam may not be at the beginning! You have 2 hours to complete this examination and may only use a basic scientific calculator and the periodic table provided. All work must be shown
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