Accepted Manuscript Title: Kinetic studies of the Decomposition of Flame Retardant Containing High Impact Polystyrene Authors: Guido Grause‚ Jun Ishibashi‚ Tomohito Kameda‚ Thallada Bhaskar‚ Toshiaki Yoshioka PII: DOI: Reference: To appear in: S0141-3910(10)00062-5 10.1016/j.polymdegradstab.2010.02.008 PDST 5967 Polymer Degradation and Stability Received Date: 17 December 2009 Revised Date: 2 February 2010 Accepted Date: 7 February 2010 Please cite this article as: Grause G‚ Ishibashi J‚ Kameda
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that is very volatile‚ it evaporates quickly because the carbon parts of ethanol can’t hydrogen bond‚ therefore its hydrogen bond isn’t as strong as water and so it evaporates faster (wisteme.com) Its latent heat of vaporisation is 846 kJ/kg while water’s is 2257 kJ/kg. It is also the most common type of alcohol used in alcoholic beverages. Its molecular formula is C2H5OH and it also has the empirical formula C2H6O. It is a very miscible solvent which means it is a very versatile solvent‚ able to
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52 Chemical Bonding and Molecular Structure 53 I. Structure of Matter (20%) B. Chemical bonding 1. Binding forces a. Types: ionic‚ covalent‚ metallic‚ hydrogen bonding‚ van der Waals (including London dispersion forces) c. Polarity of bonds‚ electronegativities 2. Molecular models a. Lewis structures TYPES OF CHEMICAL BONDING Ionic Bonding - two atoms of opposite charge electrically attracted to one another Covalent Bonding - two atoms each sharing electrons within a molecular orbital Metallic
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CHM 096 TUTORIAL 2 (Chemical Equilibrium) 1. Write the equilibrium constant expression‚ Kc‚ for each of the following reactions: a) 2NO(g) + O2(g) ⇄ 2NO2(g) b) The decomposition of solid potassium chlorate to solid potassium chloride and oxygen gas. c) 4HCl(g) + O2(g) ⇄ 2H2O(g) + 2Cl2(g) d) 2NO2(g) + 7H2(g) ⇄ 4H2O(l) + 2NH3(g) e) H2O(g) + C(s) ⇄ CO(g) + H2(g) f) The reduction of solid copper (II) oxide with hydrogen gas to produce copper metal and
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The Burning of Primary and Secondary Alcohols Year 11A Chemistry By Jarrod Ahern Abstract The aim of the investigation was to determine whether primary alcohols use less energy than secondary alcohols for fuel. The hypothesis is if primary alcohols are heated and results are taken‚ they produce a lesser heat of reaction then secondary alcohols. The method used was to find the average bond energies of three relating primary and secondary alcohols and compare it with the average theoretical
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The Adiba Shaby Scholarship Application 2013-2014 Academic Year Please complete the application. All fields are required for eligibility. Student Information Johnson Kayo McKinley Name _______________________________________________________________ Last First Middle 11651 Gorham Ave. #3 Los Angeles‚ CA 90049 Address _____________________________________________________________ Street City State ZIP Code 2889172 10 1987 Primary Telephone (___) ________________ Date of Birth ___/____/____________
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of magnesium chloride were added to water finding the heat of reaction for each trial. Depending on how many moles of magnesium chloride were present in each solution‚ the enthalpy of dissolution was then calculated which gave an average of -151.45 kJ/mol making the reaction exothermic. Magnesium chloride was compared to three other road salts to determine which of the road salts was the best for Minnesota’s winter roads. Due to the ability to lower the freezing point of water‚ the substantial value
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dissociates in a solution. These ions are good conductors of electric current in the solution. All neutralization reactions involving strong electrolytes produces same amount of energy: q = -55.90 kJ of heat per mol of H+. At a constant pressure‚ the heat of reaction equals the enthalpy change (ΔH); therefore ΔH =-55.90 kJ per mol of H+. The negative sign indicates that the heat is being released and the reaction is exothermic. In contrast to strong electrolytes‚ weak electrolytes partially ionized in water
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1 UNIT 9 CHEMICAL KINETICS 1. (c) mole 1–1 sec–1 The rate law for a reaction A + B →products‚ is rate = k [A]1[B]2. 7. Then‚ which one of the following statements is false ? (a) If [B] is held constant while [A] is doubled‚ the reaction will proceed twice as fast. (b) If [A] is held constant while [B] is reduced to one quarter‚ the rate will be halved (c) If [A] and [B] are both doubled‚ the reaction will proceed 8 times as fast. 2. Fro a first order reaction‚ a straight
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= - P kJ / mol HKA3 = q2 / a2 = +Q kJ / mol(d)KA2 + KA1 : Na2CO3(s) + 2 HCl (aq) → 2NaCl(aq) + H2O(l) + CO2 (g)KA3 + KA1 : NaHCO3 (s) + HCl (aq) → NaCl (aq) + H2O (l) + CO2 (g)(e) Energy Na2CO3 (s) + 2 HCl (aq) + H2O (l) + CO2 (g)HKA2 / kJ H 2 x HKA3 2 NaCl (aq) + 2 H2O (l) + 2 CO2 (g) 2 NaHCO3 (s) + 2 HCl (aq)(f) Na2CO3(s) + 2 HCl (aq) → 2NaCl(aq) + H2O(l) + CO2 (g) [1] HKA2 = - P kJ NaHCO3 (s) + HCl (aq) → NaCl (aq) + H2O (l) + CO2 (g) [2] HKA3 = + Q kJ Reverse
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