DOCSLIB.ORG

Copyrighted Material

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Copyrighted Material INDEX acidic regions reaction to form esters 835 A strong acid–strong base/strong base–strong absolute temperatures 299 reaction with acid anhydrides 1031 absolute uncertainties 35, 37–8 acid 473–4 reaction with acid chlorides 1031 absorbance (A) of light 575 weak acid–strong base/weak base–strong reaction with active metals 828 absorption spectra 127–8 acid 476 reaction with carboxylic acid accuracy of measurement 32–3 acidic solutions 437 derivatives 1031–2 acetaldehydes 945 alcohols 827 reaction with carboxylic acids 1028–31 acetals 955, 957–8 redox reactions in 501–3 reaction with esters 1031 as carbonyl-protecting groups 959 thiols 846–7 reaction with phosphorus halides 830 formation of 958, 993–5 acidity constants (Ka) 447 See also reaction with thionyl chlorides 830 acetic acids 433, 464, 466 Henderson–Hasselbalch equation from reduction of carbonyl compounds 826 in buffer solutions 467–8 secondary (2°) 823 Ka 447–8 esters 1010 determining values 449 solubility 1018 speciation diagrams 478 acidophiles 430 structural formula 55–6 vapour pressure variations 262 acids 432 See also diprotic acids; monoprotic tertiary (3°) 823 acids; strong acids; weak acids aldehydes 770, 833 acetones 1 13 boiling points 248–9 amino acids 1066–8 H-NMR and C-NMR spectra 913 calculating vapour pressure 413 bond enthalpies 461 acid-catalysed hydrations 956–8 electron density models 948 common 433 addition of alcohols 955–9 industrial uses 949 dissociation in aqueous solutions at 25° 462 addition of Grignard reagents 953–4 acetophenones 949, 950, 970 maximum strength 465 addition of carbon nucleophiles 955 acetylenes 716 molecular basis of strength 461–5 aliphatic 949 achiral compounds 761, 765, 772 See also oxoacids 462–4 aromatic 949 meso compounds polyprotic 433, 447, 479 boiling points 1018 achiral enols 970 strengths of 441–2 catalytic reductions 965 achiral isomers 773 superacids 465, 482 formation of imines 960–1 acid anhydrides 835, 1012 triprotic 461 formation of oximes and hydrazones 962 hydrolysis 1032, 1035 actins 1060 formation of tetrahedral carbonyl addition nomenclature 1016 actinoids 16, 548, 602 intermediates 951, 966 reaction with alcohols 1031, 1032 activation energies (Ea) 665, 666, 667 a-halogenation 970–1 reaction with ammonia and amines calculating from two rate constants 670 from hydration of alkynes 950–1 1036, 1037 second-order decomposition of nitrogen industrially important 949 acid chlorides 835, 1012, 1028, 1042 dioxide 668–70 IR spectra 889–90 hydrolysis 1032, 1035 activities 355, 523 metal hydride reductions 964–5 reaction with alcohols 1031, 1032 actual yields 98 nomenclature 947 reaction with ammonia and amines acyclic alkanes 58 nucleophilic acyl additions 1027 1036, 1037 acyl groups 1012 oxidation to carboxylic acids 967–8, 1020 acid halides 746 acyl halides 746 See also acid halides from ozonolysis of alkenes 950 formation of 1028 structure and bonding 1012 position of keto–enol equilibrium 969 nomenclature 1016 acylation of aromatic compounds 742, 746–7 preparation from oxidation of alcohols structure and bonding 1012 addition to the carbon–carbon double bond 723 950 adducts 481, 556 reaction to form 2 alcohols 826 acid ionisation constants (pKa) 448 ° alcohols in dilute aqueous solutions 827 drawing structures 483 reaction with addition of Grignard amines 855 adenines 739 reagents 951–5 a-ammonium groups 1067 adenosine diphosphates (ADP) 526, 631, 634 reduction to 1° alcohols 826, 964, 966 aromatic carboxylic acids 1024 adenosine triphosphates (ATP) 526, 31, 634 reductive amination of 962, 964 a-carboxyl groups 1067 amount of glucose in 988 solubility 948, 1018 carboxylic acids 1023–5 chair conformations 991 structural formula 56–7 interpreting 449 adhesive forces 260 structures 944 ionisable groups of amino acids 1067 adiabatic processes 300 alditols 995–6 phenols 839 adipic acids 1014 d-aldohexoses 988 phosphoric acids 623 agricultural chemicals 163 aldopentoses 990 side-chain caryboxyl groups 1067 agricultural fertilisers 622, 633 aldoses 986 acid–base indicators 472 COPYRIGHTEDAir Canada 26 MATERIALaldotetroses 988–9 pKa 479 air pollution and ways to reduce 372 aldotrioses 986, 988 colours of acid and base forms 480 airbags 498 aliphatic aldehydes 949 common 481 airconditioning, working principles behind 331 aliphatic amines 847 how they work 479–80 alanines 858, 1063 nomenclature 848–9 selecting best indicators 480–1 d-alanines 1065 aliphatic carboxylic acids 1012 acid–base reactions 432 Alcoa 605 nomenclature 1014 carboxylic acids 1023–5 alcohols 822–7, 1014 solubility 1018 group 13 620 1H-NMR spectrum 910 aliphatic dicarboxylic acids 1014 phenols 840 acid-catalysed dehydration to alkenes aliphatic hydrocarbons 698 See also alkanes acid–base reactions in water 436–42 831–3 alkadienes 720 acid–base titrations 472–81 acidity of 827 alkali metals 17 amino acids 1068 from addition of Grignard reagents to alkaline batteries 534 glycines 1069 carbonyl compounds 826–7 alkaline earth metals 17 strong acid–strong base 472–4 basicity of 827 alkaline regions weak acid–strong base 474–7 boiling points 948, 1018 strong acid–strong base/strong base–strong weak base–strong acid 474–7 functional groups 822 acid 474 acid–catalysed halogenations 970 IR spectrum 888 weak acid–strong base/weak base–strong acid–catalysed hydrations oxidation to form aldehydes 950 acid 477 aldehydes and ketones 956–8 physical properties 824–5 alkaloids 848 alkenes 728–30 preparation from alkenes 825 alkanes 698–711 aromatic compounds 744 preparation from haloalkanes 826 13C-NMR spectrum 909 mechanisms of additions 729 primary (1°) 823 boiling points 247, 708–9, 824 Index I-1141 BMIndex I-1141 1 June 2015 9:06 AM alkanes (continued) amines 847–53 anti selectivity 731 condensed and molecular formulae 699 1H-NMR spectrum 912 antibodies 1060 conformation 700–1 pKa at 25° 855 antibonding molecular orbitals 206, 208 constitutional isomerism 61–2 pKb at 25° 854–5 antibonding orbitals 265–6 formation from reduction of alkenes 731–2 basicity of 854–7 anti-cancer agents 560 high-molar mass 709 determining class of 848 anti-cancer drugs 781, 1000 IHD 876 IR spectra 889 anticoagulants 1019 IR spectrum 886–7 physical properties 851–2 antifreeze 410 isomeric 709–10 preparation from haloalkanes 852–3 anti-inflammatory drugs 781 NMR spectrum 908–9 reaction of aromatic amines with nitrous antimony 607, 610, 622, 623 nomenclature 58–63, 699, 702–3 acids 859–61 nomenclature 564 physical properties 708–11 reaction to form amides 861 valence electrons 149 reactions of 722–3 reaction with carboxylic acid apatites 266, 608, 635 structures 698, 699 derivatives 1036 aprotic solvents 805, 806, 834 alkanolates 828 reactions with acids 857–61 aqua regia 520 alkenes 698, 711, 1038 separation and purification of 857–8 arenes 698, 711–12, 734 1H-NMR spectrum 909–10 synthesis from carboxylic acids 1039 argentites 486 13C-NMR spectrum 910 synthesis into arylamines 853 argon 618 acid-catalysed dehydration from synthesis by reductive amination 963–4 close-packed structures 277 alcohols 831–3 use in pharmaceuticals 859 phase change data 268 acid-catalysed hydrations 728–30 a-amino acids 1062, 1063 Argyle diamond mine 696 addition of bromine and chlorine 730–3 d-amino acids 1065 aromatic aldehydes 949 addition of hydrogen halides 724–8 amino acids 628, 630, 1060, 1062–74 See also aromatic amines 847 addition to the carbon–carbon double peptides; polypeptides; proteins pKa and pKb at 25° 855 bond 723 pKa 1067 reaction with nitrous acids 859–61 characteristic addition reactions to 723 acidic groups 1066–8 solubility 852 cis–trans configurations 717 analysis based on charge 1073 aromatic carboxylic acids 1012 cis–trans isomers 713 analysis of 1075–6 acidity of 1024 configuration usingE,Z system 719 basic groups 1068 nomenclature 1015 designating configurations 717–19 electrophoresis 1071–3 aromatic compounds 734–42 E,Z systems 718–19 isoelectric points 1070–1 acylation 746–7 electrophilic addition reactions 723–33 in meteorites 1066 alkylation 745–6 IHD 876 other common 1065 bromination 743 IR spectrum 886, 887 pH 1069–70 chlorination 743 low-molar-mass 712, 717 protein-derived 1063–4 electrophilic aromatic substitutions 742–7 nomenclature 716–22 ratios of undissociated acids compared with Friedel–Crafts acylation 949–50 ozonlysis of 950 conjugate base 1070 aromatic dicarboxylic acids 1015 physical properties 722 separation of mixture based on aromatic hydrocarbons 734 See also benzenes preparation into alcohols 825 charges 1073–4 IR spectrum 889 reactions of 723–33 sequence analysis 1076 nomenclature 739–42 reduction to form alkanes 731–2 structural variations 1063 resonance energies 737 relative stabilities 732–3 titration of 1068–9 aromatic ketones 949 shapes of 712–13 4-aminobutanoic acids (GABA) 1065 aromatic properties 734, 738–9 alkoxides 828 b-amino alcohols 955 Hückel’s criteria 738 alkoxy groups 842 amino sugars 989 Arrhenius, Svante 432, 665 alkyl carbocations, order of stability 727 ammonia 184, 350, 482 Arrhenius equation 667–70 alkyl groups 59–60 calculating pH of ion buffers 468 arsanes 622 alkyl halides 724, 792–3 catalytic formation of 681 L-ascorbic acids 997 alkylamines 849 changing equilibrium 368–9 arsenic 610, 622 alkylation of aromatic compounds 742, 745–6 HSAB principle 486 arsenic acids 623 alkylbenzenes 1020 periodic trends in boiling points 251 arsenous acids 623 alkynes 2, 698, 711 phase diagrams 271–2 aryl grignards 952 hydration of 950–1 reaction with carboxylic acid aryl groups 734 IHD 876 derivatives 1036–7 ascorbic acids 478 IR spectrum
Load more

Recommended publications
  • High Temperature Enthalpies of the Lead Halides
    HIGH TEMPERATURE ENTHALPIES OF THE LEAD HALIDES: ENTHALPIES AND ENTROPIES OF FUSION APPROVED: Graduate Committee: Major Professor Committee Member Min fessor Committee Member X Committee Member UJ. Committee Member Committee Member Chairman of the Department of Chemistry Dean or the Graduate School HIGH TEMPERATURE ENTHALPIES OF THE LEAD HALIDES: ENTHALPIES AND ENTROPIES OF FUSION DISSERTATION Presented to the Graduate Council of the North Texas State University in Partial Fulfillment of the Requirements For the Degree of DOCTOR OF PHILOSOPHY By Clarence W, Linsey, B. S., M. S, Denton, Texas June, 1970 ACKNOWLEDGEMENT This dissertation is based on research conducted at the Oak Ridge National Laboratory, Oak Ridge, Tennessee, which is operated by the Uniofl Carbide Corporation for the U. S. Atomic Energy Commission. The author is also indebted to the Oak Ridge Associated Universities for the Oak Ridge Graduate Fellowship which he held during the laboratory phase. 11 TABLE OF CONTENTS Page LIST OF TABLES iv LIST OF ILLUSTRATIONS v Chapter I. INTRODUCTION . 1 Lead Fluoride Lead Chloride Lead Bromide Lead Iodide II. EXPERIMENTAL 11 Reagents Fusion-Filtration Method Encapsulation of Samples Equipment and Procedure Bunsen Ice Calorimeter Computer Programs Shomate Method Treatment of Data Near the Melting Point Solution Calorimeter Heat of Solution Calculations III. RESULTS AND DISCUSSION 41 Lead Fluoride Variation in Heat Contents of the Nichrome V Capsules Lead Chloride Lead Bromide Lead Iodide Summary BIBLIOGRAPHY ...... 98 in LIST OF TABLES Table Pa8e I. High-Temperature Enthalpy Data for Cubic PbE2 Encapsulated in Gold 42 II. High-Temperature Enthalpy Data for Cubic PbF2 Encapsulated in Molybdenum 48 III.
    [Show full text]
  • Chapter 11 Liquids, Solids, and Phase Changes
    Lecture Presentation Chapter 11 Liquids, Solids, and Phase Changes 11.1, 11.2, 11.3, 11.4, 11.15, 11.17, 11.26, 11.30, 11.32, 11.40, 11.42, 11.60, 11.82, 11.116 John E. McMurry Robert C. Fay Properties of Liquids Viscosity: The measure of a liquid’s resistance to flow (higher intermolecular force, higher viscosity) Surface Tension: The resistance of a liquid to spread out and increase its surface area (forms beads) (higher intermolecular force, higher surface tension) Properties of Liquids low intermolecular force – low viscosity, low surface tension high intermolecular force – high viscosity, high surface tension HW 11.1 Properties of Liquids high intermolecular force – high viscosity, high surface tension For the following molecules which has the higher intermolecular force, viscosity and surface tension ? (LD structure, VSEPRT, dipole of molecule) (if the molecules are in the liquid state) a. CHCl3 vs CH4 b. H2O vs H2 (changed from handout) c. N Cl3 vs N H Cl2 Phase Changes between Solids, Liquids, and Gases Phase Change (State Change): A change in the physical state but not the chemical identity of a substance Fusion (melting): solid to liquid Freezing: liquid to solid Vaporization: liquid to gas Condensation: gas to liquid Sublimation: solid to gas Deposition: gas to solid Phase Changes between Solids, Liquids, and Gases Enthalpy – add heat to system Entropy – add randomness to system Phase Changes between Solids, Liquids, and Gases Heat (Enthalpy) of Fusion (DHfusion ): The amount of energy required to overcome enough intermolecular forces to convert a solid to a liquid Heat (Enthalpy) of Vaporization (DHvap): The amount of energy required to overcome enough intermolecular forces to convert a liquid to a gas HW 11.2: Phase Changes between Solids, Liquids, & Gases DHfusion solid to a liquid DHvap liquid to a gas At phase change (melting, boiling, etc) : DG = DH – TDS & D G = zero (bc 2 phases in equilibrium) DH = TDS o a.
    [Show full text]
  • Cryometric Determination of the Enthalpy of Fusion of Sodium Cryolite
    Cryometric determination of the enthalpy of fusion of sodium cryolite M. MALINOVSKÝ Department of Chemical Technology of Inorganic Substances, Slovak Technical University, CS-812 37Bratislava Received 30 July 1982 Accepted for publication 22 August 1983 Using the method of classical thermal analysis a part of the liquidus of sodium cryolite in the system Na3AlF6—Na3FS04 was measured in the compo­ sition range 0—5 mole % Na3FS04. On the basis of these results the molar enthalpy of fusion of cryolite was calculated. It was found that AHf(Na3AlFft) = = 115.4 kJ mol"1; error in this result was estimated to be ±4.9 %. Методом классического термического анализа измерена часть ликви­ дуса натриевого криолита в системе Na3AlF6—Na3FS04 в интервале кон­ центраций 0—5 мол. % Na3FS04. На основании этих результатов рассчи­ тана мольная энтальпия плавления криолита. Найдено, что 1 AH,(Na3AlF6) = 115,4 кДж моль" ; точность этого результата ±4,9 %. Literature survey and theoretical Knowledge of the enthalpy of fusion of sodium hexafluoroaluminate Na3AlF6 (cryolite) is important both from theoretical and practical points of view. For example, it is needed at calculation of the thermal and energy balance and/or the thermal inertia of aluminium cells (the electrolyte contains about 90 mass % of Na3AlF6). The most precise values of the molar enthalpy of fusion AHf(i) of chemical substances can be generally obtained from calorimetric measurements. However, when we deal with substances having higher melting temperature and which are also unstable and very corrosive the calorimetric determination of the quantity AHf(i) can be less reliable. In the case of cryolite Roth and Bertram [1] found from the calorimetric 1 1 measurements ÄH,(Na3 A1F6) = 16.64 kcal mol" = 69.62 kJ mol" .
    [Show full text]
  • Thermodynamic Temperature
    Thermodynamic temperature Thermodynamic temperature is the absolute measure 1 Overview of temperature and is one of the principal parameters of thermodynamics. Temperature is a measure of the random submicroscopic Thermodynamic temperature is defined by the third law motions and vibrations of the particle constituents of of thermodynamics in which the theoretically lowest tem- matter. These motions comprise the internal energy of perature is the null or zero point. At this point, absolute a substance. More specifically, the thermodynamic tem- zero, the particle constituents of matter have minimal perature of any bulk quantity of matter is the measure motion and can become no colder.[1][2] In the quantum- of the average kinetic energy per classical (i.e., non- mechanical description, matter at absolute zero is in its quantum) degree of freedom of its constituent particles. ground state, which is its state of lowest energy. Thermo- “Translational motions” are almost always in the classical dynamic temperature is often also called absolute tem- regime. Translational motions are ordinary, whole-body perature, for two reasons: one, proposed by Kelvin, that movements in three-dimensional space in which particles it does not depend on the properties of a particular mate- move about and exchange energy in collisions. Figure 1 rial; two that it refers to an absolute zero according to the below shows translational motion in gases; Figure 4 be- properties of the ideal gas. low shows translational motion in solids. Thermodynamic temperature’s null point, absolute zero, is the temperature The International System of Units specifies a particular at which the particle constituents of matter are as close as scale for thermodynamic temperature.
    [Show full text]
  • Enthalpy of Sublimation in the Study of the Solid State of Organic Compounds
    J. Phys. Chem. B 2005, 109, 18055-18060 18055 Enthalpy of Sublimation in the Study of the Solid State of Organic Compounds. Application to Erythritol and Threitol A. J. Lopes Jesus, Luciana I. N. Tome´, M. Ermelinda Euse´bio,* and J. S. Redinha Department of Chemistry, UniVersity of Coimbra, 3004-535, Coimbra, Portugal ReceiVed: March 30, 2005; In Final Form: July 5, 2005 The enthalpies of sublimation of erythritol and L-threitol have been determined at 298.15 K by calorimetry. The values obtained for the two diastereomers differ from one another by 17 kJ mol-1. An interpretation of these results is based on the decomposition of this thermodynamic property in a term coming from the intermolecular interactions of the molecules in the crystal (∆intH°) and another one related with the conformational change of the molecules on going from the crystal lattice to the most stable forms in the gas phase (∆confH°). This last term was calculated from the values of the enthalpy of the molecules in the gas state and of the enthalpy of the isolated molecules with the crystal conformation. Both quantities were obtained by density functional theory (DFT) calculations at the B3LYP/6-311G++(d,p) level of theory. The results obtained in this study show that the most important contribution to the differences observed in the enthalpy of sublimation are the differences in the enthalpy of conformational change (13 kJ mol-1) rather than different intermolecular forces exhibited in the solid phase. This is explained by the lower enthalpy of threitol in the gas phase relative to erythritol, which is attributed to the higher strength of the intramolecular hydrogen bonds in the former.
    [Show full text]
  • Chemistry 531 Spring 2009 Problem Set 5 Solutions
    Chemistry 531 Spring 2009 Problem Set 5 Solutions 1. For the reaction CH4(g) + 2O2(g) −→ CO2(g) + 2H2O(l) use Table 4-2 on page 50 and Table 7-2 on page 171 of your text books to determine at 25◦C (a) the amount of heat liberated per mole at constant pressure; Answer: ◦ −1 ∆rHm = [2(−285.83) + (−393.509) − (−74.81)]kJ mol = −890.359kJ mol−1 (b) the maximum amount of work obtainable per mole for the reaction; Answer: ◦ −1 −1 ∆rGm = [2(−237.129) + (−394.359) − (−50.72)]kJ mol = −817.897kJ mol A = G − pV ◦ ◦ ∆rAm = ∆rGm − RT ∆ngas = −817897J mol−1−(8.3144J mol−1K−1)(298K)(−2) = −812.941kJ mol−1 = max. work (c) the maximum amount of non-pV work obtainable from the reaction per mole. Answer: ◦ −1 max. non-pV work = ∆rGm = −817.897kJ mol 2. A certain gas obeys the equation of state pVm = RT + βp 1 where β depends only on the temperature. For this gas show that ∂U ! RT 2 dβ ! = 2 ∂V T (Vm − β) dT Answer: ∂U ! ∂p ! = T − p ∂V T ∂T V RT p = Vm − β(T ) ∂p ! R RT dβ = + 2 ∂T V Vm − β (Vm − β) dT Then ∂U ! RT RT 2 dβ = + 2 − p ∂V T Vm − β (Vm − β) dT RT RT 2 dβ RT = + 2 − Vm − β (Vm − β) dT Vm − β RT 2 dβ = 2 (Vm − β) dT 3. Show that ! 2 ! ∂Cp ∂ V = −T 2 ∂p T ∂T p Answer: ∂H ! Cp = ∂T p ! ! ∂Cp ∂ ∂H = ∂p ∂p ∂T T p T ∂ ∂H ! ! ∂T ∂p T p But dH = T dS + V dp ∂H ! ∂S ! = T + V ∂p T ∂p T dG = −SdT + V dp ∂S ! ∂V ! = − ∂p T ∂T p 2 Then ∂H ! ∂V ! = V − T ∂p T ∂T p and ! ! ∂Cp ∂ ∂V = V − T ∂p ∂T ∂T T p p ∂V ! ∂V ! ∂2V ! = − − T 2 ∂T p ∂T p ∂T p ∂2V ! = −T 2 ∂T p 4.
    [Show full text]
  • Thermal Storage and Transport in Colloidal Nanocrystal-Based Materials by Minglu Liu a Dissertation Presented in Partial Fulfil
    Thermal Storage and Transport in Colloidal Nanocrystal-Based Materials by Minglu Liu A Dissertation Presented in Partial Fulfillment of the Requirements for the Degree Doctor of Philosophy Approved November 2015 by the Graduate Supervisory Committee: Robert Wang, Chair Liping Wang Konrad Rykaczewski Patrick Phelan Lenore Dai ARIZONA STATE UNIVERSITY December 2015 ABSTRACT The rapid progress of solution-phase synthesis has led colloidal nanocrystals one of the most versatile nanoscale materials, provided opportunities to tailor material's properties, and boosted related technological innovations. Colloidal nanocrystal-based materials have been demonstrated success in a variety of applications, such as LEDs, electronics, solar cells and thermoelectrics. In each of these applications, the thermal transport property plays a big role. An undesirable temperature rise due to inefficient heat dissipation could lead to deleterious effects on devices' performance and lifetime. Hence, the first project is focused on investigating the thermal transport in colloidal nanocrystal solids. This study answers the question that how the molecular structure of nanocrystals affect the thermal transport, and provides insights for future device designs. In particular, PbS nanocrystals is used as a monitoring system, and the core diameter, ligand length and ligand binding group are systematically varied to study the corresponding effect on thermal transport. Next, a fundamental study is presented on the phase stability and solid-liquid transformation of metallic (In, Sn and Bi) colloidal nanocrystals. Although the phase change of nanoparticles has been a long-standing research topic, the melting behavior of colloidal nanocrytstals is largely unexplored. In addition, this study is of practical importance to nanocrystal-based applications that operate at elevated temperatures.
    [Show full text]
  • States of Matter Chemistry 1-2 Enriched Mr
    States of Matter Chemistry 1-2 Enriched Mr. Chumbley Modern Chemistry: Chapter 10 THE KINETIC-MOLECULAR THEORY OF MATTER Section 1 p. 310 – 314 Kinetic-Molecular Theory • It is generally not possible to study individual particles, so scientists study the behavior of large groups of particles • The kinetic molecular theory was developed in the late 19th century to account for the different ways matter behaves as a solid, liquid, or gas • The kinetic-molecular theory explains that the behavior of physical systems depends on the combined actions of the molecules constituting the system KMT and Gases • Kinetic-molecular theory can be used to describe the properties and behavior of all states of matter, but is well demonstrated by gases • An ideal gas is a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory Kinetic-Molecular Theory of Gases • Gases consist of large numbers of tiny particles that are far apart relative to their size • Collisions between gas particles and between particles and container walls are elastic collisions • An elastic collision is one in which there is no net loss of kinetic energy • Gas particles are in continuous, rapid, random motion and possess kinetic energy • Kinetic energy is the energy of motion • There are no forces of attraction between gas particles • The temperature of a gas depends on the average kinetic energy of the particles of the gas Properties of Gases • Expansion • Gases do not have a definite shape or volume, but rather completely fill their container • Fluidity
    [Show full text]
  • Measurement of High Temperature Heat Content of Silicon by Drop Calorimetry
    Journal of Thermal Analysis and Calorimetry, Vol. 69 (2002) 1059–1066 MEASUREMENT OF HIGH TEMPERATURE HEAT CONTENT OF SILICON BY DROP CALORIMETRY K. Yamaguchi1* and K. Itagaki2 1Department of Materials Science and Technology, Faculty of Engineering, Iwate University, Ueda, Morioka, 020-8551, Japan 2Institute of Multidisciplinary Research for Advanced Materials, Tohoku University, Katahira, Aoba-Ku, Sendai, 980-8577, Japan Abstract Heat content of silicon has been measured in a temperature range of 700–1820 K using a drop calo- rimeter. Boron nitride was used as a sample crucible. The enthalpy of fusion and the melting point of silicon determined from the heat content-temperature plots are 48.31±0.18 kJ mol–1 and 1687±5 K, respectively. The heat content and heat capacity equations were derived using the Shomate function for the solid region and the least square method for the liquid region, respectively, and compared with the literature values. Keywords: drop calorimeter, enthalpy of fusion, heat capacity, heat content, high temperature, melting point, silicon Introduction Single crystals of silicon are important materials used in electronic device applica- tions. The solid and liquid phases coexist at the quasi-equilibrium state in conven- tional processes to fabricate the single crystal of silicon. Therefore, knowledge of the thermochemical data such as heat capacity, melting point and enthalpy of fusion is important for the analysis of fabricating processes. Furthermore, production of a sin- gle crystal of silicon having the higher quality and a larger diameter is required for the Czochralski (Cz) technique of single crystal growth. In order to achieve this demand, mathematical simulations of the transport phenomena prevailing in the Cz single crystal growth have been carried out based on the thermochemical data.
    [Show full text]
  • Arblasteros 06A SC.Docx ACCEPTED MANUSCRIPT 18/05/2020
    www.technology.matthey.com Johnson Matthey’s international journal of research exploring science and technology in industrial applications ************Accepted Manuscript*********** This article is an accepted manuscript It has been peer reviewed and accepted for publication but has not yet been copyedited, house styled, proofread or typeset. The final published version may contain differences as a result of the above procedures It will be published in the JANUARY 2021 issue of the Johnson Matthey Technology Review Please visit the website https://www.technology.matthey.com/ for Open Access to the article and the full issue once published Editorial team Manager Dan Carter Editor Sara Coles Editorial Assistant Yasmin Stephens Senior Information Officer Elisabeth Riley Johnson Matthey Technology Review Johnson Matthey Plc Orchard Road Royston SG8 5HE UK Tel +44 (0)1763 253 000 Email [email protected] ArblasterOs_06a_SC.docx ACCEPTED MANUSCRIPT 18/05/2020 A Re-assessment of the Thermodynamic Properties of Osmium Improved value for the enthalpy of fusion John W. Arblaster Droitwich, Worcestershire, UK E-mail: [email protected] The thermodynamic properties were reviewed by the author in 1995. A new assessment of the enthalpy of fusion at 68.0 ± 1.7 kJ mol-1 leads to a revision of the thermodynamic properties of the liquid phase and although the enthalpy of sublimation at 298.15 K is retained as 788 ± 4 kJ mol-1 the normal boiling point is revised to 5565 K at one atmosphere pressure. Introduction The thermodynamic properties of osmium were reviewed by the author in 1995 (1) with a further review in 2005 (2) to estimate a most likely value for the melting point at 3400 ± 50 K to replace the poor quality experimental values which were currently being quoted in the literature.
    [Show full text]
  • The Published Fusion Enthalpy and Its Influence on Solubility Estimation for Alcohols
    International Journal of Advanced Research in Chemical Science (IJARCS) Volume 6, Issue 11, 2019, PP 40-49 ISSN No. (Online) 2349-0403 DOI: http://dx.doi.org/10.20431/2349-0403.0611004 www.arcjournals.org The Published Fusion Enthalpy and its Influence on Solubility Estimation for Alcohols Moilton R. Franco Junior1*, Nattácia R. A. Felipe Rocha2, Warley A. Pereira2, Nadine P. Merlo2, Michelle G. Gomes1, Patrísia O. Rodrigues1 1Post-Graduation Program in Biofuelss – Chemistry Institute – Federal University of Uberlândia – Avenida João Naves de Ávila, Santa Monica – MG – Brazil 2 UniRV – Rio Verde University – Fazenda Fontes do Saber – Rio Verde- Goiás – Brazil. *Corresponding Author: Moilton R. Franco Junior, Post-Graduation Program in Biofuelss – Chemistry Institute – Federal University of Uberlândia – Avenida João Naves de Ávila, Santa Monica – MG – Brazil . Abstract: This paper aims to compare two different methods of estimating enthalpy of fusion and identify the one which is closer to the already published value. The n-long chain alcohols such asn-octanol(C8), dodecanol(C12), tridecanol(C13), tetradecanol(C14), pentadecanol(C15), hexadecanol(C16), heptadecanol(C17), octadecanol(C18), nonadecanol(C19)and eicosanol(C20)were the systems used for testing the methods. The experimental or estimateddata was available in the literature, and comparisons enabled the determination of the relative deviations for the compounds studied. It was expected that the enthalpy of fusion could be well evaluated by using sublimation and vaporization enthalpy as well as with the use of liquid and solid enthalpies of formation for the compound. However, when the results were compared with the literature ones, it was found that there are problems with the data published (experimental or not) because of the high relative deviations presented.
    [Show full text]
  • Math Tutor of Fusion
    DO NOT EDIT--Changes must be made through “File info” CorrectionKey=NL-A Calculations Using Enthalpies Math Tutor of Fusion When one mole of a liquid freezes to a solid, energy is released the crystal and overcome the attractive forces opposing as attractive forces between particles pull the disordered separation. This quantity of energy used to melt or freeze one particles of the liquid into a more orderly crystalline solid. mole of a substance at its melting point is called its molar When the solid melts to a liquid, the solid must absorb the enthalpy of fusion, ∆Hf . same quantity of energy in order to separate the particles of Problem-Solving TIPS • The enthalpy of fusion of a substance can be given as either joules per gram or kilojoules per mole. • Molar enthalpy of fusion is most commonly used in calculations. • The enthalpy of fusion is the energy absorbed or given off as heat when a substance melts or freezes at the melting point of the substance. • There is no net change in temperature as the change of state occurs. Samples 7.30 kJ of energy is required to melt 0.650 mol of ethylene glycol (C2H6O2) at its melting point. Calculate the molar enthalpy of fusion, ∆Hf , of ethylene glycol and the energy absorbed. energy absorbed molar enthalpy of fusion = ∆H = __ f moles of substance 7.30 kJ kJ ∆H = _ = 11.2 _ f , ethylene glycol 0.065 mol mol Determine the quantity of energy that will be needed to melt 2.50 × 105 kg of iron at its melting point, 1536°C.
    [Show full text]