General Chemistry I
General Chemistry I CHE 111
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Chapter 4 The Basic Approach to Chemical Equilibrium Text Notes I The Chemical Composition of Aqueous Solutions A Water is the most plentiful solvent on Earth and serves as the major medium for chemical analyses 03 Electrolytes 7 solutes that form ions when dissolved in water producing a solution with electrical conductivity Strong electrolytes ionized completely in water while weak electrolytes only partially ionize so a strong electrolyte solution will be a better conductor or electricity Strong electrolytes consist of acids bases and salts 0 Acids and Bases 1 BronsteadLowry Theory 7 acids donate protonsbases accept protons For a species to act as an acid a base proton acceptor must be present and vice versa The species produced when an acid gives up a proton is called the conjugate base of the parent acid Acid1 9 basel proton When a base accepts a proton a conjugate acid is produced Base proton 9 acid If the 2 processes are combined a neutralization reaction occurs Acidl base 9 basel acidz NH3 H20 9 NH4 OH39 Problem 44 Acid Conjugate Base a HOCl OCl b H20 OH c NH4 NH3 1 HCO3 CO3239 e H2PO4 HPO4239 D Amphiprotic Solvents 7 a solvent that can act as either an acid or base depending on the solute it s in methanol ethanol anhydrous acetic acid and dihydrogen phosphate ion are all examples of amphiprotic solvents H2P0439 H30 a H3PO4 H20 H2P0439 OH39 9 HPO4239 H20 zwitterions 7 an amphiprotic compound that is produced by a simple amino acid s weak acid and weak base functional groups zwitterions carry both a positive charge amino group and negative charge carboxyl group 1 Amphiprotic solvents can undergo spontaneous selfionization or autoprotolysis to form 2 different ionic species H20 H20 9 H30 OH39 Both the hydronium ion and hydroxyl ion will have concentrations of about 10397 M Problem 46 Expressions 0fAutopr0tolysis a 2H20 gt H30 0H b 2CH3COOH 9 CH3COOH2 CH3COO c 2CH3NH2 9 CH3NH3 CH3NH d 2CH3OH 9 CH3OH2 CH3O E Strong and Weak Acids and Bases 1 Strong acids dissociate completely in water weak acids partially dissociate yielding both parent acid and conjugate base 2 Acids and bases can be anionic cationic or neutral perchloric and hydrochloric acids are strong and will completely dissociate in water leaving a conjugate bases and spectator ion ammonium ion and acetic acid are weak acids and have a higher affinity for protons acetic acid can act as a differentiating solvent in which various acids dissociate to different degrees and thus have different strengths while water acts as a leveling solvent for strong acids because the strong acid will dissociate completely and have no differences in strength F Chemical Equilibrium There is never actually a complete conversion of reactants to product in a chemical reaction there is only a chemical equilibrium A chemical equilibrium state is when the ratio of concentration of reactants and products is constant 2 An equilibriumconstant expression is an algebraic equation that describes the concentration relationships that exist among reactants and products at equilibrium H3As04 3139 2H a H3As03 15 H20 This equilibrium reaction can be monitored as it moves to the right by the orange to red color change of the triiodide ion Once the color becomes constant the reactants have been used up and the triiodide ion concentration is now constant G Writing Equilibrium Constants l The concentration in uence on the position of a chemical equilibrium is quantitatively described by the equilibrium expression 2 This is a useful expression because it allows the chemist to predict the direction and completeness of a chemical reaction but the expression yields no information about the rate at which equilibrium is approached The equilibrium expression for the generalized equation WW xX 9 yY zZ would be K my ZZWW X15 Problem 4 7 a CZHSNHZ H20 9 CZHSNH3 0H Kb KwKa 100210391 231x103911 jg f OHq 433210394 CszNHzl b HCN H20 9 H30 CN Ka gi CNq 62103910 HCN c C5H5NH H20 9 C5H5N H30 Ka mggiugg gm 59x1039 CsHsNIF 1 CN H20 9 HCN 0H Kb KwKa 100x10 16x10395 0H HCN 62103910 CN e H3A504 3H20 9 3H30 Asof K1K2K3 58x10393 11x10397 32x1039 20103921 Egg 3 Aso H3ASO4 1 C03239 2H20 9 20H Hzco3 Kb KwKle 100x10 15x10394 469x103911 14 OH11EZQ21 cofl H Important Equilibrium Constants in Analytical Chemistry There are several different types of equilibrium useful for analytical chemistry ionproduct constant KW solubility product Ksp dissociation constant Ka or Kb formation constant Bu oxidationreduction constant Kredox and the distribution constant Kd Water does not appear in equilibrium constant expressions 1 The IonProduct Constant for Water aqueous solutions contain small concentrations of hydronium and hydroxide ions as a result of 2H20 9 H30 OH and the equilibrium constant can be calculated form K H30 OHH202 the concentration of water in dilute solutions is very large compared with the concentration of hydrogen and hydroxide ions so the concentration of water can be rewritten as the ion product constant for water KH202 KW H30 OH Because OH and H30 are formed only from the dissociation of water their concentrations must be equal 1 Solubility Products Ksp The Ksp is a numerical constant that describes equilibrium in a saturated solution of a sparingly soluble ionic salt Solubility S so some solid must be present in the reaction in order for a Ksp to be calculated BaIO32s a Ballm 21031 Ksp Ball 103392 Problem 49 a S Agl 103 Ksp Ag 103 52 b s so mg Ksp A612 803239 st s 48 c s A5043 13Ag Ksp 3S3 S 27s d s Pb 1CI1F1 Ksp s s s s e s cf 1 Ksp s s 82 t s Pb2 1414 Ksp S 2S2 4s3 g s Bi21 1311 Ksp S3S3 2754 h s Mn 1NH41P04quot1 Ksp s s s 8 Problem 416 mmol 103 50 ml 300M 1910393 a mmol PdCl6239 50 ml 400 mmolml 20 mmol mmol excess K 20 mmol 25mm01 10 mmol K 10 mmol K 50 ml 0200 M b mmol PdC16239 50 ml 200M 10 mmol s PdClsz39 1 K Ksp K 2 PdClGL 2S2S 4s3 6x106 s 114x10392 K 2s 2210392 M c mmol PdClsz39 added 50 ml 400M 20 mmol mmol excess PdClszquot 20 mmol 1220 mmol 10 mmol PdCl6239 10 mmol 100 ml s z 0100 s 0100 M K 2s K2 PdClGL 6x106 4s2 0100 M s x15x10395 39x10393 M l The common ion effect is responsible for the reduction in solubility of an ionic precipitate when a soluble compound combining one of the ions of the precipitate is added to the solution in equilibrium with the precipitate 2 The common ion effect is a mass action effect predicted from the Le Chatelier principle 3 The Le Chatelier principle states that the position of equilibrium in a system always shifts in a direction that tends to relieve an applied stress to the system J Writing Dissociation Constants for Acids and Bases Ka is the acid dissociation constant HNO2 H20 9 H30 NOz39 Ka mmzl HNOZ Kb is the base dissociation constant NH3 H20 9 NH4 OH39 Kb NHJHOH39D NH3 Water is not necessary in the denominator of either equation because the concentration of water is so large compared to the concentration of the weak acid or base that the dissociation does not change water appreciably Kw H30OH39 KaKb Kw KaKb K Calculating the H30 in Solutions of Weak Acids When a weak acid HA is dissolved in water 2 equilibria are established that give hydronium ions HA H20 9 H30 A Ka H30 A HA 2H20 a H3O OH Kw H30OH The hydronium produced in the rst reaction suppress the dissociation of water so that the contribution of hydronium ions from the second equation are negligible so A H30 The sum of the molar concentrations of the weak acid and its conjugate base must equal the analytical concentration of the acid CH A because the solution has no other source of A ions so cHA A HA or cHA H30 HA rearrange and get HA cHA 7 H30 the Ka expression would then be Ka 1319 CHA 7 H30 This can be further simpli ed to H30 VKaCHA Problem 419 H30 of water at 100 C at 100 C the Ksp ofwater 49x1014 M H30 V49x10391 7x10 7 M 2 Hydroxide Ion concentrations in solutions of weak acids can be found using the same approach used in nding hydronium ion concentration NH3 H20 9 NH4 OH Kb MfHOHq NH3l Analytical Chemistry Andrea Szczepanski F all 200 1 Chapter 3 Important Chemical Concepts Expressing Quantities and Concetrations 1 Important Units of Measurement A SI Units International System of Units SI Base Units Physical Quantity Name of Unit Abbreviation Mass kilogram kg Length meter In Time second s Temperature kelv in K Amount of substance mole mol Electric Current ampere Luminous Intensity candela cd Prefixes for Units giga G 109 mega M 106 kilo k 103 deci d 10391 centi c 10392 milli m 10393 micro u 10396 nano n 10399 pico p 103912 femto f 103915 atto a 103918 B The mole and millimole 1 Mole 7 amount of a chemical species Avogadro s number 6022 X 1023 of particles 19 1Lillimole 7 1mmol 10393 mol 3 Molar mass 7 mass in grams of one mole of a substance Example 35 page 76 462 gNagPO4 Molar Mass N33P04 229898 gNaX 3 309738 gp 159994 g0 X4 1639408 g per molNagPO4 Moles N33P04 462 gX 1639408 gmol 2818 X 10392 mol N33P04 Moles Na 7 2818 X 10392mol NagPOAX 3 mol Na molNa3PO4 7 845 X 10392mol Na Na ions 7 845 X 10392mol Na X 6022X 1023 7 508 X 1022 ions Analytical Chemistry Andrea Szczepanski F all 200 1 C Solutions and Their Concentrations 1 N 9 gt V Molar Concentration or Molarity 7 Number of moles of solute in one Liter of solution or millimoles solute per milliliter of solution Analytical Molarity 7 Total number of moles of a solute regardless of chemical state in one liter of solution It specifies a recipe for solution preparation Equilibrium Molarity 7 Species Molarity 7 The molar concentration of a particular species in a solution at equilibrium Percent Concentration a weight percent ww weight solute X 100 weight solution b volume percent vv volume solute X 100 volume solution c weightvolume percent wv weight solute g X 100 volume soln mL Parts Per Mlion and Parts per Billion cppm mass of solute X 106 ppm mass of solution For dilute acqueous solutions whose densities are approxilm ately 100 gmL 1 ppm 1mgL Example 322 page 77 a Molar Analytical Concentration of K3FeCN5 414mgX LMX 1g X1mol 7168X10393M 750 ml IL 103 mg 329 gmol b Molar Concentration of K 168X10393MX 3 7 503 X 10393M c Molar Concentration of FeCN3395 Moles ongFeCN5 Moles FeCN3395 168X10393M ongFeCN5 7168 X 10393M ofFeCN3395 d weightvolume ongFeCN5 0414 g X 100 00552 750 mL Analytical Chemistry Andrea Szczepanski Fall 2001 e 1Lillimoles of K in 500mL of soln 503x10393Mx107p 500 mLXEmmol 70252 mmol mL mL 0 ppm FeCN3396 Molar mass ofFeCN3395 55847 mg 12011 mg 140067 mg X6 212 mg 414 mg KgFe C11 X 212 mg Fe C1133 356 ppm 0750L 329 mg K3FCCN5 6 p 7 Functions The p value is the negative base10 logarithm of the molar concentration of a certain species pX log X The most well known pfunction is pH the negative logarithm of H3O Example 322 continued page 77 g pK for the solution log K 7 log 503x10393 M 7 298 h pFeCN5 for solution log FeCN5 log 168 X 10393 M 2775 D Density and Specific Gravity of Solutions 1 Density 7 The mass of a substance per unit volume In SI units density is expressed in units of kgL or gmL 2 Specific Gravity 7 The ratio of the mass of a substance to the mass of an equal volume of water at 4 degrees Celsius Dimensionless not associated with units of measure Example 327 page 77 Molar mass ongPO4 979943 g 169X101 g reagent X 85 g HQELX 1 molH3 4 14659015 M L reagent 100 g reagent 979943 g H3PO4 750 mL X 1L X 600 M H3PO4 45 moles 45 moles X 1L 307 mL 14659015 moles Dilute 307 mL of H3P04 to 750 mL Analytical Chemistry Andrea Szczepanski F all 200 1 11 Chemical Stoichiometry A Stoichiometry 7 The mass relationships among reacting chemical species The stoichiometry of a reaction is the relationship among the number of moles of reactants and products as shown by a balanced equation Flow Diagram Figure 32 Example 335 page 78 Balanced Equation NaZSO3 2 HClO4 02 2 NaCl H20 4 Oz nNa2503 7500 mL X 03333M 0025 moles 1000 mL n HClO4 1500 mL X 03912 M 005868 moles 1000 Mole ratio OfNazSOg to HClO4 is 12 0025 moles Nastg X 2 005 moles HClO4 HClO4 is in excess 0025 moles Nazsog X 1 mol SOZ X 640648 g SOL 10602 g SOZ 1 molNaZSOg mole Concentration of HClO4 is in excess 005868 moles 7 005 moles used in reaction 000868 moles remaining 000868 moles HClO4 00386 M Hc1o4 7500 mL 15000 mL Chapter 16 Elements of Electrochemistry Class Notes AG nFE 11 RTan AG AH TAS G Gibbs change in free energy a thermodynamic quantity E internal energy of cel F Faraday s constant n moles of electrons R 831 constant T temperature in Kelvin ln natural log ofK or 2303 log K K equilibrium coefficient H enthaply S entropy l Redox Reactions reduction 7 addition of electrons to an atom as occurs during the addition of hydrogen to a molecule or the removal of oxygen from it oxidation 7 loss of electron density from an atom as occurs upon addition of oxygen to a molecule or upon removal of hydrogen Example Cu 2a lt7 Cu E 7 0335 Zn 2e lt7 Zn E 7 o799 0335 0799 7 1134 v Eu 1134 Vols For an exothermic spontaneous reaction G lt 0 E gt 0 K gtgt 1 Reduction 9 cathode 7 more positive E Oxidation 9 anode 7 more negative E AG nFE AG 2965001134V A 21 4 k Reaction is spontaneous exothermic produces energy ll Nerstian Equation E E a In 1212121 nF A Bb E 0059 log Keq N Text Notes I Redox Reactions reaction in which electrons are transferred from one reactant to another Ce Fez lt gt Ce Fe3 Ce is the oxidizing agent or oxidant because it accepts electrons from iron and Fe is the reductant because it donated electrons to Ce A redox reaction can be split into 2 half reactions e lt gt Ce Fez lt gt Fey e The 2 half reactions must be balanced just like any other reaction The number of atoms of each element and the net charge on each side of the equation must be in balance so for the oxidation of Fe2 by MnO4 the half reactions would be MnO4 8H 5e H Mn 4H20 5Fe2 H 5Fe3 5e The net charge for the first half reaction is l 7 5 8 2 which is the same on the right side For the second half reaction it must by multiplied by 5 so that the number of electrons lost by Fe equals the number gained by MnO4 The balanced net equation for the reaction would be MnO4 5Fe2 8H H Mn 5Fe3 4H20 Problem 167 3 2Fe3 Sn 2Fe Sn Cr 3Ag Cr3 3Ag 2NO3 Cu 4H 2N0z mm Cu 2Mn04 5st03 2M ssof 4H 3H10 Ti3 FeCN63 H10 Tio FeCN6 quot ZI F H101 206 02 zce 2F 835 g 2Ag 21 Sn 2AgI Sn h U01 Zn 4H U Zn 2H10 i SHNOZ 2Mn04 E 5NO3 2Mn 3H20 j HzNNHz 103 2IF 2Cl N2 IClz 3H10 Problem 168 Oxidizing Agent Reducing Agent a Fe3 Sn b Agir Cr c NO3 Cu d MnO4 st03 e FeCN63 Ti3 f Ce4 H202 g Sn Ag h U01 Zn i MnO4 HNOz J 103 HZNNHZ redox reaction may be compared to an acidbase reaction by the equation Acid1 base lt gt base1 acid Ami Box lt gt on Bred The oxidized B will accept electrons from reductant A and A having given up e will become oxidizing agent A Redox Reactions in Electrochemical Cells A Types 1 reaction is performed by direct contact between the oxidant and the reductant in a suitable container The reactanm do not come in contact with one another salt bridge employed a salt bridge prevents the mixing of the contents of the 2 electrolyte solutions making up electrochemical cells N Problem 164 The significance between the 2 standard E potentials is that the first standard potential is for a solution that is saturated with 11 which has an 12aq activity much less than 1 The second potential is for a hypothetical half cell in which the Izaq is unity so it would have a greater potential since the driving force for the reduction would be greater at the higher 11 concentration Ill 03 Electrochemical Cell an array consisting of 2 or 3 electrodes each of which is in contact with an electrolyte solution Typically the electrolytes are in electrical contact through a salt bridge An external metal conductor connects the electrodes 1 A cathode is an electrode where reduction occurs 2 An anode is the electrode where oxidation occurs Electrochemical Cells are either galvanic or electrolytic l galvanic cells store and supply electrical energy ex Batteries 2 electrolytic cells require an external source of electrical energy for operation Reversible versus Irreversible Cells 1 in a reversible cell reversing the current reverses the cell reaction 2 in an irreversible cell reversing the current causes a different half reaction o occur at one or both of the electrodes Problem 166 The potential in the presence of base would be more negative because the nickel ion activity in the basic solution would be much less than 1 molar So the driving force for the reduction would be less and the electrode potential would be much more negative In a cell electricity is carried by movement of anions toward the anode and cations toward the catho e Electrode Potentials A the potential difference that develops between the electrodes of the cell is a measure of the tendency for the reaction to proceed from anonequilibriurn state to the condition of equilibrium Gibb s Free Energy AG nFE can If the reactants and products are in their standard states the resulting cell potential is called the standard cell potential and is related to Gibb s Free Energy Equation AG nFE RT ln Keq Cell half potentials are found by Ecell Eright Elel t Defining Electrode Potentials and Standard Electrode Potentials A An electrode potential is the potential of a cell consisting of the electrode in question acting as the right hand electrode and the standard hydrogen electrode acting as the left hand electrode B The standard electrode potential of a half reaction is defined as its electrode potential when the activities of the reactanm and producm are all unity V The Nerst Equation E E 00592n log g m a b A B The Nerst Equation relates the potential to the concentrations activity of the participanm in an electrochemical halfcell A formal potential is the electrode potential when the ratio of analytical concentrations of reactants and products of a half reaction are exactly 100 and the molar concentration of any other solutes are specified Problem 1613 E E 00592n log magi a b A B a E 0337 005922 log 100440 0297 V b Ksp CuCl 19x10 7 CuCl E 0521 005921 log 1Cu 0521 005911 log Cl Ksp E 0521 005921 log 007519x10 7 0521 005921 log 3952105 E 0521 0331 0190 V c Ksp Cu0Hz 48x10 20 011 48x10 20OHz E 0337 005922 log OHzKsp 0337 005922 log 00400 48x10 20 0337 005922 log 33321016 0337 0489 0152 V 0 n 562x10 wm11 0111 NH314 1Cuz 562x10 101281 00250 E 0337 005922 log 6032109 0337 0289 0048 V e Use equation 1523 K39MY 14KMY IMYMI Mm CT and substitute CuYquotCu CT me 36x10 9 x 6321018 22721010 CuYz 400x10 3 cT 290x10 z 4002103 250x10 z 0004Cuz 0025 22721010 1Cu 227x101000250004 14221011 E 0337 005922 log 1Cuz 0337 005922 log 14221011 0337 0003 w Problem 1624 E 0763 00296 log 1Zn2 ZnYkl 32x101 ZnYzl Y4 Zn wmxmm E 0763 00296 log jx 32x10E ZnYz when Y4 ZnYz 100 E Em E E2 0763 00296 log 100 32x10 100 125 V Professor Dr D Rahni PA CE UNIVERSITY WES T CHES T ER DYSON COLLEGE OF ART S AND SCIENCES WES T CHES T ER CAMPUS GENERAL CHEMISTRY I CHE 111 FALL 1999 Emergency Closing Number 914 773 3398 Email address nrahnipaceedu LECTURE OUTLINE Text Chemist Raymond Chang McGraw Hill Inc 63911 edition 1998 Week 4amp5 Recommended Study Guide to accompany the text Kenneth W Watkins Topic Chemistry The Study of Change Chemistry A Science for the Twenty rst Century The Scienti c Method The Study of Chemistry Classi cations of Matter The Three States of Matter Physical and Chemical Properties of Matter Measurement Handling Numbers The FactorLabel Method of SolVing Problem Atoms Molecules and Ions The Atomic Theory The Structures of the Atom The Periodic Table of the Elements Atomic Number Mass Number and Isotopes Molecules and Ions Chemical Formulas Naming Compounds Mass Relationships in Chemical Reactions Atomic Mass Molar Mass of an Element and Avogadro s Number Molecular Mass The Mass Spectrometer Percent Composition of Compounds Experimental Determination of Empirical Formulas Chemical Reactions and Chemical Equations Amounts of Reactants and Products Limiting Reagents Reaction Yield Reactions in Aqueous Solution General Properties of Aqueous Solutions Percipitation Reactions Chemistry 1 1 1 continued page 2 Top39c Lecture Outline Week Chapter 6 4 continued 10 amp 11 Atoms Acid Base Reactions Oxidation Reduction Reactions Concentration of Solutions Gravimetric Analysis Acid Base Titrations Redox Titrations EX A M I Chapters 14 5 EXAM II The Gaseous State Substances that Exist as Gases Pressure of a Gas The Gas Laws The Ideal Gas Equation Gas Stoichiometry Dalton s Law of Partial Pressures The Kinetic Molecular Theory of Gases Deviation from Ideal Behavior Thermochemist The Nature of Energy and Types of Energy Energy Changes in Chemical Reactions Enthalpy Calorimet Standard Enthalpy of Formation and Reaction Heat of Solution and Dilution Introduction to Thermodynamics Quantum Theory and the Electronic Structure of From Classical Physics to Quantum Theory The Photoelectric Effect Bohr s Theory of the Hydrogen Atom The Dual Nature of the Electron Quantum Mechanics and Quantum Numbers Atomic Orbitals Electron Con guration The BuildingUp Principal N Chapters 5 7 Periodic Relationships Among the Elements Development of the Periodic Table Periodic Classi cation of the Elements Periodic Variation in Physical Properties Ionization Energy Electron Af nity Variation in Chemical Properties of the Representative Elements continued Chemistry 111 Lecture Outline page 3 Week Chapter Top39c 13 9 Chemical Bonding I Basic Concepts Lewis Dot Symbols The Ionic Bond Lattice Energy of Ionic Compounds The Covalent Bond Electronegativity Writing Lewis Structures Formal Charge and Lewis Structure The Concept of Resonance Exceptions to the Octet Rule Bond Dissociation Energy F I N A L E X A M CUMULATIVE COURSE GRADE Exam I 15 Exam II 20 Final Exam Cumulative 30 Laboratory 25 Homework Assignment 10 Recitation and class participation While there is no provision for makeup exams such decision is only at the discretion of the professor and based upon a welldocumented reason as veri ed by the appropriate University office and only for the most compelling reason All students must pass the laboratory component in order to pass this course Homework assignment At the completion of a chapter you select and solve no less than 12 number crunching questions from the end of the chapter Whereas your degree of selecting and tackling more challenging questions will each be included in the outcome such a batch is due within a week from the completion of a chapter You will then have access to solutions in Dyson 213 by presenting a picture ID David N Rahni is Professor of Analytical Chemistry and the founder and former Director of Graduate Program in Environmental Science at Pace University Pleasantville New York In addition he serves as an adjunct professor in both the LLM Environmental Law Program at the Pace University School of Law and the Department of Dermatology at the New York Medical College He is the 1999 Chair Elect and 2000 Chair of the American Chemical Society s New York Section He was selected the 1996 Distinguished Scientist by the American Chemical Society s Westchester Section During 199394 he was J William Fulbright Senior Research Scholar at the Technical University of Denmark DTU and visiting professor at the University of Oxford UK He was also awarded a visiting professorship to DTU Denmark by the Royal Danish continued Chemistry 1 1 1 Lecture Outline page 4 Research Academy for the summer 1994 where he offered a threeday workshop on surface characterization methodology In the past he has served as an adjunct professor of chemistry at Manhattanville College has held visiting scientist positions with the IBM Thomas J Watson Research Center and CibaGeigy Research Division and has either been a visiting professor or given extended lectures at the II University of Rome the University of Florence National University of Mexico Universities of Southampton Leeds Loughborough London Copenhagen and the Danish Orsted Institute He has also served as a visiting United Nations TOKTEN Scholar in the third world presenting lectures and assisting in curriculum development in among others Tehran Guilan and the National Universities of Iran summer 1992 and 1995 He has provided consultation services to many industries and served extensively as expert witness on legal matters He is versed in the challenges faced by the higher education in the new millenium Professor Rahni has earned his PhDPostdoctoral studies in Analytical Chemistry in Professor G G Guilbault s research laboratory at the LSU University of New Orleans 198586 his MS in Chemistry at Eastern New Mexico University 1980 and his BSc in Chemistry at the National University of Iran 1979 He has published or presented extensively None hundred twenty in such diverse fields as immobilized enzyme electrochemical sensors for clinical environmental and industrial assays electrodeposition of thinfilm compositionallymodulated alloys and metal multi laminated nanostructures for r 39 39 and r 39 39 39 applications in situ pH and other key measurements in the diffusion layer of the cathode during the electrodeposition of metals process engineering the direct and indirect electrochemical investigation of oxidoreductase enzymes and proteins and their surface interactions asymmetric synthesis and mechanistic studies of congested heterocyclic phosphorous sulfur and germanium compoundsenvironmental sciences and law sustainable development and chemical education A recipient of 199798 Kenan Award for Teaching Excellence David Rahni has organized and chaired numerous workshops and symposia as typified by his current fundraising and program leadership for the Nichols Medal Symposium and Banquet the oldest Chemistry Medal in the Nation He was the General Chair and host for the 31st Middle Atlantic Regional Meeting of the American Chemical Society His past membership on the Environmental Advisory Council for the US 20th Congressional District Representative Nita M Lowey and his leadership role as a founding member in Partners for Sustainable Development NYS wide Initiatives for Economic Development and Climatic Change Conference and Rene DuBos Annual Conference on Automobile Energy and Societal Impact highlight his other leadership contributions DN Rahni PhD Professor of Chemistry and Dir Grad Prog Environmental Science PACE UNIVERSITY Pleasantville NY 105702799 voice 9147733655 Fax 9147733418 amp 3541 for more than 5 pages email nrahnipacee u httpdv on have 39 39 htm 3 3 3 ms Word syllabus chlll lecd0c
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