The Chemistry of CO 2. Walter E. Cleland, Jr. Ph.D. Department of Chemistry and Biochemistry 25 February 2008
|
|
- Lindsey McDaniel
- 6 years ago
- Views:
Transcription
1 The Chemistry of CO 2 Walter E. Cleland, Jr. Ph.D. Department of Chemistry and Biochemistry 25 February 2008
2 Outline Introduction Physical Properties Uses Production, Recovery, Purification Chemical Properties
3 Oxides of Carbon Stable Oxides of Carbon CO C O CO 2 O C O C 3 O 2 C 12 O 9 O C C C O O O O O O O O O O
4 Selected Physical Properties of CO 2 Colorless, Odorless Gas Molecular Weight Mp Critical T Critical P Density of and C Relative density of and 21.1 o C (Air=1) Solubility in water at 25 o C Henry s Law constant Gº f (CO 2 (g)) Hº f (CO 2 (g)) Sº f (CO 2 (g)) Dissociation Energy (C-O) IR (gas) UV (gas) 44.01g/mol C (5.2 atm) C (subl) 31 C atm ( psi) Kg/m ppm (wt) 392 x 10-4 mol/l atm kj/mol kj/mol 3.02 J/mol K kj/mol 2349 cm -1 (Asym C=O), cm -1 (Sym C=O; Raman), 667 cm -1 (Bending) Å
5 Phase Diagram
6 Walsh Diagram
7 Industrial Uses of CO 2 Uses Based on Physical Properties (major) Refrigeration Cleaning fluid Air conditioning Solvent for Reactions Extractions Nanopartical production Food and Agro-chemical Applications Fumigant Additive to beverages Inert atmosphere Uses Based on Chemical Properties Production of Urea Production of Salicylic acid Inorganic carbonates and pigments Production of Propylene carbonate Neutralization of caustic waste water
8 Production Sources Ammonia/Hydrogen plants CH H 2 O CO H 2 Flue gases from combustion Fermentation C 6 H 12 O 6 2 C 2 H 5 OH + 2 CO 2 Lime-kiln operations CaCO 3 CaO + CO 2 Sodium phosphate manufacture 3 Na 2 CO H 3 PO 4 2 Na 3 PO CO H 2 O Natural CO 2 gas wells
9 Recovery by Reversible Absorption Sodium or Potassium Carbonate Process K 2 CO 3 (aq) + H 2 O(l) + CO 2 (g) KHCO 3 (aq) Girbotol Amine Process 2 HOCH 2 CH 2 NH 2 (aq) + H 2 O(l) + CO 2 (g) (HOCH 2 CH 2 NH 3 ) 2 CO 3 (aq)
10 Purification Permanganate Process 3 H 2 S + 2KMnO CO 2 3 S + 2 MnO KHCO H 2 O Dichromate Process 3 H 2 S + K 2 Cr 2 O 7 + H 2 O + 2 CO 2 3 S + 2 Cr(OH) KHCO 3
11 Chemical Properties General Reactivity Aqueous chemistry Reactions of Industrial Importance Biological Reactions Organic Reactions Coordination Chemistry Reactions incorporating CO 2 without Reduction Reactions with Reduction
12 General Reactivity Not very reactive at ordinary temperature ; nonreactive ; stable ; inert Many reactions of CO 2 are thermodynamically favorable, but kinetically slow Ex: M 2 SiO CO 2 2 MCO 3 + SiO 2
13 Aqueous Chemistry Species involved: CO 2, H 2 CO 3, HCO 3-, CO 3 2-, H +, OH -, [H 2 CO 3* ] = [CO 2 (aq)] + [H 2 CO 3 ] Equilibrium concentrations described completely by system of 5 equations CO 2 + H 2 O H 2 CO 3 K 1 = 1.67 x 10-3 H 2 CO * 3 H + + HCO - 3 K 2 = 4.47 x 10-7 H 2 CO 3 H + + HCO - 3 K a = 2.68 x 10-4 HCO - 3 H + + CO 2-3 K 3 =4.68 x H 2 O H + + OH - K w = 1.0 x C T = [H 2 CO 3* ] + [HCO 3- ] + [CO 2-3 ] Carbonates insoluble K sp (CaCO 3 ) = 2.8 x 10-9 ; K sp (MgCO 3 ) = 3.5 x 10-8
14 Slow Kinetics for Reactions of At ph < 8 CO 2 CO 2 + H 2 O H 2 CO 3 (slow) H 2 CO 3 + OH - HCO 3- (fast) At ph > 10 CO 2 + OH - HCO 3 - (slow) HCO 3- + OH - CO 3 2- (fast) At ph 8-10 both sets of equilibria are important.
15 Important Reactions of CO 2, At high temperature 2 C + O 2 2 CO C + O 2 CO 2 C + H 2 O CO + H 2 CO and O 2 Hº = kj/mol Hº = kj/mol Hº = kj/mol 2 CO C + CO 2 Hº = kj/mol CO 2 CO + 1/2 O 2 Also CO 2 + H 2 CO + H 2 O (reverse of water-gas shift rxn) CO NH 3 NH 4 O 2 CNH 2 NH 2 CONH 2 + H 2 O
16 Basic Organic Reactions
17 Coordination Chemistry CO 2 is a poor ligand A number of complexes and bonding modes known Important for activation of CO 2 in reduction reactions
18 Reactions of M-CO 2 With Protons or other electrophile M-CO 2 + 2H + + 2e - M-CO + H 2 O M-CO 2 + R + M-C(O)OR Hydride insertion M-H + CO 2 M-O 2 CH With External Phosphine M-CO 2 + PR 3 M-CO + O=PR 3 With Coordinated Isonitrile M(CNR)(CO 2 ) RNCO + M-CO
19 Biological Reactions Ubiquitous in Nature Animal metabolism C 6 H 6 O O 2 6 CO H 2 O + energy Photosynthesis is reverse of above reaction Numerous enzymes catalyze reactions of CO 2 Carbonic anhydrase (Zn 2+ ) - H 2 CO 3 CO 2 RuBisCO (Mg 2+ ) - carboxylation of ribose Carbon monoxide dehydrogenase (Ni,Fe) - CO 2 CO
20 Use of CO 2 as C 1 Feedstock Conversion reactions (CO 2 not reduced) Carboxylates, lactones RCOOR Carbamates, RR NCOOR Ureas, RR NCONRR Isocyanates, RNCO Carbonates, ROC(O)OR Reduction of CO 2 Formates, HCOO - Oxalates, - O 2 C-CO 2 - Formaldehyde, H 2 CO Carbon Monoxide, CO Methanol, CH 3 OH Methane, CH 4
21 Carboxylation Reactions C-C bond formation Direct carbonylation in ionic liquid from imidazoliumcarbonate N-C, O-C bond formation also known
22 Metal Salen complexes as catalysts Production of Polycarbonates from Epoxides and CO 2 Plastics from CO 2
23 CO 2 Hydrogenation to form Formic Acid
24 Production of Methanol CO + 2 H 2 CH 3 OH CO H 2 CH 3 OH Cu-Zn-O catalyst, ºC, 5-10 MPa Up to 30% CO 2 added to syngas feedstock significantly improves yield CO 2 + H 2 O CH 3 OH Cascade of enzymes CO 2 HCOO - (formate dehydrogenase) HCOO - CH 2 O (formaldehyde dehydrogenase) CH 2 O CH 3 OH (methanol dehydrogenase)
25 Photoelectrochemical Reduction In anhydrous,aprotic solvent, reduction potential of CO 2 to CO 2 - is -2.2V vs NHE! Large kinetic overvoltage Yield of photochemical conversion is low Proton assisted multielectron reductions more favorable CO 2 + 2H + + 2e - HCO 2 H CO H + + 6e - CH 3 OH + H 2 O -0.61V -0.38V
26 References Cotton,F.A.; Wilkinson, G.; Murillo,C.A.; Bochmann, M.; Advanced Inorganic Chemistry 6th ed.; Wiley-Interscience: New York, Greenwood, N.N.; Earnshaw, A.; Chemistry of the Elements; Pergamon: New York, Aresta, M. Carbon Dioxide Reduction and Uses as a Chemical Feedstock. In Activation of Small Molecules: Organometallic and Bioinorganic Perspectives; Tolman, W.B., Ed.; Wiley-VCH: Weinheim, Stumm, W.; Morgan, J.J.; Aquatic Chemistry: Chemical Equilibria and Rates in Natural Waters; Wiley: New York, Ballou, R.W. Carbon Dioxide. In Kirk-Othmer Encyclopedia of Chemical Technology; Wiley: New York, 2005; Vol. 4, pp Tommasi, I.; Sorrentino, F.; Utilization of 1,3-dialkylimidazolium-2-carboxylates as CO 2 -carriers in the presence of Na + and K + : Application in the Synthesis of Carboxylates, Monomethylcarbonate Anions and Halogen-free Ionic Liquids. Tetrahedron Letters 2005, 46, Darrensbourg, D.J.; Making Plastics from Carbon Dioxide: Salen Metal Complexes as Catalysts for the Production of Polycarbonates from Epoxides and CO 2. Chem. Rev. 2007, 107, Leitner, W. Carbon Dioxide as a Raw Material: The Synthesis of Formic Acid and Its Derivatives from CO 2. Angewante Chemie International Edition in English 1995, 34,
EXAM OF SCIENTIFIC CULTURE MAJOR CHEMISTRY. CO 2 hydrogenation
EXAM OF SCIETIFIC CULTURE MAJOR CHEMISTRY CO 2 hydrogenation One possibility to limit CO 2 imprint on the global warming is to reduce CO 2 to more usable forms such as hydrocarbons. These can serve as
More informationSectional Solutions Key
Sectional Solutions Key 1. For the equilibrium: 2SO 2 (g) + O 2 (g) 2SO 3 (g) + 188 kj, the number of moles of sulfur trioxide will increase if: a. the temperature of the system is increased (at constant
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationCH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
More informationProperties of Compounds
Chapter 6. Properties of Compounds Comparing properties of elements and compounds Compounds are formed when elements combine together in fixed proportions. The compound formed will often have properties
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationUnit 1 - Foundations of Chemistry
Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its
More informationRevision of Important Concepts. 1. Types of Bonding
Revision of Important Concepts 1. Types of Bonding Electronegativity (EN) often molecular often ionic compounds Bonding in chemical substances Bond energy: Is the energy that is released when a bond is
More informationSolubility of gases in water: Henry s Law concentration dissolved / partial pressure of the gas K H (units mol L -1 atm -1 ) = c X /p X
CHEM/TOX 336 Lecture 11/12 Dissolved Gases in Natural Water Dissolved Solids in Natural Water Solubility of gases in water: Henry s Law concentration dissolved / partial pressure of the gas K H (units
More information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More informationLe Châtelier's Principle. Chemical Equilibria & the Application of Le Châtelier s Principle to General Equilibria. Using Le Châtelier's Principle
Chemical Equilibria & the Application of Le Châtelier s Principle to General Equilibria CHEM 107 T. Hughbanks Le Châtelier's Principle When a change is imposed on a system at equilibrium, the system will
More informationAmmonia * Andrew R. Barron. 1 Synthesis. 2 Structure
OpenStax-CNX module: m32956 1 Ammonia * Andrew R. Barron This work is produced by OpenStax-CNX and licensed under the Creative Commons Attribution License 3.0 Ammonia (NH 3 ) is a colorless, pungent gas
More informationChapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary
Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen s electronegativity is high (3.5) and hydrogen s is low (2.1)
More informationF322: Chains, Energy and Resources Rates and Equilibria
F322: Chains, Energy and Resources 2.3.2 Rates and Equilibria 1. Dilute aqueous hydrogen peroxide, H 2 O 2 (aq), is used to sterilise contact lenses. Dilute H 2 O 2 (aq) slowly decomposes at room temperature
More informationCHAPTER Describing Chemical Reactions Reactants Products. New substances produced The arrow means yields TYPES OF EQUATIONS.
CHAPTER 11 Chemical Reactions 11.1 Describing Chemical Reactions Reactants Products New substances produced The arrow means yields Where do Chemical Reactions occur? Everywhere!!! In living organisms In
More informationShifting Equilibrium. Section 2. Equilibrium shifts to relieve stress on the system. > Virginia standards. Main Idea. Changes in Pressure
Section 2 Main Ideas Equilibrium shifts to relieve stress on the system. Some ionic reactions seem to go to completion. Common ions often produce precipitates. > Virginia standards CH.3.f The student will
More information10/26/2010. An Example of a Polar Reaction: Addition of H 2 O to Ethylene. to Ethylene
6.5 An Example of a Polar Reaction: Addition of H 2 O to Ethylene Addition of water to ethylene Typical polar process Acid catalyzed addition reaction (Electophilic addition reaction) Polar Reaction All
More information10.3 Types of Chemical Reactions
10.3 Types of Chemical Reactions Chemical equations follow certain patterns Combination (synthesis ) The number of possible chemical is very large. However, there are a limited number of structural patterns
More informationCHEMpossible. Final Exam Review
CHEMpossible Final Exam Review 1. Given the following pair of reactions and their equilibrium constants: 2NO 2 (g) 2NO (g) + O 2 (g) K c = 15.5 2NO (g) + Cl 2 (g) 2 NOCl (g) K c = 3.20 10-3 Calculate a
More informationDissolved Gases in Natural Water Dissolved Solids in Natural Water
Dissolved Gases in Natural Water Dissolved Solids in Natural Water Solubility of gases in water: Henry's Law concentration dissolved / partial pressure of the gas K H (units mol L -1 atm -1 ) = c X /p
More informationChem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria)
Name: Date: Exam #: _ Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria) Multiple Choice Identify the letter of the choice that best completes the statement or answers
More informationChapter 14 THE GROUP 14 ELEMENTS. Exercises
Chapter 14 THE GROUP 14 ELEMENTS Exercises 14.1 (a) Li 2 C 2 (s) + 2 H 2 O(l) 2 LiOH(aq) + C 2 H 2 (g) (b) SiO 2 (s) + 2 C(s) Si(l) + 2 CO(g) (c) CuO(s) + CO(g) Cu(s) + CO 2 (g) (d) Ca(OH) 2 (aq) + CO
More informationSolubility Equilibria
Solubility Equilibria Heretofore, we have investigated gas pressure, solution, acidbase equilibriums. Another important equilibrium that is used in the chemistry lab is that of solubility equilibrium.
More informationCAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
Centre Number Candidate Number Candidate Name CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/2 PAPER 2 OCTOBER/NOVEMBER
More informationChemistry 122 Wrap-Up Review Kundell
Chapter 11 Chemistry 122 Wrap-Up Review Kundell 1. The enthalpy (heat) of vaporization for ethanol (C 2 H 5 OH) is 43.3 kj/mol. How much heat, in kilojoules, is required to vaporize 115 g of ethanol at
More informationChemistry 112, Spring 2006 Prof. Metz Final Exam Name Each question is worth 4 points, unless otherwise noted
Chemistry 112, Spring 2006 Prof. Metz Final Exam Name Each question is worth 4 points, unless otherwise noted 1. The predominant intermolecular attractive force in solid sodium is: (A) metallic (B) ionic
More informationAP Chemistry. 4. Which atom in its ground state has the most unpaired electrons? a. Ge b. As c. Se d. Br e. Ga
Name AP Chemistry Take Home Quiz Due Thursday, 1/9/2014 Bubble the correct answer on your scantron for each of the following. 1. Barium sulfate is LEAST soluble in a 0.01-molar solution of which of the
More information(b) Describe, and explain, what would happen to the position of the NO 2 /N 2 O 4 equilibrium if the following changes are made
1. Nitrogen dioxide, NO 2, and dinitrogen tetroxide, N 2 O 4, take part in the following equilibrium. 2NO 2 (g) N 2 O 4 (g) ΔH = 58 kj mol 1 (a) State le Chatelier s principle. (b) Describe, and explain,
More informationSection 3 Environmental Chemistry
Section 3 Environmental Chemistry 1 Environmental Chemistry Definitions Chemical Reactions Stoichiometry Photolytic Reactions Enthalpy and Heat of Reaction Chemical Equilibria ph Solubility Carbonate Systems
More informationChemistry 1A Fall 2010 Exam 2 Key Chapters 4 (part), 5, 6, and 7 (part)
Chemistry 1A Fall 010 Exam Key Chapters 4 (part), 5, 6, and 7 (part) You might find the following useful. 0.008314 kj ΔH = ΔE + (Δn)RT R = K mol 0.00418 kj q = C calδt + m w g C H rxn = Σ H f (products)
More information(g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (c) Chromium(III) sulfate: ; (h) Dinitrogen tetroxide:
1. Name each of the following compounds: (a) Ca(OCl) 2 : ; (b) (NH 4 ) 3 PO 4 : ; (c) K 2 Cr 2 O 7 : ; (d) HBrO 2 : ; (e) PF 5 : ; (f) B 2 O 3 : ; (g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (i) Na 2 C 2 O 4
More informationCH 221 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak
More informationChapter 6: Chemical Bonds
Chapter 6: Chemical Bonds Section 6.1: Ionic Bonding I. Stable Electron Configurations Group # II. III. Ionic Bonds Group # A. Transfer of Electrons Group # B. Formation of Ions Group # C. Formation of
More informationWYSE Academic Challenge 2004 Sectional Chemistry Solution Set
WYSE Academic Challenge 2004 Sectional Chemistry Solution Set 1. Answer: d. Assume 100.0 g of the compound. Thus, we have 40.00 g of carbon, or 40.00/12.01 = 3.33 mol C. We have 6.71 g of hydrogen, or
More informationChapter 19 Chemical Thermodynamics
Chapter 19. Chemical Thermodynamics Sample Exercise 19.2 (p. 819) Elemental mercury is a silver liquid at room temperature. Its normal freezing point is -38.9 o C, and its molar enthalpy of fusion is H
More informationChem 101 Review. Fall 2012
Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table
More informationChapter 4 Electrolytes and Aqueous Reactions. Dr. Sapna Gupta
Chapter 4 Electrolytes and Aqueous Reactions Dr. Sapna Gupta Aqueous Solutions Solution - a homogeneous mixture of solute + solvent Solute: the component that is dissolved Solvent: the component that does
More informationEquilibrium. What is equilibrium? Hebden Unit 2 (page 37 69) Dynamic Equilibrium
Equilibrium What is equilibrium? Hebden Unit (page 37 69) Dynamic Equilibrium Hebden Unit (page 37 69) Experiments show that most reactions, when carried out in a closed system, do NOT undergo complete
More informationReaction Rate and Equilibrium Chapter 19 Assignment & Problem Set
Reaction Rate and Equilibrium Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Reaction Rate and Equilibrium 2 Study Guide: Things You Must Know
More informationChanna Asela
Reproducing the following contents by amending or deleting the author s name and contact numbers is prohibited. You may email or print without any amendment. Underline the most suitable answer 1995-I-2
More information0620 Chemistry Paper 3 (Extended) Paper 32 O/N/10. Paper 32 M/J/10. Paper 3 O/N/09
0620 Chemistry Paper 3 (Extended) Paper 32 O/N/10 no. 1 properties of elements and compounds 4,21 44, 266 2 zinc and zinc blende chemistry, distillation 8,2,23 90,19,280 3 breaking down MnO 2, rate of
More informationAngel International SchoolManipay
Grade OL Angel International SchoolManipay 2 nd Term Examination March, 2016 Chemistry Duration: 3 Hours 1. Which property is common to calcium, potassium and sodium? a) Their atoms all lose two electrons
More informationBasic Concepts of Chemistry and Chemical Calculations. The ratio of the average mass factor to one twelfth of the mass of an atom of carbon-12
Basic Concepts of Chemistry and Chemical Calculations Relative Atomic mass: The relative atomic mass is defined as the ratio of the average atomic mass factor to the unified atomic mass unit. (Or) The
More informationHonors text: Ch 10 & 12 Unit 06 Notes: Balancing Chemical Equations
Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely
More informationRedox Worksheet 1: Numbers & Balancing Reactions
Name: Date: Per: Redox Worksheet 1: Numbers & Balancing Reactions Assigning Oxidation Number rules: Elements and Compounds have an oxidation number/total of 0 Group I and II In addition to the elemental
More informationPractice I: Chemistry IGCSE
Practice I: Chemistry IGCSE cristian.obiol@gmail.com 1) Explain the following processes related to changes of states of matter. -Melting:... -Vaporization:... -Freezing:... -Condensation:... -Sublimation:...
More informationChapter 1 Reactions of Organic Compounds. Reactions Involving Hydrocarbons
Chapter 1 Reactions of Organic Compounds Reactions Involving Hydrocarbons Reactions of Alkanes Single bonds (C-C) are strong and very hard to break, therefore these compounds are relatively unreactive
More information2) Solve for protons neutrons and electrons for the bromide ION.
1) Write the formulas for the following a) Calcium nitride c)lithium hydroxide b) Iron (III) sulfide d) sulfuric acid 2) Solve for protons neutrons and electrons for the bromide ION. 3) Write the electron
More information2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression.
Practice Problems for Chem 1B Exam 1 Chapter 14: Chemical Equilibrium 1. Which of the following statements is/are CORRECT? 1. For a chemical system, if the reaction quotient (Q) is greater than K, products
More informationBonus Final Exam 3. 1 Calculate the heat of reaction,δh 0 rxn, for the following reaction as written at 298 K: g 2H 2 CH 4. g CF 4.
Bonus Final Exam 3 1 Calculate the heat of reaction,δh rxn, for the following reaction as written at 298 K: CH 4 2F 2 CF 4 2H 2 substance CH 4 CF 4 ΔH f kj/mol 75 68 (A) ΔH rxn 23 kj (B) ΔH rxn 914 kj
More informationFinal S2 (2011) - Practice Test - Ch 11, 12, 13, 14, 15, 16, 18, 19, 22, 23
Final S2 (2011) - Practice Test - Ch 11, 12, 13, 14, 15, 16, 18, 19, 22, 23 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. If 12.0 g of a gas at 2.5 atm
More informationChapter 18. Reversible Reactions. A chemical reaction in which the products can react to re-form the reactants is called a reversible reaction.
Section 1 The Nature of Chemical Equilibrium Reversible Reactions A chemical reaction in which the products can react to re-form the reactants is called a reversible reaction. Section 1 The Nature of Chemical
More informationelemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another.
CHEMICAL TYPES HANDOUT In these reactions, a free element reacts with a compound to form another compound and release one of the elements of the original compound in the elemental state. There are two
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationTopic 1: Quantitative chemistry
covered by A-Level Chemistry products Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant 1.1.1 Apply the mole concept to substances. Moles and Formulae 1.1.2 Determine the number
More informationChemistry 20 Unit 3A Solutions FITB Notes. Topic A Classification of Solutions
Chemistry 20 Unit 3A Solutions FITB Notes General Outcome: Topic A Classification of Solutions Matter is a substance with and A substance is a type of matter with one definite formula (elements, compounds)
More informationCHEMISTRY: A Study of Matter
Review Sheet: Unit 6 Name KEY I. Fill in the blanks with the most appropriate term: Common names of substances like milk of magnesia or lime usually give no information about the chemical composition of
More informationChapter 15 THE GROUP 15 ELEMENTS. Exercises
Chapter 15 THE GROUP 15 ELEMENTS Exercises 15.2 (a) NH 4 NO 2 (aq) N 2 (g) + 2 H 2 O(l) (b) (NH 4 ) 2 SO 4 (aq) + 2 NaOH(aq) Na 2 SO 4 (aq) + 2 NH 3 (g) + 2 H 2 O(l) (c) 3 NH 3 (g) + H 3 PO 4 (aq) (NH
More informationChapter Test B. Chapter: Chemical Equilibrium. following equilibrium system? 2CO(g) O 2 (g) ^ 2CO 2 (g)
Assessment Chapter Test B Chapter: Chemical Equilibrium PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. What is
More informationCHEMISTRY CP Name: Period:
CHEMISTRY CP Name: Period: CHEMISTRY SPRING FINAL REVIEW SHEET NOTE: Below are concepts that we have covered in class throughout the second semester. Questions are organized by chapter/concept to help
More informationChem. 1A Midterm 2 Version A
Chem. 1A Midterm 2 Version A Name Student Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units and for the incorrect number of significant figures.
More informationS 8 + F 2 SF 6 4/9/2014. iclicker Participation Question: Balance the following equation by inspection: H + + Cr 2 O 7 + C 2 H 5 OH
Today: Redox Reactions Oxidations Reductions Oxidation Numbers Half Reactions Balancing in Acidic Solution Balancing in Basic Solution QUIZ 3 & EXAM 3 moved up by one day: Quiz 3 Wednesday/Thursday next
More information15.1: Hydrocarbon Reactions
15.1: Hydrocarbon Reactions Halogenation An alkane will react with a halogen to produce a halalkane and the corresponding hydrogen halide. The catalyst is ultraviolet radiation. Reaction 1 methane chlorine
More informationConservation The Law of Conservation of Matter states that matter cannot be created or destroyed in ordinary chemical reactions. This means that no
Chemical Reactions Conservation The Law of Conservation of Matter states that matter cannot be created or destroyed in ordinary chemical reactions. This means that no atoms can be lost or gained. This
More informationUnit-8 Equilibrium. Rate of reaction: Consider the following chemical reactions:
Unit-8 Equilibrium Rate of reaction: Consider the following chemical reactions: 1. The solution of sodium chloride and silver nitrate when mixed, there is an instantaneous formation of a precipitate of
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions Chapter 4 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A solution is a homogenous mixture of 2 or more substances. The solute
More informationChem 130 Name Exam 2 October 11, Points Part I: Complete all of problems 1-9
Chem 130 Name Exam October 11, 017 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and significant
More informationAP Chem Chapter 14 Study Questions
Class: Date: AP Chem Chapter 14 Study Questions 1. A burning splint will burn more vigorously in pure oxygen than in air because a. oxygen is a reactant in combustion and concentration of oxygen is higher
More informationChemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions
Chemical Reactions Ch. 11 Chemical Reactions when a substance changes identity Reactants - original Products - resulting law of conservation of mass total mass of reactants = total mass of products In
More information(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion
AP Chemistry - Problem Drill 08: Chemical Reactions No. 1 of 10 1. What type is the following reaction: H 2 CO 3 (aq) + Ca(OH) 2 (aq) CaCO 3 (aq) + 2 H 2 O (l)? (A) Composition (B) Decomposition (C) Single
More informationChemistry 2000 Lecture 14: Redox reactions
Chemistry 2000 Lecture 14: Redox reactions Marc R. Roussel February 8, 2018 Marc R. Roussel Chemistry 2000 Lecture 14: Redox reactions February 8, 2018 1 / 12 Review: Oxidation states The oxidation state
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions
More informationCHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A
CHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A 1. Consider a balloon filled with 5 L of an ideal gas at 20 C. If the temperature of the balloon is increased by 70 C and the external pressure acting on the
More informationUnit 5: Spontaneity of Reaction. You need to bring your textbooks everyday of this unit.
Unit 5: Spontaneity of Reaction You need to bring your textbooks everyday of this unit. THE LAWS OF THERMODYNAMICS 1 st Law of Thermodynamics Energy is conserved ΔE = q + w 2 nd Law of Thermodynamics A
More informationChem 1A Dr. White Fall Handout 4
Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular
More informationChapter 10: Carboxylic Acids and Their Derivatives
Chapter 10: Carboxylic Acids and Their Derivatives The back of the white willow tree (Salix alba) is a source of salicylic acid which is used to make aspirin (acetylsalicylic acid) The functional group
More informationChapter 3 Chemical Reactions
Chapter 3 Chemical Reactions Jeffrey Mack California State University, Sacramento Chemical Reactions Reactants: Zn + I 2 Product: ZnI 2 Chemical Reactions Evidence of a chemical reaction: Gas Evolution
More informationALE 23. Balancing Redox Reactions. How does one balance a reaction for both matter and charge?
Name Chem 163 Section: Team Number: ALE 23. Balancing Redox Reactions (Reference: Section 4.5 (pp. 158 166) and 21.1 Silberberg 5 th edition) How does one balance a reaction for both matter and charge?
More informationGeneral Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
More informationRedox, ph, pe OUTLINE 9/12/17. Equilibrium? Finish last lecture Mineral stability Aquatic chemistry oxidation and reduction: redox
Redox, ph, pe Equilibrium? OUTLINE Finish last lecture Mineral stability Aquatic chemistry oxidation and reduction: redox Reading: White p555-563 1 Question of the day? So what about the CO 2 system? CO
More informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
More informationIn terms of production, nitric acid is the third most widely produced acid across the world.
In terms of production, nitric acid is the third most widely produced acid across the world. It has a wide range of uses in agriculture, industry and medicine where it is used as a fertiliser and in the
More informationCHEMISTRY HIGHER LEVEL
*P15* PRE-LEAVING CERTIFICATE EXAMINATION, 2008 CHEMISTRY HIGHER LEVEL TIME: 3 HOURS 400 MARKS Answer eight questions in all These must include at least two questions from Section A All questions carry
More informationChapter 5. Chemical reactions
Chapter 5 Chemical reactions Chemical equations CaO(s) + CO 2 (g) CaCO 3 (s) + CO(g) Chemical equation - representation of a chemical reaction; uses the symbols of the elements and formulae of the compounds
More informationNanoscale pictures: Figs. 5.1, 5.4, and 5.5
Solutions and concentration Solution: a homogeneous mixture of two or more substances. Example: water, sugar, flavor mixture (Coke). The substances are physically combined, not chemically combined or bonded
More informationCHEMICAL REACTIONS. Discuss breaking/forming bonds 10/29/2012. Products Reactants
CHEMICAL REACTIONS - Page 321 Products Reactants Reactants: Zn + I 2 Product: Zn I 2 Discuss breaking/forming bonds Chemical Reaction or Change process in which one or more substances are converted into
More informationStoichiometry. Mole Concept. Balancing Chemical Equations
Stoichiometry The story so far The structure of an atom protons, neutrons & electrons Electron structure & the Periodic Table Shapes of electron orbitals (Quantum Numbers) Essential and toxic elements
More informationCHEM 101A EXAM 1 SOLUTIONS TO VERSION 1
CHEM 101A EXAM 1 SOLUTIONS TO VERSION 1 Multiple-choice questions (3 points each): Write the letter of the best answer on the line beside the question. Give only one answer for each question. B 1) If 0.1
More informationChemical Equations and Chemical Reactions
Chemical Equations Chemical Equations and Chemical Reactions Chemical equations are concise representations of chemical reactions. Chemical Equations Symbols Used in Chemical Equations The formulas of
More informationChapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions. Dr. Sapna Gupta
Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions Dr. Sapna Gupta Types of Reactions Two classifications: one how atoms are rearrangement and the other is chemical
More informationACP Chemistry (821) - Mid-Year Review
ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference
More informationAqueous Equilibria, Part 2 AP Chemistry Lecture Outline
Aqueous Equilibria, Part 2 AP Chemistry Lecture Outline Name: The Common-Ion Effect Suppose we have a weak acid and a soluble salt of that acid. CH 3 COOH NaCH 3 COO CH 3 COOH CH 3 COO + H + Since NaCH
More informationChapter 8. Chemical Equations and Reactions
Chapter 8 Chemical Equations and Reactions Chemical Equations Represents, w/ symbols & formulas, the reactants & products in a chemical reaction Requirements Must represent the known facts Must contain
More informationTheophylline (TH), the structure of which is presented below, is a bronchial-dilator used for the treatment of asthma.
1 EXAM SCIETIIC CULTURE CEMISTRY PRBLEM 1: Theophylline (T), the structure of which is presented below, is a bronchial-dilator used for the treatment of asthma. 3 C 7 1 3 9 1.1 Structural study and acid-base
More informationChemistry course ACME Faculty, EHVE course B.Sc. Studies, I year, I semester. Inorganic chemistry. Oxidation state. Oxidation state.
-- Chemistry course ACME Faculty, EHVE course B.Sc. Studies, I year, I semester Leszek Niedzicki, PhD, Eng. Inorganic chemistry Particle Particle can be a simple atom system, i.e.: atom (usually of metal
More informationCHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total.
Name Exam No. F CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total. Multiple Choice. (20 questions, 3 points each = 60 points total) Mark the letter on the scantron form corresponding to the one best
More information2H 2 (g) + O 2 (g) 2H 2 O (g)
Mass A AP Chemistry Stoichiometry Review Pages Mass to Mass Stoichiometry Problem (Review) Moles A Moles B Mass B Mass of given Amount of given Amount of unknown Mass of unknown in grams in Moles in moles
More informationChem A Ch. 9 Practice Test
Name: Class: Date: Chem A Ch. 9 Practice Test Matching Match each item with the correct statement below. a. product d. balanced equation b. reactant e. skeleton equation c. chemical equation 1. a new substance
More informationReactions in Aqueous Solution
1 Reactions in Aqueous Solution Chapter 4 For test 3: Sections 3.7 and 4.1 to 4.5 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 2 A solution is a homogenous
More information