EIT Review S2012 Part 2 Dr. J. Mack CSUS Department of Chemistry
... • Concentration data can be used to calculate equilibrium constants for both aqueous and gaseous systems. • In these cases, the symbol K is sometimes given the subscript “c” for “concentration,” as in Kc. • For gases, however, equilibrium constant expressions can be written in another way: in ...
... • Concentration data can be used to calculate equilibrium constants for both aqueous and gaseous systems. • In these cases, the symbol K is sometimes given the subscript “c” for “concentration,” as in Kc. • For gases, however, equilibrium constant expressions can be written in another way: in ...
Chapter 4 "Reactions in Aqueous Solution"
... solutes2, are dispersed uniformly throughout the substance in the greater amount, the solvent3. An aqueous solution4 is a solution in which the solvent is water, whereas in a nonaqueous solution, the solvent is a substance other than water. Familiar examples of nonaqueous solvents are ethyl acetate, ...
... solutes2, are dispersed uniformly throughout the substance in the greater amount, the solvent3. An aqueous solution4 is a solution in which the solvent is water, whereas in a nonaqueous solution, the solvent is a substance other than water. Familiar examples of nonaqueous solvents are ethyl acetate, ...
chemical bonding i: basic concepts
... complexes. Dissolve white anhydrous CuCl2 in water; it turns light blue due to the complex [Cu(H2O)6]2+. Add ammonia to this and it turns deep blue as some of the water is replaced by ammonia to form complexes such as [Cu(NH3)4(H2O)2]2+. Coordinate covalent bonds occur in the formation of transition ...
... complexes. Dissolve white anhydrous CuCl2 in water; it turns light blue due to the complex [Cu(H2O)6]2+. Add ammonia to this and it turns deep blue as some of the water is replaced by ammonia to form complexes such as [Cu(NH3)4(H2O)2]2+. Coordinate covalent bonds occur in the formation of transition ...
Exam 2 Key
... 3. The terms strong electrolyte and weak electrolyte are used in multiple contexts. Discuss how these terms are used in each of the contexts below. Use a maximum of three sentences per context. (8 points) a. When describing a compound: When describing a compound, the term electrolyte refers to the c ...
... 3. The terms strong electrolyte and weak electrolyte are used in multiple contexts. Discuss how these terms are used in each of the contexts below. Use a maximum of three sentences per context. (8 points) a. When describing a compound: When describing a compound, the term electrolyte refers to the c ...
Unit 10 complete 2016-2017
... a. How many moles of hydrogen would be needed to produce 5.0 moles of water? b. How many moles of oxygen would be needed to produce 5.0 moles of water? 2. Ethane, C2H6, can undergo combustion. a. If 4.50 moles of ethane are available how many moles of carbon dioxide can be produced? b. If 4.50 moles ...
... a. How many moles of hydrogen would be needed to produce 5.0 moles of water? b. How many moles of oxygen would be needed to produce 5.0 moles of water? 2. Ethane, C2H6, can undergo combustion. a. If 4.50 moles of ethane are available how many moles of carbon dioxide can be produced? b. If 4.50 moles ...
Honors Chemistry
... a. How many moles of hydrogen would be needed to produce 5.0 moles of water? b. How many moles of oxygen would be needed to produce 5.0 moles of water? 2. Ethane, C2H6, can undergo combustion. a. If 4.50 moles of ethane are available how many moles of carbon dioxide can be produced? b. If 4.50 moles ...
... a. How many moles of hydrogen would be needed to produce 5.0 moles of water? b. How many moles of oxygen would be needed to produce 5.0 moles of water? 2. Ethane, C2H6, can undergo combustion. a. If 4.50 moles of ethane are available how many moles of carbon dioxide can be produced? b. If 4.50 moles ...
Unit 8 Chemical Equilibrium Focusing on Acid
... simplest integer coefficients, and include physical states for all substances. (a) Copper(II) chloride and potassium carbonate solutions are mixed. (b) Ethene (ethylene) reacts with hydrogen chloride to form chloroethane. (c) Aluminium foil reacts with hydrochloric acid. (d) Ammonia undergoes simple ...
... simplest integer coefficients, and include physical states for all substances. (a) Copper(II) chloride and potassium carbonate solutions are mixed. (b) Ethene (ethylene) reacts with hydrogen chloride to form chloroethane. (c) Aluminium foil reacts with hydrochloric acid. (d) Ammonia undergoes simple ...
Chemistry Honours - SCS Autonomous College
... Markownikoff addition), mechanism of oxymercuration-demercuration, hydroborationoxidation, ozonolysis, reduction (catalytic and chemical), syn and anti-hydroxylation (oxidation). 1,2-and 1,4-addition reactions in conjugated dienes and, Diels-Alder reaction; Allylic and benzylic bromination and mecha ...
... Markownikoff addition), mechanism of oxymercuration-demercuration, hydroborationoxidation, ozonolysis, reduction (catalytic and chemical), syn and anti-hydroxylation (oxidation). 1,2-and 1,4-addition reactions in conjugated dienes and, Diels-Alder reaction; Allylic and benzylic bromination and mecha ...
Nordonia Hills City Schools Honors Chemistry Course of Study
... In a chemical process, recognize that there is an ideal ratio of reactants. 2. Apply ideal ratio concept to reaction coefficients in a balanced equation. 3. Solve stoichiometric problems involving moles and mass. 4. Identify limiting reactant to determine the quantity of product (s) formed. 5. Calcu ...
... In a chemical process, recognize that there is an ideal ratio of reactants. 2. Apply ideal ratio concept to reaction coefficients in a balanced equation. 3. Solve stoichiometric problems involving moles and mass. 4. Identify limiting reactant to determine the quantity of product (s) formed. 5. Calcu ...
PDF - mockies – Mockiesgateacademy
... Eg. Consider the following reaction 2 H2 + O2 → 2H2O In this reaction one molecule of oxygen reacts with two molecules of hydrogen. So it would be desirable to take the molecules of H2 and oxygen in the ratio 2:1, so that the reactants are completely consumed during the reaction. But atoms and mole ...
... Eg. Consider the following reaction 2 H2 + O2 → 2H2O In this reaction one molecule of oxygen reacts with two molecules of hydrogen. So it would be desirable to take the molecules of H2 and oxygen in the ratio 2:1, so that the reactants are completely consumed during the reaction. But atoms and mole ...
Document
... group is MORE positive than it was in the C-O-H group By increasing the number of highly electronegative O, more electrons were drawn away from that C, making it more positive. ...
... group is MORE positive than it was in the C-O-H group By increasing the number of highly electronegative O, more electrons were drawn away from that C, making it more positive. ...
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chap15pptlecture_chapte.ppt [Read-Only]
... If a reaction can be expressed as the sum of two or more reactions, the equilibrium constant for the overall reaction is given by the product of the equilibrium constants of the individual reactions. ...
... If a reaction can be expressed as the sum of two or more reactions, the equilibrium constant for the overall reaction is given by the product of the equilibrium constants of the individual reactions. ...
chapter_14 Equilibr
... do not appear in the equilibrium constant expressions. 3. The equilibrium constant is a dimensionless quantity. 4. In quoting a value for the equilibrium constant, you must specify the balanced equation and the temperature. 5. If a reaction can be expressed as a sum of two or more reactions, the equ ...
... do not appear in the equilibrium constant expressions. 3. The equilibrium constant is a dimensionless quantity. 4. In quoting a value for the equilibrium constant, you must specify the balanced equation and the temperature. 5. If a reaction can be expressed as a sum of two or more reactions, the equ ...
Document
... do not appear in the equilibrium constant expressions. 3. The equilibrium constant is a dimensionless quantity. 4. In quoting a value for the equilibrium constant, you must specify the balanced equation and the temperature. 5. If a reaction can be expressed as a sum of two or more reactions, the equ ...
... do not appear in the equilibrium constant expressions. 3. The equilibrium constant is a dimensionless quantity. 4. In quoting a value for the equilibrium constant, you must specify the balanced equation and the temperature. 5. If a reaction can be expressed as a sum of two or more reactions, the equ ...
... The theoretical yield is the maximum amount of product that could be formed from given amounts of reactants. 7. The amount of product that actually forms when a chemical reaction is carried actual out in a laboratory is called the ______________________ yield. 8. Is the following sentence true or fa ...
Unit 6- Math of Chemistry
... • What is the percent composition of O in KClO3? • 1st: Determine formula mass of element and of the compound • 2nd: % of element = element formula mass/ total formula mass x 100 ...
... • What is the percent composition of O in KClO3? • 1st: Determine formula mass of element and of the compound • 2nd: % of element = element formula mass/ total formula mass x 100 ...
2014 International Practice Exam: Chemistry
... when you have finished. . . . Sign your name, and write today’s date. Look up when you have finished. . . . Now print your full legal name where indicated. Are there any questions? . . . Turn to the back cover and read it completely. Look up when you have finished. . . . Are there any questions? . . ...
... when you have finished. . . . Sign your name, and write today’s date. Look up when you have finished. . . . Now print your full legal name where indicated. Are there any questions? . . . Turn to the back cover and read it completely. Look up when you have finished. . . . Are there any questions? . . ...
Equilibrium
... The value of the equilibrium constant for any reaction can be determined by experiment. As detailed in the above section, the equilibrium position for a given reaction does not depend on the starting concentrations, so the equilibrium constant has the same value regardless of the initial amounts of ...
... The value of the equilibrium constant for any reaction can be determined by experiment. As detailed in the above section, the equilibrium position for a given reaction does not depend on the starting concentrations, so the equilibrium constant has the same value regardless of the initial amounts of ...
Lab Manual Quantitative Analytical Method
... flasks. Measure between 0.20 – 0.25 g of potassium hydrogen phthalate into each. conical flask. Record Clean, rinse well (with deionized water), and dry three 125-mL or 250-mL Conical flasks. Measure between 0.20 – 0.25 g of potassium hydrogen phthalate into each Conical flask. Record the exact weig ...
... flasks. Measure between 0.20 – 0.25 g of potassium hydrogen phthalate into each. conical flask. Record Clean, rinse well (with deionized water), and dry three 125-mL or 250-mL Conical flasks. Measure between 0.20 – 0.25 g of potassium hydrogen phthalate into each Conical flask. Record the exact weig ...
20. Chemical Equilibrium
... Setting up an equilibrium expression is an extremely useful skill after you become aware of what information it can provide. In other words, what good is Keq? One way to determine the value of Keq for a particular reaction is to allow the reaction to proceed at a given temperature in such a way as t ...
... Setting up an equilibrium expression is an extremely useful skill after you become aware of what information it can provide. In other words, what good is Keq? One way to determine the value of Keq for a particular reaction is to allow the reaction to proceed at a given temperature in such a way as t ...
File - cpprashanths Chemistry
... Q29.Discuss oxides of nitrogen.Give structure and calculate the oxidation number of nitrogen in each of them.Arrange the oxides in order of increasing acid strength. Nitrogen forms a wide range of oxided .The oxidation number of nitrogen in these oxides varies from +1 to +5.The oxides are 1)N2O din ...
... Q29.Discuss oxides of nitrogen.Give structure and calculate the oxidation number of nitrogen in each of them.Arrange the oxides in order of increasing acid strength. Nitrogen forms a wide range of oxided .The oxidation number of nitrogen in these oxides varies from +1 to +5.The oxides are 1)N2O din ...
EDEXCEL A LeveL - Hodder Education
... 2 What steps should the students take to ensure that all the b) How much copper, in moles, combines with one mole of copper oxide is reduced to copper? oxygen in red copper oxide? 3 Start a spreadsheet program on a computer and open up c) What is the formula of red copper oxide? a new spreadsheet ...
... 2 What steps should the students take to ensure that all the b) How much copper, in moles, combines with one mole of copper oxide is reduced to copper? oxygen in red copper oxide? 3 Start a spreadsheet program on a computer and open up c) What is the formula of red copper oxide? a new spreadsheet ...
Soft X-Ray-Induced Decomposition of Amino Acids: An XPS, Mass
... (8–10). Amino acids, which are the building blocks of proteins, are among the simplest organic molecules of biological relevance and thus serve as convenient model systems in studies of radiation damage. Radiation-induced chemical modifications in the solid state can be monitored by X-ray photoelect ...
... (8–10). Amino acids, which are the building blocks of proteins, are among the simplest organic molecules of biological relevance and thus serve as convenient model systems in studies of radiation damage. Radiation-induced chemical modifications in the solid state can be monitored by X-ray photoelect ...
Chemical Reactions
... Sodium metal reacts with water to produce aqueous sodium hydroxide and hydrogen. How many grams of sodium are needed to produce 50.0g of hydrogen? A balanced chemical equation is needed before any calculations can be made. ...
... Sodium metal reacts with water to produce aqueous sodium hydroxide and hydrogen. How many grams of sodium are needed to produce 50.0g of hydrogen? A balanced chemical equation is needed before any calculations can be made. ...
Lewis acid catalysis
In Lewis acid catalysis of organic reactions, a metal-based Lewis acid acts as an electron pair acceptor to increase the reactivity of a substrate. Common Lewis acid catalysts are based on main group metals such as aluminum, boron, silicon, and tin, as well as many early (titanium, zirconium) and late (iron, copper, zinc) d-block metals. The metal atom forms an adduct with a lone-pair bearing electronegative atom in the substrate, such as oxygen (both sp2 or sp3), nitrogen, sulfur, and halogens. The complexation has partial charge-transfer character and makes the lone-pair donor effectively more electronegative, activating the substrate toward nucleophilic attack, heterolytic bond cleavage, or cycloaddition with 1,3-dienes and 1,3-dipoles.Many classical reactions involving carbon–carbon or carbon–heteroatom bond formation can be catalyzed by Lewis acids. Examples include the Friedel-Crafts reaction, the aldol reaction, and various pericyclic processes that proceed slowly at room temperature, such as the Diels-Alder reaction and the ene reaction. In addition to accelerating the reactions, Lewis acid catalysts are able to impose regioselectivity and stereoselectivity in many cases.Early developments in Lewis acid reagents focused on easily available compounds such as TiCl4, BF3, SnCl4, and AlCl3. The relative strengths of these (and other) Lewis acids may be estimated from NMR spectroscopy by the Childs method or the Gutmann-Beckett method. Over the years, versatile catalysts bearing ligands designed for specific applications have facilitated improvement in both reactivity and selectivity of Lewis acid-catalyzed reactions. More recently, Lewis acid catalysts with chiral ligands have become an important class of tools for asymmetric catalysis.Challenges in the development of Lewis acid catalysis include inefficient catalyst turnover (caused by catalyst affinity for the product) and the frequent requirement of two-point binding for stereoselectivity, which often necessitates the use of auxiliary groups.