'Equilibrium constants' diaporamas de présentation

Fundamental relations: The thermodynamic functions The molecular partition function

Chapter 20 Statistical thermodynamics: the machinery. Fundamental relations: The thermodynamic functions The molecular partition function Using statistical thermodynamics Mean energies Heat capacities Equation of state Residual entropies Equilibrium constants.

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Chapter 14 Chemical Equilibrium

Chemistry: A Molecular Approach , 1 st Ed. Nivaldo Tro. Chapter 14 Chemical Equilibrium. Roy Kennedy Massachusetts Bay Community College Wellesley Hills, MA. 2008, Prentice Hall. Hemoglobin. protein (Hb) found in red blood cells that reacts with O 2

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Reaction Rates and Equilibrium

Reaction Rates and Equilibrium. Chapter 18. 18.1. Rates of Reaction.

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Activity

Activity. Introduction 1.) Hydration Ions do not act as independent particles in solvent (water) Surrounded by a shell of solvent molecules . Oxygen has a partial negative charge and hydrogen partial positive charge. Oxygen binds cations. Hydrogen binds anions. Activity. Introduction

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Chapter 14 Chemical Equilibrium

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Complex-Induced Proximity Effect in Directed Ortho and Remote Metallation Methodologies

Complex-Induced Proximity Effect in Directed Ortho and Remote Metallation Methodologies. February 5 2008 Louis-Philippe Beaulieu. Outline. Background Information Complex-Induced Proximity Effect: The concept

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Section 06

Section 06. General Concepts of Chemical Equilibrium. General Concepts: Chemical Equilibrium. Chemical Reactions: The Rate Concept aA + bB ?? cC + dD Rate f = k f [A] a [B] b Rate r = k r [C] c [D] d Rate f = Rate r k f [A] a [B] b = k r [C] c [D] d Molar Equilibrium Constant K

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Control of Oxides of Nitrogen from Stationary Sources

Control of Oxides of Nitrogen from Stationary Sources. Oxides of Nitrogen. The gaseous oxides of nitrogen include: N2O:nitrous oxide NO:nitric oxide (free radical) N2O3: nitrogen trioxide NO2:Nitrogen dioxide (free radical) N2O5:nitrogen pentoxide An unstable form NO3 also exists.

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Chapter 16. Chemical Reactions Rates and Equilibria

Chapter 16. Chemical Reactions Rates and Equilibria. The rate of a chemical reaction shows how fast it goes. The equilibrium position of a chemical reaction shows how far it goes. How Do Chemical Reactions Occur?.

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Chapter 14 Chemical Equilibrium

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Unit 4: Equilibrium

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Chapter 15 Chemical Equilibrium

Chapter 15 Chemical Equilibrium. The Concept of Equilibrium. The double arrow implies the process is dynamic. Consider Forward reaction: A ? B Rate = k f [A] Reverse reaction: B ? A Rate = k r [B] At equilibrium k f [A] = k r [B]. The Concept of Equilibrium.

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Chapter 19, part II Notes

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Factors Affecting Reaction Rates

Factors Affecting Reaction Rates. Factors Affecting Reaction Rates. There are several factors affect reaction rates Concentration Surface area (Particle size) Temperature Catalysts Inhibitors. Catalysts.

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Chapter 9: Chemical Equilibrium

Chapter 9: Chemical Equilibrium. The forward and reverse reaction are both taking place at the same rate. Production and Decomposition of Ammonia. Forward Reaction: N 2 (g) + 3H 2 (g) ? 2NH 3 (g). Reverse Reaction: 2NH 3 (g) ? N 2 (g) + 3H 2 (g).

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Weak Acids and Bases

Weak Acids and Bases.

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Solubility

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Thermodynamic Equilibrium Constant

Thermodynamic Equilibrium Constant The equilibrium constant expressions which use concentrations are called concentration equilibrium constants. For example, in the reaction: AB D A + B We can write K = [A][B]/[AB]

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Introduction to Equilibrium

Introduction to Equilibrium. AP Chemistry. Equilibrium. Defined as the state when the concentrations of all reactants and products remain constant over time. This occurs when the rate of the forward = rate of the reverse reaction.

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Reversible Reactions and Equilibrium

Reversible Reactions and Equilibrium. OBJECTIVES Describe how the amounts of reactants and products change in a chemical system at equilibrium. Identify three stresses that can change the equilibrium position of a chemical system.

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