'Effective collisions' diaporamas de présentation

Chemical Kinetics CHAPTER 14 Chemistry: The Molecular Nature of Matter, 6 th edition

Chemical Kinetics CHAPTER 14 Chemistry: The Molecular Nature of Matter, 6 th edition By Jesperson , Brady, & Hyslop. CHAPTER 14 Chemical Kinetics. Learning Objectives: Factors Affecting Reaction Rate : Concentration State Surface Area Temperature Catalyst

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Reaction Rates & Equilibrium

Reaction Rates & Equilibrium. Unit 9 *Start with visual from Phet. In order for a reaction to take place, the reacting molecules must collide into each other. Once molecules collide they may react together or they may not, depending on two factors -

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Rates of Reactions

Rates of Reactions. Measurements & Graphs Factors affecting Rate of a Reaction Experiments to show how the rate is affected by various factors. What is meant by the rate of a reaction?. A measure of how fast a reaction is taking place. Different reaction occur at different rates.

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Chapter 8: Kinetics and Equilibrium

Chapter 8: Kinetics and Equilibrium. Do Now: Answer these questions. 1. What type of energy is related to the temperature of a substance? (think about definition of temperature) 2. If the temperature of a substance is increased, what do you think happens to the speed of its particles?

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by Steven S. Zumdahl & Don J. DeCoste University of Illinois

Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Don J. DeCoste University of Illinois. Chapter 17 Equilibrium. Collision Theory of Kinetics.

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Thermodynamics

Thermodynamics. Tells if a reaction will occur. Kinetics. Tells how fast a reaction will occur. Reaction Rate. Speed of the reaction. Found experimentally. Measure change in concentration of a reactant or a product over time. Rate = ?Conc ?time. How do you measure rates?.

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Introductory Chemistry , 3 rd Edition Nivaldo Tro

Introductory Chemistry , 3 rd Edition Nivaldo Tro. Chapter 15 Chemical Equilibrium. Basic Principles of Chemistry Online Southeast Missouri State University Cape Girardeau, MO. 2009, Prentice Hall. Equilibrium vs. Disequilibrium.

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Unit 14 Equilibrium

Unit 14 Equilibrium. The Concept of Equilibrium. Ex) elevator, football game, moving walkway. 1. Reversible Reactions : Chemical reaction in which the products can regenerate the original reactants . A double arrow is used to express a reversible reaction.

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Chapter 12 – Chemical Kinetics

Chapter 12 – Chemical Kinetics. Second order Rate Law Zero Order Rate Law Reaction Mechanism Model for Chemical Kinetics Collision Catalysis Heterogeneous Catalysis Homogeneous Catalysis. Second-Order Rate Law. For a A  products in a second-order reaction, Integrated rate law is

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Kinetics

Kinetics. Kinetics. Kinetics - rates of chemical reactions and the mechanisms by which they occur Rate of a chemical reaction - change in the concentration of products and reactants in a given time. Collision Theory. Molecules must have effective collisions in order to react

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Kinetics & Equilibrium

Kinetics & Equilibrium. Chemical Kinetics. The area of chemistry that is concerned with reaction __________ and reaction __________ is called chemical __________ . The rate of a reaction depends on the collision __________ of the reactants and on the collision efficiency.

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Catalysts

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O8-#51-52 BASE ACID ? SALT WATER

O8-#51-52 BASE ACID ? SALT WATER 51) K OH + H Cl ? K Cl + H 2 O COMBINE THE METAL K FROM THE BASE WITH THE NON METAL Cl FROM THE ACID TO FORM YOUR SALT. THE OH FROM THE BASE AND THE H FROM

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THE COLLISION THEORY

THE COLLISION THEORY. For the reaction A + B ? C , A and B must collide For the reaction A ? B + C , A must collide with itself or with the walls of the container. Effective Collisions.

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Catalysis

Catalysis. Lowering of Activation Energy by a Catalyst. Catalysts Increase the Number of Effective Collisions. Heterogeneous Catalysis. Heterogeneous Catalysis. Heterogeneous Catalysis. Heterogeneous Catalysis.

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RATES OF REACTION

RATES OF REACTION. Rates of Reaction. The rate of a chemical reaction is the speed at which the reaction occurs (i.e. speed at which the reactants are used or products are produced). Rate can be measured by the: 1) change in mass of reactants or products . 2) change in pH

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