Chapter 9 complete - Collision Theory of Reactions A...

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Collision Theory of Reactions A chemical reaction occurs when • collisions between molecules have sufficient energy to break the bonds in the reactants • molecules collide with the proper orientation • bonds between atoms of the reactants (N 2 and O 2 ) are broken and new bonds (NO) form
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Collision Theory of Reactions A chemical reaction does not take place if the • collisions between molecules do not have sufficient energy to break the bonds in the reactants • molecules are not properly aligned
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Activation Energy The activation energy • is the minimum energy needed for a reaction to take place upon proper collision of reactants
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Reaction Rate and Temperature Reaction rate • is the speed at which reactant is used up • is the speed at which product forms • increases when temperature rises because reacting molecules move faster, thereby providing more colliding molecules with energy of activation
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Reaction Rate and Concentration Increasing the concentration of reactants • increases the number of collisions • increases the reaction rate
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Reaction Rate and Catalysts A catalyst • speeds up the rate of a reaction • lowers the energy of activation • is not used up during the reaction
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Factors that Increase Reaction Rate
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Learning Check State the effect of each on the rate of reaction as: I) increases D) decreases N) no change A. increasing the temperature B. removing some of the reactants C. adding a catalyst D. placing the reaction flask in ice E. increasing the concentration of a reactant I D I D I
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Learning Check Indicate the effect of each factor listed on the rate of the following reaction as I) increases, D) decreases, or N) none: 2CO( g ) + O 2 ( g ) 2CO 2 ( g ) A. raising the temperature B. removing O 2 C. adding a catalyst D. lowering the temperature I D I D
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Lecture 32: Chemical Equilibrium Goals: Use the concept of reversible reactions to explain chemical equilibrium. Calculate the equilibrium constant for a reversible reaction given the concentrations of reactants and products at equilibrium. Outline (Timberlake 9.2-9.4): Chemical Equilibrium (9.2) Equilibrium Constants (9.3) Using Equilibrium Constants (9.4) Problems for Extra Practice: 9.11, 9.13, 9.15, 9.17, 9.19, 9.21, 9.23, 9.25
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Energy Diagram The activation energy • is the minimum energy needed for a reaction to take place upon proper collision of reactants D H rxn = (+)
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Conditions Required for Reaction to Occur 1. Collision Reactants must collide 2. Orientation Reactant must align properly to break and form bonds 3. Energy Collision must provide the energy of activation
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Reaction Rate Rate of Reaction = Change in concentration Change in time
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Reversible Reactions • Suppose SO 2 and O 2 are present initially. As they collide, the forward reaction begins. 2SO
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This note was uploaded on 01/18/2012 for the course CHEM 120A taught by Professor Leahmiller during the Fall '11 term at University of Washington.

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Chapter 9 complete - Collision Theory of Reactions A...

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