04 Notes - Intro to Equilibrium

04 Notes - Intro to Equilibrium - reaction Reaction must be...

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Aim: What types of systems can exhibit equilibrium? QQ: Explain how two different factors affect the rate of a chemical reaction. Do Now: What does the word “equilibrium” mean? Equilibrium: A state where two opposing processes are occurring at equal rates. Water In Water Out In order for a system to be at equilibrium, the process must be reversible. A B This means two reactions are occurring… 1. A B (forward) 2. B A (reverse) Phase Equilibrium Rate of vaporization = rate of condensation Exists between liquid and vapor phase Must be a closed system H 2 O (l) H 2 O (g) Solution Equilibrium Rate of dissolving = rate of precipitation Occurs in saturated solutions only NaCl (s) Na + (aq) + Cl - (aq) Chemical Equilibrium Rate of forward reaction = rate of reverse
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Unformatted text preview: reaction Reaction must be reversible Dynamic Equilibrium A system at equilibrium has not stopped reacting! A system is at equilibrium when: Rates of forward and reverse reactions are equal Concentrations of reactants and products are constant Net change of the reaction is equal to zero Notice the difference between the two graphs! Conclusions: Only reversible reactions can be at equilibrium Equilibrium means that two opposite processes are occurring at the same rate Three types of equilibrium systems exist: o Phase – occurs between a liquid and vapor o Solution – must be saturated o Chemical – reaction must be reversible At equilibrium, concentrations of product and reactant are constant and rates are equal...
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This note was uploaded on 01/01/2012 for the course CHEM 101 taught by Professor Donahue during the Spring '11 term at Long Island U..

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04 Notes - Intro to Equilibrium - reaction Reaction must be...

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