Lecture10 - Chemistry 132 Lecture 10 Introduction to...

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Chemistry 132 – Lecture 10 – Introduction to Equilibrium (Oxtoby Chapter 9) Chemical Equilibrium Chemical reactions left to themselves ultimately come to a state of equilibrium . Chemical equilibria display all of the following characteristics: The system is closed . Nothing is entering or leaving the system. They show no macroscopic evidence of change They are reached through spontaneous processes. A dynamic balance of forward and reverse processes exists within them. The same equilibrium is reached regardless of the direction from which it was approached. 1
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Chemistry 132 – Lecture 10 – Introduction to Equilibrium (Oxtoby Chapter 9) If we could follow the concentrations of reactant and product molecules from the time the reaction started until equilibrium was reached, the following trends would be noted. Consider the reaction A + 2B 3C in which equal amounts of A and B were added to the reaction vessel. C equilibrium reached [conc] A B time Notice from the graph that concentrations continue to change until equilibrium has been reached. At this point, the concentration values level out. Despite the fact that the concentrations are not changing, forward and reverse reactions are still occurring, but they are occurring at the same rate (speed). 2
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Chemistry 132 – Lecture 10 – Introduction to Equilibrium (Oxtoby Chapter 9) A few important points should be noted about equilibrium: At equilibrium, continuous exchange between reactants and products continues at a molecular level, despite the fact that concentrations or reactants and products
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This note was uploaded on 12/01/2010 for the course APPLIED SC 131 taught by Professor Professornewstead during the Fall '09 term at Queens University.

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Lecture10 - Chemistry 132 Lecture 10 Introduction to...

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