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Equilibrium Systems

Equilibrium Systems. 15.1a: Closed Systems & Reaction Equilibrium. Closed System. in order for equilibrium to be studied there must be a boundary between the system and the surroundings gaseous systems must be closed systems where no matter can enter or exit

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Equilibrium Systems

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  1. Equilibrium Systems 15.1a: Closed Systems & Reaction Equilibrium

  2. Closed System • in order for equilibrium to be studied there must be a boundary between the system and the surroundings • gaseous systems must be closed systems where no matter can enter or exit • collision-reaction theory is used to explain chemical systems, both fast and slow • not all rxtn’s are quantitative, forward and reverse rxtn’s can occur simultaneously in a closed system

  3. Forward Reaction arrow points from left to right ----> reactants form products Reverse Reaction arrow points from right to left <---- products form reactants Closed system con’t When both arrows are shown it is considered an equilibrium equation --------> <--------

  4. Equilibrium two opposing changes occur at equal rates dynamic – not static

  5. Equilibrium • dynamic equilibrium • may seem like no changes are occurring but there are changes • no NET changes • When did this reaction reach it?

  6. at equilibrium, forward and reverse reaction rates are equal

  7. Chemical Equilibrium The state of a chemical reaction in which its forward and reverse reactions occur at equal rates so that the concentration of the reactants and products does not change with time.

  8. Reaction Equilibrium • position of an equilibrium can be determined using % yield • yield of product compared to maximum possible yield at equilibrium (actual/theoretical) • four categories of reactions at equilibrium • % yield description @ equilibrium • Negligible non-spontaneous • < 50% reactants favoured • > 50% products favoured • > 99.9% quantatative -----> --------> <-------- --------> <--------

  9. lies “to the left” more reactants less products lies “to the right” less reactants more products If reactants are mixed and concentrations do not change could already be at equilibrium reaction rates are so slow that change is too difficult to detect Equilibrium Position

  10. ICE Tables • are used to organize data and calculations • Initial, Change, Equilibrium • see sample 15.1 p. 681

  11. Text p682 #4 & 6 Define the following phase equilibrium solubility equilibrium chemical reaction equilibrium forward rxtn reverse rxtn Homework

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