CH0002 - Lecture 6

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  1. What is an equilibrium?
    Where there is no tendency for a further change to occur.
  2. What is a reversible reaction?
    • A reversible reaction is one which can be made to go in either direction depending on the conditions.
    • The happen in Closed Systems!
  3. What is a dynamic equilibirum?
    A dynamic equilibrium is a chemical equilibrium between a forward reaction and the reverse reaction where the rate of the reactions are equal.
  4. What are two examples of dynamic equilibria?
    • Br2 (l)  <----> Br2 (g) 
    • Solubilisation
    • PbCl2 (s)  <---->  PbCl2 (aq) 
  5. What are 4 points about dynamic equilibria?
    The Macroscopic properties are constant (for given T, P and initial concentrations)

    The Processes on a molecular scale are in balance, therefore no net change occurs

    The equilibrium can be obtained from either side of the equation.

    The equilibrium only exists in a closed system.
  6. What is an equilibrium constant?
    A reaction has a fixed equilibrium constant which describes the extent to which the reaction proceeds.

    If you allow the reaction to reach equilibrium and then measure the equilibrium concentrations of everything, you can combine these concentrations into an expression known as an equilibrium constant.
  7. How do you calculate an equilibrium constant?
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    • [A] = concentration of A in mol dm-3 
    • = Mole numbers in front of each substance in the chemical equation.
  8. What is Le Chantelier's Principle?
    If a system at equilibrium is subjected to a change, processes occur which tend to counteract the change.
  9. What factors can affect the equilibrium of a reaction?
    • Changes in temperature and pressure.
    • Changes in concentration
  10. What would happen if you changed the conditions of a reaction by increasing the pressure?
    According to Le Chatelier, the position of equilibrium will move in such a way as to counteract the change. That means that the position of equilibrium will move so that the pressure is reduced again.

    Pressure is caused by gas molecules hitting the sides of their container. The more molecules you have in the container, the higher the pressure will be. The system can reduce the pressure by reacting in such a way as to produce fewer molecules.

    In this case, there are 3 molecules on the left-hand side of the equation, but only 2 on the right. By forming more C and D, the system causes the pressure to reduce.
  11. What would happen if you changed the conditions by decreasing the pressure?
    The equilibrium will move in such a way that the pressure increases again.
  12. When increasing the pressure of a reaction, what happens if there are the same number of molecules on both sides of the equilibrium reaction?
    In this case, increasing the pressure has no effect whatsoever on the position of the equilibrium.

    Because you have the same numbers of molecules on both sides, the equilibrium can't move in any way that will reduce the pressure again.
  13. How does a change in temperature affect the equilibrium of a reaction?
    Increasing the temperature of a system in dynamic equilibrium favours the endothermic reaction. The system counteracts the change you have made by absorbing the extra heat.

    Decreasing the temperature of a system in dynamic equilibrium favours the exothermic reaction. The system counteracts the change you have made by producing more heat.
  14. What is the solubility product?
    The solubility product is the equilibrium constant for a solubility equilibrium.

    It is written as Ksp 
  15. What is different about the solubility product equation?
    No terms are included for the solid, since molar concentration of a pure solid is constant independent of the amount present.
  16. Give an example of a solubility product?
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  19. What is the water ionisation constant for the auto-ionisation of water?
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  20. How can you work out the units for solubility products?
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CH0002 - Lecture 6
2014-04-28 09:46:57
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