Chemical Equilibrium

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Author:
Anonymous
ID:
192080
Filename:
Chemical Equilibrium
Updated:
2013-01-10 13:38:45
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Chemistry
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Description:
Advanced Higher Chemistry - Unit Two - Chemical Equilibrium
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  1. When is a chemical reaction in equilibrium?
    When the rate of the forward reaction equals the rate of the reverse reaction
  2. How would you describe the concentrations of reactants and products at equilibrium?
    They are constant but not always equal
  3. How can you change the position of equilibrium of a reaction?
    • By altering the concentration of a reactant or product
    • By changing the pressure if there are different numbers of moles of gases on both sides of the balanced equation
    • By altering the temperature
  4. What symbol is given for the equilibrium constant?
    K
  5. For the general reaction:
    aA + bB ↔ cC + dD
    what is the equation for the equilibrium constant?
    K = [C]c [D]d / [A]a [B]b
  6. What is the difference between homogeneous equilibrium and heterogeneous equilibrium?
    In homogeneous equilibrium all the species are in the same phase whereas in heterogeneous equilibrium the species are in more than one phase
  7. What value are the concentrations of pure solids or pure liquids given in the equilibrium equation?
    1
  8. Do equilibrium constants have units?
    No
  9. What is the extent of the reaction when the value of Kc is <10-3?
    Effectively no reaction
  10. What is the extent of the reaction when the value of Kc is between 10-3 and 103?
    There are significant quantities of reactants and products at equilibrium
  11. What is the extent of the reaction when the value of Kc is >103?
    The reaction effectively goes to completion
  12. Are equilibrium constants effected by particular concentrations or pressures of a species in a reaction?
    No
  13. What does Le Chatlier's principle state?
    That when a reaction at equilibrium is subject to change the composition alters in such a way as to minimise the effects of that change
  14. What does a rise in temperature cause in endothermic reactions?
    A rise in temperature causes an increase in the value of K and an increase in the yield of the product(s)
  15. What does a rise in temperature cause in exothermic reactions?
    A rise in temperature causes a decrease in the value of K and a decrease in the yield of the product(s)
  16. What effect does a catalyst have on the equilibrium constant?
    No effect

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