A-LEVEL NOTES
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A-LEVEL NOTES

A-LEVEL AQA ChEMISTRY NOTES 
equilibrium constant kp for homogenous systems


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Partial Pressure
  • Mole fractions indicate the fraction of a mixture occupied by a particular gas
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  • Partial pressure is the pressure each gas in a mixture would exert on its own. The partial pressure of a gas A is denoted by  or p(A) or PA.
  • The total pressure of a gas mixture is the sum of all partial pressures from each gas.
  • The amount of pressure a gas exerts in a fixed volume depends on how many particles there are – more particles means greater pressure.
  • p(A) = mole partial pressure of gas A X total pressure
          p(A) partial pressure of gas A (kPa)
          mole of fraction of gas A (mol)
          total pressure (kPa)

​Equilibrium Constant, Kp
  • Kp is an equilibrium constant associated with equilibrium reactions, only involving gases. It is written in terms of partial pressures rather than concentrations.
  • For the equilibrium reaction:
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  • The units of Kp are variable and depend on the specific reaction that is under consideration
  • Temperature can affect the position of equilibrium
    • Increasing the temperature will cause the position of equilibrium to shift in the endothermic direction. Increasing Kp
    • Decreasing the temperature will cause the position of equilibrium to shift in the exothermic direction. Decreasing Kp
  • Pressure can affect the position of equilibrium
    • Increasing the pressure will shift the position of equilibrium to the side with less moles of gas
    • Decreasing the pressure will shift the position of equilibrium to the side with more moles of gas
  • Changing pressure will not affect the value of Kp; instead, the position of equilibrium will shift to keep Kp constant.
  • Catalysts do not affect the value of Kp. Instead, it affects how quickly equilibrium is reached.

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