3.1.10 Equilibrium constant Kp for homogeneous systems

• Both the position of equilibrium and the value of Kc or Kp will change if temperature is altered.
• In this equilibrium which is exothermic in the forward direction

  N2 (g)+ 3 H2 (g)  ⇌ 2 NH3 (g)

  If temperature is increased the reaction will shift to oppose the change and move in the backwards endothermic direction. The position of equilibrium shifts left. The value of Kp gets smaller as there are fewer products.
• partial pressure of gas 1 = ( mole fraction of gas 1 ) x total pressure
• mole fraction = number of moles of a gas/ total number of moles of all gases
• Kp is measured in kPa
• Round brackets are used in kP