Kp

• Partial pressure = Total pressure * mole fraction
• Mole fraction = Number of moles of species A / Total number of moles of all gas species
• For reaction containing gas, its difficult to measure concentration of a gas. Instead the quantity of each gas in an equilibrium mixture is partial pressure
• aA(g) + bB(g) ⇌ cC(g) =dD(g)

  Kp = P(C)^c * P(D)^d / P(A)^a * P(B)^b

  P(C) is the partial pressure of species C

  Its not square brackets because its not concentrations
• Temperature affects Kp but pressure and catalyst doesn't affect Kp