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K p

K p. K p. The equilibrium constant in terms of partial pressures. Mole fraction. Partial pressures. Partial pressure, p The contribution of a gas towards the total pressure Partial pressure = mole fraction x Total pressure. 3 5. 2 5. x (N 2 ) = = 0.4. x (O 2 ) = = 0.6.

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K p

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  1. Kp

  2. Kp The equilibrium constant in terms of partial pressures

  3. Mole fraction

  4. Partial pressures Partial pressure, p The contribution of a gas towards the total pressure Partial pressure = mole fraction x Total pressure 3 5 2 5 x(N2) = = 0.4 x(O2) = = 0.6 A gas mixture with a total pressure of 320 kPa contains 2 molof N2(g) and 3 molof O2(g). Mole fractions Partial pressures Sum of partial pressures = Total pressure p(N2)+ p(O2) = 128+ 192= 320 kPa • p(N2) = x(N2)P = 0.4x 320 • = 128 kPa • p(O2) = x(O2)P = 0.6 x 320 • = 192 kPa

  5. What is Kp Kp = Similar to Kc but partial pressures used in place of concentration Equilibrium: 2SO2(g) + O2(g) ⇌ 2SO3(g) Units: Kp =

  6. Calculating Kp Kp = x Equilibrium: 2SO2(g) + O2(g) ⇌ 2SO3(g) Partial pressures: SO2(g), 74 kPa; O2(g), 23 kPa; SO3(g), 142 kPa = 0.160 kPa–1 Kp = x

  7. Heterogeneous equilibria Equilibrium contains different phases Equilibrium: CaCO3(s) ⇌ CaO(s) + CO2(g) Kp expression contains only gaseous species Kp = p(CO2) Solid species are omitted (solids have no gas pressure)

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