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Understanding Equilibrium Constants Using Partial Pressures in Gas Mixtures

Learn how to calculate equilibrium constants using partial pressures in gas mixtures through examples and formulas. Understand the relationship between partial pressures, mole fractions, and total pressure in equilibrium reactions.

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Understanding Equilibrium Constants Using Partial Pressures in Gas Mixtures

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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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