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Equilibrium Pressure

Equilibrium Pressure. If the values at equilibrium are given in partial pressure, then solving for the constant is the same, but use K p instead of K c . What makes them different: Kc = equilibrium constant based on molarity and concentration.

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Equilibrium Pressure

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  1. Equilibrium Pressure • If the values at equilibrium are given in partial pressure, then solving for the constant is the same, but use Kp instead of Kc. • What makes them different:Kc = equilibrium constant based on molarity and concentration. Kp = equilibrium constant based on partial pressures in atm.

  2. The mole ratio in a mixture gas is proportional to the partial pressures of each of the gases. • Dalton’s Law of Partial Pressures – the total pressure in a system is equal to the sum of the individual pressures. • Total = Pressure of + Pressure of ….Pressure Gas #1 Gas #2

  3. 2 NO2 (g) 2 NO (g) + O2 (g) • Determine the Kp for the above reaction when at equilibrium, the pressure of nitrogen dioxide is 0.425 atm, nitrogen monoxide is 0.270 atm, and oxygen is 0.100 atm. • Kp = [NO]2 [O2] [NO2]2 • Kp = [0.270]2 [0.100] [0.425]2 • Kp= 0.0404

  4. Relationship between Kc and Kp We use the Ideal Gas Law, and derive the relationship between Kc and Kp. Kp= Kc(RT)n Kp = Equilibrium constant in partial pressure Kc = Equilibrium constant in molar concentrations R = Ideal Gas constant (always 0.082) T = Temperature (in Kelvin) n = Change in moles of GASES ONLY (moles of gas products) – (moles of gas reactants)

  5. 2 NO2 (g) 2 NO (g) + O2 (g) • At equilibrium, the pressure of nitrogen dioxide is 0.425 atm, nitrogen monoxide is 0.270 atm, and oxygen is 0.100 atm. Determine the Kp for the above reaction.

  6. CO(g) + Cl2(g)  COCl2(g) • At equilibrium the concentrations at 740C are [CO] = 0.012 M, [Cl2] = 0.054 M, and [COCl2] = 0.14 M. Calculate the equilibrium constants Kc and Kp. • Start with the equilibrium expression for Kc: Kc = [COCl2] [CO][Cl2] Kc = [0.14 M] = 216 [0.012][0.054]

  7. CO(g) + Cl2(g)  COCl2(g) • At equilibrium the concentrations at 740C are [CO] = 0.012 M, [Cl2] = 0.054 M, and [COCl2] = 0.14 M. Calculate the equilibrium constants Kc and Kp. • To solve for Kp we use the Ideal gas law eq.Kp= Kc(RT)n Kp= 216 x (.082 x 347)(1-2) Kp = 7.6

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