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Learning Goals
• identify common equilibrium constants, including Keq, Ksp, Kw, Ka, Kb and write the expressions for each
• solve problems related to equilibrium by performing calculations involving concentrations of reactants and products
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Equilibrium Law
• mathematical description of chemical system at equilibrium
• defined by the equilibrium constant, K• Complete Inv. 7.2.1 on p. 473-474
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Writing Equilibrium Law EquationsFor aA + bB cC + dD,
K = [C]c[D]d (omit units) [A]a[B]b
• omit (s) and (l)
• include only (aq) and (g)
Ex. H2(g) + S(l) H2S(g)
Ex. NH3(g) + H2O(l) NH4+
(aq) + OH-(aq)
p. 431 #1-3, p. 434 #1
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Calculating K
• Write the equilibrium law equation.• Substitute [ ]eq
• K can be used to predict the equilibrium position (Review Equilibrium Position table in lesson 1 and add a column for K.)
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• Sample Problem 2 (p. 430)
In a closed vessel at 500°C, N2(g) + 3 H2(g) 2 NH3(g)
The equil. conc. of N2, H2 and NH3, respectively, are 1.50 x 10-5 M, 3.45 x 10-1 M and 2.00 x 10-4 M. Calculate K.
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• Sample Problem 3 (p. 431)
In a closed vessel at 500°C, 2 NH3(g) N2(g) + 3 H2(g)
The equil. conc. of N2, H2 and NH3, respectively, are 1.50 x 10-5 M, 3.45 x 10-1 M and 2.00 x 10-4 M. Calculate K.
K (synthesis of ammonia)K’ (decomposition of ammonia)Mathematical relationship b/w K and K’?
K = 1/K’
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What does the magnitude of K tell us about the equilibrium position?
A. In a closed system at 25°C,2 CO(g) + O2(g) 2 CO2(g) K = 3.3 x 1091
B. Decomposition of water at 1000°C,2 H2O(g) 2 H2(g) + O2(g) K = 7.3 x 10-10
C. NO2(g) + NO(g) N2O(g) + O2(g) K = 0.951
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Homework
• p. 436 #1-6