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Mastering Equilibrium Constants & Problem Solving in Equilibrium Law

Enhance your understanding of common equilibrium constants such as Keq, Ksp, Kw, Ka, and Kb. Learn to write expressions for each and tackle equilibrium problems by calculating concentrations of reactants and products effectively.

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Mastering Equilibrium Constants & Problem Solving in Equilibrium Law

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  1. 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
  2. Equilibrium Law mathematical description of chemical system at equilibrium defined by the equilibrium constant, K Complete Inv. 7.2.1 on p. 473-474
  3. Writing Equilibrium Law Equations For aA + bBcC + 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
  4. 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.)
  5. 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.
  6. 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’
  7. 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
  8. Homework p. 436 #1-6
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