HW#7 Kc = 5 x 1012 CHEM 185 Skills Class 1. Consider the following equilibrium: Equilibrium 2 NO (g) + O2 (g) 2 NO2 (g) a. Calculate the equilibrium constants, Kc, for the following reactions: O2(g) NO2 (g) NO (g) + 2 NO2 (g) NO2 (g) 2 NO (g) + O2(g) NO (g) + ½ O2 (g) b. Calculate the value of K, at 298 K for 2 NO (g) + O2 (g) 2 NO2 (g)

(Q97) What is the value of the equilibrium constant (Keg) for the following hypothetical reaction: 2 W (g) + X (g) 3 Y (g) Using the related hypothetical equations should be helpful: X (g) + 1/2 Y (g) W (g) + 1/2 Z (g) K = 0.211 2 Y + Z 3 X (g) K2 = 140

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8.2 mol NH3 are placed in a 10.5 L container at some temperature and allowed to come to equilibrium as per the reaction below. At equilibrium, 2.2 moles remained. What is the value of Kc for the following reaction at the temperature of the experiment? 2 NH3(g)  N2(g) + 3 H2(g)

Given the following reaction what is the expression for Kc? 2SO2(g)+O2(g)->2SO3(g) a.What is the expression for the equilibrium constant?       b.If the equilibrium constant for this reaction is 3.70 X 10-7, are the products or the reactants favored?         c.What is the equilibrium constant for the reverse reaction?         d.What is the equilibrium constant for the reaction below? 6 SO3(g)-> 6 SO2(g)+3O2(g)