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The equilibrium constant, K, is 24 x 10^1 at a certain temperature for the reaction

The equilibrium constant, K, is 24 x 10^1 at a certain temperature for the reaction 2NO (g) ↔ N 2 (g) + O 2 (g) For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift?

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The equilibrium constant, K, is 24 x 10^1 at a certain temperature for the reaction

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  1. The equilibrium constant, K, is 24 x 10^1 at a certain temperature for the reaction • 2NO (g) ↔ N2 (g) + O2 (g) • For which of the following sets of conditions is the system at equilibrium? • For those that are not at equilibrium, in which direction will the system shift? • A 1.0 L flask contains 0.024 mol NO, 2.0 mol N2, and 2.6 mol O2 • A 2.0 L flask contains 0.032 mol NO, 0.062 mol N2 and 4.0 mol O2 • A 3.0-L flask contains 0.060 mol NO, 2.4 mol N2, and 1.7 mol O2

  2. At a particular temperature, 12.0 mol of SO3 is placed into a 3.0-L rigid container, and the SO3 dissociates by the reaction SO3 (g) ↔ 2SO2 (g) + O2 (g) At equilibrium, 3.0 mol of SO2 is present. Calculate the K for this reaction.

  3. At 2200 oC, Kp = 0.050 for the reaction N2 (g) + O2 (g)↔ 2NO (g) What is the partial pressure of NO in equilibrium with N2 and O2 that were placed in a flask at initial pressures of 0.80 and 0.20 atm respectively?

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