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1.) The compound NOCl decomposes to nitric oxide and chlorine according to the following equation: 2 NOCl (g) → 2 NO (g) + Cl2 (g) Suppose that 0.420 mol NOCl is placed in a 3.00-L flask at a given temperature. When equilibrium has been established, it is found that the concentration of NO is 0.0830 M. Calculate the equilibrium constant for this reaction
2.) The following reaction has an equilibrium constant, Kc, of 6.20 x 102 at a particular temperature: N2 (g) + 3 H2 (g) → 2 NH3 (g) You have a container in which the concentration of N2 is 0.35 M, the the concentration of H2 is 0.12 M, and the concentration of NH3 is 0.44 M. (a) Calculate the value of the reaction quotient Q. (b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed to reach equilibrium.
3.) The equilibrium constant, Kc, for the reaction 2 NOCl (g) + → 2 NO (g) + Cl2 (g) is 3.90 x 10-3. (a) What is Kc for the reaction 2 NO (g) + Cl2 (g) → 2 NOCl (g) (b) What is Kc for the reaction NOCl (g) → NO (g) + 1/2 Cl2 (g). For the reaction 2 NOCl (g) à 2 NO (g) + Cl2 (g) KP is 2.8 x 101 at 600°C. Calculate KC for the reaction at this temperature
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