1. Chemical Equilibrium Chapter 15

2. 15.8 Write the expressions for the equilibrium constants K P of these thermal decompositions:

3. 15.14 Consider the following equilibrium process at 700 o C: Analysis shows that there are 2.50 moles of H 2, 1.35 x 10 -5 mole of S 2, and 8.70 moles of H 2 S present in a 12.0-L flask at equilibrium. Calculate the equilibrium constant K c for the reaction.

4. 15.32 A sample of pure NO 2 gas heated to 1000 K decomposes: The equilibrium constant K P is 158. Analysis shows that the partial pressure of O 2 is 0.25 atm at equilibrium. Calculate the pressure of NO and NO 2 in the mixture.

5. 15.48 Consider the equilibrium process: Predict the direction of the shift in equilibrium when (a) the temperature is raised, (b) more chlorine gas is added to the reaction mixture, (c) some PCl 3 is removed from the mixture, (d) the pressure on the gases is increased, and (e) a catalyst is added to the reaction mixture.

6. 15.52 Consider the reaction at equilibrium in a closed container: What would happen if (a) the volume is increased, (b) some CaO is added to the mixture, (c) some CaCO 3 is removed, (d) some CO 2 is added to the mixture, (e) a few drops of an NaOH solution are added to the mixture, (f) a few drops of an HCl solution are added to the mixture (ignore the reaction between CO 2 and water), and (g) the temperature is increased.

7. Practice exercise, p. 491 The equilibrium constant (K c ) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine is 6.5 x 10 4 at 35 o C. In a certain experiment, 2.0 x 10 -2 mole of NO, 8.3 x 10 -3 mole of Cl 2, and 6.8 moles of NOCl are mixed in a 2.0-L flask. In which direction will the system proceed to reach equilibrium?