Key Begins on Page 3.1. Write equilibrium constant expressions for the following reactions. For gases, use either pressures orconcentrations.a) 2 H2O2 (g) 2 H2O (g) + O2 (g)b) C (s) + CO2 (g) 2 CO (g)c) CO (g) + ½ O2 (g) CO2 (g)d) (NH4)2CO3 (s) 2 NH3 (g) + CO2 (g) + H2O (g)2. Three moles of pure SO3 are placed in a 800 L flask at 1150 K. At equilibrium, 0.58 mol of O2 has formed.Calculate Kc for the reaction at 1150 K.2 SO3 (g) 2 SO2 (g) + O2 (g)3. Neither PbCl2 nor PbF2 is appreciably soluble in water. If solid PbCl2 and solid PbF2 are places in equal amountsof water in separate beakers, in which beaker is the concentration of Pb2+ greater? Equilibrium constants forthese solids dissolving in water arePbCl2 (s) Pb2+ (aq) + 2 Cl – (aq) Kc = 1.7 x 10 –5PbF2 (s) Pb2+ (aq) + 2 F – (aq) Kc = 3.7 x 10 –84. How does the reaction quotient for a reaction differ from the equilibrium constant for that reaction?Chem 132 Chapter 145. At 2300 K the equilibrium constant for the formation of NO (g) is Kc = 1.7 x 10 –3.N2 (g) + O2 (g) 2 NO (g)a) If analysis show that the concentration of N2 and O2 are 0.25 M, and that of NO is 0.0042 M, is thesystem at equilibrium?b) If the system is not at equilibrium, in which direction does the reaction proceed?c) When the system is at equilibrium, what are the equilibrium concentrations?6. Sulfuryl chloride, SO2Cl2, is a compound with very irritating vapors; it is used as a reagent in the synthesis oforganic compounds. When heated to a sufficiently high temperature id decomposes to SO2 and Cl2.SO2Cl2 (g) SO2 (g) + Cl2 (g) Kc = 0.045 at 375 oCa) In a 1.00 L flask you place 6.70 g of SO2Cl2 and heat it to 375 oC. What is the concentration of each ofthe compounds in the system when equilibrium is achieved?b) What are the concentrations of SO2Cl2, SO2, and Cl2 at equilibrium in the 1.00 L flask at 375 oC if youbegin with a mixture of SO2Cl2 (6.70 g) and Cl2 (1 atm)?c) Do the fractions of SO2Cl2 in parts (a) and (b) agree with your expectation based on Le Chatelier'sprinciple?7. The decomposition of calcium carbonateCaCO3 (s) CaO (s) + CO2 (g)is an endothermic process. Using Le Chatelier's principle, explain how increasing the temperature affects theequilibrium. If more CaCO3 is added to the flask in which this equilibrium exists, how is the equilibriumaffected? What if some additional CO2 is placed in the flask?Chem 132 Chapter 14Chem 132 Chapter 14Chem 132 Chapter