Consider phosgene, COCl2(g). It is an important intermediate inthe manufacture of some plastics. It can decompose into carbonmonoxide and chlorine gases. Its ΔHf° is -220.1 kJ/mole. a) Writethe balanced chemical equation for the decomposition of phosgeneincluding an equilibrium arrow and the states in ( ). b) Write theequilibrium constant expression for this decomposition. c) At500°C, after the reaction has reached equilibrium, Pcarbon monoxide= 0.413 atm, Pchlorine = 0.237 atm, and Pphosgene = 0.217.Calculate Kp at 500°C. d) Initially, a flask is charged with 0.689atm phosgene, 0.250 atm chlorine, and 0.333 atm carbon monoxide.After equilibrium is established at 500°C, the new pressure onphosgene is 0.501 atm. Calculate the pressures of chlorine andcarbon monoxide at equilibrium. e) [For the first part, you cannotuse the equilibrium shortcut; both Kp and the concentrations aretoo large to be considered negligible…quadratic equation ahead…] i)Initially a second flask contains 0.750 atm of chlorine, 0.750 atmcarbon monoxide, and 0.500 atm phosgene. What is the pressure ofeach gas when equilibrium is established? ii) Suppose enoughphosgene is added to the flask to raise the pressure temporarily to2.00 atm. According to Le Chatelier’s Principle, in which directionwill the reaction shift to get back to equilibrium? f) According toLe Chatelier’s Principle, explain which direction the reaction willshift to get back to equilibrium if: i) the reaction is transferredinto a flask that is larger in volume? ii) helium gas is added?iii) the temperature is increased? iv) aplatinum-iridium-magnesium-palladium (PIMP) catalyst is added?
