Ethylene oxide is an important organic intermediate in the chemical industry. The standard Gibbs energy change at 298 K for the reaction C₂H₄ + ½O₂ ⇆ C₂H₄O is -79.79 kJ/ mole. This large negative value of ΔG°_T indicates that equilibrium is far to the right at 298 K. However, the direct oxidation of ethylene must be promoted by a catalyst selective to this reaction to prevent the complete combustion of ethylene to carbon dioxide and water. Even with such a catalyst, it is thought that the reaction will have to be carried out at a temperature of about 550 K in order to obtain a reasonable reaction rate. Since the reaction is exothermic, an increase in temperature will have an adverse effect on the equilibrium. Is the reaction feasible (from an equilibrium standpoint) at 550 K, assuming that a suitable catalyst selective for this reaction is available? For ethylene oxide, ΔH^f₂₉₈ = -52.63 kJ/mol. Heat capacity equations (in J/mole-K) for the temperature range involved may be approximated by C_P,_C2H4O = 6.57 + 0.1389 T(K); C_P,C2H4 = 15.40 + 0.0937 T(K); C_P,O2  26.65 + 0.0084 T(K)