The oxidation of nitric oxide NO+21O2NO2 takes place in an isothermal batch reactor. The reactor is charged with a mixture containing 20.0 volume percent NO and the balance air at an initial pressure of 380kPa (absolute). (a) Assuming ideal gas behavior, determine the composition of the mixture (component mole fractions) and the final pressure (kPa) if the conversion of NO is 90%. (b) Suppose the pressure in the reactor eventually equilibrates (leveis out) at 360kPa. What is the equilibrium percent conversion of NO? Calculate the reaction equilibrium constant at the prevailing temperature, Kp[(atm)0.5], defined as Kp=(pNO)(pO2)0.5(pNO2) where pi(atm) is the partial pressure of species i(NO2,NO,O2) at equilibrium