The oxidation of nitric oxide NO+1/2O2NO2 takes place in an isothermal batch reactor. The reactor is charged with a mixture containing 24.0 volume percent NO and the balance air at an initial pressure of 350.0kPa (absolute). Composition and Final Pressure Assuming ideal-gas behavior, determine the composition of the mixture (component mole fractions) and the final pressure (kPa) if the conversion of NO is 85.0%. yNO= yNO2= yO2= yN2= Pfinal=kPa Suppose the pressure in the reactor really equilibrates (levels out) at 330.0kPa. What is the equilibrium percent conversion of NO for that case? Calculate the reaction equilibrium constant at the prevailing temperature, Kp[(atm)0.5], defined as Kp=pNO(pO2)0.5pNO2 where pi(atm) is the partial pressure of species i(NO2,NO,O2) at equilibrium. Conversion = % Kp=