The oxidation of nitric oxide 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 380 kPa (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 (levels out) at 360 kPa. What is the equilibrium percent conversion of NO? Calculate the reaction equilibrium constant at the prevailing temperature, K_p [(atm)^?0.5], defined as where p_i (atm) is the partial pressure of species?i (NO₂, NO, O₂) at equilibrium.

Transcribed Image Text:

NO + O₂ = NO₂ (PNO₂) (PNO) (PO₂).5 K₂ =