The oxidation of nitric oxide
takes place in an isothermal batch reactor at 25°C. 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 ?nal 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,
where pi(atm) is the partial pressure of species i (NO3, NO, O2) at equilibrium.
(c) Assuming that KPdepends only on temperature, estimate the ?nal pressure and composition in the reactor if the feed ratio of NO to O2and the initial pressure are the same as in Part (a), but the feed to the reactor is pure O2instead of air.
(d) Replace the partial pressures in the expression for KP, and use the result to explain how reactor pressure in?uences the conversion of NO to NO2.
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