The oxidation of nitric oxide

Reference no: EM13311169

The oxidation of nitric oxide NO + 1/2O2 <--> NO2

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 kPa (absolute).

a) Assuming idea gas behavior, determine the composition of the mixture (component mole fraction) 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? Calbulate the reaction equilibrium constant at the prevailing temperature, Kp[(atm)^-0.5], defined as

Kp=(pNO2)/[(pNO)(pO2)^0.5]

where pi(atm) is the partial pressure of species i (NO2,NO,O2) at equilibrium.

Reference no: EM13311169

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