The oxidation of nitric oxide NO +1/2 O2 → NO2 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 350.0 kPa (absolute). Suppose the pressure in the reactor really equilibrates (levels out) at 327.8 kPa. 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 (see picture) where pi(atm) is the partial pressure of species i (NO2, NO, O2) at equilibrium.  Find the conversion percent and Kp

Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
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The oxidation of nitric oxide

NO +1/2 O→ NO2


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 350.0 kPa (absolute).

Suppose the pressure in the reactor really equilibrates (levels out) at 327.8 kPa. 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 (see picture)

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

Find the conversion percent and Kp 

 

 

PNO2
Kp
PNo (Po,)
0.5
Transcribed Image Text:PNO2 Kp PNo (Po,) 0.5
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