Question: The production of NO by the direct oxidation of nitrogen occurs naturally in internal combustion engines. This reaction is also used to produce nitric oxide commercially in electric arcs in the Berkeland-Eyde process. If air is used as the feed, compute the equilibrium conversion of oxygen at 1 bar total pressure over the temperature range of 1300 – 1500oC. Air contains 21 mol% oxygen and 79% N2. Request: You do not need to know what the Berkeland-Eyde process is to solve this reaction equilibrium problem. But can you still help me with solving the equilibrium conversion knowing the numerical information provided? Thank you!
Question: The production of NO by the direct oxidation of nitrogen occurs naturally in internal combustion engines. This reaction is also used to produce nitric oxide commercially in electric arcs in the Berkeland-Eyde process. If air is used as the feed, compute the equilibrium conversion of oxygen at 1 bar total pressure over the temperature range of 1300 – 1500oC. Air contains 21 mol% oxygen and 79% N2. Request: You do not need to know what the Berkeland-Eyde process is to solve this reaction equilibrium problem. But can you still help me with solving the equilibrium conversion knowing the numerical information provided? Thank you!
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
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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The production of NO by the direct oxidation of nitrogen occurs naturally in internal combustion engines. This reaction is also used to produce nitric oxide commercially in electric arcs in the Berkeland-Eyde process. If air is used as the feed, compute the equilibrium conversion of oxygen at 1 bar total pressure over the temperature range of 1300 – 1500oC. Air contains 21 mol% oxygen and 79% N2.
Request:
You do not need to know what the Berkeland-Eyde process is to solve this reaction equilibrium problem. But can you still help me with solving the equilibrium conversion knowing the numerical information provided? Thank you!
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