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In order to obtain the necessary amount of Hydrogen in the HyL Process and to be able to reduce the iron oxide ores to iron, the necessary Hydrogen is obtained from a catalytic reaction of Methane with water by the reaction: CH4 + 2H2O => CO2 + 4H2. Where products and reactants are gaseous. The conditions of the above reaction are inputs at 125ºC and outputs at 35ºC, consider a base calculation of 20,000 gmol/hrs of Hydrogen to be obtained. Make the Matter and Energy Balance considering 85% conversion and 25% Excess water.  What would be the would be the outlet temperature if 200,000 Kcal/hrs are given and the incoming flows are at 25ºC, with the same conversion and excess conditions?

In order to obtain the necessary amount of Hydrogen in the HyL Process and to be able to reduce the iron oxide ores to iron, the necessary Hydrogen is obtained from a catalytic reaction of Methane with water by the reaction: CH4 + 2H2O => CO2 + 4H2. Where products and reactants are gaseous. The conditions of the above reaction are inputs at 125ºC and outputs at 35ºC, consider a base calculation of 20,000 gmol/hrs of Hydrogen to be obtained. Make the Matter and Energy Balance considering 85% conversion and 25% Excess water.  What would be the would be the outlet temperature if 200,000 Kcal/hrs are given and the incoming flows are at 25ºC, with the same conversion and excess conditions?

Introduction to Chemical Engineering Thermodynamics
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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In order to obtain the necessary amount of Hydrogen in the HyL Process and to be able to reduce the iron oxide ores to iron, the necessary Hydrogen is obtained from a catalytic reaction of Methane with water by the reaction: CH4 + 2H2O => CO2 + 4H2. Where products and reactants are gaseous. The conditions of the above reaction are inputs at 125ºC and outputs at 35ºC, consider a base calculation of 20,000 gmol/hrs of Hydrogen to be obtained. Make the Matter and Energy Balance considering 85% conversion and 25% Excess water. 
What would be the would be the outlet temperature if 200,000 Kcal/hrs are given and the incoming flows are at 25ºC, with the same conversion and excess conditions?

 

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