Hydrogen gas can be produced by heating methane gas CH4 and water vapor with a nickel catalyst to a temperature of 1000C. The reaction also produces carbon monoxide, i.e. carbon monoxide. Write the balanced reaction equation for one mole of methane. Calculate the standard enthalpy ΔrH⊖ for this reaction and standard entropy ΔrS⊖. Assuming that ΔrH⊖ and ΔrS⊖ remain constant over this temperature range, determine the Gibbs energy of the reaction at 1000C
Hydrogen gas can be produced by heating methane gas CH4 and water vapor with a nickel catalyst to a temperature of 1000C. The reaction also produces carbon monoxide, i.e. carbon monoxide. Write the balanced reaction equation for one mole of methane. Calculate the standard enthalpy ΔrH⊖ for this reaction and standard entropy ΔrS⊖. Assuming that ΔrH⊖ and ΔrS⊖ remain constant over this temperature range, determine the Gibbs energy of the reaction at 1000C
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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Hydrogen gas can be produced by heating methane gas CH4 and water vapor with a nickel catalyst to a temperature of 1000C. The reaction also produces carbon monoxide, i.e. carbon monoxide. Write the balanced reaction equation for one mole of methane. Calculate the standard enthalpy ΔrH⊖ for this reaction
and standard entropy ΔrS⊖. Assuming that ΔrH⊖ and ΔrS⊖ remain constant over this temperature range, determine the Gibbs energy of the reaction at 1000C Is the methane reaction spontaneous,why?
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