Nitrosyl bromide, NOBr, decomposes according to the equation NOBr(g) → NO(g) + 1/2 Br₂(g) where ∆G˚ at 4.0e+02 ˚C is 9.83 kJ. What is the value of the equilibrium constant at 4.0e+02˚C?
Nitrosyl bromide, NOBr, decomposes according to the equation NOBr(g) → NO(g) + 1/2 Br₂(g) where ∆G˚ at 4.0e+02 ˚C is 9.83 kJ. What is the value of the equilibrium constant at 4.0e+02˚C?
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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Nitrosyl bromide, NOBr, decomposes according to the equation
NOBr(g) → NO(g) + 1/2 Br₂(g)
where ∆G˚ at 4.0e+02 ˚C is 9.83 kJ. What is the value of the equilibrium constant at 4.0e+02˚C?
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