Bromine and water react to form hydrogen bromide and oxygen, like this: 2 Br,(g) + 2 H,O(g) - 4 HBr(g) + 0,(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of bromine, water, hydrogen bromide, and oxygen has the following composition: compound pressure at equilibrium Br2 75.1 atm H,0 27.5 atm HBr 6.09 atm O2 68.3 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K, = 0
Bromine and water react to form hydrogen bromide and oxygen, like this: 2 Br,(g) + 2 H,O(g) - 4 HBr(g) + 0,(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of bromine, water, hydrogen bromide, and oxygen has the following composition: compound pressure at equilibrium Br2 75.1 atm H,0 27.5 atm HBr 6.09 atm O2 68.3 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K, = 0
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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