Let's go back to the original equilibrium position established by the reaction, with the equilibrium molarity for oxygen gas as 0.150 M. The temperature for the reaction is now changed to 578 K, and the new equilibrium molarity for oxygen gas is found to be 0.055 M. Is the reaction endothermic or exothermic, as written? Circle and explain your answer below. endothermic exothermic
Let's go back to the original equilibrium position established by the reaction, with the equilibrium molarity for oxygen gas as 0.150 M. The temperature for the reaction is now changed to 578 K, and the new equilibrium molarity for oxygen gas is found to be 0.055 M. Is the reaction endothermic or exothermic, as written? Circle and explain your answer below. endothermic exothermic
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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Transcribed Image Text:Nitrogen and oxygen gases react reversibly to produce gaseous N2O4 in a
4.00 L container being held at 278 K. 2.00 mols of each reactant and 1.00 mol of
the product are initially placed into the container, and once the reaction
establishes equilibrium, the molarity of oxygen gas is measured as 0.150 M.
Answer the questions below.
Transcribed Image Text:Let's go back to the original equilibrium position established by
the reaction, with the equilibrium molarity for oxygen gas as 0.150 M. The
temperature for the reaction is now changed to 578 K, and the new equilibrium
molarity for oxygen gas is found to be 0.055 M. Is the reaction endothermic or
exothermic, as written? Circle and explain your answer below.
endothermic
exothermic
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