IV. At 800 K, 2.00 moles of NO are mixed with 1.00 mole of O₂. The reaction 2 NO(g) + O₂ (g) = 2 NO: (g) comes to equilibrium at a total pressure of 1 bar. Analysis of the system shows that 0.71 moles of oxygen are present at equilibrium. a) Calculate the equilibrium constant for the reaction. b) Calculate AG" for the reaction at 800 K. (
IV. At 800 K, 2.00 moles of NO are mixed with 1.00 mole of O₂. The reaction 2 NO(g) + O₂ (g) = 2 NO: (g) comes to equilibrium at a total pressure of 1 bar. Analysis of the system shows that 0.71 moles of oxygen are present at equilibrium. a) Calculate the equilibrium constant for the reaction. b) Calculate AG" for the reaction at 800 K. (
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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Solve correctly please, this much data info given.
![IV. At 800 K, 2.00 moles of NO are mixed with 1.00 mole of O₂. The reaction
2 NO(g) + O₂(g) = 2 NO₂ (g)
comes to equilibrium at a total pressure of 1 bar. Analysis of the system shows that 0.71 moles of
oxygen are present at equilibrium.
a) Calculate the equilibrium constant for the reaction.
b) Calculate AG for the reaction at 800 K. (](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F47b0c065-d829-4cdd-bbb4-fc0ba1d88dca%2F722c72f1-aef8-4fa7-be22-3dc935ea92f7%2F4hd1ups_processed.jpeg&w=3840&q=75)
Transcribed Image Text:IV. At 800 K, 2.00 moles of NO are mixed with 1.00 mole of O₂. The reaction
2 NO(g) + O₂(g) = 2 NO₂ (g)
comes to equilibrium at a total pressure of 1 bar. Analysis of the system shows that 0.71 moles of
oxygen are present at equilibrium.
a) Calculate the equilibrium constant for the reaction.
b) Calculate AG for the reaction at 800 K. (
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