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Given the equilibrium constant values at 500 K and constant pressure:​
​N2(g) + ½ O2(g) N2O(g) ​Kc = 2.70 * 10-18​​ N2O4(g) 2 NO2(g) ​Kc = 4.60 * 10-3​​ ½ N2(g) + O2(g) NO2(g) ​Kc = 4.10 * 10-9 Determine the Kc value for:​ 2 N2O (g) + 3 O2(g) 2 N2O4(g) a) 3.44​x 10–6​ b) 1.83 x 106​ c) 5.29 x 10–3​ d) 1.24 x 105​e) 2.76 x 106

Given the equilibrium constant values at 500 K and constant pressure:​
​N2(g) + ½ O2(g) N2O(g) ​Kc = 2.70 * 10-18​​ N2O4(g) 2 NO2(g) ​Kc = 4.60 * 10-3​​ ½ N2(g) + O2(g) NO2(g) ​Kc = 4.10 * 10-9 Determine the Kc value for:​ 2 N2O (g) + 3 O2(g) 2 N2O4(g) a) 3.44​x 10–6​ b) 1.83 x 106​ c) 5.29 x 10–3​ d) 1.24 x 105​e) 2.76 x 106

Introduction to Chemical Engineering Thermodynamics
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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Given the equilibrium constant values at 500 K and constant pressure: ​
​N2(g) + ½ O2(g) N2O(g) ​Kc = 2.70 * 10-18 ​​ N2O4(g) 2 NO2(g) ​Kc = 4.60 * 10-3 ​​ ½ N2(g) + O2(g) NO2(g) ​Kc = 4.10 * 10-9 Determine the Kc value for:​ 2 N2O (g) + 3 O2(g) 2 N2O4(g) a) 3.44​x 10–6​ b) 1.83 x 106​ c) 5.29 x 10–3​ d) 1.24 x 105​e) 2.76 x 106
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