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1) Production of a diprotic acid H2XO4 involves 3 steps as shown below: 1. X(s) + O2(g)=XO2 (g) AH= -45 kJ/mol 2. 2XO2 (g) + O2(g) = 2XO3 (g) AH= 17 kJ/mol 3. 2XO3 (g) + H2O(g) = H2X04 (1) AH= -76 kJ/mol a) Write equilibrium expressions for each of the steps above (K1, K2, K3). b) The reactions above where carried at 273 K, and the equilibrium constants were determined to be 1.5 x 1043, 4.5 x 1011, and 2.8 x 1012 respectively. Determine the overall reaction and its equilibrium constant at 273 K. c) Given the equilibrium constant for K1, calculate the equilibrium pressure of XO2 if the initial concentration of O2 is 2 atm. d) Given the equilibrium constant for K2, determine the total pressure of gases at equilibrium if the initial concentration of XO2 and O2 was 1 atm. e) State Le Châtelier's principle and describe its application to each of the reactions described above and to the overall reaction.

1) Production of a diprotic acid H2XO4 involves 3 steps as shown below: 1. X(s) + O2(g)=XO2 (g) AH= -45 kJ/mol 2. 2XO2 (g) + O2(g) = 2XO3 (g) AH= 17 kJ/mol 3. 2XO3 (g) + H2O(g) = H2X04 (1) AH= -76 kJ/mol a) Write equilibrium expressions for each of the steps above (K1, K2, K3). b) The reactions above where carried at 273 K, and the equilibrium constants were determined to be 1.5 x 1043, 4.5 x 1011, and 2.8 x 1012 respectively. Determine the overall reaction and its equilibrium constant at 273 K. c) Given the equilibrium constant for K1, calculate the equilibrium pressure of XO2 if the initial concentration of O2 is 2 atm. d) Given the equilibrium constant for K2, determine the total pressure of gases at equilibrium if the initial concentration of XO2 and O2 was 1 atm. e) State Le Châtelier's principle and describe its application to each of the reactions described above and to the overall reaction.

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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Can you please help with d) if possible, with others too (except point c))

1) Production of a diprotic acid H2XO4 involves 3 steps as shown below: 1. X(s) + O2(g) = XO2 (g) AH= -45 kJ/mol 2. 2XO2 (g) + O2(g) = 2XO3 (g) AH= 17 kJ/mol 3. 2XO3 (g) + H2O(g) = H2XO4 (1) AH= -76 kJ/mol a) Write equilibrium expressions for each of the steps above (K1, K2, K3). b) The reactions above where carried at 273 K, and the equilibrium constants were determined to be 1.5 x 1043, 4.5 x 1011, and 2.8 x 1012 respectively. Determine the overall reaction and its equilibrium constant at 273 K. c) Given the equilibrium constant for K1, calculate the equilibrium pressure of XO2 if the initial concentration of O2 is 2 atm. d) Given the equilibrium constant for K2, determine the total pressure of gases at equilibrium if the initial concentration of XO2 and O2 was 1 atm. e) State Le Châtelier's principle and describe its application to each of the reactions described above and to the overall reaction.
Transcribed Image Text:1) Production of a diprotic acid H2XO4 involves 3 steps as shown below: 1. X(s) + O2(g) = XO2 (g) AH= -45 kJ/mol 2. 2XO2 (g) + O2(g) = 2XO3 (g) AH= 17 kJ/mol 3. 2XO3 (g) + H2O(g) = H2XO4 (1) AH= -76 kJ/mol a) Write equilibrium expressions for each of the steps above (K1, K2, K3). b) The reactions above where carried at 273 K, and the equilibrium constants were determined to be 1.5 x 1043, 4.5 x 1011, and 2.8 x 1012 respectively. Determine the overall reaction and its equilibrium constant at 273 K. c) Given the equilibrium constant for K1, calculate the equilibrium pressure of XO2 if the initial concentration of O2 is 2 atm. d) Given the equilibrium constant for K2, determine the total pressure of gases at equilibrium if the initial concentration of XO2 and O2 was 1 atm. e) State Le Châtelier's principle and describe its application to each of the reactions described above and to the overall reaction.
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