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-) 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.

-) 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.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Hello! Can you please help with d) 

and if possible with others too (except 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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