-) 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.
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Chapter6: Thermochemistry
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Problem 105AE: Combustion of table sugar produces CO2(g) and H2O( l). When 1.46 g table sugar is combusted in a...
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Hello! Can you please help with d)
and if possible with others too (except c)
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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