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
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
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
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The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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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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