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The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?
Correct answer is between '1.12,1.17'. Can you explain this answer?
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The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ...
Fe(s) CO2(g) is given by:
Kc = [CO2][Fe]/[CO][Fe3O4]
where [CO2], [Fe], [CO], and [Fe3O4] represent the equilibrium concentrations of the respective species.
The equilibrium expression can be simplified by assuming that the solid Fe3O4 is in excess and its concentration remains constant at the start and end of the reaction. In this case, the equilibrium constant can be written as:
Kc = [CO2][Fe]/[CO]
where [Fe] represents the initial concentration of Fe in the reaction mixture.
The value of Kc depends on the temperature at which the reaction is carried out. At a given temperature, the equilibrium constant remains constant and is a measure of the extent to which the reaction proceeds in the forward or reverse direction.
Experimental determination of the equilibrium constant involves measuring the concentrations of the reactants and products at equilibrium and plugging them into the equilibrium expression. The equilibrium constant can also be calculated from thermodynamic data using the standard free energy change of the reaction.
Kc = [CO2][Fe]/[CO][Fe3O4]
where [CO2], [Fe], [CO], and [Fe3O4] represent the equilibrium concentrations of the respective species.
The equilibrium expression can be simplified by assuming that the solid Fe3O4 is in excess and its concentration remains constant at the start and end of the reaction. In this case, the equilibrium constant can be written as:
Kc = [CO2][Fe]/[CO]
where [Fe] represents the initial concentration of Fe in the reaction mixture.
The value of Kc depends on the temperature at which the reaction is carried out. At a given temperature, the equilibrium constant remains constant and is a measure of the extent to which the reaction proceeds in the forward or reverse direction.
Experimental determination of the equilibrium constant involves measuring the concentrations of the reactants and products at equilibrium and plugging them into the equilibrium expression. The equilibrium constant can also be calculated from thermodynamic data using the standard free energy change of the reaction.
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The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer?
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The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer?.
The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer? for Chemistry 2024 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer? covers all topics & solutions for Chemistry 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer?.
Solutions for The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer? in English & in Hindi are available as part of our courses for Chemistry.
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The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer?, a detailed solution for The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer? has been provided alongside types of The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice The equilibrium constant for the reversible reaction Fe3O4(s) + CO(g) ↔ 3FeO(s) + CO2(g) at 600oC is 1.00. If a mixture initially consisting of 1 mole of Fe3O4, 2 mole of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated at constant total pressure of 5 atm, how many moles of CO2 will be present at equilibrium?Correct answer is between '1.12,1.17'. Can you explain this answer? tests, examples and also practice Chemistry tests.
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