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A 10 moles of pcl5 are heated in a vessel of 1litre capacity At equilibrium the degree of dissociation of pcl5 is 0.6find kc?
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Introduction
To find the equilibrium constant (Kc) for the dissociation of PCl5, we start with the balanced reaction:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
Initial Conditions
- Number of moles of PCl5 = 10 moles
- Volume of the vessel = 1 L
- Initial concentration of PCl5 = 10 moles/L = 10 M
Degree of Dissociation
- Given degree of dissociation (α) = 0.6
- At equilibrium, the amount of PCl5 that dissociates = α × Initial moles = 0.6 × 10 = 6 moles
Equilibrium Concentrations
- Moles of PCl5 remaining = Initial moles - Moles dissociated
- = 10 - 6 = 4 moles
- Moles of PCl3 formed = 6 moles
- Moles of Cl2 formed = 6 moles
Since the volume of the vessel is 1 L, the concentrations at equilibrium are:
- [PCl5] = 4 moles/1 L = 4 M
- [PCl3] = 6 moles/1 L = 6 M
- [Cl2] = 6 moles/1 L = 6 M
Expression for Kc
The expression for the equilibrium constant (Kc) is given by:
Kc = [PCl3][Cl2] / [PCl5]
Calculating Kc
Substituting the equilibrium concentrations into the expression:
Kc = (6)(6) / (4)
Kc = 36 / 4 = 9
Conclusion
The equilibrium constant Kc for the dissociation of PCl5 at the given conditions is:
Kc = 9
To find the equilibrium constant (Kc) for the dissociation of PCl5, we start with the balanced reaction:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
Initial Conditions
- Number of moles of PCl5 = 10 moles
- Volume of the vessel = 1 L
- Initial concentration of PCl5 = 10 moles/L = 10 M
Degree of Dissociation
- Given degree of dissociation (α) = 0.6
- At equilibrium, the amount of PCl5 that dissociates = α × Initial moles = 0.6 × 10 = 6 moles
Equilibrium Concentrations
- Moles of PCl5 remaining = Initial moles - Moles dissociated
- = 10 - 6 = 4 moles
- Moles of PCl3 formed = 6 moles
- Moles of Cl2 formed = 6 moles
Since the volume of the vessel is 1 L, the concentrations at equilibrium are:
- [PCl5] = 4 moles/1 L = 4 M
- [PCl3] = 6 moles/1 L = 6 M
- [Cl2] = 6 moles/1 L = 6 M
Expression for Kc
The expression for the equilibrium constant (Kc) is given by:
Kc = [PCl3][Cl2] / [PCl5]
Calculating Kc
Substituting the equilibrium concentrations into the expression:
Kc = (6)(6) / (4)
Kc = 36 / 4 = 9
Conclusion
The equilibrium constant Kc for the dissociation of PCl5 at the given conditions is:
Kc = 9
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A 10 moles of pcl5 are heated in a vessel of 1litre capacity At equilibrium the degree of dissociation of pcl5 is 0.6find kc?
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A 10 moles of pcl5 are heated in a vessel of 1litre capacity At equilibrium the degree of dissociation of pcl5 is 0.6find kc? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A 10 moles of pcl5 are heated in a vessel of 1litre capacity At equilibrium the degree of dissociation of pcl5 is 0.6find kc? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 10 moles of pcl5 are heated in a vessel of 1litre capacity At equilibrium the degree of dissociation of pcl5 is 0.6find kc?.
A 10 moles of pcl5 are heated in a vessel of 1litre capacity At equilibrium the degree of dissociation of pcl5 is 0.6find kc? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A 10 moles of pcl5 are heated in a vessel of 1litre capacity At equilibrium the degree of dissociation of pcl5 is 0.6find kc? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 10 moles of pcl5 are heated in a vessel of 1litre capacity At equilibrium the degree of dissociation of pcl5 is 0.6find kc?.
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