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One mole of pure pcl5 is placed in an evacuated container and maintained at 250°C the equilibrium is established at total pressure of 2 atm what is partial pressure of chlorine at equilibrium?
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One mole of pure pcl5 is placed in an evacuated container and maintain...
Understanding the Reaction
When one mole of pure PCl5 is placed in a container, it can dissociate into PCl3 and Cl2 according to the equilibrium reaction:
PCl5 ⇌ PCl3 + Cl2
Initial Conditions
- Initial moles of PCl5 = 1
- Moles of PCl3 = 0
- Moles of Cl2 = 0
Setting Up the Equilibrium
Let "x" be the amount of PCl5 that dissociates at equilibrium:
- Moles of PCl5 at equilibrium = 1 - x
- Moles of PCl3 at equilibrium = x
- Moles of Cl2 at equilibrium = x
Total Moles at Equilibrium
Total moles at equilibrium = (1 - x) + x + x = 1 + x
Using Total Pressure
Given that the total pressure at equilibrium is 2 atm:
P = (Total moles) × (RT/V)
Since R and V are constants, we can use the ideal gas law to express the pressure in terms of moles. Here, P = 2 atm:
2 atm = (1 + x) × (P/RT)
Finding "x"
To find the partial pressures, we need to express the moles in terms of total pressure. Using Dalton's Law:
Partial pressure of Cl2 = (moles of Cl2 / total moles) × total pressure
Substituting for total moles:
Partial pressure of Cl2 = (x / (1 + x)) × 2 atm
Equilibrium Condition
At equilibrium, we know that the system must balance. If we assume that PCl5 dissociates completely (x = 1), then:
Total moles = 1 + 1 = 2
Partial pressure of Cl2 = (1 / 2) × 2 atm = 1 atm
Conclusion
Thus, the partial pressure of chlorine (Cl2) at equilibrium is 1 atm.
When one mole of pure PCl5 is placed in a container, it can dissociate into PCl3 and Cl2 according to the equilibrium reaction:
PCl5 ⇌ PCl3 + Cl2
Initial Conditions
- Initial moles of PCl5 = 1
- Moles of PCl3 = 0
- Moles of Cl2 = 0
Setting Up the Equilibrium
Let "x" be the amount of PCl5 that dissociates at equilibrium:
- Moles of PCl5 at equilibrium = 1 - x
- Moles of PCl3 at equilibrium = x
- Moles of Cl2 at equilibrium = x
Total Moles at Equilibrium
Total moles at equilibrium = (1 - x) + x + x = 1 + x
Using Total Pressure
Given that the total pressure at equilibrium is 2 atm:
P = (Total moles) × (RT/V)
Since R and V are constants, we can use the ideal gas law to express the pressure in terms of moles. Here, P = 2 atm:
2 atm = (1 + x) × (P/RT)
Finding "x"
To find the partial pressures, we need to express the moles in terms of total pressure. Using Dalton's Law:
Partial pressure of Cl2 = (moles of Cl2 / total moles) × total pressure
Substituting for total moles:
Partial pressure of Cl2 = (x / (1 + x)) × 2 atm
Equilibrium Condition
At equilibrium, we know that the system must balance. If we assume that PCl5 dissociates completely (x = 1), then:
Total moles = 1 + 1 = 2
Partial pressure of Cl2 = (1 / 2) × 2 atm = 1 atm
Conclusion
Thus, the partial pressure of chlorine (Cl2) at equilibrium is 1 atm.
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One mole of pure pcl5 is placed in an evacuated container and maintained at 250°C the equilibrium is established at total pressure of 2 atm what is partial pressure of chlorine at equilibrium?
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One mole of pure pcl5 is placed in an evacuated container and maintained at 250°C the equilibrium is established at total pressure of 2 atm what is partial pressure of chlorine at equilibrium? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about One mole of pure pcl5 is placed in an evacuated container and maintained at 250°C the equilibrium is established at total pressure of 2 atm what is partial pressure of chlorine at equilibrium? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for One mole of pure pcl5 is placed in an evacuated container and maintained at 250°C the equilibrium is established at total pressure of 2 atm what is partial pressure of chlorine at equilibrium?.
One mole of pure pcl5 is placed in an evacuated container and maintained at 250°C the equilibrium is established at total pressure of 2 atm what is partial pressure of chlorine at equilibrium? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about One mole of pure pcl5 is placed in an evacuated container and maintained at 250°C the equilibrium is established at total pressure of 2 atm what is partial pressure of chlorine at equilibrium? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for One mole of pure pcl5 is placed in an evacuated container and maintained at 250°C the equilibrium is established at total pressure of 2 atm what is partial pressure of chlorine at equilibrium?.
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