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1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).?
Most Upvoted Answer
1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel h...
Answers :
Write the eqn. first,
PCl5 -------> PCl3 + Cl2
Use ideal gas eqn. to get the value of n .i.e moles
and use concentration for finding of Kp instead of using partial pressure.
Kp = pcl3*cl2/pcl5
2 years ago
PCL5=> PCL3 + CL2 3 mol 0 mol 0 mol no.moles initially 3(3-x) 3x 3x no.of moles at equi. now,
on using
PV=nRT [P=2.05 , V=100 , R=0.0821 , T=227 DEGREE CELCIUS MEANS 500K]
=> 2.05*100=n*0.0821*500
=> 205=41.05n
=> n=4.9[ we can take approx 5]
total number of moles at equilibrium
=>3-3x+3x+3x+1=5[we have taken 1 here because we have to add no. of moles of Cl2]
=> 3x+4=5
=> x=0.33[degree of dissociation]
frome here we can find Kp also that will be 0.205atm
Write the eqn. first,
PCl5 -------> PCl3 + Cl2
Use ideal gas eqn. to get the value of n .i.e moles
and use concentration for finding of Kp instead of using partial pressure.
Kp = pcl3*cl2/pcl5
2 years ago
PCL5=> PCL3 + CL2 3 mol 0 mol 0 mol no.moles initially 3(3-x) 3x 3x no.of moles at equi. now,
on using
PV=nRT [P=2.05 , V=100 , R=0.0821 , T=227 DEGREE CELCIUS MEANS 500K]
=> 2.05*100=n*0.0821*500
=> 205=41.05n
=> n=4.9[ we can take approx 5]
total number of moles at equilibrium
=>3-3x+3x+3x+1=5[we have taken 1 here because we have to add no. of moles of Cl2]
=> 3x+4=5
=> x=0.33[degree of dissociation]
frome here we can find Kp also that will be 0.205atm
Community Answer
1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel h...
Given:
- 1 mole of Cl2(g) and 3 moles of PCl5(g)
- Placed in a 100 L vessel
- Heated to 227 degrees Celsius
- Equilibrium pressure is 2.05 atm
To find:
- Degree of dissociation of PCl5(g)
- Kp for the reaction, PCl5(g) = PCl3 + Cl2(g)
Solution:
Step 1: Write the balanced equation:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
Step 2: Set up the ICE table:
Let x be the degree of dissociation of PCl5.
Initial moles:
PCl5(g): 3 moles
PCl3(g): 0 moles
Cl2(g): 1 mole
Change in moles:
PCl5(g): -x moles
PCl3(g): +x moles
Cl2(g): +x moles
Equilibrium moles:
PCl5(g): (3 - x) moles
PCl3(g): x moles
Cl2(g): (1 + x) moles
Step 3: Calculate the equilibrium pressure:
Since the volume of the vessel is given as 100 L, we can assume ideal behavior and use the ideal gas law to calculate the equilibrium pressure.
PV = nRT
For PCl5(g):
P(PCl5) = (3 - x) moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K
For PCl3(g):
P(PCl3) = x moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K
For Cl2(g):
P(Cl2) = (1 + x) moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K
The total equilibrium pressure is given as 2.05 atm:
2.05 atm = P(PCl5) + P(PCl3) + P(Cl2)
Step 4: Solve for x:
Substitute the calculated pressures into the equation:
2.05 atm = (3 - x) moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K + x moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K + (1 + x) moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K
Simplify and solve for x.
Step 5: Calculate Kp:
Kp is the equilibrium constant for the reaction, which can be calculated using the equilibrium partial pressures.
Kp = (P(PCl3) * P(Cl2)) / P(PCl5)
Substitute the calculated pressures into the equation to find Kp.
Conclusion:
- The degree of dissociation of PCl5(g) can be calculated by solving the equation derived from the ICE table.
- The
- 1 mole of Cl2(g) and 3 moles of PCl5(g)
- Placed in a 100 L vessel
- Heated to 227 degrees Celsius
- Equilibrium pressure is 2.05 atm
To find:
- Degree of dissociation of PCl5(g)
- Kp for the reaction, PCl5(g) = PCl3 + Cl2(g)
Solution:
Step 1: Write the balanced equation:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
Step 2: Set up the ICE table:
Let x be the degree of dissociation of PCl5.
Initial moles:
PCl5(g): 3 moles
PCl3(g): 0 moles
Cl2(g): 1 mole
Change in moles:
PCl5(g): -x moles
PCl3(g): +x moles
Cl2(g): +x moles
Equilibrium moles:
PCl5(g): (3 - x) moles
PCl3(g): x moles
Cl2(g): (1 + x) moles
Step 3: Calculate the equilibrium pressure:
Since the volume of the vessel is given as 100 L, we can assume ideal behavior and use the ideal gas law to calculate the equilibrium pressure.
PV = nRT
For PCl5(g):
P(PCl5) = (3 - x) moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K
For PCl3(g):
P(PCl3) = x moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K
For Cl2(g):
P(Cl2) = (1 + x) moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K
The total equilibrium pressure is given as 2.05 atm:
2.05 atm = P(PCl5) + P(PCl3) + P(Cl2)
Step 4: Solve for x:
Substitute the calculated pressures into the equation:
2.05 atm = (3 - x) moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K + x moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K + (1 + x) moles / 100 L * 0.0821 L·atm/mol·K * (227 + 273) K
Simplify and solve for x.
Step 5: Calculate Kp:
Kp is the equilibrium constant for the reaction, which can be calculated using the equilibrium partial pressures.
Kp = (P(PCl3) * P(Cl2)) / P(PCl5)
Substitute the calculated pressures into the equation to find Kp.
Conclusion:
- The degree of dissociation of PCl5(g) can be calculated by solving the equation derived from the ICE table.
- The
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1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).?
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1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).?.
1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).?.
Solutions for 1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).? in English & in Hindi are available as part of our courses for NEET.
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1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).?, a detailed solution for 1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).? has been provided alongside types of 1 mole of Cl2(g) and 3 moles of PCl5(g) are placed in a 100 l vessel heated to 227 degree Celsius. The equilibrium pressure is 2.05atm. Assuming ideal behavior, calculate the degree of dissociation of PCl5(g) and Kp for the reaction, PCl5(g) = PCl3 + Cl2(g).? theory, EduRev gives you an
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