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20g CaCO3 is taken in a 10 L container at 827°C. for the equilibrium CaCO3 --> CaO + CO2 Kp = 1.1 find the percentage of CaCo3 that remains unreacted?
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20g CaCO3 is taken in a 10 L container at 827°C. for the equilibrium C...
Calculation of Percentage of CaCO3 Remaining
- Given information:
- Initial amount of CaCO3 = 20g
- Volume of container = 10 L
- Temperature = 827°C
- Equilibrium reaction: CaCO3 --> CaO + CO2
- Kp = 1.1
Step 1: Calculate the moles of CaCO3
Molar mass of CaCO3 = 100.09 g/mol
Moles of CaCO3 = 20g / 100.09 g/mol = 0.1997 mol
Step 2: Calculate the partial pressures of CaO and CO2 at equilibrium
Since 1 mol of CaCO3 produces 1 mol of CaO and 1 mol of CO2,
Partial pressure of CaO = x atm
Partial pressure of CO2 = x atm
Step 3: Calculate the total pressure at equilibrium
Total pressure at equilibrium = P(CaO) + P(CO2) = 2x atm
Step 4: Use the equilibrium constant (Kp) to find the value of x
Kp = P(CaO) * P(CO2) / P(CaCO3)
1.1 = x * x / (0.1997 - x)
Step 5: Solve for x
After solving the equation, we get x = 0.4106 atm
Step 6: Calculate the percentage of CaCO3 remaining
Percentage of CaCO3 remaining = (Moles of CaCO3 remaining / Moles of CaCO3 initially) * 100
Moles of CaCO3 remaining can be calculated using the value of x obtained above.
Therefore, the percentage of CaCO3 that remains unreacted can be calculated using the above steps.
- Given information:
- Initial amount of CaCO3 = 20g
- Volume of container = 10 L
- Temperature = 827°C
- Equilibrium reaction: CaCO3 --> CaO + CO2
- Kp = 1.1
Step 1: Calculate the moles of CaCO3
Molar mass of CaCO3 = 100.09 g/mol
Moles of CaCO3 = 20g / 100.09 g/mol = 0.1997 mol
Step 2: Calculate the partial pressures of CaO and CO2 at equilibrium
Since 1 mol of CaCO3 produces 1 mol of CaO and 1 mol of CO2,
Partial pressure of CaO = x atm
Partial pressure of CO2 = x atm
Step 3: Calculate the total pressure at equilibrium
Total pressure at equilibrium = P(CaO) + P(CO2) = 2x atm
Step 4: Use the equilibrium constant (Kp) to find the value of x
Kp = P(CaO) * P(CO2) / P(CaCO3)
1.1 = x * x / (0.1997 - x)
Step 5: Solve for x
After solving the equation, we get x = 0.4106 atm
Step 6: Calculate the percentage of CaCO3 remaining
Percentage of CaCO3 remaining = (Moles of CaCO3 remaining / Moles of CaCO3 initially) * 100
Moles of CaCO3 remaining can be calculated using the value of x obtained above.
Therefore, the percentage of CaCO3 that remains unreacted can be calculated using the above steps.
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20g CaCO3 is taken in a 10 L container at 827°C. for the equilibrium CaCO3 --> CaO + CO2 Kp = 1.1 find the percentage of CaCo3 that remains unreacted?
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20g CaCO3 is taken in a 10 L container at 827°C. for the equilibrium CaCO3 --> CaO + CO2 Kp = 1.1 find the percentage of CaCo3 that remains unreacted? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about 20g CaCO3 is taken in a 10 L container at 827°C. for the equilibrium CaCO3 --> CaO + CO2 Kp = 1.1 find the percentage of CaCo3 that remains unreacted? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 20g CaCO3 is taken in a 10 L container at 827°C. for the equilibrium CaCO3 --> CaO + CO2 Kp = 1.1 find the percentage of CaCo3 that remains unreacted?.
20g CaCO3 is taken in a 10 L container at 827°C. for the equilibrium CaCO3 --> CaO + CO2 Kp = 1.1 find the percentage of CaCo3 that remains unreacted? for UPSC 2024 is part of UPSC preparation. The Question and answers have been prepared according to the UPSC exam syllabus. Information about 20g CaCO3 is taken in a 10 L container at 827°C. for the equilibrium CaCO3 --> CaO + CO2 Kp = 1.1 find the percentage of CaCo3 that remains unreacted? covers all topics & solutions for UPSC 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 20g CaCO3 is taken in a 10 L container at 827°C. for the equilibrium CaCO3 --> CaO + CO2 Kp = 1.1 find the percentage of CaCo3 that remains unreacted?.
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