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Consider the reaction, 2X(g) + 3Y(g) → Z(g)
Where gases X and Y are insoluble and inert to water and Z form a basic solution. In an experiment 3 mole each of X and Y are allowed to react in 15 lit flask at 500 K. When the reaction is complete, 5L of water is added to the flask and temperature is reduced to 300 K. The pressure in the flask is (neglect aqueous tension)
- a)1.64 atm
- b)2.46 atm
- c)4.92 atm
- d)3.28 atm
Correct answer is option 'B'. Can you explain this answer?
Most Upvoted Answer
Consider the reaction, 2X(g) + 3Y(g) →Z(g)Where gases X and Y ar...
The reaction is
2X(g) + 3Y(g) → Z(g)
2 moles of X reacts with 3 moles of Y to form 1mole of Z.
Now 3 moles of X and 3 moles of Y are present in the flask. Y is the limiting reagent. (Tocheck LR, divide the no of moles by stoichiometric coff. of that element. The least value will be LR)
After reaction, 1 mole of X is remaining and 1 mole of Z is formed, X is insoluble in water whereas Z is soluble in water.
Thus, the pressure in the flask is due to 1 mole of X.
The total volume of the flask is 15 L. The volume of water is 5 L. Thus the volume of gas is 15-5 = 10L.
The ideal gas equation is pV = nRT
Hence ,
p = nRT/V = 1×0.0821×300/10
= 2.46 atm
2X(g) + 3Y(g) → Z(g)
2 moles of X reacts with 3 moles of Y to form 1mole of Z.
Now 3 moles of X and 3 moles of Y are present in the flask. Y is the limiting reagent. (Tocheck LR, divide the no of moles by stoichiometric coff. of that element. The least value will be LR)
After reaction, 1 mole of X is remaining and 1 mole of Z is formed, X is insoluble in water whereas Z is soluble in water.
Thus, the pressure in the flask is due to 1 mole of X.
The total volume of the flask is 15 L. The volume of water is 5 L. Thus the volume of gas is 15-5 = 10L.
The ideal gas equation is pV = nRT
Hence ,
p = nRT/V = 1×0.0821×300/10
= 2.46 atm
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Community Answer
Consider the reaction, 2X(g) + 3Y(g) →Z(g)Where gases X and Y ar...
Given:
- Reaction: 2X(g) + 3Y(g) → Z(g)
- Gases X and Y are insoluble and inert to water
- Z forms a basic solution
- 3 moles of X and Y are allowed to react in a 15 L flask at 500 K
- When the reaction is complete, 5 L of water is added to the flask
- Temperature is reduced to 300 K
To find: Pressure in the flask
Solution:
1. Calculate the initial number of moles of X and Y
- Total number of moles of X and Y = 3 + 3 = 6 moles
2. Calculate the number of moles of Z produced
- From the balanced equation, 2 moles of X reacts with 3 moles of Y to produce 1 mole of Z
- Therefore, 3 moles of X reacts with 4.5 moles of Y to produce (3/2) moles of Z
- Total number of moles of Z produced = (3/2) moles
3. Calculate the total number of moles of gas present after the reaction
- Total number of moles of gas = initial number of moles of X and Y - moles of X and Y reacted + moles of Z produced
- Total number of moles of gas = 6 - 3 - 4.5 + 1.5 = 0.5 moles
4. Calculate the pressure of the gas before water is added
- Using the ideal gas equation: PV = nRT
- P = (nRT)/V
- P = (0.5 mol x 0.0821 L atm mol^-1 K^-1 x 500 K)/15 L = 6.173 atm
5. Calculate the moles of Z in the solution after water is added
- Assuming Z is completely dissolved in water, the number of moles of Z in the solution is equal to the number of moles of Z produced
- Moles of Z in solution = (3/2) moles
6. Calculate the moles of water added
- Using the ideal gas equation: PV = nRT
- n = PV/RT
- n = (1 atm x 5 L)/(0.0821 L atm mol^-1 K^-1 x 300 K) = 0.204 moles
7. Calculate the new total number of moles of gas present after water is added
- Total number of moles of gas = moles of gas before water is added + moles of Z in solution + moles of water added
- Total number of moles of gas = 0.5 + (3/2) + 0.204 = 2.204 moles
8. Calculate the final pressure of the gas
- Using the ideal gas equation: PV = nRT
- P = (nRT)/V
- P = (2.204 mol x 0.0821 L atm mol^-1 K^-1 x 300 K)/(15 L) = 2.46 atm
Therefore, the pressure in the flask after adding water and reducing the temperature is 2.46 atm (Option B is correct).
- Reaction: 2X(g) + 3Y(g) → Z(g)
- Gases X and Y are insoluble and inert to water
- Z forms a basic solution
- 3 moles of X and Y are allowed to react in a 15 L flask at 500 K
- When the reaction is complete, 5 L of water is added to the flask
- Temperature is reduced to 300 K
To find: Pressure in the flask
Solution:
1. Calculate the initial number of moles of X and Y
- Total number of moles of X and Y = 3 + 3 = 6 moles
2. Calculate the number of moles of Z produced
- From the balanced equation, 2 moles of X reacts with 3 moles of Y to produce 1 mole of Z
- Therefore, 3 moles of X reacts with 4.5 moles of Y to produce (3/2) moles of Z
- Total number of moles of Z produced = (3/2) moles
3. Calculate the total number of moles of gas present after the reaction
- Total number of moles of gas = initial number of moles of X and Y - moles of X and Y reacted + moles of Z produced
- Total number of moles of gas = 6 - 3 - 4.5 + 1.5 = 0.5 moles
4. Calculate the pressure of the gas before water is added
- Using the ideal gas equation: PV = nRT
- P = (nRT)/V
- P = (0.5 mol x 0.0821 L atm mol^-1 K^-1 x 500 K)/15 L = 6.173 atm
5. Calculate the moles of Z in the solution after water is added
- Assuming Z is completely dissolved in water, the number of moles of Z in the solution is equal to the number of moles of Z produced
- Moles of Z in solution = (3/2) moles
6. Calculate the moles of water added
- Using the ideal gas equation: PV = nRT
- n = PV/RT
- n = (1 atm x 5 L)/(0.0821 L atm mol^-1 K^-1 x 300 K) = 0.204 moles
7. Calculate the new total number of moles of gas present after water is added
- Total number of moles of gas = moles of gas before water is added + moles of Z in solution + moles of water added
- Total number of moles of gas = 0.5 + (3/2) + 0.204 = 2.204 moles
8. Calculate the final pressure of the gas
- Using the ideal gas equation: PV = nRT
- P = (nRT)/V
- P = (2.204 mol x 0.0821 L atm mol^-1 K^-1 x 300 K)/(15 L) = 2.46 atm
Therefore, the pressure in the flask after adding water and reducing the temperature is 2.46 atm (Option B is correct).
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Consider the reaction, 2X(g) + 3Y(g) →Z(g)Where gases X and Y are insoluble and inert to water and Z form a basic solution. In an experiment 3 mole each of X and Y are allowed to react in 15 lit flask at 500 K. When the reaction is complete, 5L of water is added to the flask and temperature is reduced to 300 K. The pressure in the flask is (neglect aqueous tension)a)1.64 atm b)2.46 atmc)4.92 atmd)3.28 atmCorrect answer is option 'B'. Can you explain this answer? for Class 11 2026 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Consider the reaction, 2X(g) + 3Y(g) →Z(g)Where gases X and Y are insoluble and inert to water and Z form a basic solution. In an experiment 3 mole each of X and Y are allowed to react in 15 lit flask at 500 K. When the reaction is complete, 5L of water is added to the flask and temperature is reduced to 300 K. The pressure in the flask is (neglect aqueous tension)a)1.64 atm b)2.46 atmc)4.92 atmd)3.28 atmCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2026 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Consider the reaction, 2X(g) + 3Y(g) →Z(g)Where gases X and Y are insoluble and inert to water and Z form a basic solution. In an experiment 3 mole each of X and Y are allowed to react in 15 lit flask at 500 K. When the reaction is complete, 5L of water is added to the flask and temperature is reduced to 300 K. The pressure in the flask is (neglect aqueous tension)a)1.64 atm b)2.46 atmc)4.92 atmd)3.28 atmCorrect answer is option 'B'. Can you explain this answer?.
Consider the reaction, 2X(g) + 3Y(g) →Z(g)Where gases X and Y are insoluble and inert to water and Z form a basic solution. In an experiment 3 mole each of X and Y are allowed to react in 15 lit flask at 500 K. When the reaction is complete, 5L of water is added to the flask and temperature is reduced to 300 K. The pressure in the flask is (neglect aqueous tension)a)1.64 atm b)2.46 atmc)4.92 atmd)3.28 atmCorrect answer is option 'B'. Can you explain this answer? for Class 11 2026 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Consider the reaction, 2X(g) + 3Y(g) →Z(g)Where gases X and Y are insoluble and inert to water and Z form a basic solution. In an experiment 3 mole each of X and Y are allowed to react in 15 lit flask at 500 K. When the reaction is complete, 5L of water is added to the flask and temperature is reduced to 300 K. The pressure in the flask is (neglect aqueous tension)a)1.64 atm b)2.46 atmc)4.92 atmd)3.28 atmCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2026 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Consider the reaction, 2X(g) + 3Y(g) →Z(g)Where gases X and Y are insoluble and inert to water and Z form a basic solution. In an experiment 3 mole each of X and Y are allowed to react in 15 lit flask at 500 K. When the reaction is complete, 5L of water is added to the flask and temperature is reduced to 300 K. The pressure in the flask is (neglect aqueous tension)a)1.64 atm b)2.46 atmc)4.92 atmd)3.28 atmCorrect answer is option 'B'. Can you explain this answer?.
Solutions for Consider the reaction, 2X(g) + 3Y(g) →Z(g)Where gases X and Y are insoluble and inert to water and Z form a basic solution. In an experiment 3 mole each of X and Y are allowed to react in 15 lit flask at 500 K. When the reaction is complete, 5L of water is added to the flask and temperature is reduced to 300 K. The pressure in the flask is (neglect aqueous tension)a)1.64 atm b)2.46 atmc)4.92 atmd)3.28 atmCorrect answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 11. Download more important topics, notes, lectures and mock test series for Class 11 Exam by signing up for free.
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