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In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]
- a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
- b)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogen
- c)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
- d)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogen
Correct answer is option 'C'. Can you explain this answer?
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Verified Answer
In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen w...
It is given that only 50% of the expected product is formed hence only 10 litre of NH3 is formed N2 used = 5 litres, left = 30 – 5 = 25 litres H2 used = 15 litres, left = 30 – 15 = 15 litres
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In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen w...
**Given Information:**
- 30 litres of dihydrogen (H2)
- 30 litres of dinitrogen (N2)
- Yield of only 50% of the expected product
**Haber Process:**
The Haber process is a chemical reaction that converts nitrogen gas (N2) and hydrogen gas (H2) into ammonia (NH3). The reaction is as follows:
N2 + 3H2 ⇌ 2NH3
**Calculating the Theoretical Yield:**
To determine the theoretical yield of ammonia, we need to consider the stoichiometry of the reaction. From the balanced equation, we can see that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.
- Number of moles of nitrogen (N2) = (30 L N2) / (22.4 L/mol) = 1.34 moles
- Number of moles of hydrogen (H2) = (30 L H2) / (22.4 L/mol) = 1.34 moles
Since the reaction has a 1:3 ratio between nitrogen and hydrogen, we can determine that the limiting reactant is nitrogen. Therefore, the maximum number of moles of ammonia that can be produced is 2/1 * 1.34 = 2.68 moles.
**Calculating the Actual Yield:**
The question states that the yield is only 50% of the expected product. Therefore, the actual yield of ammonia is 50% of 2.68 moles, which is 1.34 moles.
**Calculating the Remaining Reactants:**
Since the reaction is not complete, there will be some nitrogen and hydrogen remaining after the reaction. From the balanced equation, we can see that the stoichiometry of the reaction is 1:3 between nitrogen and hydrogen. Therefore, for every 1 mole of nitrogen reacted, 3 moles of hydrogen are reacted.
- Moles of nitrogen reacted = 1.34 moles
- Moles of hydrogen reacted = 3 * 1.34 moles = 4.02 moles
Since there was a 50% yield, the moles of reactants consumed are also halved. Therefore, the moles of nitrogen and hydrogen remaining are:
- Moles of nitrogen remaining = 1.34 moles / 2 = 0.67 moles
- Moles of hydrogen remaining = 4.02 moles / 2 = 2.01 moles
**Converting Moles to Litres:**
To determine the composition of the gaseous mixture, we need to convert the remaining moles of nitrogen and hydrogen back into litres.
- Volume of nitrogen remaining = (0.67 moles) * (22.4 L/mol) = 14.97 L
- Volume of hydrogen remaining = (2.01 moles) * (22.4 L/mol) = 45.04 L
**Composition of Gaseous Mixture:**
The composition of the gaseous mixture at the end is given by the remaining moles/volumes of each gas.
- Ammonia (NH3): 1.34 moles = 1.34 * 22.4 L = 29.94 L
- Nitrogen (N2): 0.67 moles =
- 30 litres of dihydrogen (H2)
- 30 litres of dinitrogen (N2)
- Yield of only 50% of the expected product
**Haber Process:**
The Haber process is a chemical reaction that converts nitrogen gas (N2) and hydrogen gas (H2) into ammonia (NH3). The reaction is as follows:
N2 + 3H2 ⇌ 2NH3
**Calculating the Theoretical Yield:**
To determine the theoretical yield of ammonia, we need to consider the stoichiometry of the reaction. From the balanced equation, we can see that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.
- Number of moles of nitrogen (N2) = (30 L N2) / (22.4 L/mol) = 1.34 moles
- Number of moles of hydrogen (H2) = (30 L H2) / (22.4 L/mol) = 1.34 moles
Since the reaction has a 1:3 ratio between nitrogen and hydrogen, we can determine that the limiting reactant is nitrogen. Therefore, the maximum number of moles of ammonia that can be produced is 2/1 * 1.34 = 2.68 moles.
**Calculating the Actual Yield:**
The question states that the yield is only 50% of the expected product. Therefore, the actual yield of ammonia is 50% of 2.68 moles, which is 1.34 moles.
**Calculating the Remaining Reactants:**
Since the reaction is not complete, there will be some nitrogen and hydrogen remaining after the reaction. From the balanced equation, we can see that the stoichiometry of the reaction is 1:3 between nitrogen and hydrogen. Therefore, for every 1 mole of nitrogen reacted, 3 moles of hydrogen are reacted.
- Moles of nitrogen reacted = 1.34 moles
- Moles of hydrogen reacted = 3 * 1.34 moles = 4.02 moles
Since there was a 50% yield, the moles of reactants consumed are also halved. Therefore, the moles of nitrogen and hydrogen remaining are:
- Moles of nitrogen remaining = 1.34 moles / 2 = 0.67 moles
- Moles of hydrogen remaining = 4.02 moles / 2 = 2.01 moles
**Converting Moles to Litres:**
To determine the composition of the gaseous mixture, we need to convert the remaining moles of nitrogen and hydrogen back into litres.
- Volume of nitrogen remaining = (0.67 moles) * (22.4 L/mol) = 14.97 L
- Volume of hydrogen remaining = (2.01 moles) * (22.4 L/mol) = 45.04 L
**Composition of Gaseous Mixture:**
The composition of the gaseous mixture at the end is given by the remaining moles/volumes of each gas.
- Ammonia (NH3): 1.34 moles = 1.34 * 22.4 L = 29.94 L
- Nitrogen (N2): 0.67 moles =
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In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen w...
C is correct.
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In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer?
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In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer?.
In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer?.
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In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer?, a detailed solution for In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer? has been provided alongside types of In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end? [2003]a)20 litres ammonia, 25 litres nitrogen, 15 litres hydrogenb)20 litres ammonia, 20 litres nitrogen, 20 litres hydrogenc)10 litres ammonia, 25 litres nitrogen, 15 litres hydrogend)20 litres ammonia, 10 litres nitrogen, 30 litres hydrogenCorrect answer is option 'C'. Can you explain this answer? tests, examples and also practice Class 11 tests.
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