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340g of mixture of nitrogen and hydrogen in the correct ratio gave 20% yield of ammonia.the produced mass of ammonia would be
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Mass of Nitrogen and Hydrogen Mixture:
Given that the mass of the nitrogen and hydrogen mixture is 340g.
Yield of Ammonia:
The yield of ammonia is 20%, which means that only 20% of the reactants actually convert into ammonia.
Determining the Mass of Ammonia Produced:
To determine the mass of ammonia produced, we need to consider the balanced chemical equation for the reaction between nitrogen and hydrogen to form ammonia:
N₂ + 3H₂ → 2NH₃
From the balanced equation, we can see that for every 1 mole of nitrogen (N₂) and 3 moles of hydrogen (H₂), we obtain 2 moles of ammonia (NH₃). To calculate the mass of ammonia produced, we need to know the molar masses of nitrogen, hydrogen, and ammonia.
The molar mass of nitrogen (N₂) is approximately 28 g/mol, while the molar mass of hydrogen (H₂) is approximately 2 g/mol. The molar mass of ammonia (NH₃) is approximately 17 g/mol.
Calculating the Moles of Nitrogen and Hydrogen:
To determine the moles of nitrogen and hydrogen in the given mixture, we need to divide their masses by their respective molar masses.
Moles of nitrogen = mass of nitrogen / molar mass of nitrogen
Moles of hydrogen = mass of hydrogen / molar mass of hydrogen
Calculating the Moles of Ammonia Produced:
From the balanced equation, we know that 1 mole of nitrogen reacts to form 2 moles of ammonia. Therefore, the moles of ammonia produced can be calculated as follows:
Moles of ammonia = moles of nitrogen × (2 moles of ammonia / 1 mole of nitrogen)
Calculating the Mass of Ammonia Produced:
To find the mass of ammonia produced, we multiply the moles of ammonia by the molar mass of ammonia:
Mass of ammonia = moles of ammonia × molar mass of ammonia
Since we know that the yield of ammonia is 20%, we can calculate the actual mass of ammonia produced by multiplying the calculated mass by the yield percentage:
Actual mass of ammonia produced = mass of ammonia × (yield percentage / 100)
Conclusion:
By following the steps outlined above, we can determine the mass of ammonia produced from a given mass of nitrogen and hydrogen mixture.
Given that the mass of the nitrogen and hydrogen mixture is 340g.
Yield of Ammonia:
The yield of ammonia is 20%, which means that only 20% of the reactants actually convert into ammonia.
Determining the Mass of Ammonia Produced:
To determine the mass of ammonia produced, we need to consider the balanced chemical equation for the reaction between nitrogen and hydrogen to form ammonia:
N₂ + 3H₂ → 2NH₃
From the balanced equation, we can see that for every 1 mole of nitrogen (N₂) and 3 moles of hydrogen (H₂), we obtain 2 moles of ammonia (NH₃). To calculate the mass of ammonia produced, we need to know the molar masses of nitrogen, hydrogen, and ammonia.
The molar mass of nitrogen (N₂) is approximately 28 g/mol, while the molar mass of hydrogen (H₂) is approximately 2 g/mol. The molar mass of ammonia (NH₃) is approximately 17 g/mol.
Calculating the Moles of Nitrogen and Hydrogen:
To determine the moles of nitrogen and hydrogen in the given mixture, we need to divide their masses by their respective molar masses.
Moles of nitrogen = mass of nitrogen / molar mass of nitrogen
Moles of hydrogen = mass of hydrogen / molar mass of hydrogen
Calculating the Moles of Ammonia Produced:
From the balanced equation, we know that 1 mole of nitrogen reacts to form 2 moles of ammonia. Therefore, the moles of ammonia produced can be calculated as follows:
Moles of ammonia = moles of nitrogen × (2 moles of ammonia / 1 mole of nitrogen)
Calculating the Mass of Ammonia Produced:
To find the mass of ammonia produced, we multiply the moles of ammonia by the molar mass of ammonia:
Mass of ammonia = moles of ammonia × molar mass of ammonia
Since we know that the yield of ammonia is 20%, we can calculate the actual mass of ammonia produced by multiplying the calculated mass by the yield percentage:
Actual mass of ammonia produced = mass of ammonia × (yield percentage / 100)
Conclusion:
By following the steps outlined above, we can determine the mass of ammonia produced from a given mass of nitrogen and hydrogen mixture.
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340g of mixture of nitrogen and hydrogen in the correct ratio gave 20% yield of ammonia.the produced mass of ammonia would be
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340g of mixture of nitrogen and hydrogen in the correct ratio gave 20% yield of ammonia.the produced mass of ammonia would be 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 340g of mixture of nitrogen and hydrogen in the correct ratio gave 20% yield of ammonia.the produced mass of ammonia would be covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 340g of mixture of nitrogen and hydrogen in the correct ratio gave 20% yield of ammonia.the produced mass of ammonia would be.
340g of mixture of nitrogen and hydrogen in the correct ratio gave 20% yield of ammonia.the produced mass of ammonia would be 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 340g of mixture of nitrogen and hydrogen in the correct ratio gave 20% yield of ammonia.the produced mass of ammonia would be covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 340g of mixture of nitrogen and hydrogen in the correct ratio gave 20% yield of ammonia.the produced mass of ammonia would be.
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