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A gaseous compound of nitrogen and hydrogen contains 12.5%(by mass) of hydrogen. The density of the compound relative to hydrogen is 16. The molecular formula of the compound is :
- a)NH2
- b)NH3
- c)N3H
- d)N2H4
Correct answer is option 'D'. Can you explain this answer?
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Verified Answer
A gaseous compound of nitrogen and hydrogen contains 12.5%(by mass) of...
Empirical formula = NH2
Since Vapour density = 16
∴ mol. wt. = 32
∵ Molecular formula = n × Emp. formula = 2 × NH2
= N2H4
Most Upvoted Answer
A gaseous compound of nitrogen and hydrogen contains 12.5%(by mass) of...
Given information:
- The gaseous compound contains 12.5% hydrogen by mass.
- The compound has a density relative to hydrogen of 16.
To find:
- The molecular formula of the compound.
Solution:
Step 1: Determine the empirical formula
The empirical formula gives the simplest ratio of the atoms present in a compound.
Assuming we have 100g of the compound:
- The mass of hydrogen in the compound = 12.5g (12.5% of 100g)
- The mass of nitrogen in the compound = 100g - 12.5g = 87.5g (total mass - mass of hydrogen)
Calculate the moles of hydrogen and nitrogen:
- Moles of hydrogen = mass/molar mass = 12.5g/1g/mol = 12.5 mol
- Moles of nitrogen = mass/molar mass = 87.5g/14g/mol = 6.25 mol
Divide by the smallest number of moles:
- Divide the number of moles of each element by the smallest number of moles to obtain the simplest whole number ratio.
- In this case, the smallest number of moles is 6.25 mol (moles of nitrogen).
- Moles of hydrogen in the empirical formula = 12.5 mol / 6.25 mol = 2
- Moles of nitrogen in the empirical formula = 6.25 mol / 6.25 mol = 1
Therefore, the empirical formula of the compound is NH2.
Step 2: Determine the molecular formula
The molecular formula gives the actual number of atoms of each element present in a compound.
Calculate the molar mass of the empirical formula:
- Molar mass of nitrogen = 14g/mol
- Molar mass of hydrogen = 1g/mol
Molar mass of NH2 = (1g/mol * 2) + 14g/mol = 16g/mol
Calculate the ratio of the molar mass of the compound to the molar mass of the empirical formula:
- Ratio = molar mass of compound / molar mass of empirical formula
= density of compound / density of empirical formula
Given that the density of the compound relative to hydrogen is 16, we can write:
16 = molar mass of compound / 16g/mol
Calculate the molar mass of the compound:
Molar mass of compound = 16g/mol * 16 = 256g/mol
Calculate the ratio of the molar masses:
- Ratio = 256g/mol / 16g/mol = 16
Since the ratio is 16, it means that the molecular formula is 16 times the empirical formula.
Final Answer:
The molecular formula of the compound is N2H4 (16 times the empirical formula NH2). Therefore, the correct answer is option D).
- The gaseous compound contains 12.5% hydrogen by mass.
- The compound has a density relative to hydrogen of 16.
To find:
- The molecular formula of the compound.
Solution:
Step 1: Determine the empirical formula
The empirical formula gives the simplest ratio of the atoms present in a compound.
Assuming we have 100g of the compound:
- The mass of hydrogen in the compound = 12.5g (12.5% of 100g)
- The mass of nitrogen in the compound = 100g - 12.5g = 87.5g (total mass - mass of hydrogen)
Calculate the moles of hydrogen and nitrogen:
- Moles of hydrogen = mass/molar mass = 12.5g/1g/mol = 12.5 mol
- Moles of nitrogen = mass/molar mass = 87.5g/14g/mol = 6.25 mol
Divide by the smallest number of moles:
- Divide the number of moles of each element by the smallest number of moles to obtain the simplest whole number ratio.
- In this case, the smallest number of moles is 6.25 mol (moles of nitrogen).
- Moles of hydrogen in the empirical formula = 12.5 mol / 6.25 mol = 2
- Moles of nitrogen in the empirical formula = 6.25 mol / 6.25 mol = 1
Therefore, the empirical formula of the compound is NH2.
Step 2: Determine the molecular formula
The molecular formula gives the actual number of atoms of each element present in a compound.
Calculate the molar mass of the empirical formula:
- Molar mass of nitrogen = 14g/mol
- Molar mass of hydrogen = 1g/mol
Molar mass of NH2 = (1g/mol * 2) + 14g/mol = 16g/mol
Calculate the ratio of the molar mass of the compound to the molar mass of the empirical formula:
- Ratio = molar mass of compound / molar mass of empirical formula
= density of compound / density of empirical formula
Given that the density of the compound relative to hydrogen is 16, we can write:
16 = molar mass of compound / 16g/mol
Calculate the molar mass of the compound:
Molar mass of compound = 16g/mol * 16 = 256g/mol
Calculate the ratio of the molar masses:
- Ratio = 256g/mol / 16g/mol = 16
Since the ratio is 16, it means that the molecular formula is 16 times the empirical formula.
Final Answer:
The molecular formula of the compound is N2H4 (16 times the empirical formula NH2). Therefore, the correct answer is option D).
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A gaseous compound of nitrogen and hydrogen contains 12.5%(by mass) of hydrogen. The density of the compound relative to hydrogen is 16. The molecular formula of the compound is :a)NH2b)NH3c)N3Hd)N2H4Correct answer is option 'D'. Can you explain this answer?
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A gaseous compound of nitrogen and hydrogen contains 12.5%(by mass) of hydrogen. The density of the compound relative to hydrogen is 16. The molecular formula of the compound is :a)NH2b)NH3c)N3Hd)N2H4Correct answer is option 'D'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A gaseous compound of nitrogen and hydrogen contains 12.5%(by mass) of hydrogen. The density of the compound relative to hydrogen is 16. The molecular formula of the compound is :a)NH2b)NH3c)N3Hd)N2H4Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A gaseous compound of nitrogen and hydrogen contains 12.5%(by mass) of hydrogen. The density of the compound relative to hydrogen is 16. The molecular formula of the compound is :a)NH2b)NH3c)N3Hd)N2H4Correct answer is option 'D'. Can you explain this answer?.
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