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An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound is
- a)C4H8N4
- b)C2H4N2
- c)C12H24N12
- d)C16H32N16
Correct answer is option 'A'. Can you explain this answer?
Most Upvoted Answer
An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm...
Given:
- Mass of carbon (C) = 48 gm
- Mass of hydrogen (H) = 8 gm
- Mass of nitrogen (N) = 56 gm
- Volume of 1.0 g of the compound = 200 ml at NTP
To Find:
- Molecular formula of the compound
Solution:
Step 1: Calculate the moles of each element:
- Moles of carbon (C) = Mass of carbon (C) / Molar mass of carbon (C)
- Moles of hydrogen (H) = Mass of hydrogen (H) / Molar mass of hydrogen (H)
- Moles of nitrogen (N) = Mass of nitrogen (N) / Molar mass of nitrogen (N)
The molar mass of carbon (C) is 12 g/mol, the molar mass of hydrogen (H) is 1 g/mol, and the molar mass of nitrogen (N) is 14 g/mol.
Moles of carbon (C) = 48 gm / 12 g/mol = 4 mol
Moles of hydrogen (H) = 8 gm / 1 g/mol = 8 mol
Moles of nitrogen (N) = 56 gm / 14 g/mol = 4 mol
Step 2: Find the empirical formula of the compound:
The empirical formula represents the simplest whole number ratio of the atoms present in a compound.
The empirical formula can be determined by dividing the moles of each element by the smallest number of moles.
Since the smallest number of moles is 4, we divide the moles of each element by 4.
Empirical formula: C1H2N1
Step 3: Calculate the molar mass of the empirical formula:
Molar mass of the empirical formula = (Molar mass of carbon (C) × Number of carbon atoms) + (Molar mass of hydrogen (H) × Number of hydrogen atoms) + (Molar mass of nitrogen (N) × Number of nitrogen atoms)
Molar mass of the empirical formula = (12 g/mol × 1) + (1 g/mol × 2) + (14 g/mol × 1) = 12 g/mol + 2 g/mol + 14 g/mol = 28 g/mol
Step 4: Calculate the number of empirical formula units in 1.0 g:
Number of empirical formula units = Mass of the compound / Molar mass of the empirical formula
Number of empirical formula units = 1.0 g / 28 g/mol = 0.0357 mol
Step 5: Determine the molecular formula:
The molecular formula represents the actual number of atoms of each element in a compound.
The molecular formula can be determined by multiplying the empirical formula by a whole number (n).
Molecular formula = Empirical formula × n
To find the value of 'n', we divide the number of empirical formula units (0.0357 mol) by the number of moles of the empirical formula (0.0357 mol).
n = Number of empirical formula units / Number of moles of the empirical formula
n = 0.0357 mol / 0.0357 mol = 1
Therefore, the molecular formula is the same
- Mass of carbon (C) = 48 gm
- Mass of hydrogen (H) = 8 gm
- Mass of nitrogen (N) = 56 gm
- Volume of 1.0 g of the compound = 200 ml at NTP
To Find:
- Molecular formula of the compound
Solution:
Step 1: Calculate the moles of each element:
- Moles of carbon (C) = Mass of carbon (C) / Molar mass of carbon (C)
- Moles of hydrogen (H) = Mass of hydrogen (H) / Molar mass of hydrogen (H)
- Moles of nitrogen (N) = Mass of nitrogen (N) / Molar mass of nitrogen (N)
The molar mass of carbon (C) is 12 g/mol, the molar mass of hydrogen (H) is 1 g/mol, and the molar mass of nitrogen (N) is 14 g/mol.
Moles of carbon (C) = 48 gm / 12 g/mol = 4 mol
Moles of hydrogen (H) = 8 gm / 1 g/mol = 8 mol
Moles of nitrogen (N) = 56 gm / 14 g/mol = 4 mol
Step 2: Find the empirical formula of the compound:
The empirical formula represents the simplest whole number ratio of the atoms present in a compound.
The empirical formula can be determined by dividing the moles of each element by the smallest number of moles.
Since the smallest number of moles is 4, we divide the moles of each element by 4.
Empirical formula: C1H2N1
Step 3: Calculate the molar mass of the empirical formula:
Molar mass of the empirical formula = (Molar mass of carbon (C) × Number of carbon atoms) + (Molar mass of hydrogen (H) × Number of hydrogen atoms) + (Molar mass of nitrogen (N) × Number of nitrogen atoms)
Molar mass of the empirical formula = (12 g/mol × 1) + (1 g/mol × 2) + (14 g/mol × 1) = 12 g/mol + 2 g/mol + 14 g/mol = 28 g/mol
Step 4: Calculate the number of empirical formula units in 1.0 g:
Number of empirical formula units = Mass of the compound / Molar mass of the empirical formula
Number of empirical formula units = 1.0 g / 28 g/mol = 0.0357 mol
Step 5: Determine the molecular formula:
The molecular formula represents the actual number of atoms of each element in a compound.
The molecular formula can be determined by multiplying the empirical formula by a whole number (n).
Molecular formula = Empirical formula × n
To find the value of 'n', we divide the number of empirical formula units (0.0357 mol) by the number of moles of the empirical formula (0.0357 mol).
n = Number of empirical formula units / Number of moles of the empirical formula
n = 0.0357 mol / 0.0357 mol = 1
Therefore, the molecular formula is the same
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An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound isa)C4H8N4b)C2H4N2c)C12H24N12d)C16H32N16Correct answer is option 'A'. Can you explain this answer?
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An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound isa)C4H8N4b)C2H4N2c)C12H24N12d)C16H32N16Correct answer is option 'A'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound isa)C4H8N4b)C2H4N2c)C12H24N12d)C16H32N16Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound isa)C4H8N4b)C2H4N2c)C12H24N12d)C16H32N16Correct answer is option 'A'. Can you explain this answer?.
An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound isa)C4H8N4b)C2H4N2c)C12H24N12d)C16H32N16Correct answer is option 'A'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound isa)C4H8N4b)C2H4N2c)C12H24N12d)C16H32N16Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound isa)C4H8N4b)C2H4N2c)C12H24N12d)C16H32N16Correct answer is option 'A'. Can you explain this answer?.
Solutions for An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound isa)C4H8N4b)C2H4N2c)C12H24N12d)C16H32N16Correct answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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ample number of questions to practice An organic compound on analysis gave C = 48 gm, H = 8 gm and N = 56 gm. Volume of 1.0 g of the compound was found to be 200 ml at NTP. Molecular formula of the compound isa)C4H8N4b)C2H4N2c)C12H24N12d)C16H32N16Correct answer is option 'A'. Can you explain this answer? tests, examples and also practice JEE tests.
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