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0.0833 mole of a carbohydrate of empirical formula CH2O contains 1.00 g of hydrogen. The molecular formula of the carbohydrate is
- a)C5H10O5
- b)C3H4O3
- c)C12H22O11
- d)C6H12O6
Correct answer is option 'D'. Can you explain this answer?
Most Upvoted Answer
0.0833 mole of a carbohydrate of empirical formula CH2O contains 1.00 ...
- Empirical formula = CH2O.
- Empirical formula weight = 12 + 2×1 + 16 = 30 g/mol.
- Let the molecular formula be (CH2O)n = CnH2nOn.
- Moles of carbohydrate = 0.0833 mol.
- Mass of hydrogen in 0.0833 mol = 1.00 g.
- Molecular formula = CnH2nOn, so 2n hydrogen atoms per molecule.
- Atomic mass of hydrogen = 1 g/mol, so mass of hydrogen in 1 mole of carbohydrate = 2n g.
- For 0.0833 moles, mass of hydrogen = 0.0833 × 2n = 1.00 g.
- Solving: 2n × 0.0833 = 1.00
n = 1.00 / (2 × 0.0833) ≈ 6. - Molecular formula = C6H12O6.
Verification:
- Molecular weight of C6H12O6 = 6×12 + 12×1 + 6×16 = 180 g/mol.
- Hydrogen mass in 1 mole = 12 g.
- In 0.0833 moles, hydrogen mass = 12 × 0.0833 ≈ 1.00 g, which matches.
Thus, the correct answer is D. C6H12O6.
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Community Answer
0.0833 mole of a carbohydrate of empirical formula CH2O contains 1.00 ...
Understanding the Problem
To determine the molecular formula of the carbohydrate, we start with the information given:
- Empirical formula: CH2O
- Moles of carbohydrate: 0.0833 moles
- Mass of hydrogen: 1.00 g
Calculating Moles of Hydrogen
- The empirical formula CH2O contains 2 moles of H per mole of the compound.
- Therefore, in 0.0833 moles of CH2O, the moles of hydrogen can be calculated as follows:
- Moles of H = 0.0833 moles CH2O * 2 moles H/1 mole CH2O = 0.1666 moles H
Converting Moles of Hydrogen to Grams
- To find the mass of hydrogen:
- Mass of H = moles of H * molar mass of H (1 g/mol)
- Mass of H = 0.1666 moles * 1 g/mol = 0.1666 g of H
This indicates a discrepancy as we need to consider that the given mass of hydrogen is 1.00 g.
Finding the Molecular Formula
- To find the molecular formula, we must determine the molar mass of the entire carbohydrate.
- The mass of hydrogen (1.00 g) suggests that the actual number of moles of H in the molecular formula is higher.
Molecular Formula Calculation
- Since there are 1.00 g of hydrogen, the moles of H in the molecular formula is 1.00 g / 1 g/mol = 1.00 mole of H.
- The ratio of moles (1.00 mole of H) to empirical formula (0.1666 moles) is approximately 6.
- Therefore, the molecular formula is (C1H2O1) * 6 = C6H12O6.
Conclusion
Thus, the molecular formula of the carbohydrate is C6H12O6, which corresponds to option 'D'.
To determine the molecular formula of the carbohydrate, we start with the information given:
- Empirical formula: CH2O
- Moles of carbohydrate: 0.0833 moles
- Mass of hydrogen: 1.00 g
Calculating Moles of Hydrogen
- The empirical formula CH2O contains 2 moles of H per mole of the compound.
- Therefore, in 0.0833 moles of CH2O, the moles of hydrogen can be calculated as follows:
- Moles of H = 0.0833 moles CH2O * 2 moles H/1 mole CH2O = 0.1666 moles H
Converting Moles of Hydrogen to Grams
- To find the mass of hydrogen:
- Mass of H = moles of H * molar mass of H (1 g/mol)
- Mass of H = 0.1666 moles * 1 g/mol = 0.1666 g of H
This indicates a discrepancy as we need to consider that the given mass of hydrogen is 1.00 g.
Finding the Molecular Formula
- To find the molecular formula, we must determine the molar mass of the entire carbohydrate.
- The mass of hydrogen (1.00 g) suggests that the actual number of moles of H in the molecular formula is higher.
Molecular Formula Calculation
- Since there are 1.00 g of hydrogen, the moles of H in the molecular formula is 1.00 g / 1 g/mol = 1.00 mole of H.
- The ratio of moles (1.00 mole of H) to empirical formula (0.1666 moles) is approximately 6.
- Therefore, the molecular formula is (C1H2O1) * 6 = C6H12O6.
Conclusion
Thus, the molecular formula of the carbohydrate is C6H12O6, which corresponds to option 'D'.
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0.0833 mole of a carbohydrate of empirical formula CH2O contains 1.00 g of hydrogen. The molecular formula of the carbohydrate isa)C5H10O5b)C3H4O3c)C12H22O11d)C6H12O6Correct answer is option 'D'. Can you explain this answer? for NEET 2026 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 0.0833 mole of a carbohydrate of empirical formula CH2O contains 1.00 g of hydrogen. The molecular formula of the carbohydrate isa)C5H10O5b)C3H4O3c)C12H22O11d)C6H12O6Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for NEET 2026 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 0.0833 mole of a carbohydrate of empirical formula CH2O contains 1.00 g of hydrogen. The molecular formula of the carbohydrate isa)C5H10O5b)C3H4O3c)C12H22O11d)C6H12O6Correct answer is option 'D'. Can you explain this answer?.
0.0833 mole of a carbohydrate of empirical formula CH2O contains 1.00 g of hydrogen. The molecular formula of the carbohydrate isa)C5H10O5b)C3H4O3c)C12H22O11d)C6H12O6Correct answer is option 'D'. Can you explain this answer? for NEET 2026 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 0.0833 mole of a carbohydrate of empirical formula CH2O contains 1.00 g of hydrogen. The molecular formula of the carbohydrate isa)C5H10O5b)C3H4O3c)C12H22O11d)C6H12O6Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for NEET 2026 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 0.0833 mole of a carbohydrate of empirical formula CH2O contains 1.00 g of hydrogen. The molecular formula of the carbohydrate isa)C5H10O5b)C3H4O3c)C12H22O11d)C6H12O6Correct answer is option 'D'. Can you explain this answer?.
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