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Choose the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively and its molecular mass is 160.
- a)FeO
- b)Fe3O4
- c)Fe2O3
- d)FeO2
Correct answer is option 'C'. Can you explain this answer?
Most Upvoted Answer
Choose the molecular formula of an oxide of iron in which the mass per...
For element Fe, mole of atoms = 69.9/56 = 1.25
For element O, Mole of atoms = 30.1/16 = 1.88
Mole ratio of Fe = 1.25/1.25 = 1
Mole ratio of O = 1.88/1.25 = 1.5
Simplest whole number ratio of Fe and O = 2, 3
Empirical formula of compoimd = Fe2O3
Molecular mass of Fe2O3 = 160
Molecular formula = Fe2O3
For element O, Mole of atoms = 30.1/16 = 1.88
Mole ratio of Fe = 1.25/1.25 = 1
Mole ratio of O = 1.88/1.25 = 1.5
Simplest whole number ratio of Fe and O = 2, 3
Empirical formula of compoimd = Fe2O3
Molecular mass of Fe2O3 = 160
Molecular formula = Fe2O3
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Choose the molecular formula of an oxide of iron in which the mass per...
To determine the molecular formula of the oxide of iron, we need to consider the given information about the mass percent of iron and oxygen, as well as the molecular mass.
Given:
Mass percent of iron (Fe) = 69.9%
Mass percent of oxygen (O) = 30.1%
Molecular mass = 160
To find the molecular formula, we need to determine the ratio of iron to oxygen atoms in the compound.
Let's assume the compound has x moles of iron and y moles of oxygen.
1. Calculating the mass of iron and oxygen:
The mass of iron can be calculated using the mass percent:
Mass of iron = (Mass percent of iron / 100) * Total mass of the compound
= (69.9 / 100) * 160
= 111.84 g
Similarly, the mass of oxygen can be calculated:
Mass of oxygen = (Mass percent of oxygen / 100) * Total mass of the compound
= (30.1 / 100) * 160
= 48.16 g
2. Determining the moles of iron and oxygen:
Moles of iron = Mass of iron / Atomic mass of iron
= 111.84 g / 55.85 g/mol (atomic mass of Fe)
≈ 2 moles
Moles of oxygen = Mass of oxygen / Atomic mass of oxygen
= 48.16 g / 16 g/mol (atomic mass of O)
≈ 3 moles
3. Simplifying the ratio of iron to oxygen atoms:
To simplify the ratio, we divide the number of moles by the smallest value, which is 2 in this case.
Moles of iron (Fe) = 2 / 2 = 1
Moles of oxygen (O) = 3 / 2 ≈ 1.5
Since we need whole numbers for the ratio of atoms, we multiply both moles by 2 to get a whole number:
Moles of iron (Fe) = 1 * 2 = 2
Moles of oxygen (O) = 1.5 * 2 = 3
Therefore, the molecular formula of the oxide of iron is Fe2O3, which corresponds to option C.
Given:
Mass percent of iron (Fe) = 69.9%
Mass percent of oxygen (O) = 30.1%
Molecular mass = 160
To find the molecular formula, we need to determine the ratio of iron to oxygen atoms in the compound.
Let's assume the compound has x moles of iron and y moles of oxygen.
1. Calculating the mass of iron and oxygen:
The mass of iron can be calculated using the mass percent:
Mass of iron = (Mass percent of iron / 100) * Total mass of the compound
= (69.9 / 100) * 160
= 111.84 g
Similarly, the mass of oxygen can be calculated:
Mass of oxygen = (Mass percent of oxygen / 100) * Total mass of the compound
= (30.1 / 100) * 160
= 48.16 g
2. Determining the moles of iron and oxygen:
Moles of iron = Mass of iron / Atomic mass of iron
= 111.84 g / 55.85 g/mol (atomic mass of Fe)
≈ 2 moles
Moles of oxygen = Mass of oxygen / Atomic mass of oxygen
= 48.16 g / 16 g/mol (atomic mass of O)
≈ 3 moles
3. Simplifying the ratio of iron to oxygen atoms:
To simplify the ratio, we divide the number of moles by the smallest value, which is 2 in this case.
Moles of iron (Fe) = 2 / 2 = 1
Moles of oxygen (O) = 3 / 2 ≈ 1.5
Since we need whole numbers for the ratio of atoms, we multiply both moles by 2 to get a whole number:
Moles of iron (Fe) = 1 * 2 = 2
Moles of oxygen (O) = 1.5 * 2 = 3
Therefore, the molecular formula of the oxide of iron is Fe2O3, which corresponds to option C.
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Choose the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively and its molecular mass is 160.a)FeOb)Fe3O4c)Fe2O3d)FeO2Correct answer is option 'C'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Choose the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively and its molecular mass is 160.a)FeOb)Fe3O4c)Fe2O3d)FeO2Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Choose the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively and its molecular mass is 160.a)FeOb)Fe3O4c)Fe2O3d)FeO2Correct answer is option 'C'. Can you explain this answer?.
Choose the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively and its molecular mass is 160.a)FeOb)Fe3O4c)Fe2O3d)FeO2Correct answer is option 'C'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Choose the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively and its molecular mass is 160.a)FeOb)Fe3O4c)Fe2O3d)FeO2Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Choose the molecular formula of an oxide of iron in which the mass per cent of iron and oxygen are 69.9 and 30.1 respectively and its molecular mass is 160.a)FeOb)Fe3O4c)Fe2O3d)FeO2Correct answer is option 'C'. Can you explain this answer?.
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