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Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:
- a)8000-10000
- b)10000-10200
- c)10000-10300
- d)10000-10500
Correct answer is option 'C'. Can you explain this answer?
Most Upvoted Answer
Molybdenum crystallizes in a bcc-structure with unit cell dimensions o...
We know that d = (zM) /(Na)*(a³) and
z = 2 for bcc
Substituting for M (96 g/mol), Na (Avogadro number), and a (0.314nm),
We get d = 10298 kg/m³
Hence, option c is correct.
z = 2 for bcc
Substituting for M (96 g/mol), Na (Avogadro number), and a (0.314nm),
We get d = 10298 kg/m³
Hence, option c is correct.
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Molybdenum crystallizes in a bcc-structure with unit cell dimensions o...
Molybdenum Density Calculation
Given:
- Crystal structure of molybdenum: bcc
- Unit cell dimensions: 0.314 nm
- Atomic mass of molybdenum: 96
To find: Density of molybdenum in kg/m3
Solution:
1. Calculate the volume of the unit cell
- Volume of a bcc unit cell = (4 * r/√3)^3
- Here, r = 0.314 nm/2 = 0.157 nm (radius is half of the unit cell dimension)
- Volume of the unit cell = (4 * 0.157 nm/√3)^3
- Volume of the unit cell = 1.787 x 10^-29 m^3
2. Calculate the number of atoms in the unit cell
- There are 2 atoms in a bcc unit cell
- Therefore, number of atoms in the unit cell = 2
3. Calculate the mass of one unit cell
- Mass of one unit cell = number of atoms x atomic mass
- Mass of one unit cell = 2 x 96 g/mol
- Mass of one unit cell = 192 g/mol
4. Convert the mass of one unit cell to kg
- Mass of one unit cell = 192 g/mol x 1 kg/1000 g
- Mass of one unit cell = 0.192 kg
5. Calculate the density of molybdenum
- Density = mass/volume
- Density = 0.192 kg/1.787 x 10^-29 m^3
- Density = 1.075 x 10^4 kg/m3
Answer: The density of molybdenum is in the range of 10000-10300 kg/m3, which is option C.
Given:
- Crystal structure of molybdenum: bcc
- Unit cell dimensions: 0.314 nm
- Atomic mass of molybdenum: 96
To find: Density of molybdenum in kg/m3
Solution:
1. Calculate the volume of the unit cell
- Volume of a bcc unit cell = (4 * r/√3)^3
- Here, r = 0.314 nm/2 = 0.157 nm (radius is half of the unit cell dimension)
- Volume of the unit cell = (4 * 0.157 nm/√3)^3
- Volume of the unit cell = 1.787 x 10^-29 m^3
2. Calculate the number of atoms in the unit cell
- There are 2 atoms in a bcc unit cell
- Therefore, number of atoms in the unit cell = 2
3. Calculate the mass of one unit cell
- Mass of one unit cell = number of atoms x atomic mass
- Mass of one unit cell = 2 x 96 g/mol
- Mass of one unit cell = 192 g/mol
4. Convert the mass of one unit cell to kg
- Mass of one unit cell = 192 g/mol x 1 kg/1000 g
- Mass of one unit cell = 0.192 kg
5. Calculate the density of molybdenum
- Density = mass/volume
- Density = 0.192 kg/1.787 x 10^-29 m^3
- Density = 1.075 x 10^4 kg/m3
Answer: The density of molybdenum is in the range of 10000-10300 kg/m3, which is option C.
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Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:a)8000-10000b)10000-10200c)10000-10300d)10000-10500Correct answer is option 'C'. Can you explain this answer? for Chemistry 2025 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:a)8000-10000b)10000-10200c)10000-10300d)10000-10500Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Chemistry 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:a)8000-10000b)10000-10200c)10000-10300d)10000-10500Correct answer is option 'C'. Can you explain this answer?.
Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:a)8000-10000b)10000-10200c)10000-10300d)10000-10500Correct answer is option 'C'. Can you explain this answer? for Chemistry 2025 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:a)8000-10000b)10000-10200c)10000-10300d)10000-10500Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for Chemistry 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:a)8000-10000b)10000-10200c)10000-10300d)10000-10500Correct answer is option 'C'. Can you explain this answer?.
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Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:a)8000-10000b)10000-10200c)10000-10300d)10000-10500Correct answer is option 'C'. Can you explain this answer?, a detailed solution for Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:a)8000-10000b)10000-10200c)10000-10300d)10000-10500Correct answer is option 'C'. Can you explain this answer? has been provided alongside types of Molybdenum crystallizes in a bcc-structure with unit cell dimensions of 0.314 nm. Considering the atomic mass of molybdenum to be 96, its density (in kg m–3) is in the range of:a)8000-10000b)10000-10200c)10000-10300d)10000-10500Correct answer is option 'C'. Can you explain this answer? theory, EduRev gives you an
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