Calculations Involving Unit Cell Dimensions
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NEET DIGITAL LIBRARY
CHXII01:THE SOLID STATE

318671 Aluminium has fcc structure. The length of the unit cell is \({\rm{404}}\,{\rm{pm}}\). If the density of the metal is \(2.7 \mathrm{~g} \mathrm{~cm}^{-3}\), the molar mass of \(\mathrm{Al}\) atom is

1 \(28 \mathrm{~g} \mathrm{~mol}^{-1}\)
2 \(30 \mathrm{~g} \mathrm{~mol}^{-1}\)
3 \(26.80 \mathrm{~g} \mathrm{~mol}^{-1}\)
4 \(25 \mathrm{~g} \mathrm{~mol}^{-1}\)
CHXII01:THE SOLID STATE

318672 An element has a bcc structure with cell edge of \(288 \mathrm{pm}\). The density of element is \(7.2 \mathrm{~g} \mathrm{~cm}^{-3}\). What is the atomic mass of an element?

1 25.89
2 51.78
3 77.68
4 62.43
MHTCET - 2020
CHXII01:THE SOLID STATE

318673 A metallic element crystallises in simple cubic lattice. If edge length of the unit cell is \({\rm{3}}\mathop {\rm{A}}\limits^{\rm{^\circ }} \), with density \(8 \mathrm{~g} / \mathrm{cc}\). What is the number of unit cells in \(100 \mathrm{~g}\) of the metal?
\((\) Molar mass of metal \(=108 \mathrm{~g} / \mathrm{mol})\)

1 \(1.33 \times 10^{20}\)
2 \(2.7 \times 10^{22}\)
3 \(2 \times 10^{24}\)
4 \(5 \times 10^{23}\)
MHTCET - 2020
CHXII01:THE SOLID STATE

318674 The atomic radius of atom is r. Total volume of atoms present in a fcc unit cell of an element is

1 \(\dfrac{24}{3} \pi r^{3}\)
2 \(\dfrac{12}{3} \pi \mathrm{r}^{3}\)
3 \(\dfrac{16}{3} \pi \mathrm{r}^{3}\)
4 None
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CHXII01:THE SOLID STATE

318671 Aluminium has fcc structure. The length of the unit cell is \({\rm{404}}\,{\rm{pm}}\). If the density of the metal is \(2.7 \mathrm{~g} \mathrm{~cm}^{-3}\), the molar mass of \(\mathrm{Al}\) atom is

1 \(28 \mathrm{~g} \mathrm{~mol}^{-1}\)
2 \(30 \mathrm{~g} \mathrm{~mol}^{-1}\)
3 \(26.80 \mathrm{~g} \mathrm{~mol}^{-1}\)
4 \(25 \mathrm{~g} \mathrm{~mol}^{-1}\)
CHXII01:THE SOLID STATE

318672 An element has a bcc structure with cell edge of \(288 \mathrm{pm}\). The density of element is \(7.2 \mathrm{~g} \mathrm{~cm}^{-3}\). What is the atomic mass of an element?

1 25.89
2 51.78
3 77.68
4 62.43
MHTCET - 2020
CHXII01:THE SOLID STATE

318673 A metallic element crystallises in simple cubic lattice. If edge length of the unit cell is \({\rm{3}}\mathop {\rm{A}}\limits^{\rm{^\circ }} \), with density \(8 \mathrm{~g} / \mathrm{cc}\). What is the number of unit cells in \(100 \mathrm{~g}\) of the metal?
\((\) Molar mass of metal \(=108 \mathrm{~g} / \mathrm{mol})\)

1 \(1.33 \times 10^{20}\)
2 \(2.7 \times 10^{22}\)
3 \(2 \times 10^{24}\)
4 \(5 \times 10^{23}\)
MHTCET - 2020
CHXII01:THE SOLID STATE

318674 The atomic radius of atom is r. Total volume of atoms present in a fcc unit cell of an element is

1 \(\dfrac{24}{3} \pi r^{3}\)
2 \(\dfrac{12}{3} \pi \mathrm{r}^{3}\)
3 \(\dfrac{16}{3} \pi \mathrm{r}^{3}\)
4 None
For More Updates join with Us
CHXII01:THE SOLID STATE

318671 Aluminium has fcc structure. The length of the unit cell is \({\rm{404}}\,{\rm{pm}}\). If the density of the metal is \(2.7 \mathrm{~g} \mathrm{~cm}^{-3}\), the molar mass of \(\mathrm{Al}\) atom is

1 \(28 \mathrm{~g} \mathrm{~mol}^{-1}\)
2 \(30 \mathrm{~g} \mathrm{~mol}^{-1}\)
3 \(26.80 \mathrm{~g} \mathrm{~mol}^{-1}\)
4 \(25 \mathrm{~g} \mathrm{~mol}^{-1}\)
CHXII01:THE SOLID STATE

318672 An element has a bcc structure with cell edge of \(288 \mathrm{pm}\). The density of element is \(7.2 \mathrm{~g} \mathrm{~cm}^{-3}\). What is the atomic mass of an element?

1 25.89
2 51.78
3 77.68
4 62.43
MHTCET - 2020
CHXII01:THE SOLID STATE

318673 A metallic element crystallises in simple cubic lattice. If edge length of the unit cell is \({\rm{3}}\mathop {\rm{A}}\limits^{\rm{^\circ }} \), with density \(8 \mathrm{~g} / \mathrm{cc}\). What is the number of unit cells in \(100 \mathrm{~g}\) of the metal?
\((\) Molar mass of metal \(=108 \mathrm{~g} / \mathrm{mol})\)

1 \(1.33 \times 10^{20}\)
2 \(2.7 \times 10^{22}\)
3 \(2 \times 10^{24}\)
4 \(5 \times 10^{23}\)
MHTCET - 2020
CHXII01:THE SOLID STATE

318674 The atomic radius of atom is r. Total volume of atoms present in a fcc unit cell of an element is

1 \(\dfrac{24}{3} \pi r^{3}\)
2 \(\dfrac{12}{3} \pi \mathrm{r}^{3}\)
3 \(\dfrac{16}{3} \pi \mathrm{r}^{3}\)
4 None
NEET DIGITAL LIBRARY
CHXII01:THE SOLID STATE

318671 Aluminium has fcc structure. The length of the unit cell is \({\rm{404}}\,{\rm{pm}}\). If the density of the metal is \(2.7 \mathrm{~g} \mathrm{~cm}^{-3}\), the molar mass of \(\mathrm{Al}\) atom is

1 \(28 \mathrm{~g} \mathrm{~mol}^{-1}\)
2 \(30 \mathrm{~g} \mathrm{~mol}^{-1}\)
3 \(26.80 \mathrm{~g} \mathrm{~mol}^{-1}\)
4 \(25 \mathrm{~g} \mathrm{~mol}^{-1}\)
CHXII01:THE SOLID STATE

318672 An element has a bcc structure with cell edge of \(288 \mathrm{pm}\). The density of element is \(7.2 \mathrm{~g} \mathrm{~cm}^{-3}\). What is the atomic mass of an element?

1 25.89
2 51.78
3 77.68
4 62.43
MHTCET - 2020
CHXII01:THE SOLID STATE

318673 A metallic element crystallises in simple cubic lattice. If edge length of the unit cell is \({\rm{3}}\mathop {\rm{A}}\limits^{\rm{^\circ }} \), with density \(8 \mathrm{~g} / \mathrm{cc}\). What is the number of unit cells in \(100 \mathrm{~g}\) of the metal?
\((\) Molar mass of metal \(=108 \mathrm{~g} / \mathrm{mol})\)

1 \(1.33 \times 10^{20}\)
2 \(2.7 \times 10^{22}\)
3 \(2 \times 10^{24}\)
4 \(5 \times 10^{23}\)
MHTCET - 2020
CHXII01:THE SOLID STATE

318674 The atomic radius of atom is r. Total volume of atoms present in a fcc unit cell of an element is

1 \(\dfrac{24}{3} \pi r^{3}\)
2 \(\dfrac{12}{3} \pi \mathrm{r}^{3}\)
3 \(\dfrac{16}{3} \pi \mathrm{r}^{3}\)
4 None
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