$X -$ ray diffraction studies show that copper crystallises in an $F C C$ unit cell with cell edge of $3.608 ˚ A$ . In a separate experiment, copper is determined to have a density of $8.92 g / c m^{3}$ , calculate the atomic (molar) mass of the copper.

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Solution

In $F C C$ Lattice, number of atoms/unit cell $= 4$
$∴$ $M = \frac{d N_{A} a^{3}}{Z} = \frac{8.92 \times 6.023 \times 10^{23} \times {(3.608 \times 10^{- 8})}^{3}}{4}$
$∴$ Atomic mass of $C u = 63.1$ g/mol

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X-ray diffraction studies show that copper crystallizes in an fcc unit cell with cell edge of 3.608 × 10^-8 cm. In a separate experiment, copper is determined to have a density of 8.92 g/cm³, calculate the atomic mass of copper.

Q. Copper crystallises into a fcc structure and the unit cell has length of edge

3.61 \times 10^{- 8} c m

calculate the density of copper if the molar mass of Cu is

63.5 g m o l^{- 1}

Q. Copper crystallises in fcc lattice with a unit cell edge of 361 pm. The radius of the copper atom is :

Copper crystallises into a fcc lattice with edge length 3.61 × 10⁻⁸ cm. Show that the calculated density is in agreement with its measured value of 8.92 g cm⁻³.

Q. Copper crystallises as an FCC unit cell. If the atomic radius of copper is

1.28 ˚ A

, then what is the edge length (in

˚ A

) of the unit cell?

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X−ray diffraction studies show that copper crystallises in an FCC unit cell with cell edge of 3.608 ˚A. In a separate experiment, copper is determined to have a density of 8.92 g/cm3, calculate the atomic (molar) mass of the copper.

In FCC Lattice, number of atoms/unit cell =4∴ M=dNAa3Z=8.92×6.023×1023×(3.608×10−8)34∴ Atomic mass of Cu=63.1 g/mol

$X -$ ray diffraction studies show that copper crystallises in an $F C C$ unit cell with cell edge of $3.608 ˚ A$ . In a separate experiment, copper is determined to have a density of $8.92 g / c m^{3}$ , calculate the atomic (molar) mass of the copper.

In $F C C$ Lattice, number of atoms/unit cell $= 4$
$∴$ $M = \frac{d N_{A} a^{3}}{Z} = \frac{8.92 \times 6.023 \times 10^{23} \times {(3.608 \times 10^{- 8})}^{3}}{4}$
$∴$ Atomic mass of $C u = 63.1$ g/mol