When silver crystallizes, it forms face centered cubic cells, if the volume of unit cells 6.84 × 1 0 − 23 cm 3 . Calculate the density of silver. (Molar mass of silver is 108 g/mol, N A = 6.022 × 1

Question

When silver crystallizes, it forms face centered cubic cells, if the volume of unit cells 6.84 × 1 0 − 23 cm 3 . Calculate the density of silver. (Molar mass of silver is 108 g/mol, N A ​ = 6.022 × 1 0 23 )

TestHub · Accepted Answer

For a face-centered cubic (fcc) unit cell, the number of atoms per unit cell is $Z = 4$ .

The density of the unit cell is given by the formula:

$d = \frac{Z \times M}{N _{A} \times V}$

Substituting the given values:

$d = \frac{4 \times 108}{6.022 \times 1 0 ^{23} \times 6.84 \times 1 0 ^{- 23}}$

$d = \frac{432}{41.19}$

$d = 10.49 gm cm^{- 3}$

Answer: $10.49 gm cm^{- 3}$

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