Question

When gold crystallizes it forms face centered cubic cell. The unit cell edge length is 408 pm. Calculate

the density of gold. Molar mass of gold is 197 g/mol.​

Answer 1

Answer:

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Explanation:

atoms are in contact along the diagonal of the unit cell.

4r= sqrt 2 a, where a is the edge length of unit cell and r is the radius of atom. Substituting values in the above

expression, we get √2 × 407 4 r = = 143.9 pm Number of atoms per unit cell (FCC) = 4 Volume of 1 unit cell = (407 × 10−¹2)³ m³ = 6.741 * 10 ^ - 29 * m ^ 3 = 2.824 * 10 ^ - 28 * m ^ 3

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Mass of 1 unit cell 197 x 4788 amu = -24 ¹kg

1.66 × 10-27 × 788 kg = 1.30808 × 10

Density 1.30808 x 10-24 6.741 × 10-29 19404.83 kg/m³ = 19.4 g/cm³