An element has hcp packing with a hexagonal unit cell. Its density is 21000 kg/m3 and the unit cell volume is 2.94 x 10-23 mL. Calculate the molar mass (g/mol) of the element to three significant figures.

The same principles apply from your earlier post.

12.0

To calculate the molar mass of the element, we need to use the formula:

Molar Mass = (Density * Unit Cell Volume) / Avogadro's Number

First, let's convert the unit cell volume from mL to cubic meters:
2.94 x 10^(-23) mL = 2.94 x 10^(-26) m^3

Now, we can substitute the values into the formula:

Molar Mass = (21000 kg/m^3 * 2.94 x 10^(-26) m^3) / 6.022 x 10^23 mol^(-1)

Molar Mass = (21000 * 2.94 x 10^(-26)) / 6.022 x 10^23

Molar Mass ≈ 1.03 x 10^(-3) g/mol

Rounding to three significant figures, the molar mass of the element is approximately 1.03 x 10^(-3) g/mol.