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Iron has body centred cubic cell with a ...

Iron has body centred cubic cell with a cell edge of 286.5 pm. The density of iron is 7.87 g `cm^(-3)`. Use this information to calculate Avogadro's number. (Atomic mass of Fe = 56 `mol^(-3)`)

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For bcc arrangment, `Z = 2 , rho = 7.87 g cm^(-3) `
`M = 56 g mol^(-1)`
Edge length , `a = 286.65 xx 10^(-12) m = 286.65 xx 10^(-10) cm`
`rho = (Z xx M)/(a^3 xx N_A)`
or `N_A = (Z xx M)/(rho^3 xx a^3)`
`= (2 xx (56 g mol^(-1)))/((7.87 g cm^(-3)) xx (286.65 xx 10^(-10) cm)^3)`
`= 6.04 xx 10^23 mol^(-1)`.
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