Phosphorus crystallizes in several different forms, one of which is a simple cube with an edge length of 238 pm. What is the density of phosphorus in the simple cubic crystal fo…

Question

asked Jan 11, 2021 219k views

1 Answer

Gianluca Paris · Answer 1 · 2021-01-15T17:57:00+0000

Answer: The density of phosphorus is

Step-by-step explanation:

To calculate the density of phosphorus, we use the equation:

$\rho=(Z* M)/(N_(A)* a^(3))$

where,

$\rho$ = density

Z = number of atom in unit cell = 1 (CCP)

M = atomic mass of phosphorus = 31 g/mol

N_(A) = Avogadro's number =
6.022* 10^(23)

a = edge length of unit cell =
238pm=238* 10^(-10)cm (Conversion factor:
)

Putting values in above equation, we get:

$\rho=(1* 31)/(6.022* 10^(23)* (238* 10^(-10))^3)\\\\\rho=3.81g/cm^3$

Hence, the density of phosphorus is