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An element crystallizes in a f.c.c. lattice with cell edge of 250 pm. Calculate the density if 300 g of this element contain 2 × 10^24 atoms. - Chemistry

ConceptCalculations Involving Unit Cell Dimensions

Question

An element crystallizes in a f.c.c. lattice with a cell edge of 250 pm. Calculate the density if 300 g of this element contains 2 × 1024 atoms.

Solution

Given:  a = 250 pm = 250 × 10−12 m

z = 4

m =  250 × 10-10 cm 2 × 1024 atom weighs = 300g

m=M/N_A(M" is molar mass")

"molar mass, M ="(300xx6.02xx10^23)/(2xx10^24)=90.3" g/mol"

"Density, "d=(zM)/(a^3N_A)

d=(4xx90.3)/((250)^3xx10^-36xx6.02xx10^23)=38.4" g/cm"^3

Therefore, the density of the given element is 38.4 g/cm3

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Solution An element crystallizes in a f.c.c. lattice with cell edge of 250 pm. Calculate the density if 300 g of this element contain 2 × 10^24 atoms. Concept: Calculations Involving Unit Cell Dimensions.
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