At 100, ^circ C,copper (Cu) has FCC unit cell | vedclass

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(D) The density $(d)$ of a unit cell is given by the formula: $d = \frac{Z 	imes M}{N_A 	imes a^3}$For an $FCC$ unit cell,the number of atoms per un

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$\frac{422}{x^3}$

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(D) The density $(d)$ of a unit cell is given by the formula: $d = \frac{Z 	imes M}{N_A 	imes a^3}$For an $FCC$ unit cell,the number of atoms per unit cell $(Z) = 4$.The atomic mass of $Cu$ $(M) = 63.55\, g\, mol^{-1}$.The Avogadro constant $(N_A) = 6.023 	imes 10^{23}\, mol^{-1}$.The edge length $(a) = x\, \mathring{A} = x 	imes 10^{-8}\, cm$.Substituting these values into the formula:$d = \frac{4 	imes 63.55}{(6.023 	imes 10^{23}) 	imes (x 	imes 10^{-8})^3}$$d = \frac{254.2}{6.023 	imes 10^{23} 	imes x^3 	imes 10^{-24}}$$d = \frac{254.2}{0.6023 	imes x^3} \approx \frac{422}{x^3}\, g\, cm^{-3}$

At $100\, ^\circ C$,copper $(Cu)$ has $FCC$ unit cell structure with cell edge length $x\, \mathring{A}$. What is the approximate density of $Cu$ (in $g\, cm^{-3}$) at this temperature? [Atomic mass of $Cu = 63.55\, u$]

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