Calculate the number of unit cells in 0.4 g | vedclass

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Question

(C) The mass of the metal is given as $m = 0.4 \ g$. The product of density $(ho)$ and volume of the unit cell $(V = a^3)$ is given as $ho 	imes

Vedclass · Accepted Answer

$3.3 	imes 10^{21}$

Vedclass · Answer

(C) The mass of the metal is given as $m = 0.4 \ g$. The product of density $(ho)$ and volume of the unit cell $(V = a^3)$ is given as $ho 	imes a^3 = 1.2 	imes 10^{-22} \ g$. The number of unit cells is calculated by dividing the total mass of the metal by the mass of one unit cell. $	ext{Number of unit cells} = \frac{	ext{Total mass}}{	ext{Mass of one unit cell}} = \frac{m}{ho 	imes a^3}$. Substituting the values: $\frac{0.4 \ g}{1.2 	imes 10^{-22} \ g} = 3.33 	imes 10^{21}$. Therefore,the number of unit cells is $3.3 	imes 10^{21}$.

Calculate the number of unit cells in $0.4 \ g$ of metal if the product of density and volume of the unit cell is $1.2 \times 10^{-22} \ g$.

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