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15. If the density of copper is $8.96 \mathrm{~g} / \mathrm{cm}^{3}$, how many copper atoms are in a copper cube that has a volume of $10 \mathrm{~cm}^{3}$ ?
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Answer from Sia

Posted 6 months ago

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Answer

The number of copper atoms in the cube is calculated to be approximately $8.96 \times 10^{23}$ atoms.

Key Concept

Calculating the number of atoms in a sample involves finding the mass, converting it to moles, and then using Avogadro's number.

Explanation

The mass of the copper cube is found using its density and volume. This mass is then converted to moles using the molar mass of copper. Finally, the number of atoms is found by multiplying the number of moles by Avogadro's number.

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