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We have to determine the mass of one atom of copper in grams.

The **mass of one atom** of an element can be determined using its **average atomic mass and Avogadro’s number (N _{A})**.

The average atomic mass of copper can be looked up in the periodic table.

Cu = 63.55 g/mol

Avogadro’s number (N_{A}) = 6.022x10^{23} particles/mol

The number of atoms in an element can be calculated using this formula:

$\overline{){\#}{}{\mathrm{of}}{}{\mathrm{atoms}}{}{=}{}\frac{\mathrm{mass}\left(\mathrm{m}\right)}{\mathrm{Molar}\mathrm{mass}\left(\mathrm{M}\right)}{\times}{{\mathrm{N}}}_{{\mathrm{A}}}}$

We can rearrange this equation to isolate mass.

$\overline{){\mathrm{mass}}{}\left(\mathrm{m}\right){=}{}\frac{\#\mathrm{of}\mathrm{atoms}\times \mathrm{Molar}\mathrm{mass}\left(\mathrm{M}\right)}{{\mathrm{N}}_{\mathrm{A}}}}$

What is the mass of one atom of copper in grams?

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Based on our data, we think this problem is relevant for Professor Martin's class at NCSU.