We’re asked to **determine how many atoms are present in a cube of silver** metal that **measures 1.050 cm on each edge **given its density.

**We can calculate the # of Ag (silver) atoms using the following steps:**

**Step 1: **Determine the** volume of the silver cube**. Recall that the * volume of a cube* is given by the equation:

$\overline{){\mathbf{Volume}}{\mathbf{=}}{{\mathbf{l}}}^{{\mathbf{3}}}}$

*l = length of edge of a cube*

**Step 2: **Determine the** mass of the silver cube** from the given density from the equation:

$\overline{){\mathbf{density}}{\mathbf{=}}\frac{\mathbf{mass}}{\mathbf{volume}}}\phantom{\rule{0ex}{0ex}}$

This means that: **Mass = density x volume**

**Step 3**: Determine atoms Ag. The flow of the solution will be like this:

** mass Ag (molar mass Ag) ** → moles Ag

You are given a cube of silver metal that measures 1.050 cm on each edge. The density of silver is 10.5 g/cm^{3}.

How many atoms are in this cube?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Mole Concept concept. You can view video lessons to learn Mole Concept. Or if you need more Mole Concept practice, you can also practice Mole Concept practice problems.