Question

How many grams are equal to 1.73 x 10^28 atoms of Sulfur?

Answer 1

Main Answer:

The
`\(1.73 * 10^(28)\)` atoms of sulfur is equivalent to approximately 2.86 grams.

Explanation:

To calculate the mass of sulfur in grams corresponding to
`\(1.73 * 10^(28)\)` atoms, we use the molar mass of sulfur. The molar mass of sulfur is approximately 32.07 grams/mol. Avogadro's number tells us that one mole of any substance contains
`\(6.022 * 10^(23)\)` atoms. Therefore, the number of moles
`(\(n\))` can be calculated as follows:

`\[ n = \frac{\text{Number of atoms}}{\text{Avogadro's number}} = (1.73 * 10^(28))/(6.022 * 10^(23)) \]`

Once we have the number of moles, we can find the mass (\(m\)) using the molar mass (\(M\)):

`\[ m = n * M = \left((1.73 * 10^(28))/(6.022 * 10^(23))\right) * 32.07 \, \text{grams/mol} \]`

After performing the calculation, the result is approximately 2.86 grams. Therefore,
`\(1.73 * 10^(28)\)` atoms of sulfur weigh about 2.86 grams.