calculate the number of atoms in 10.0g of sulfur
To calculate the number of atoms in a given mass of a substance, you need to follow these steps:
1. Determine the molar mass of the substance: The molar mass of an element is the mass of one mole of atoms in grams. The molar mass of sulfur (S) can be found on the periodic table, which is approximately 32.06 g/mol.
2. Convert the given mass (10.0g) of sulfur to moles: To do this, divide the given mass by the molar mass of sulfur:
Moles = Mass (g) / Molar mass (g/mol)
Moles = 10.0g / 32.06g/mol
This calculation gives you the number of moles of sulfur.
3. Use Avogadro's number: Avogadro's number is a fundamental constant that represents the number of atoms or molecules in one mole of a substance. It is approximately 6.022 x 10^23 particles/mol.
4. Multiply the number of moles of sulfur by Avogadro's number: This calculation will give you the number of atoms present in the given mass of sulfur.
Number of atoms = Moles of sulfur x Avogadro's number
Therefore, the formula is:
Number of atoms = Moles of sulfur × 6.022 x 10^23
Now, let's calculate the number of atoms in 10.0g of sulfur:
Molar mass of sulfur (S) = 32.06 g/mol
Moles of sulfur = 10.0g / 32.06g/mol ≈ 0.312 moles
Number of atoms = 0.312 moles × 6.022 x 10^23 ≈ 1.88 x 10^23 atoms
So, there are approximately 1.88 x 10^23 atoms in 10.0g of sulfur.