Which has more atoms: 3.0 g iron, Fe, or 2.0 g of sulfur, S?
Calculate mols of each.
mols Fe = 3.0/atomic mass Fe.
mols S = 2.0/atomic mass S.
The one with more mols will have more atoms since 1 mol of each material will have 5.02 x 10^23 atoms.
To determine which substance has more atoms, we need to compare the number of moles for each element.
1. Calculate the number of moles for iron (Fe):
First, find the molar mass of iron (Fe) from the periodic table.
The molar mass of Fe is approximately 55.845 g/mol.
Using the formula:
Number of moles = mass (g) / molar mass (g/mol)
Number of moles of iron = 3.0 g / 55.845 g/mol
Number of moles of iron ≈ 0.05 mol
2. Calculate the number of moles for sulfur (S):
Similarly, find the molar mass of sulfur (S) from the periodic table.
The molar mass of S is approximately 32.06 g/mol.
Number of moles of sulfur = 2.0 g / 32.06 g/mol
Number of moles of sulfur ≈ 0.062 mol
3. Compare the number of moles:
From the calculations, we can see that we have more moles of sulfur than iron.
4. Compare the number of atoms:
Since 1 mole of any substance contains Avogadro's number (6.022 x 10^23) of atoms, we can calculate the number of atoms for each element.
Number of atoms of iron = Number of moles of iron × Avogadro's number
Number of atoms of iron ≈ 0.05 mol × 6.022 x 10^23 atoms/mol
Number of atoms of sulfur = Number of moles of sulfur × Avogadro's number
Number of atoms of sulfur ≈ 0.062 mol × 6.022 x 10^23 atoms/mol
Now that we have the number of atoms for each element, we can compare them.