To determine which sample contains the least number of atoms, we need to compare the number of moles of each sample. Avogadro's number (6.022 × 10^23) represents the number of atoms in one mole of a substance.
Sample: 58 mol Number of atoms = 58 mol * (6.022 × 10^23 atoms/mol) ≈ 3.499 × 10^25 atoms
Sample: 5.8 × 10^-10 g To convert the mass to moles, we need to know the molar mass of the element. Without knowing the specific element, we cannot calculate the number of atoms.
Sample: 0.0058 kg To convert the mass to moles, we need to know the molar mass of the element. Without knowing the specific element, we cannot calculate the number of atoms.
Sample: 580 amu Atomic mass unit (amu) is a unit used to express the mass of atoms or molecules. One amu is defined as exactly 1/12th the mass of a carbon-12 atom. To convert from amu to grams, we use the molar mass of carbon-12, which is 12 g/mol. Mass of sample in grams = 580 amu * (1 g/6.022 × 10^23 amu) ≈ 9.63 × 10^-23 g To convert the mass to moles: Moles = Mass (g) / Molar mass (g/mol) Moles = (9.63 × 10^-23 g) / (12 g/mol) ≈ 8.03 × 10^-24 mol Number of atoms = 8.03 × 10^-24 mol * (6.022 × 10^23 atoms/mol) ≈ 4.84 atoms
Comparing the calculated values, we see that the sample with 580 amu contains the least number of atoms, with approximately 4.84 atoms.