Find the mass of 1.6 mol of magnesium, Mg. How many atoms are present in such a sample?
grams = moles x molar mass
1 mole contains 6.022E23 atoms.
To find the mass of 1.6 moles of magnesium (Mg), you need to know the molar mass of Mg. The molar mass of an element is the mass of one mole of that element. You can find the molar mass of an element on the periodic table.
The atomic mass of Mg is approximately 24.31 g/mol. So, the molar mass of Mg is 24.31 g/mol.
To find the mass of 1.6 moles of Mg, you can use the formula:
Mass = Number of moles × Molar mass
So, for 1.6 moles of Mg:
Mass = 1.6 mol × 24.31 g/mol
Mass = 38.89 g
Therefore, the mass of 1.6 moles of Mg is approximately 38.89 grams.
To find the number of atoms present in such a sample, you need to use Avogadro's number, which states that 1 mole of any substance contains 6.022 × 10^23 particles (atoms, molecules, or ions).
Since 1 mole of Mg contains 6.022 × 10^23 atoms, you can calculate the number of atoms in 1.6 moles of Mg by multiplying the number of moles by Avogadro's number:
Number of atoms = Number of moles × Avogadro's number
Number of atoms = 1.6 mol × 6.022 × 10^23 atoms/mol
Number of atoms = 9.6352 × 10^23 atoms
Therefore, there are approximately 9.6352 × 10^23 atoms in 1.6 moles of Mg.