Answer :
The amount of atoms in 38.1 g of barium chloride (BaCl2) is determined using Avogadro's number and the molar mass of BaCl2. The calculation results in approximately 3.3 x 10^23 atoms.
The number of atoms in a sample can be determined using Avogadro's number, which states that one mole of any substance contains 6.022 x 10^23 particles (atoms, molecules, etc.). Therefore, we firstly need to find out how many moles our sample of barium chloride has.
The molar mass of barium chloride (BaCl2) is about 208.23 g/mol, which we can find by adding the atomic masses of its component atoms according to the periodic table.
Therefore, the number of moles in 38.1 g BaCl2 = 38.1 g / 208.23 g/mol = 0.183 moles. Then we multiply this by Avogadro's number, 0.183 moles * 6.022 x 10^23 atoms/mole. But remember, each unit of BaCl2 has 3 atoms (1 barium and 2 chlorine).
So the total number of atoms= 0.183 moles * 6.022 x 10^23 atoms/mole * 3 atoms/unit = 3.3 x 10^23 atoms.
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