1. Determine the number of atoms per formula unit:
* Barium phosphate (Ba₃(PO₄)₂) has:
* 3 barium (Ba) atoms
* 2 phosphorus (P) atoms
* 8 oxygen (O) atoms
* Total: 3 + 2 + 8 = 13 atoms per formula unit
2. Calculate the number of formula units:
* Avogadro's number tells us that there are 6.022 x 10²³ formula units in one mole of any substance.
* Therefore, 0.0350 mol of barium phosphate contains:
* 0.0350 mol * (6.022 x 10²³ formula units/mol) = 2.108 x 10²² formula units
3. Calculate the total number of atoms:
* Multiply the number of formula units by the number of atoms per formula unit:
* (2.108 x 10²² formula units) * (13 atoms/formula unit) = 2.74 x 10²³ atoms
Therefore, there are approximately 2.74 x 10²³ atoms present in 0.0350 mol of barium phosphate.
