Final answer:
To find the number of phosphorus atoms in 168 kg of phosphorus, convert the mass to grams, find the number of moles, and then multiply by Avogadro's number.
Step-by-step explanation:
To determine the number of phosphorus atoms in 168 kg of phosphorus, we need to use Avogadro's number and the molar mass of phosphorus.
First, we need to convert 168 kg to grams by multiplying it by 1000, which gives us 168,000 g.
Next, we divide the mass of phosphorus by its molar mass to find the number of moles, and then multiply that by Avogadro's number (6.022 × 10^23) to find the number of atoms.
The molar mass of phosphorus is 30.97 g/mol. So, the calculation would be: (168,000 g / 30.97 g/mol) × (6.022 × 10^23 atoms/mol) = 3.09 × 10^26 phosphorus atoms.