Final answer:
To find the mass of 1.8×1023 atoms of phosphorus, the given number of atoms is divided by Avogadro's number to determine the moles, and then multiplied by the molar mass of phosphorus. The calculation results in approximately 9.291 grams.
Step-by-step explanation:
To calculate the mass of 1.8×1023 atoms of phosphorus, we need to relate this number to Avogadro's number, which is approximately 6.022×1023 atoms per mole, and the molar mass of phosphorus. The molar mass of phosphorus (P) is approximately 30.97 g/mol. To find the number of moles represented by 1.8×1023 atoms of phosphorus, we divide the given number of atoms by Avogadro's number:
Number of moles = (1.8×1023 atoms P) / (6.022×1023 atoms/mol) = 0.3 mol P
Next, we multiply the number of moles by the molar mass of phosphorus to find the mass:
Mass = (0.3 mol P) × (30.97 g/mol) = 9.291 g P
Therefore, 1.8×1023 atoms of phosphorus weigh approximately 9.291 grams.