Final answer:
The mass of 1.20×10^23 atoms of phosphorus is calculated by using Avogadro's number and the molar mass of phosphorus, resulting in approximately 6.18×10^-2 g, which doesn't match any of the provided options, indicating a possible typo or miscalculation.
Step-by-step explanation:
The mass in grams of 1.20×1023 atoms of phosphorus can be calculated using Avogadro's number and the molar mass of phosphorus. Avogadro's number is 6.022×1023 atoms/mol and the molar mass of phosphorus is approximately 30.97 g/mol.
You can use the following relationship to determine the mass:
By inserting the known values, we get:
Mass = (1.20×1023 atoms) × (30.97 g/mol) / (6.022×1023 atoms/mol)
After calculating, the mass of 1.20×1023 atoms of phosphorus is found to be approximately 6.1812×10-2 g. When converting to scientific notation with two significant figures, the mass is 6.18×10-2 g. None of the provided options match this calculated value; thus, it seems that there may be a typo or miscalculation in the options given.