Final answer:
To find the number of grams of phosphorus (P) in 3.3×10^28 atoms of P, you can use the concept of molar mass. The molar mass of phosphorus (P) is approximately 30.973761 g/mol. So, you can calculate the number of grams of phosphorus (P) in 3.3×10^28 atoms by multiplying the number of atoms by the molar mass.
Step-by-step explanation:
To find the number of grams of phosphorus (P) in 3.3×10^28 atoms of P, you can use the concept of molar mass. The molar mass of phosphorus (P) is approximately 30.973761 g/mol.
So, you can calculate the number of grams of phosphorus (P) in 3.3×10^28 atoms by:
Number of grams = Number of atoms × Molar mass
= 3.3×10^28 atoms × 30.973761 g/mol
= 1.02×10^30 g
To determine the mass of phosphorus in 3.3 \u00d7 1028 atoms P, calculate the number of moles using Avogadro's number and then multiply by the molar mass of phosphorus, resulting in approximately 16,970 grams.
To calculate the mass of phosphorus from the number of atoms, use Avogadro's number and the molar mass of phosphorus. Avogadro's number (6.022 \u00d7 1023 atoms/mol) tells us how many atoms are in one mole of a substance, while the molar mass (30.973761 grams per mole for phosphorus) tells us the mass of one mole of that substance. Here's how you can do the calculation:
First, calculate the number of moles of phosphorus atoms in 3.3 \u00d7 1028 atoms:
Number of moles = Number of atoms \u00f7 Avogadro's number
Number of moles = 3.3 \u00d7 1028 atoms / 6.022 \u00d7 1023 atoms/mol
Number of moles \u2248 548 moles of phosphorous (rounded to three significant figures)
Next, calculate the mass from the moles of phosphorus:
Mass = moles \u00d7 molar mass
Mass = 548 moles \u00d7 30.973761 g/mol
Mass = u2248 16,970 g of phosphorus (rounded to three significant figures)
Therefore, 3.3 \u00d7 1028 atoms of phosphorus correspond to approximately 16,970 grams of phosphorus.