What is the weight of 6.3 × 10
21
atoms of
phosphorus?
Answer in units of g
To calculate the weight of 6.3 x 10^21 atoms of phosphorus, you will need to use the concept of molar mass and Avogadro's number. Here are the steps to get the answer:
1. Find the molar mass of phosphorus (P) from the periodic table. The molar mass of phosphorus is approximately 31.0 g/mol.
2. Determine the number of moles of phosphorus atoms by dividing the given number of atoms by Avogadro's number. Avogadro's number is approximately 6.022 x 10^23 atoms/mol.
Number of moles = (6.3 x 10^21 atoms) / (6.022 x 10^23 atoms/mol)
3. Calculate the weight (mass) of phosphorus by multiplying the number of moles by the molar mass.
Weight of phosphorus = (Number of moles of P) x (Molar mass of P)
So, let's do the calculations:
Number of moles = (6.3 x 10^21 atoms) / (6.022 x 10^23 atoms/mol)
= 6.3 x 10^21 / 6.022 x 10^23
≈ 0.1047 moles
Weight of phosphorus = (Number of moles of P) x (Molar mass of P)
= 0.1047 moles x 31.0 g/mol
≈ 3.24 grams
Therefore, the weight of 6.3 x 10^21 atoms of phosphorus is approximately 3.24 grams.