Question

Calculate the mass, in grams, of 962 atoms of iron, Fe(1 mol of Fe has a mass of 55.85 g ).

Answer 1

To calculate the mass of 962 atoms of iron, convert atoms to moles using Avogadro's number and then to grams using the molar mass of iron. The final mass of 962 atoms of iron is approximately 8.92 ×
`10^{-20` grams.

Step-by-step explanation:

To calculate the mass of 962 atoms of iron, we must first understand the concept of a mole. A mole is a unit that represents a specific number of particles, often atoms or molecules. Avogadro's number, which is approximately 6.022 ×
`10^{23`, represents the number of particles in one mole. Therefore, we can calculate the mass of 962 atoms of iron by first converting atoms to moles and then using the molar mass of iron to find the mass in grams.

Step 1: Convert atoms to moles using Avogadro's number:

962 atoms Fe × (1 mol Fe / 6.022 ×
`10^{23` atoms) = 1.598 ×
`10^{-21` mol Fe

Step 2: Convert moles to grams using the molar mass of iron (55.85 g/mol):

1.598 ×
`10^{-21` mol Fe × (55.85 g/mol) = 8.919 ×
`10^{-20` g Fe

We can round our final answer to three significant figures:

8.92 ×
`10^{-20` g Fe