The mass of a sample of boron atoms is 5.60 g. How many boron atoms are in this sample? Show your work here.
5.60/10.81 * 6.02 * 10^23
To determine the number of boron atoms in a given sample, we need to use the concept of molar mass and Avogadro's number.
1. Locate the molar mass of boron. The molar mass is the mass of one mole of a substance. For boron, the molar mass is approximately 10.81 g/mol.
2. Calculate the number of moles by dividing the mass of the sample by the molar mass. In this case, 5.60 g / 10.81 g/mol ≈ 0.5172 mol.
3. Use Avogadro's number, which is approximately 6.022 x 10^23 atoms/mol, to relate the number of moles to the number of atoms. Multiply the number of moles by Avogadro's number: 0.5172 mol x (6.022 x 10^23 atoms/mol) ≈ 3.114 x 10^23 atoms.
Therefore, there are approximately 3.114 x 10^23 boron atoms in the 5.60 g sample.