How many carbon atoms are there in a diamond (pure carbon) with a mass of 50 ?

It's 50mg. I really don't understand how to do this.

It is milligrams, so divide by 1000

The atomic weight in grams is the mass of 6*10^23 atoms (Avagadro's number)

To determine the number of carbon atoms in a diamond with a mass of 50 grams (assuming pure carbon), we need to use the concept of molar mass and Avogadro's number.

1. Find the molar mass of carbon (C). The molar mass of carbon is approximately 12.01 g/mol.

2. Use the molar mass to calculate the number of moles of carbon in the diamond by dividing the mass of the diamond (50 grams) by the molar mass of carbon (12.01 g/mol):

Number of moles = Mass of diamond (grams) / Molar mass of carbon (grams/mol)
= 50 g / 12.01 g/mol

3. Now, we can use Avogadro's number, which is approximately 6.022 x 10^23 atoms/mol, to determine the number of carbon atoms in the diamond. Multiply the number of moles of carbon by Avogadro's number:

Number of atoms = Number of moles × Avogadro's number
= (50 g / 12.01 g/mol) × (6.022 x 10^23 atoms/mol)

By following these steps, you can calculate the number of carbon atoms in a diamond with a mass of 50 grams.

grams? kilograms ? Carats ?

If grams (pretty big)

6*10^23 carbon atoms weigh 12 grams
so
50 grams * 6*10^23 / 12 = 25*10^23 = 2.5*10^24 atoms