Question

Diamond is one form of elemental carbon. An engagement ring contains a diamond weighing 1.25 carats (1 carat = 200 mg). How many atoms are present in the diamond?

a) 3.25 × 10^22 atoms

b) 1.25 × 10^24 atoms

c) 2.5 × 10^22 atoms

d) 6.25 × 10^23 atoms

Answer 1

A diamond ring weighing 1.25 carats contains approximately 1.25 x 10²² atoms of carbon. None of the given choices are correct.

Step-by-step explanation:

In 1 carat, there are 200 mg of diamond. So, in a 1.25 carat diamond ring, the weight of the diamond is 1.25 carats x 200 mg/carat = 250 mg.

The molar mass of carbon is 12.01 g/mol. To find the number of moles, we can convert the weight of the diamond to grams (250 mg = 0.250 g) and then divide by the molar mass: 0.250 g / 12.01 g/mol = 0.0208 mol.

Avogadro's number tells us that there are 6.022 x 10²³ atoms in 1 mole. To find the number of atoms, we can multiply the number of moles by Avogadro's number: 0.0208 mol x 6.022 x 10²³ atoms/mol = 1.25 x 10²² atoms.

Hence, all options are incorrect.