How many carbon atoms are there in a diamond (pure carbon) with a mass of "48" mg?

3.47 * 10²³ C atoms

Solution:

Data Given:

Mass of Diamond = 48 mg = 0.048 g

M. Mass of Diamond = 12.01 g. mol⁻¹ (as it is purely Carbon)

Step 1: Calculate Moles of Diamond as,

Moles = Mass : M. Mass

Putting values,

Moles = 0.048 g : 12.01 g. mol⁻¹

Moles = 0.576 mol

Step 2: Calculate number of Carbon atoms,

As 1 mole of any substance contains 6.022 * 10²³ particles (Avogadro's Number) then the relation for Moles and Number of Carbon atoms can be written as,

Moles = Number of C Atoms : 6.022 * 10²³ Atoms. mol⁻¹

Solving for Number of C atoms,

Number of C atoms = Moles * 6.022 * 10²³ Atoms. mol⁻¹

Putting value of moles,

Number of C atoms = 0.576 mol * 6.022 * 10²³ Atoms. mol⁻¹

Number of C atoms = 3.47 * 10²³ C atoms