Ask Question
12 February, 02:18

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

+1
Answers (1)
  1. 12 February, 05:10
    0
    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
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “How many carbon atoms are there in a diamond (pure carbon) with a mass of "48" mg? ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers