Answer :

Answer:

3.01 × 10²³ atoms C

General Formulas and Concepts:

Chemistry

Atomic Structure

  • Reading a Periodic Table
  • Using Dimensional Analysis
  • Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

Math

Pre-Algebra

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right

Explanation:

Step 1: Define

6.00 g C

Step 2: Identify Conversions

Avogadro's Number

Molar Mass of C - 12.01 g/mol

Step 3: Convert

[tex]6.00 \ g \ C(\frac{1 \ mol \ C}{12.01 \ g \ C} )(\frac{6.022 \cdot 10^{23} \ atoms \ C}{1 \ mol \ C} )[/tex] = 3.00849 × 10²³ atoms C

Step 4: Check

We are given 3 sig figs. Follow sig fig rules and round.

3.00849 × 10²³ atoms C ≈ 3.01 × 10²³ atoms C

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Rewritten by : Barada