Mole
Definition
The SI unit for the amount of a substance, equal to 6.022 × 10²³ particles (atoms, molecules, or ions) — known as Avogadro's number.
Why is Mole Important?
Mole is an essential chemistry concept used in laboratories, pharmaceutical development, environmental science, and industrial processes. Understanding this concept is critical for accurate chemical calculations, safe laboratory practices, and optimizing reactions.
Our chemistry calculators provide instant, accurate results for complex conversions and calculations, making lab work more efficient and reducing the risk of errors in critical measurements.
What is a Mole?
The mole (mol) is the SI unit for the amount of a substance, defined as exactly 6.02214076 × 10²³ particles (atoms, molecules, ions, or other entities). This number is known as Avogadro's number. The mole bridges the gap between the atomic scale and the human scale — allowing chemists to count atoms by weighing them.
Why Moles Matter
| Without Moles | With Moles |
|---|---|
| "Mix 1.204×10²⁴ molecules of H₂ with 6.022×10²³ molecules of O₂" | "Mix 2 mol H₂ with 1 mol O₂" |
| Individual atoms are ~10⁻²⁶ kg | 1 mol of atoms weighs the molar mass in grams |
Molar Mass Reference
| Substance | Molar Mass (g/mol) | Meaning |
|---|---|---|
| Hydrogen (H₂) | 2.016 | 1 mol H₂ weighs 2.016 g |
| Carbon (C) | 12.011 | 1 mol C weighs 12.011 g |
| Water (H₂O) | 18.015 | 1 mol H₂O = 18 mL ≈ 1 tbsp |
| Sodium chloride (NaCl) | 58.44 | 1 mol NaCl ≈ 2 tbsp table salt |
| Glucose (C₆H₁₂O₆) | 180.16 | 1 mol glucose ≈ ¾ cup sugar |