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Amount of Substance Converter

Convert between different units of amount of substance measurement including moles, millimoles, and more.

Common Amount of Substance Conversions

Mole (SI Base Unit)

  • 1 mol = 1,000 mmol (millimoles)
  • 1 mol = 1,000,000 μmol (micromoles)
  • 1 mol = 1 g-mol (gram-mole)
  • 1 mol = 0.001 kmol (kilomoles)

Practical Units

  • 1 mmol = 0.001 mol
  • 1 kmol = 1,000 mol
  • 1 lb-mol = 453.59237 mol
  • 1 μmol = 10⁻⁶ mol

Most Common Conversions

  • 1 mol = 1,000 mmol
  • 1 mmol = 0.001 mol
  • 1 mol = 1 g-mol
  • 1 g-mol = 1 mol
  • 1 g-mol = 0.001 kmol
  • 1 kmol = 1,000 g-mol
  • 1 lb-mol ≈ 453.59 mol
  • 1 mol ≈ 0.002205 lb-mol

Real-World Examples

  • Water (18 g): 1 mole = 6.022 × 10²³ molecules
  • Table Salt (NaCl, 58.44 g): 1 mole = 6.022 × 10²³ formula units
  • Glucose (C₆H₁₂O₆, 180 g): 1 mole = 6.022 × 10²³ molecules
  • Oxygen Gas (O₂, 32 g): 1 mole at STP = 22.4 liters
  • Carbon-12 (12 g): Exactly 1 mole (by definition)
  • Blood Glucose Normal Range: 4-6 mmol/L (fasting)
  • Vitamin C Tablet: ~500 mg ≈ 2.8 mmol ascorbic acid

About Amount of Substance

Amount of substance (symbol: n) is one of the seven SI base quantities. It measures the number of elementary entities (atoms, molecules, ions, electrons, or other particles) in a sample. The SI unit is the mole (mol).

The Mole

The mole is defined as exactly 6.02214076 × 10²³ elementary entities (Avogadro's number, NA). This definition was adopted in 2019 as part of the SI redefinition. One mole of any substance contains the same number of entities as there are atoms in exactly 12 grams of carbon-12.

Formula

The amount of substance is calculated as:

n = N / NA

Where:

  • n = amount of substance (in moles)
  • N = number of elementary entities
  • NA = Avogadro constant (6.02214076 × 10²³ mol⁻¹)

Relationship to Mass

Amount of substance relates to mass through molar mass (M):

n = m / M

Where:

  • m = mass (in grams)
  • M = molar mass (in g/mol)

Gram-mole vs Mole

The gram-mole (g-mol) is essentially the same as the mole. It explicitly emphasizes that the molar mass is expressed in grams. In practice, "mole" and "gram-mole" are interchangeable, with 1 mol = 1 g-mol. Similarly, the pound-mole (lb-mol) is used in some engineering contexts where mass is measured in pounds.

Submultiples in Practice

  • Millimole (mmol): Commonly used in clinical chemistry and medicine (e.g., blood glucose levels)
  • Micromole (μmol): Used for trace amounts in biochemistry and pharmacology
  • Nanomole (nmol): Used in molecular biology and analytical chemistry
  • Picomole (pmol): Used in high-sensitivity analytical techniques
  • Kilomole (kmol): Used in industrial chemistry and chemical engineering for large-scale processes

Historical Note

The word "mole" comes from the Latin word moles, meaning "massive structure" or "heap." It was introduced in 1897 by German chemist Wilhelm Ostwald. Before the 2019 redefinition, the mole was defined as the amount of substance containing as many entities as there are atoms in 12 grams of carbon-12. The new definition fixes Avogadro's number exactly, making the mole independent of the kilogram.

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