Mole-Mass-Particle Converter

Convert between moles, mass (grams), and number of particles. Enter any one value with the molar mass to calculate the other two.

Stoichiometry

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結果

How to Use

1
Enter molar mass or select an element
Input the molar mass of your substance in g/mol. For pure elements, you can select from the periodic table to auto-fill the value.
2
Enter the known quantity
Type the amount in moles, grams, or number of particles (molecules or atoms) into the corresponding field.
3
Read the converted values
The tool simultaneously displays all three quantities so you can verify stoichiometric amounts needed for a reaction or present in a sample.

About

The mole-mass-particle triangle is the conceptual backbone of quantitative chemistry. Every stoichiometric calculation — predicting how much product a reaction produces, determining limiting reagents, or standardizing a solution — ultimately rests on the ability to move fluidly between macroscopic masses in grams and microscopic counts of molecules.

Avogadro's constant (6.022×10²³ mol⁻¹) makes this bridge possible. Because atoms and molecules are extraordinarily small, laboratory-scale quantities of matter contain astronomical numbers of particles. One gram of hydrogen contains roughly 6×10²³ atoms; one milliliter of water contains about 3.3×10²² molecules. The mole collapses this enormous number into a manageable unit aligned with the periodic table: the molar mass of any substance in g/mol equals its formula weight in amu.

This converter is designed to reinforce the dimensional relationships that students and researchers navigate daily in the laboratory. Whether you are weighing out a precise amount of reagent, calculating theoretical yield, or checking whether a synthesized batch matches expected molecular weight by elemental analysis, facility with mole conversions is essential to chemical fluency.

FAQ

What is a mole and why is it used in chemistry?

A mole is the SI unit for amount of substance, defined since 2019 as exactly 6.02214076×10²³ entities (Avogadro's constant). The mole bridges the macroscopic scale, where we measure mass in grams, and the atomic scale, where chemical reactions occur one molecule at a time. One mole of any element has a mass in grams numerically equal to its atomic weight on the periodic table, making mass-to-mole conversions straightforward.

What is Avogadro's number and how was it determined?

Avogadro's constant (NA = 6.022×10²³ mol⁻¹) is the number of particles in one mole. Historically it was determined through X-ray crystallography (measuring unit cell dimensions of known crystals), electrolysis (Faraday's constant / electron charge), and Brownian motion studies. The 2019 SI redefinition fixed its value exactly, inverting the relationship: now Avogadro's constant defines the mole rather than being derived from it.

How do I convert grams to moles?

Divide the mass in grams by the molar mass in g/mol: moles = mass (g) / molar mass (g/mol). The molar mass of a compound is the sum of the atomic masses of all its constituent atoms from the periodic table. For example, water (H₂O) has molar mass = 2(1.008) + 15.999 = 18.015 g/mol, so 36.03 g of water contains exactly 2.000 moles.

What is the difference between molecular mass and molar mass?

Molecular mass (or molecular weight) refers to the mass of a single molecule expressed in atomic mass units (amu or Da), where 1 amu = 1/12 the mass of a carbon-12 atom. Molar mass refers to the mass of one mole of that substance expressed in g/mol. Numerically they are the same number but the units differ: water has molecular mass 18.015 amu and molar mass 18.015 g/mol. This numerical equality is a consequence of how the amu and the mole are defined.

How do I find the moles in a solution from volume and molarity?

Molarity (M, mol/L) multiplied by volume in liters gives moles: n = M × V(L). For example, 250 mL (0.250 L) of a 2.0 mol/L HCl solution contains 0.250 × 2.0 = 0.50 mol of HCl. This relationship is the basis for all volumetric titration calculations and is the link between the mole-converter (mass-based) and dilution-based approaches to quantifying amounts.

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