Universal mole converter: between moles, grams, particles, and volume of gas at STP. Complete stoichiometry conversion tool for chemistry.
The mole calculator is a comprehensive conversion tool that translates between moles, grams, number of particles, and gas volume at standard temperature and pressure (STP). The mole is the central unit in chemistry that connects the macroscopic world we can measure with the microscopic world of atoms and molecules.
One mole of any substance contains exactly 6.02214076 × 10²³ particles (Avogadro's number) and occupies 22.414 liters at STP if it is an ideal gas. These relationships allow chemists to convert freely between mass, mole count, particle number, and gas volume — the four fundamental quantities in stoichiometry.
This calculator handles all six possible pairwise conversions among these four quantities. Enter any one known quantity along with the molar mass, and instantly obtain the other three. It includes presets for common substances, handles multiple units, and provides a detailed breakdown of each conversion step.
For best results, combine calculator output with direct observation and periodic check-ins with a veterinarian or qualified advisor. Small adjustments made early usually improve comfort, safety, and long-term outcomes more than large corrective changes made later.
This universal mole converter handles every common stoichiometry conversion in one place. Enter any quantity and get all related values instantly — no need for separate calculators for each conversion type. This mole calculator helps you compare outcomes quickly and reduce avoidable mistakes when making day-to-day care decisions. Use the estimate as a planning baseline and confirm final decisions with a qualified professional when risk is high.
Core Relationships: - Mass (g) = Moles × Molar Mass (g/mol) - Particles = Moles × 6.022 × 10²³ - Volume at STP (L) = Moles × 22.414 Derived: - Moles = Mass / Molar Mass = Particles / 6.022×10²³ = Volume(STP) / 22.414
Result: 132.03 g, 1.807 × 10²⁴ molecules, 67.24 L at STP
Three moles of CO₂: mass = 3 × 44.01 = 132.03 g; particles = 3 × 6.022 × 10²³ = 1.807 × 10²⁴ molecules; gas volume at STP = 3 × 22.414 = 67.24 L.
Chemistry students benefit from visualizing the relationships between mass, moles, particles, and gas volume as a road map. Moles sit at the center, connected to mass (via molar mass), to particles (via Avogadro's number), and to gas volume (via molar volume at STP). Any conversion between non-adjacent quantities passes through moles as an intermediate step.
The concept evolved over centuries. John Dalton's atomic theory (1808) established that atoms have definite masses. Avogadro's hypothesis (1811) related gas volumes to particle counts. The actual number was first estimated by Josef Loschmidt in 1865. In 2019, the mole was redefined to be exactly 6.02214076 × 10²³, removing its dependence on the carbon-12 definition.
Advanced applications extend the mole concept to solution chemistry (molarity = moles/liter), thermochemistry (enthalpy per mole), and electrochemistry (Faraday's constant = charge per mole of electrons). The mole unifies all quantitative chemistry by providing a standard way to count particles.
A mole is the SI unit for amount of substance. It represents exactly 6.02214076 × 10²³ entities (atoms, molecules, ions, etc.). It allows chemists to count particles by weighing them.
STP (Standard Temperature and Pressure) is 0°C (273.15 K) and 1 atm (101.325 kPa). At STP, one mole of any ideal gas occupies exactly 22.414 liters, providing a simple mole-to-volume conversion.
This value comes from the ideal gas law: V = nRT/P. With n = 1 mol, R = 0.08206 L·atm/(mol·K), T = 273.15 K, and P = 1 atm, V = 22.414 L. Real gases deviate slightly from this value.
Divide the mass by the molar mass to get moles, then multiply by Avogadro's number. This calculator does both steps: particles = (mass / MW) × 6.022 × 10²³.
The 22.414 L molar volume only applies to ideal gases at STP. Liquids and solids have much smaller molar volumes that depend on density. For example, one mole of water is only 18.07 mL.
Both contain 6.022 × 10²³ entities, but a mole of O₂ molecules contains 2 × 6.022 × 10²³ = 1.204 × 10²⁴ individual oxygen atoms since each molecule has 2 atoms.