Mole Gram Particles Converter
Convert between moles, grams and particles using molar mass and Avogadro constant.
What can you convert?
This tool treats moles as the central bridge. If you enter grams, it divides by molar mass to reach moles. If you enter particles, it divides by Avogadro's number. Once moles are known, grams and particles are calculated from the same amount of substance.
| Known input | Required data | Calculator path |
|---|---|---|
| Moles | Formula or molar mass | moles -> grams and particles |
| Grams | Formula or molar mass | grams / molar mass -> moles |
| Particles | Formula or molar mass | particles / 6.02214076e23 -> moles |
| Manual molar mass | g/mol value | Use when the formula is not needed or not supported |
Formula map
Worked examples
1 mole of H2O: molar mass is about 18.015 g/mol, so 1 mol = 18.015 g and 6.02214076 x 10^23 molecules.
58.44 g of NaCl: NaCl has molar mass about 58.44 g/mol, so 58.44 g is about 1.000 mol or 6.02214076 x 10^23 formula units.
6.02214076 x 10^23 CO2 molecules: that is 1 mol of CO2, which has mass about 44.01 g.
How the conversion diagram helps
The visual map shows why mole conversions feel repetitive: every path passes through moles. Grams depend on molar mass, particles depend on Avogadro's number, and moles connect both sides. When a problem feels confusing, decide which box you already know, convert to moles, then move to the requested box.
Where this converter is useful
- Changing grams of a reagent into moles for a balanced equation.
- Finding the number of molecules in a given sample mass.
- Checking molarity preparation problems after molar mass is known.
- Comparing formula units for ionic compounds with molecules for covalent compounds.
- Reviewing Avogadro's number before stoichiometry exams.
Common mistakes
- Multiplying by molar mass when converting grams to moles; grams to moles should divide.
- Using atomic mass for one element when the compound needs full molar mass.
- Calling particles only molecules; ionic compounds are often counted as formula units.
- Forgetting scientific notation, especially for particle counts near 10^23.
- Rounding molar mass too aggressively before a multi-step stoichiometry problem.
Rounding and result checking
Particle counts are usually very large, so scientific notation is expected. Grams should scale with molar mass: one mole of glucose is much heavier than one mole of water because each formula unit contains more atoms. Keep a few extra digits in molar mass during calculation, then round the final answer to the significant figures from the measured input.
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FAQs
How to convert grams to moles?
Divide the mass by the molar mass: moles = mass (g) ÷ molar mass (g/mol). Find the molar mass from the chemical formula and the periodic table, then divide. Examples: 18 g of H2O ÷ 18 g/mol = 1 mol; 49 g of H2SO4 ÷ 98 g/mol = 0.5 mol; 11 g of CO2 ÷ 44 g/mol = 0.25 mol. From there you can find particles (× 6.022 × 10^23), gas volume at STP (× 22.4 L), or use mole ratios from a balanced equation to find amounts of other species in the reaction.
How do you convert moles into grams?
Multiply moles by molar mass: mass (g) = moles × molar mass (g/mol). Examples: 0.5 mol of NaCl × 58.5 g/mol = 29.25 g; 2 mol of CO2 × 44 g/mol = 88 g; 0.25 mol of H2SO4 × 98 g/mol = 24.5 g. Common use cases: weighing out a solute for a target molarity, calculating product mass from a balanced equation, or working out mass changes during a reaction.
How many moles are in 88.0 grams of CO2?
2.00 mol. Molar mass of CO2 = 12.01 + 2 × 16.00 = 44.01 g/mol. Moles = 88.0 ÷ 44.01 = 2.00 mol. That sample contains 2.00 × 6.022 × 10^23 = 1.20 × 10^24 CO2 molecules and would occupy 2.00 × 22.4 = 44.8 L at STP.
How many moles are in 15 grams of lithium?
About 2.16 mol. Atomic mass of Li = 6.94 g/mol, so moles = 15 ÷ 6.94 = 2.16 mol. That corresponds to 2.16 × 6.022 × 10^23 ≈ 1.30 × 10^24 lithium atoms. Lithium reacts with water (2Li + 2H2O → 2LiOH + H2), but more slowly than sodium or potassium because of its lower reduction potential difference and higher hydration enthalpy.
How many grams are in 2.4 moles of sulfur?
76.9 g, treating sulfur as atomic S. Molar mass of S = 32.06 g/mol, so mass = 2.4 × 32.06 = 76.94 g. Solid elemental sulfur at room temperature actually exists as S8 rings (256.5 g/mol), so if a problem specifies S8, the answer would instead be 2.4 × 256.5 = 615.6 g — read the formula carefully.
How many grams are in 88.1 moles of magnesium?
About 2142 g (≈ 2.14 kg). Atomic mass of Mg = 24.31 g/mol, so mass = 88.1 × 24.31 = 2141.7 g. That sample contains 88.1 × 6.022 × 10^23 ≈ 5.31 × 10^25 Mg atoms.
How many moles are in 2.3 grams of phosphorus?
About 0.074 mol of P atoms. Atomic mass of P = 30.97 g/mol, so moles = 2.3 ÷ 30.97 = 0.0743 mol. If the problem refers specifically to white phosphorus (P4, molar mass ≈ 123.9 g/mol), the answer is instead 2.3 ÷ 123.9 = 0.0186 mol of P4.
How many moles are in 22 grams of argon?
About 0.551 mol. Argon is monatomic with atomic mass 39.95 g/mol, so moles = 22 ÷ 39.95 = 0.551 mol. That gives roughly 0.551 × 6.022 × 10^23 ≈ 3.32 × 10^23 atoms, occupying 0.551 × 22.4 ≈ 12.3 L at STP.
How many particles are in a mole?
6.022 × 10^23 particles. This is Avogadro's number, named after Amedeo Avogadro. The 'particles' are whatever discrete entity the substance is made of: atoms (for elements), molecules (for covalent compounds), or formula units (for ionic compounds). Since the 2019 SI redefinition, the value is fixed by definition: NA = 6.02214076 × 10^23 mol^-1 exactly.
How many particles equals 8.1 mol of C2H4O?
About 4.88 × 10^24 molecules. Particles = moles × NA = 8.1 × 6.022 × 10^23 = 4.878 × 10^24 molecules. Each C2H4O molecule contains 7 atoms (2 C + 4 H + 1 O), so the total atom count is 7 × 4.878 × 10^24 = 3.41 × 10^25 atoms. C2H4O is the molecular formula for both acetaldehyde (CH3CHO) and ethylene oxide; specify the structure when it matters.
How many moles are contained in 3.131 × 10^24 particles?
5.20 mol. Moles = particles ÷ NA = (3.131 × 10^24) ÷ (6.022 × 10^23) = 5.199 ≈ 5.20 mol. Same arithmetic regardless of whether the particles are atoms, molecules, ions, or formula units.
How many particles are in 1 mol of lithium?
6.022 × 10^23 atoms — that is the definition of a mole. Lithium is a metal that exists as discrete atoms (not molecules), so the particles are atoms. Mass check: 1 mol × 6.94 g/mol = 6.94 g of lithium contains 6.022 × 10^23 atoms. In a Li-ion battery, charge transfer scales with electrons per Li ion: 1 mol of Li transferred carries 1 mol of electrons (96,485 C — Faraday's constant).
How many particles are in 1.75 moles of carbon?
About 1.054 × 10^24 atoms. Particles = 1.75 × 6.022 × 10^23 = 1.054 × 10^24 carbon atoms. By mass that sample is only 1.75 × 12.01 = 21.0 g — a short pencil's worth of graphite, but already a sextillion atoms.
How many particles are in 2 moles?
1.204 × 10^24 particles, regardless of substance. The mole is just a count: 2 × 6.022 × 10^23 = 1.204 × 10^24 of whatever entity the formula represents. For an ionic substance like NaCl, 2 mol contains 1.204 × 10^24 formula units, which is 2.408 × 10^24 individual ions (one Na+ and one Cl- per unit). Mass differs by substance: 2 mol of H2 weighs about 4 g; 2 mol of Cu weighs about 127 g.
How many particles are in 3 moles?
1.807 × 10^24 particles. Particles = 3 × 6.022 × 10^23 = 1.8066 × 10^24. At STP, 3 mol of an ideal gas occupies 3 × 22.4 = 67.2 L. In electrochemistry, 3 mol of electrons carries 3 × 96,485 ≈ 289,455 C of charge.
How many representative particles are in 2.5 mol H2O2?
About 1.506 × 10^24 molecules. Particles = 2.5 × 6.022 × 10^23 = 1.5055 × 10^24 H2O2 molecules. Each molecule has 4 atoms, so the atom count is 4 × 1.506 × 10^24 = 6.02 × 10^24 atoms. Molar mass of H2O2 = 34.01 g/mol, so 2.5 mol weighs 85 g. Hydrogen peroxide decomposes to water and oxygen (2H2O2 → 2H2O + O2), accelerated by MnO2 or the enzyme catalase — the basis of the 'elephant's toothpaste' demo.