Mole to Grams Calculator
Convert moles to grams using molar mass with step-by-step chemistry help.
Mole Conversion Formulas
Moles to Grams: grams = moles × molar mass (g/mol)
Grams to Moles: moles = grams ÷ molar mass (g/mol)
Avogadro\'s Number: 1 mol = 6.022 × 10²³ particles
Common Molar Masses (Reference)
| Compound/Element | Formula | Molar Mass (g/mol) |
|---|---|---|
| Water | H₂O | 18 |
| Sodium Chloride | NaCl | 58.5 |
| Glucose | C₆H₁₂O₆ | 180 |
| Calcium Hydroxide | Ca(OH)₂ | 74 |
| Oxygen | O₂ | 32 |
Frequently Asked Questions
What is a mole in chemistry?
A mole is a unit for counting particles. 1 mole = 6.022 × 10²³ particles (atoms, molecules, ions). Avogadro's number. Used to connect macroscopic (grams) to atomic scale.
What is molar mass?
Mass of one mole of substance in g/mol. For elements: atomic mass from periodic table. For compounds: sum atomic masses of all atoms. Example: H₂O = 2(1) + 16 = 18 g/mol.
How do I convert moles to grams?
Multiply moles by molar mass: grams = moles × molar mass (g/mol). Example: 2 mol H₂O × 18 g/mol = 36 g.
How do I convert grams to moles?
Divide grams by molar mass: moles = grams ÷ molar mass (g/mol). Example: 36 g H₂O ÷ 18 g/mol = 2 mol.
How do I find molar mass?
Look up atomic masses on periodic table. For each element, multiply atomic mass by # of atoms. Sum all. Example: NaCl = 23 + 35.5 = 58.5 g/mol.
Why is mole-to-gram conversion important?
Stoichiometry: calculating reactants/products in reactions. Labs: measuring chemicals by mass, not particles. Balancing equations requires mole ratios.
What is Avogadro's number?
6.022 × 10²³ particles per mole. Defined value. Links atomic scale to macroscopic scale. Allows counting trillions of atoms by weighing grams.
Can I use molar mass for any substance?
Yes, for molecular compounds, ionic compounds, elements. Molar mass = average atomic mass × number of atoms. Works for solids, liquids, gases.
How do subscripts in formulas affect molar mass?
Subscripts show number of atoms. Ca(OH)₂: Ca (40) + 2×O (16) + 2×H (1) = 74 g/mol. Higher subscripts = higher molar mass.
What is the relationship between moles, grams, and particles?
moles = grams ÷ molar mass. particles = moles × Avogadro's number. These three conversions solve most chemistry stoichiometry.
Why do we use moles instead of counting atoms directly?
Atoms are too small to count individually. Moles provide a practical unit bridging atomic and laboratory scales. Makes calculations manageable.
What are common mistakes in mole-gram conversion?
Forgetting subscripts in molar mass. Using wrong atomic masses. Not converting units. Confusing molarity (mol/L) with molar mass (g/mol).