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ChemBench
From raw masses to the simplest formula.
Each element's mass is divided by its atomic weight to get moles, then every mole value is divided by the smallest one — this converts arbitrary masses into the simplest whole-number ratio of atoms.
The empirical formula is the simplest ratio (CH₂O), while the molecular formula could be a multiple of it (C₆H₁₂O₆ for glucose) — empirical formula alone can't tell you which multiple without also knowing the molar mass.
Molar mass of any chemical formula (e.g. H2O, C6H12O6, Ca(OH)2).
OpenPercent composition of an element within a chemical formula.
OpenPercent yield from actual and theoretical reaction yields.
OpenIdentify which reactant runs out first in a reaction.
OpenEmpirical formula
CH2O
What you entered
Moles of C
mass ÷ atomic weight= 3.3303Moles of H
mass ÷ atomic weight= 6.6468Moles of O
mass ÷ atomic weight= 3.3315Divide each by the smallest mole value
÷ 3.3303= C: 1, H: 1.9959, O: 1.0004Result
Empirical formula: CH2O
The simplest whole-number mole ratio of these elements gives the empirical formula CH2O.