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Mole Converter & Gas Stoichiometry

Enter a chemical formula and a quantity in grams, moles, molecules, or liters at STP. The tool converts to all other units and shows the step-by-step dimensional analysis.

Input

Results

Molar Mass
18.015 g/mol
Grams
18 g
Moles
0.999167 mol
Molecules
6.0171 x 10^23
Liters at STP
22.3953 L

Mole Map

MolesGramsMoleculesLiters (STP)÷ 18.02× 18.02× 6.022×10²³÷ 6.022×10²³× 22.4 L÷ 22.4 L

Step-by-Step Dimensional Analysis

1. Determine molar mass

M(H2O)=18.015 g/molM(\text{H2O}) = 18.015 \text{ g/mol}

2. Convert grams to moles

n=mM=1818.015=0.999167 moln = \frac{m}{M} = \frac{18}{18.015} = 0.999167 \text{ mol}

3. Calculate molecules

N=n×NA=0.999167×6.022×1023=6.0171×1023N = n \times N_A = 0.999167 \times 6.022 \times 10^{23} = 6.0171 \times 10^{23}

4. Calculate volume at STP

V=n×22.414=0.999167×22.414=22.3953 LV = n \times 22.414 = 0.999167 \times 22.414 = 22.3953 \text{ L}

Reference Guide

Molar Mass

The molar mass (M) is the mass of one mole of a substance, equal to the sum of atomic masses of all atoms in the formula.

n=mMn = \frac{m}{M}

Avogadro's Number

One mole contains exactly 6.022 x 10^23 particles (atoms, molecules, or formula units).

N=n×NA=n×6.022×1023N = n \times N_A = n \times 6.022 \times 10^{23}

Molar Volume at STP

At standard temperature and pressure (0 C, 1 atm), one mole of any ideal gas occupies 22.4 liters.

V=n×22.414 L/molV = n \times 22.414 \text{ L/mol}

Dimensional Analysis

Convert between units by multiplying by conversion factors so that unwanted units cancel. The mole sits at the center of all conversions.