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Grams per cm³ to Grams per Liter Density Converter
↔ Convert g/L to g/cm³ instead

Common Conversions

g/cm³ g/L
0.001 1
0.005 5
0.01 10
0.05 50
0.1 100
0.5 500
1 1000
2 2000
5 5000
10 10000

Why this conversion matters in chemistry

Solvent density tables run in g/cm³ at 20 °C — water at 0.998, methanol at 0.791, dichloromethane at 1.326. Gas-phase work and dilute aqueous concentrations live in g/L. Multiplying by 1000 brings a liquid density up to the same scale: DCM at 1326 g/L sits a thousand-fold above CO₂ vapor at about 2 g/L, which is most of why a gas-phase mass-balance feels different from a liquid one. The conversion is also the routine step when a chemistry-table density has to feed a volumetric reagent-charge calculation expressed in g/L.

Formula

g/L = g/cm³ × 1000

Worked Examples

1 g/cm³ = 1000 g/L

Water density at 4 °C — the conversion's calibration anchor.

0.001293 g/cm³ = 1.293 g/L

Air density at old STP (0 °C, 1 atm) — illustrating how gas-phase values fall when scaled out of g/cm³.

2.165 g/cm³ = 2165 g/L

The crystallographic density of solid sodium chloride — useful as a reference for any halite-related calculation.

Frequently Asked Questions

How do I convert g/cm³ to g/L?
Multiply by 1000. The relationship is exact, since 1 L is exactly 1000 cm³ by definition.
How much denser are liquids than gases?
Typical liquid densities run 700–1500 g/L; gas densities at STP are 0.1–5 g/L. So liquids are roughly 200–1000 times denser than gases — the gap that makes gases compressible and liquids effectively not.
How does a solution concentration in g/L relate to molarity?
Molarity is g/L divided by molar mass. So 58.44 g/L of NaCl, divided by NaCl's 58.44 g/mol, gives exactly 1 M — the textbook calibration that links gravimetric concentration and molar concentration.