Molar specific heats for some common gases at constant volume. Gases - Explosion and Flammability Concentration Limitsįlame and explosion limits for gases like propane, methane, butane, acetylene and more. tolerable concentration levels for some industrial gases.Ībsolute (dynamic) viscosities of some common gases. Online density converter with commonly used units.ĭangerous vs. Potential biogas production from animal manure.Ĭhemical, physical and thermal properties of n-Butane.ĭensities of common products - Imperial and SI-units. Typical composition of biogas produced from household waste. Specific heat of Benzene Gas - C6H6 - at temperatures ranging 250 - 900 K.Ĭarbon - Nitrogen ratios for biogas produced from various raw materials. Material properties of gases, fluids and solids - densities, specific heats, viscosities and more.ĭry air is a mixture of gases where the average molecular weight (or molar mass) can be calculated by adding the weight of each component.īenzene Gas - Specific Heat vs. Definitions and convertion calculators.Īir, LNG, LPG and other common gas properties, pipeline capacities, sizing of relief valves. You can divide pounds per cubic foot by 32.2 for a rough value in slugs.ĭensities of solids, liquids and gases. Note that even if pounds per cubic foot is often used as a measure of density in the U.S., pounds are really a measure of force, not mass. Even if not flammable, it could collect in the lower floor or level of a confined space and displace air, possibly presenting an asphyxiation hazard to individuals entering the lower part of that space.1) NTP - Normal Temperature and Pressure - is defined as 20 oC (293.15 K, 68 oF) and 1 atm ( 101.325 kN/m 2, 101.325 kPa, 14.7 psia, 0 psig, 30 in Hg, 760 torr)Ģ) STP - Standard Temperature and Pressure - is defined as 0 oC (273.15 K, 32 oF) and 1 atm (101.325 kN/m 2, 101.325 kPa, 14.7 psia, 0 psig, 30 in Hg, 760 torr) The density has implications for container storage and personnel safety-if a container can release a dense gas, its vapour could sink and, if flammable, collect until it is at a concentration sufficient for ignition. With this definition, the vapour density would indicate whether a gas is denser (greater than one) or less dense (less than one) than air. This can be seen by dividing the molecular weight of Acetone, 58.1 by that of air, 28.97, which equals 2. That means acetone vapour is twice as heavy as air. For example, acetone has a vapour density of 2 in relation to air. For this use, air has a molecular weight of 28.97 atomic mass units, and all other gas and vapour molecular weights are divided by this number to derive their vapour density. In many web sources, particularly in relation to safety considerations at commercial and industrial facilities in the U.S., vapour density is defined with respect to air, not hydrogen. Vapour density is a dimensionless quantity. (and thus: molar mass = ~2 × vapour density)įor example, vapour density of mixture of NO 2 and N 2O 4 is 38.3. vapour density = molar mass of gas / molar mass of H 2 vapour density = molar mass of gas / 2.016 vapour density = 1⁄ 2 × molar mass Vapour density = mass of n molecules of gas / mass of n molecules of hydrogen gas. It may be defined as mass of a certain volume of a substance divided by mass of same volume of hydrogen. Vapour density is the density of a vapour in relation to that of hydrogen.

Water vapor density