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# Converter Parts Per Million (ppm)

Parts Per Million (ppm) Converter for Gases This converter calculates the measured value in units of [ppm] into units of [mg/m^{3}] and visa versa. The unit ppm is used in several branches in different ways. The use of ppm therefore has to be specified in the input fields below, in the way it should convert the value with the proper unit. For more theory about the use of ppm, please see the documentation below. |

## Molecular Weight :

In the input field of Molecular Weight you could either choose from the drop-down list, or you could fill in the value of the molecular weight of the gas. If the molecular weight is unknown to you, please try our Molecular Weight Calculator.

By entering either the concentration in units of [ppm] or in units of [mg/m^{3}], the value will be converted directly and displayed in the field at the bottom. The significance is automatically determined. Use extra zero’s to expand the significance.

**Definition** Parts Per Million (ppm) in proportion of:** Volume Mole Weight**measured in: ** Air WaterMolecular Weight **(Calculate) [Select Common Gas] Ammonia [NH3] Argon [Ar] Carbon Dioxide [CO2] Carbon Monoxide [CO] Helium [He] Hydrogen [H2] Hydrogen Sulfide [H2S] Krypton [Kr] Methane [CH4] Neon [Ne] Nitric Oxide [NO] Nitrogen [N2] Nitrogen Dioxide [NO2] Nitrous Oxide [N2O] Oxygen [O2] Ozone [O3] Sulfur Dioxide [SO2] Water [H2O] Xenon [Xe]*M* =g/mol**Concentration** expressed in units of ppm*X _{ppm}* =ppm expressed in units of mg/m

^{3}

*X*=mg/m

_{mg/m}3^{3}

**Converted Concentration**

*X*=

*Copyright © 1998-2008 Lenntech Water Treatment & Air Purification Holding B.V.Version 1.7*[ Converters ] [ Calculators ] [ Periodic Table ]

FORMULAS:

Parts per Million by Volume (or mole) in AirIn air pollution literature ppm applied to a gas, always means parts per million by volume or by mole. These are identical for an ideal gas, and practically identical for most gases of air pollution interest at 1 atm. Another way of expressing this value is ppmv. [1]

One part per million (by volume) is equal to a volume of a given gas mixed in a million volumes of air:A micro liter volume of gas in one liter of air would therefore be equal to 1 ppm:Today’s more and more there is an interest to express gas concentrations in metric units, i.e. *µ*g/m^{3}. Although expressing gaseous concentrations in *µ*g/m^{3} units, has the advantage of metric expression, it has the disadvantage of being greatly influenced by changes in temperature and pressure. Additionally, because of difference in molecular weight, comparisons of concentrations of different gases are difficult. [2]

To convert ppmv to a metric expression like *µ*g/m^{3}, the density of the concerning gas is needed. The density of gas can be calculated by the Law of Avogadro’s, which says: equal volumes of gases, at the same temperature and pressure, contain the same number of molecules. This law implies that 1 mole of gas at STP a volume of 22.71108 liters (dm^{3}) enfolds, also mentioned as the molar volume of ideal gas. Standard Temperature and Pressure (STP) is defined as a condition of 100.00 kPa (1 bar) and 273.15 K^{ }(0^{°}C), which is a standard of IUPAC. [3] The amount of moles of the concerning gas can be calculated with the molecular weight.Where:*V _{m}* =standard molar volume of ideal gas (at 1 bar and 273.15 K) [3][22.71108 L/mol]

*M*=molecular weight of gas[g/mol]For converting ppm by mole, the same equation can be used. This can be made clear by the following notation:By checking the dimensions of the most right part of the equation, there will be found a dimensionless value, like the concentration in ppm is.To calculate the concentration in metric dimensions, with other temperature and pressure conditions the Ideal Gas Law comes in handy. The volume (

*V*) divided by the number of molecules (n) represents the molar volume (

*V*) of the gas with a temperature (

_{n}*T*) and pressure (

*P*).Where:

*V*

_{n}=specific molar volume of ideal gas (at pressure

*P*and temperature

*T*)[L/mol]

*V*=volume of the gas[m

^{3}]

*n*=amount of molecules[mol]

*R*=universal gas law constant [3][8.314510 J K

^{-1}mol

^{-1}] or [m

^{3 }Pa K

^{-1}mol

^{-1}]

*T*=temperature[K]

*P*=pressure[Pa]With this equation it comes clear that the percentage notation by ppm is much more useful, because the independency of the temperature and pressure.

**Parts per Million by Weight in Water :**

The concentration in ppm of gas in water is meanly meant by weight. To express this concentration with metric units the density of water is needed.

The density of pure water has to be by definition 1000.0000 kg/m^{3} at a temperature of 3.98°C and standard atmospheric pressure, till 1969. Till then this was mean definition for the kilogram. Today’s the kilo is defined as being equal to the mass of the international prototype of the kilogram [4].

## Water with a high purity (VSMOW) at a temperature of 4°C (IPTS-68) and standard atmospheric pressure has a density of 999.9750 kg/m^{3}. [5]

The density of water is effected by the temperature, pressure and impurities, i.e. dissolved gasses or the salinity of the water. Even the concerning concentration of gas dissolved in the water is affecting the density of the solution. By nature there’s a chance that water contains a certain concentration of Deuterium which influences the density of the water. This concentration is also called the isotopic composition [6].

Accurate calculations on these conversions are only possible when the density of the water is measured. In practice the density of water is therefore set to 1.0 ·10^{3} kg/m^{3}. When calculating the conversion with this value you gets:Where:*? _{w}* =density of water[1.0 ·10

^{3}kg/m

^{3}] Reference[1] Never, N. ,

*Air Pollution Control Engineering*. McGraw-HILL, Singapore 1995.

[2] Godish, T. ,

*Air Quality. Lewis Publishers*, Michigan 1991.

[3] Cohen, E.R. and Taylor, B.N.,

*J. Res. Nat. Bur. Stand.*

**92**(1987) 85-95. (International Union of Pure and Applied Chemistry (IUPAC))

[4] n/a,

*Kilogram*. International prototype of the kilogram, www.bipm.org/en/scientific/mass/prototype.html.

[5] Marsh, K.N., Ed.,

*Recommended Reference Materials for the Realization of Physicochemical Properties*. Blackwell Scientific Publications, Oxford.

[6] www.iapws.org/faq1/isotope.htm

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