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Thus, the number of molecules in a specific volume of gas is independent of the size or mass of the gas molecules when related to an ideal gas approximate. It is very important to note that we apply an ideal gas or perfect gas definition (a hypothetical gas consisting of identical particles of zero volume, with no intermolecular forces, but the ability to interchange momentum with identical gas molecules) to a real gas such as hydrogen or nitrogen so we can statistically approximate the real gas behavior.
As an example, equal volumes of molecular hydrogen and nitrogen would contain the same number of molecules, as long as they are at the same temperature and pressure and observe ideal or perfect gas behavior. Whilst this is not the real world case, it is statistically very close.
However, this above equation is just a trivial one, which is valid for all homogeneous substances, including homogeneous liquids and solids. This relation is easy to deduce; its validity was assumed before Avogadro's work.
The most important consequence of Avogadro's law is the following: The ideal gas constant has the same value for all gases. This means that the constant
has the same value for all gases, independent of the size or mass of the gas molecules. This statement is nontrivial, and it embodies Avogadro's ingenious insight into the nature of ideal gases. It took decades to prove Avogadro's law based on the kinetic theory of gases.
One mole of an ideal gas occupies 22.4 liters (dm³) at STP, and occupies 24.45 litres at SATP (Standard Ambient Temperature and Pressure = 25 degrees C and 1 atm/101.3kPa). This volume is often referred to as the molar volume of an ideal gas. Real gases may deviate from this value.
The number of molecules in one mole is called Avogadro's number: approximately 6.022×1023 particles per mole.
|This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Avogadro's_law". A list of authors is available in Wikipedia.|