Search results
Results From The WOW.Com Content Network
Historically, the mole was defined as the amount of substance in 12 grams of the carbon-12 isotope.As a consequence, the mass of one mole of a chemical compound, in grams, is numerically equal (for all practical purposes) to the mass of one molecule or formula unit of the compound, in daltons, and the molar mass of an isotope in grams per mole is approximately equal to the mass number ...
Thus, the solid is composed of a certain number of moles of such entities. In yet other cases, such as diamond, where the entire crystal is essentially a single molecule, the mole is still used to express the number of atoms bound together, rather than a count of molecules. Thus, common chemical conventions apply to the definition of the ...
By mole fraction (i.e., by quantity of molecules), dry air contains 78.08% nitrogen, 20.95% oxygen, 0.93% argon, 0.04% carbon dioxide, and small amounts of other trace gases (see Composition below for more detail). Air also contains a variable amount of water vapor, on average around 1% at sea level, and 0.4% over the entire atmosphere.
The laws describing the behaviour of gases under fixed pressure, volume, amount of gas, and absolute temperature conditions are called gas laws.The basic gas laws were discovered by the end of the 18th century when scientists found out that relationships between pressure, volume and temperature of a sample of gas could be obtained which would hold to approximation for all gases.
Acumatica – Acumatica Cloud ERP; BatchMaster Software – BatchMaster ERP; Consona Corporation – AXIS ERP, Intuitive ERP, Made2Manage ERP; CGI Group – CGI Advantage; CGram Software – CGram Enterprise; Consona Corporation – Cimnet Systems, Compiere professional edition, Encompix ERP; Ciright Systems – Ciright ERP
For a given mass of an ideal gas, the volume and amount (moles) of the gas are directly proportional if the temperature and pressure are constant. The law is named after Amedeo Avogadro who, in 1812, [ 2 ] [ 3 ] hypothesized that two given samples of an ideal gas, of the same volume and at the same temperature and pressure, contain the same ...
The atmospheric pressure is roughly equal to the sum of partial pressures of constituent gases – oxygen, nitrogen, argon, water vapor, carbon dioxide, etc.. In a mixture of gases, each constituent gas has a partial pressure which is the notional pressure of that constituent gas as if it alone occupied the entire volume of the original mixture at the same temperature. [1]
[9] Any extensive quantity E for a sample can be divided by the sample's volume, to become the "E density" for the sample; similarly, any extensive quantity "E" can be divided by the sample's mass, to become the sample's "specific E"; extensive quantities "E" which have been divided by the number of moles in their sample are referred to as ...