Search results
Results from the WOW.Com Content Network
The ideal gas equation can be rearranged to give an expression for the molar volume of an ideal gas: = = Hence, for a given temperature and pressure, the molar volume is the same for all ideal gases and is based on the gas constant: R = 8.314 462 618 153 24 m 3 ⋅Pa⋅K −1 ⋅mol −1, or about 8.205 736 608 095 96 × 10 −5 m 3 ⋅atm⋅K ...
Specific volume is commonly applied to: Molar volume; Volume (thermodynamics) Partial molar volume; Imagine a variable-volume, airtight chamber containing a certain number of atoms of oxygen gas. Consider the following four examples: If the chamber is made smaller without allowing gas in or out, the density increases and the specific volume ...
Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law , but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products.
Carbon dioxide is the lasing medium in a carbon-dioxide laser, which is one of the earliest type of lasers. Carbon dioxide can be used as a means of controlling the pH of swimming pools, [141] by continuously adding gas to the water, thus keeping the pH from rising. Among the advantages of this is the avoidance of handling (more hazardous) acids.
Figure 2 is an example of a generalized compressibility factor graph derived from hundreds of experimental PVT data points of 10 pure gases, namely methane, ethane, ethylene, propane, n-butane, i-pentane, n-hexane, nitrogen, carbon dioxide and steam.
Specific volume is the volume occupied by a unit of mass of a material. [1] In many cases, the specific volume is a useful quantity to determine because, as an intensive property, it can be used to determine the complete state of a system in conjunction with another independent intensive variable .
In his 1803 publication about the quantity of gases absorbed by water, [1] William Henry described the results of his experiments: … water takes up, of gas condensed by one, two, or more additional atmospheres, a quantity which, ordinarily compressed, would be equal to twice, thrice, &c. the volume absorbed under the common pressure of the atmosphere.
The volume of such a mixture is slightly less than the sum of the volumes of the components. Thus, by the above definition, the term "40% alcohol by volume" refers to a mixture of 40 volume units of ethanol with enough water to make a final volume of 100 units, rather than a mixture of 40 units of ethanol with 60 units of water.