To find the atomicity of an ideal gas you can use γ = Cp/Cv.
Atomicity of a gas is the number of an element present in one molecule of that element.The gases can be:-monoatomic .E.g-Helium(He),diatomic,E.g-Hydrogen(H2),triatomic,E.g-Ozone(O3),polyatomic,E.g-Sulphur(S8).
The atomicity of a gas can be determined by comparing its vapor density to its atomic weight. In this case, if the vapor density is 28 and the atomic weight is 14, the atomicity of the gas is 2. This means that each molecule of the gas consists of 2 atoms.
Neon is an inert gas (noble gas), natural, atomic number 10; it is a monoatomic ags and its atomicity is 1. neon is used as filling gas in red lamps, in lasers, in plasma displays, in cryogenic applications, etc.
To calculate the atomicity of ammonium phosphate, first determine the formula of ammonium phosphate, NH4)3PO4. The atomicity is then determined by adding the total number of atoms in the formula, which is 12 (4 nitrogen atoms from ammonium and 8 atoms from phosphate). So, the atomicity of ammonium phosphate is 12.
the atomicity of ozone is 3 hehehehe./////////////......................
The atomicity of neon is 1, meaning it exists as individual atoms. Phosphorus can exist in several allotropes with different atomicities: white phosphorus has an atomicity of 4, red phosphorus has an atomicity of 1, and black phosphorus has an atomicity of 1.
Atomicity means which can not be broken into further small parts. like in database,dept_id can be considered as atomic value of dept table as it cannot be broken into further values.please visithttp://sanchit-tricks.blogspot.comfor latest tricks and hacks.
Helium is a noble gas with an atomic number of 2, meaning it has a total of 2 protons in its nucleus. It is considered monatomic, existing as single atoms rather than forming molecules with other atoms.
The atomicity of oxygen in ozone is 3. This means that each molecule of ozone contains three oxygen atoms.
Hydrogen has an atomicity of 1, meaning that its molecules consist of single hydrogen atoms.
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