Density of liquid at any temperature t is given by dt=do /(1+ga at) the equation applies to
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The ideal gas law, also called the general gas equation, is the equation of state of a hypothetical ideal gas. It is a good approximation of the behavior of many gases under many conditions, although it has several limitations. It was first stated by Émile Clapeyron in 1834 as a combination of the empirical Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law.[1] The ideal gas law is often written in an empirical form:
{\displaystyle PV=nRT}PV=nRT
where {\displaystyle P}P, {\displaystyle V}V and {\displaystyle T}T are the pressure, volume and temperature; {\displaystyle n}n is the amount of substance; and {\displaystyle R}R is the ideal gas constant. It is the same for all gases. It can also be derived from the microscopic kinetic theory, as was achieved (apparently independently) by August Krönig in 1856[2] and Rudolf Clausius in 1857.[3]
Note that this law makes no comment as to whether a gas heats or cools during compression or expansion. An ideal gas may not change temperature, but most gases like air are not ideal and follow the Joule–Thomson effect.[dubious – discuss]
This equation will apply to all liquids.
• Density is just the mass for a chosen amount (volume) of the solid. The standard unit of measurement for water's density is gram/ml.
• The atoms in liquids are close together. Although they are haphazardly arranged, they are still firmly packed, giving liquids high densities. The density of a substance as a liquid is typically only somewhat less than its density as a solid.