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Isotherms of an ideal gas for different temperatures. The curved lines are rectangular hyperbolae of the form y = a/x. They represent the relationship between pressure (on the vertical axis) and volume (on the horizontal axis) for an ideal gas at different temperatures: lines that are farther away from the origin (that is, lines that are nearer to the top right-hand corner of the diagram ...
where F is the gravitational force acting between two objects, m 1 and m 2 are the masses of the objects, r is the distance between the centers of their masses, and G is the gravitational constant. The first test of Newton's law of gravitation between masses in the laboratory was the Cavendish experiment conducted by the British scientist Henry ...
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.
The molar gas constant (also known as the gas constant, universal gas constant, or ideal gas constant) is denoted by the symbol R or R. It is the molar equivalent to the Boltzmann constant , expressed in units of energy per temperature increment per amount of substance , rather than energy per temperature increment per particle .
The sound speed in an ideal gas depends only on its temperature: =. Deduction of the form valid for ideal gases In an ideal gas the isoentropic transformation is described by the Poisson's law : d ( p ρ − γ ) s = 0 {\displaystyle d\left(p\rho ^{-\gamma }\right)_{s}=0} where γ is the heat capacity ratio , a constant for the material.
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The inset in Fig. B shows the mixture states which are a combination of the saturated liquid and vapor states that exist at each end of the line, intersections of the mixture line and its isotherm. However, these mixture states are not part of the surface generated by the van der Waals equation; they are not solutions of the equation.