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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 following table lists the Van der Waals constants (from the Van der Waals equation) for a number of common gases and volatile liquids. [ 1 ] To convert from L 2 b a r / m o l 2 {\displaystyle \mathrm {L^{2}bar/mol^{2}} } to L 2 k P a / m o l 2 {\displaystyle \mathrm {L^{2}kPa/mol^{2}} } , multiply by 100.
The conversion procedure for some units (for example, the Mach unit of speed) are built into Module:Convert as they are too complex to be specified in a table. That is indicated by entering a code (which must be the same as used in the module) in the Extra column.
The constants listed here are known values of physical constants expressed in SI units; that is, physical quantities that are generally believed to be universal in nature and thus are independent of the unit system in which they are measured. Many of these are redundant, in the sense that they obey a known relationship with other physical ...
mph ≡ 1 mi/h = 0.447 04 m/s: mile per minute: mpm ≡ 1 mi/min = 26.8224 m/s: mile per second: mps ≡ 1 mi/s = 1 609.344 m/s: speed of light in vacuum: c: ≡ 299 792 458 m/s = 299 792 458 m/s: speed of sound in air: s: 1225 to 1062 km/h (761–660 mph or 661–574 kn) [note 1] ≈ 340 to 295 m/s: Note
Expansion rate between 2 points in free space 1 m apart under Hubble's law. [1] ... 110: 70: 1 × 10 −7: Typical ... 320 km/h or 200 mph is a parameter sometimes ...
(mph) (km/h) (m/s) Subsonic <0.8 <530 <609 <980 <273 Most often propeller-driven and commercial turbofan aircraft with high aspect-ratio (slender) wings, and rounded features like the nose and leading edges. The subsonic speed range is that range of speeds within which, all of the airflow over an aircraft is less than Mach 1.
For gases, departure from 3 R per mole of atoms is generally due to two factors: (1) failure of the higher quantum-energy-spaced vibration modes in gas molecules to be excited at room temperature, and (2) loss of potential energy degree of freedom for small gas molecules, simply because most of their atoms are not bonded maximally in space to ...