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L −1 M T −2: intensive Entropy: S: Logarithmic measure of the number of available states of a system J/K L 2 M T −2 Θ −1: extensive, scalar Force: F →: Transfer of momentum per unit time newton (N = kg⋅m⋅s −2) L M T −2: extensive, vector Frequency: f: Number of (periodic) occurrences per unit time hertz (Hz = s −1) T −1 ...
newton per coulomb (N⋅C −1), or equivalently, volt per meter (V⋅m −1) energy: joule (J) Young's modulus: pascal (Pa) or newton per square meter (N/m 2) eccentricity: unitless Euler's number (2.71828, base of the natural logarithm) unitless electron: unitless elementary charge: coulomb (C) force
The two points P and P ' (red) are antipodal because they are ends of a diameter PP ', a segment of the axis a (purple) passing through the sphere's center O (black). P and P ' are the poles of a great circle g (green) whose points are equidistant from each (with a central right angle). Any great circle s (blue) passing through the poles is ...
Both definitions are also valid for the diameter of a sphere. In more modern usage, the length d {\displaystyle d} of a diameter is also called the diameter. In this sense one speaks of the diameter rather than a diameter (which refers to the line segment itself), because all diameters of a circle or sphere have the same length, this being ...
For example, the atomic mass constant is exactly known when expressed using the dalton (its value is exactly 1 Da), but the kilogram is not exactly known when using these units, the opposite of when expressing the same quantities using the kilogram.
is the number of collisions made (in ideal conditions, perfectly elastic with no friction) by an object of mass m initially at rest between a fixed wall and another object of mass b 2N m, when struck by the other object. [1] (This gives the digits of π in base b up to N digits past the radix point.)
It is defined as exactly 6.022 140 76 × 10 23 mol −1. Avogadro number The total number of individual molecules in one mole of a substance, by definition equaling exactly 6.022 140 76 × 10 23. Avogadro's law
In statistical physics, the kinetic theory of gases applies Newton's laws of motion to large numbers (typically on the order of the Avogadro number) of particles. Kinetic theory can explain, for example, the pressure that a gas exerts upon the container holding it as the aggregate of many impacts of atoms, each imparting a tiny amount of momentum.