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The ratio of the number of discrete constituent particles (such as molecules, atoms, or ions) to the amount of a substance, defined as exactly 6.022 140 76 × 10 23 mol −1. Avogadro number The number of discrete constituent particles in one mole of a substance, defined as exactly 6.02214076 × 10 23.
One lb-mol is equal to 453.592 37 g‑mol, [6] which is the same numerical value as the number of grams in an international avoirdupois pound. Greenhouse and growth chamber lighting for plants is sometimes expressed in micromoles per square metre per second, where 1 mol photons ≈ 6.02 × 10 23 photons. [ 7 ]
20 Presumably from the practice, in counting sheep or large herds of cattle, of counting orally from one to twenty, and making a score or notch on a stick, before proceeding to count the next twenty. [3] [4] A distance of twenty yards in ancient archery and gunnery. [5] Threescore: 60 Three score (3x20) Large: 1,000 Slang for one thousand ...
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
List of orders of magnitude for molar concentration; Factor (Molarity) SI prefix Value Item 10 −24: yM 1.66 yM: 1 elementary entity per litre [1]: 8.5 yM: airborne bacteria in the upper troposphere (5100/m 3) [2]
510-07-6 C 20 H 26 O 3: Crotogoudin: 1252665-39-6 C 20 H 27 NO 11: amygdalin: 29883-15-6 C 20 H 28 O 2: tretinoin: 302-79-4 C 20 H 30 O 3: Neotripterifordin: C 20 H 32 O 5: prostacyclin: C 20 H 32 O 5: prostaglandin E2: C 20 H 34 O 5: dinoprost: C 20 H 42: eicosane: 112-95-8 C 21 H 16 FN 7: AMG 319: 1608125-21-8 C 21 H 18 FN 5 O 5 S ...
In the International System of Units (SI), the coherent unit for molar concentration is mol/m 3. However, most chemical literature traditionally uses mol/dm 3, which is the same as mol/L. This traditional unit is often called a molar and denoted by the letter M, for example: 1 mol/m 3 = 10 −3 mol/dm 3 = 10 −3 mol/L = 10 −3 M = 1 mM = 1 ...
The molar mass of atoms of an element is given by the relative atomic mass of the element multiplied by the molar mass constant, M u ≈ 1.000 000 × 10 −3 kg/mol ≈ 1 g/mol. For normal samples from Earth with typical isotope composition, the atomic weight can be approximated by the standard atomic weight [ 2 ] or the conventional atomic weight.