gram molecular weight - The mass of a substance divided by the molecular weight of the substance expressed in grams.
the fundamental unit of mass of a substance. A mole of any substance is the number of grams or pounds indicated by its molecular weight. For example, water has a molecular weight of approximately 18. Therefore, a gram-mole of water is 18 grams of water; a poundmole or water is 18 pounds of water. See molecular weight.
a unit of measurement of the physical quantity named 'abundance' ( also: 'amount of substance'); 1 mole is defined as the abundance of a system which contains the number of constituents equal to the number of atoms in exactly 12 grams of the carbon-12 isotope. The number of items in 1 mole is called Avogadro's number ( = 6.0222 E+23 mol-). Abbreviated as 'mol', e.g. = 32.2 g/mol.
A quantity of a compound whose weight in grams is numerically equal to its molecular weight expressed in atomic mass units. Avogadro's number of molecules: 6.023 ¥ 1023 molecules.
M grams of a substance, where M is its relative molecular mass (molecular weight); this will be 6 x 1E23 molecules of the substance.
The number of hydrogen atoms in one gram of hydrogen, equal to . When counting the number of molecules in a gas, it is often convenient to count them in moles.
amount of a substance that contains 6.02 * 1023 particles
The formula weight in grams of an element or compound; or a quantity of chemical substance that contains 6.02 x 1023 formula units of the substance.
an amount of a substance equal in grams to the sum of the atomic weights.
Unit quantity in chemistry. Amount of a substance in grams (gram mole) or pounds (pound mole) which corresponds to the sum of the atomic weights of all the atoms appearing in the molecule. Sometimes referred to as a mol.
6.02 x 1023 atoms of an element or 6.02 x 1023 molecules of a chemical compound. The weight of one mole of an element is equal to its atomic weight in grams; the weight of one mole of a compound is equal to its molecular weight in grams.
The SI unit of amount of substance equal to the number of particles ( atoms, ions, molecules, electrons, photons) as there are atoms in 12 grams of 12C. This number is equal to 6.023 x 10exp23.
A quantity of an element or compound having a mass in grams equal to the element’s atomic weight or to the compound’s molecular weight.
a certain quantity of matter
a chemical measurement of quantity
a fixed number, similar to a dozen, which describes a number of particles as well as quantity of mass
a given number (Avogadro's number) of something
a gram equivalent weight of an element in a liter of water
an incredibly large number because atoms are so very tiny
a quantity equal to 6.023 x 1023
Not a small furry animal! A mole refers to a large number, 6 x 1023, which is the number of carbon atoms present in 12g of carbon.
The quantity (in grams) of a chemical which equals the molecular weight. This amount equals 6.023 x 1023 molecules (Avogadro's number) of the substance (e.g. sodium chloride has a molecular weight of 58.5 so one mole of salt equals 58.5 g).
The mass of a material equal to the combined mass of 6.023 1023 atoms or molecules of the material.
the amount of a material which contains Avogadro's number of molecules and whose mass in grams is numerically equal to the molecular mass of the substance
One mole represents the number 6.02 × 1023 which is the number of atoms inside 12 grams of carbon-12.
The amount of substance that contains the same number of elementary particles as are found in exactly 12 g of carbon-12.
Avogadro's number (6.02 X 1023 atoms) of a substance.
the quantity of a given substance that contains as many molecules or formula units as the number of atoms in exactly 12 g of carbon- 12. The amount of substance containing Avogadro's number of molecules or formula units
the amount of a species (compound, element, or ion) whose mass (in grammes, g) is equal to its atomic or molecular mass. It is usually abreviated as mol.
One mole is the mass numerically equal (in grams) to the relative molecular mass of a substance. It is the amount of substance of a system that contains as many elementary units (6.023 exp23) as there are atoms of carbon in 0.012 kg of the pure nuclide C12; the elementary unit must be specified and may be an atom, molecule, ion, electron, photon, or even a specified group of such units.
In dermatology, a pigmented spot on the skin, Also called a nevus. In gynecology, a mass within the uterus formed of partly developed products of conception. In biochemistry, the molecular weight of a substance. In more technical terms, a mole is the number of atoms in exactly 12 g of carbon-12. Mole in this sense is short for molecular weight.
The amount of a substance containing the same number of atoms, formula units, molecules, or ions as there are in exactly 12 grams of Carbon-12. This "Avagadro's number" is phenomenally large; it is (approximately) 602,000,000,000,000,000,000,000.
SI unit for measuring a substance; equal to 0.012 kg of carbon 12.
The measure of the number of objects or particles. One mole is 6.02 x 1023 objects (Avogadro's number). The mole of a pure substance contains a mass (in grams) equal to the atomic mass of the substance. For example, carbon has an atomic mass of exactly 12.0 units; therefore, a mole of carbon is 12 grams.
a unit of mass equal to the molecular weight of the substance
An amount equal to the number of carbon atoms in exactly 12 grams of the C12
(SI) A mole of a substance is the molecular weight of the substance in grams. ie. NaCl has a molecualr weight of 58.443 therefore 1 mole of NaCl is 58.443 grams.
The amount of a substance that contains 6.0225 × 10 23 (Avogadro's number) of atoms or molecules.
For a given molecule, one mole is the mass numerically equal to its molecular weight. A gram mole is the mass in grams equal to the molecular weight. A pound-mole is the weight in pounds equal to the molecular weight.
The SI fundamental unit for "amount of substance." A mole is, generally speaking, Avogadro's number of atoms, molecules, or other elementary particles; however, in the more precise SI definition, a mole is equal to the number of carbon atoms in 12.01 g of carbon.
Gram-molecular weight. The sum of the atomic weights of all the atoms of any molecule, in grams.
The fundamental unit for measuring chemical compounds (abbreviated mol). One mole equals the molecular weight of a compound in grams. The number of molecules in a mole is equal to 6.02 x 1023 (Avogadro's number).
A mass: in this context a mass of cells originating from the conceptus.
The quantity of a compound or element that has a weight in grams numerically equal to its molecular weight. Also referred to as gram molecule or gram molecular weight.
The molecular weight of a substance, usually expressed in grams.
Weight of a substance in grams equal to the molecular weight; 1 mole of a substance contains the same number of particles as 1 mole of any other substance.
An amount equal to Avogadro's number or 6.02 × 1023. One mole of atoms is equal to 6.02 × 1023atoms.
the number equal to the number of carbon atoms in exactly 12 grams of pure 12C: Avogadro's number. One mole represents 6.02 x 1023 units.
The mole (symbol: mol) is the SI base unit that measures an amount of substance. One mole contains Avogadro's number (approximately 6.022) entities. A mole is much like "a dozen" in that both units can describe any set of elementary objects, although the mole's use is usually limited to measurement of subatomic, atomic, and molecular structures.