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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.
Relative atomic and molecular masses as defined are dimensionless. Molar masses when expressed in g/mol have almost identical numerical values as relative atomic and molecular masses. For example, the molar mass and molecular mass of methane, whose molecular formula is CH 4, are calculated respectively as follows:
Relative atomic mass (symbol: A r; sometimes abbreviated RAM or r.a.m.), also known by the deprecated synonym atomic weight, is a dimensionless physical quantity defined as the ratio of the average mass of atoms of a chemical element in a given sample to the atomic mass constant.
Quantity (Common Name/s) (Common) Symbol/s Defining Equation SI Units Dimension Relative atomic mass of an element : A r, A, m ram = /The average mass is the average of the T masses m i (X) corresponding the T isotopes of X (i is a dummy index labelling each isotope):
The relative isotopic mass, then, is the mass of a given isotope (specifically, any single nuclide), when this value is scaled by the mass of carbon-12, where the latter has to be determined experimentally. Equivalently, the relative isotopic mass of an isotope or nuclide is the mass of the isotope relative to 1/12 of the mass of a carbon-12 atom.
The molar mass constant, usually denoted by M u, is a physical constant defined as one twelfth of the molar mass of carbon-12: M u = M(12 C)/12. [1] The molar mass of an element or compound is its relative atomic mass (atomic weight) or relative molecular mass (molecular weight or formula weight) multiplied by the molar mass constant.
Universal Mass Calculator Freeware: UMC is programmed as a mass spectrometry tool to assist interpreting measurement results, mainly derived from molecular or quasi-molecular ions. It can be used for the calculation of: Mass deviation (mmu or ppm) of measured mass from given empirical formula; Mass differences of two empirical formulas
It can be converted into a measure of mass (with dimension M) by multiplying it with the dalton, also known as the atomic mass constant. Among various variants of the notion of atomic weight (A r, also known as relative atomic mass) used by scientists, the standard atomic weight (A r °) is the most common and practical.