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Information about Molar Mass

Molar mass, symbol M,[1] is the mass of one mole of a substance (chemical element or chemical compound).[2] It is a physical property which is characteristic of each pure substance. The base SI unit for mass is the kilogram[1] but, for both practical and historical reasons, molar masses are almost always quoted in grams per mole (g/mol or g mol–1), especially in chemistry.

Molar mass is closely related to the molecular weight (M.W.), formula weight (F.W.) or relative molar mass (Mr) of a compound, and to the atomic weight of an element. However, it should be distinguished from the molecular mass, which is the mass of one molecule. The dalton, symbol Da, is also sometimes used as a unit of molar mass, especially in biochemistry, with the definition 1 Da = 1 g/mol, despite the fact that it is strictly a unit of molecular mass (1 Da = 1.660 538 782(83)×10–27 kg).[3][4]

Molar masses are almost never measured directly. They may be calculated from standard atomic weights, and are often listed in chemical catalogues and on material safety data sheets (MSDS). Molar masses typically vary between:
1–238 g/mol for atoms of naturally-occuring elements;
10–1000 g/mol for simple chemical compounds;
1000–5,000,000 g/mol for polymers, proteins, DNA fragments, etc.

Molar masses of elements

Main article: atomic weight
The molar mass of atoms of an element is given by the atomic weight of the element[5] multiplied by the molar mass constant, Mu = 1×10–3 kg/mol = 1 g/mol:[6]
M(H) = 1.007 97(7) × 1 g/mol = 1.007 94(7) g/mol
M(S) = 32.065(5) × 1 g/mol = 32.065(5) g/mol
M(Cl) = 35.453(2) × 1 g/mol = 35.453(2) g/mol
M(Fe) = 55.845(2) × 1 g/mol = 55.854(2) g/mol
Multiplying by the molar mass constant ensures that the calculation is dimensionally correct: atomic weights are dimensionless quantities (ie, pure numbers) whereas molar masses have units (in this case, g/mol).

Some elements are usually encountered as molecules, eg hydrogen (H2), sulfur (S8), chlorine (Cl2). The molar mass of molecules of these elements is the molar mass of the atoms multiplied by the number of atoms in each molecule:
M(H2) = 2 × 1.007 97(7) × 1 g/mol = 2.015 88(14) g/mol
M(S8) = 8 × 32.065(5) × 1 g/mol = 256.52(4) g/mol
M(Cl2) = 2 × 35.453(2) × 1 g/mol = 70.906(4) g/mol

Molar masses of compounds

The molar mass of a compound is given by the sum of the atomic weights of the atoms which form the compound multiplied by the molar mass constant, Mu:
M(NaCl) = [22.989 769 28(2) + 35.453(2)] × 1 g/mol = 58.443(2) g/mol
M(C12H22O11) = ([12 × 12.0107(8)] + [22 ×1.007 94(7)] + [11 ×15.9994(3)]) × 1 g/mol = 486.424(10) g/mol


An average molar mass may be defined for mixtures of compounds.[1] This is particularly important in polymer science, where different polymer molecules may contain different numbers of monomer units (non-uniform polymers).[7]

Related properties

Molecular weight (M.W.) and formula weight (F.W.) are older terms for what is now more correctly called the relative molar mass (Mr).[2] This is a dimensionless quantity (ie, a pure number, without units) equal to the molar mass divided by the molar mass constant.[8]

Molecular mass

Main article: Molecular mass
The molecular mass (m) is the mass of a given molecule: it is measured in daltons (Da) or atomic mass units (u), where 1 Da = 1 u = 1.660 538 782(83)×10–27 kg).[3][4] Different molecules of the same compound may have different molecular masses because they contain different isotopes of an element. The molar mass is a measure of the average molecular mass of all the molecules in a sample, and is usually the more appropriate measure when dealing with macroscopic (weighable) quantities of a substance.

Molecular masses are calculated from the relative atomic masses[9] of each nuclide, while molar masses are calculated from the atomic weights of each element. The atomic weight takes into account the isotopic distribution of the element in a given sample (usually assumed to be "normal"). For example, water has a molar mass of 18.0153(3) g/mol, but individual water molecules have molecular masses which range between 18.010 564 6863(15) u (1H216O) and 22.027 7364(9) u (2H218O).

The distinction between molar mass and molecular mass is important because relative molecular masses can be measured directly by mass spectrometry, often to a precision of a few parts per million. This is accurate enough to directly determine the chemical formula of a molecule.[10]

Precision and uncertainties

The precision to which a molar mass is known depends on the precision of the atomic weights from which it was calculated. Most atomic weights are known to a precision of at least one part in ten-thousand, often much better[5] (the atomic weight of lithium is a notable, and serious,[11] exception). This is adequate for almost all normal uses in chemistry: it is more precise than most chemical analyses, and exceeds the purity of most laboratory reagents.

The precision of atomics weights, and hence of molar masses, is limited by the knowledge of the isotopic distribution of the element. If a more accurate value of the molar mass is required, it is necessary to determine the isotopic distribution of the sample in question, which may be different from the standard distribution used to calculate the standard atomic weight. The isotopic distributions of the different elements in a sample are not necessarily independant of one another: for example, a sample which has been distilled will be enriched in the lighter isotopes of all the elements present. This complicates the calculation of the standard uncertainty in the molar mass.

A useful convention for normal laboratory work is to quote molar masses to two decimal places for all calculations. This is more accurate than is usually required, but avoids rounding errors during calculations. When the molar mass is greater than 1000 g/mol, it is rarely appropriate to use more than one decimal place. These conventions are followed in most tabulated values of molar masses.[12]

Measurement

While molar masses are almost always, in practice, calculated from atomic weights, they can also be measured in certain cases. Such measurements are much less precise than modern mass spectrometric measurements of atomic weights and molecular masses, and are of mostly historical interest. All of the procedures rely on colligative propeties, and any dissociation of the compound must be taken into account.

Vapour density

Main article: Vapour density
The measurement of molar mass by vapour density relies on the principle, first enounced by Amadeo Avogadro, that equal volumes of gases under identical conditions contain equal numbers of particles. This principle is included in the ideal gas equation:
:
where n is the amount of substance. The vapour density (ρ) is given by
:.
Combining these two equations gives an expression for the molar mass in terms of the vapour density for conditions of known pressure and temperature.
:

Freezing-point depression

Main article: Freezing-point depression
The freezing point of a solution is lower than that of the pure solvant, and the freezing-point depression (ΔT) is directly proportional to the amount concentration for dilute solutions. When the amount concentration is expressed as a molality, the proportionality constant is known as the cryoscopic constant (Kf) and is characteristic for each solvant. If w represents the mass fraction of the solute in solution, and assuming no dissociation of the solute, the molar mass is given by
:.

Boiling-point elevation

Main article: Boiling-point elevation
The boiling point of a solution of an involatile solute is higher than that of the pure solvant, and the boiling-point elevation (ΔT) is directly proportional to the amount concentration for dilute solutions. When the amount concentration is expressed as a molality, the proportionality constant is known as the ebullioscopic constant (Kb) and is characteristic for each solvant. If w represents the mass fraction of the solute in solution, and assuming no dissociation of the solute, the molar mass is given by
:.

References

1. ^ International Union of Pure and Applied Chemistry (1993). Quantities, Units and Symbols in Physical Chemistry (2nd Edn). Oxford: Blackwell Science. ISBN 0-632-03583-8. p. 41. Electronic version.
2. ^ International Union of Pure and Applied Chemistry. "relative molar mass". Compendium of Chemical Terminology Internet edition.
3. ^ Bureau International des Poids et Mesures (2006). The International System of Units (SI) (8th Edn). ISBN 92-822-2213-6. p. 126.
4. ^ CODATA value: atomic mass constant. NIST. Retrieved on 2007-10-14.
5. ^ International Union of Pure and Applied Chemistry Commission on Isotopic Abundances and Atomic Weights (2006). "Atomic Weights of the Elements 2005". Pure Appl. Chem. 78: 2051–66. DOI:10.1351/pac200678112051. 
6. ^ Mohr, Peter J.; Taylor, Barry N. (2005). "CODATA recommended values of the fundamental physical constants: 2002". Rev. Mod. Phys. 77: 1–107. DOI:0034-6861/2005/77(1)/1(107). 
7. ^ International Union of Pure and Applied Chemistry (1984). "Note on the terminology for molar masses in polymer science". J. Polym. Sci., Polym. Lett. Ed. | volume = 22 | pages = 57.  Metanomski, W. V. (1991). Compendium of Macromolecular Nomenclature, pp. 47–73. ISBN 0-63202-847-5. 
8. ^">^">#ref_rf-9">^ Atomic Weights and Isotopic Compositions for All Elements. NIST. Retrieved on 2007-10-14.
10. ^">#ref_rf-9">^ Atomic Weights and Isotopic Compositions for All Elements. NIST. Retrieved on 2007-10-14.
10. ^">^">#ref_rf-10">^ Author Guidelines – Article Layout. Royal Society of Chemistry">^">#ref_rf-9">^ Atomic Weights and Isotopic Compositions for All Elements. NIST. Retrieved on 2007-10-14.
10. ^">#ref_rf-10">^ Author Guidelines – Article Layout. Royal Society of Chemistry">RSC Publishing. Retrieved on 2007-10-14.
11. #ref_rf-11

External links

Mass is a fundamental concept in physics, roughly corresponding to the intuitive idea of "how much matter there is in an object". Mass is a central concept of classical mechanics and related subjects, and there are several definitions of mass within the framework of relativistic
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The mole (symbol: mol) is the SI base unit that measures an amount of substance. One mole contains Avogadro's number (approximately 6.0221023) entities.

A mole is much like "a dozen" in that both are absolute numbers (having no units) and can describe any type of
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chemical element, or element, is a type of atom that is defined by its atomic number; that is, by the number of protons in its nucleus. The term is also used to refer to a pure chemical substance composed of atoms with the same number of protons.
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International System of Units (abbreviated SI from the French Le Système international d'unités) is the modern form of the metric system.
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kilogram or kilogramme (symbol: kg) is the SI base unit of mass. The kilogram is defined as being equal to the mass of the International Prototype Kilogram (IPK), which is almost exactly equal to the mass of one liter of water.
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atomic mass (ma) is the mass of an atom at rest, most often expressed in unified atomic mass units.[1] The atomic mass may be considered to be the total mass of protons, neutrons and electrons in a single atom (when the atom is motionless).
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molecular mass (abbreviated Mr) of a substance, formerly also called molecular weight and abbreviated as MW, is the mass of one molecule of that substance, relative to the unified atomic mass unit u (equal to 1/12 the mass of one atom of carbon-12).
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The unified atomic mass unit (u), or dalton (Da), is a small unit of mass used to express atomic and molecular masses. It is defined to be one twelfth of the mass of an unbound atom of the carbon-12 nuclide, at rest and in its ground state.
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Biochemistry is the study of the chemical processes in living organisms.[1] The word "biochemistry" comes from the Greek word βιοχημεία biochēmeia, which means "the chemistry of life.
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material safety data sheet (MSDS) is a form containing data regarding the properties of a particular substance. An important component of product stewardship and workplace safety, it is intended to provide workers and emergency personnel with procedures for handling or
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polymer is a substance composed of molecules with large molecular mass composed of repeating structural units, or monomers, connected by covalent chemical bonds. The word is derived from the Greek, πολυ, polu, "many"; and μέρος, meros,
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Proteins are large organic compounds made of amino acids arranged in a linear chain and joined together by peptide bonds between the carboxyl and amino groups of adjacent amino acid residues.
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atomic mass (ma) is the mass of an atom at rest, most often expressed in unified atomic mass units.[1] The atomic mass may be considered to be the total mass of protons, neutrons and electrons in a single atom (when the atom is motionless).
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atom (Greek ἄτομος or átomos meaning "indivisible") is the smallest particle still characterizing a chemical element.
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chemical element, or element, is a type of atom that is defined by its atomic number; that is, by the number of protons in its nucleus. The term is also used to refer to a pure chemical substance composed of atoms with the same number of protons.
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atomic mass (ma) is the mass of an atom at rest, most often expressed in unified atomic mass units.[1] The atomic mass may be considered to be the total mass of protons, neutrons and electrons in a single atom (when the atom is motionless).
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The molar mass constant, symbol Mu, is a physical constant which relates atomic weight and molar mass. Its value is defined to be 1×10–3 kg/mol.
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dimension (Latin, "measured out") is a parameter or measurement required to define the characteristics of an object—i.e., length, width, and height or size and shape.
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molecule is defined as a sufficiently stable electrically neutral group of at least two atoms in a definite arrangement held together by strong chemical bonds.[1][2] In organic chemistry and biochemistry, the term molecule
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1, −1
(amphoteric oxide)
Electronegativity 2.20 (Pauling scale) More

Atomic radius 25 pm
Atomic radius (calc.) 53 pm
Covalent radius 37 pm
Van der Waals radius 120 pm
Miscellaneous

Thermal conductivity (300 K) 180.
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6
(strongly acidic oxide)
Electronegativity 2.58 (Pauling scale)
Ionization energies
(more) 1st: 999.6 kJmol−1
2nd: 2252 kJmol−1
3rd: 3357 kJmol−1

Atomic radius 100 pm
Atomic radius (calc.
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1, 3, 5, 7
(strongly acidic oxide)
Electronegativity 3.16 (Pauling scale)
Ionization energies
(more) 1st: 1251.2 kJmol−1
2nd: 2298 kJmol−1
3rd: 3822 kJmol−1

Atomic radius 100 pm
Atomic radius (calc.
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atomic mass (ma) is the mass of an atom at rest, most often expressed in unified atomic mass units.[1] The atomic mass may be considered to be the total mass of protons, neutrons and electrons in a single atom (when the atom is motionless).
..... Click the link for more information.
atom (Greek ἄτομος or átomos meaning "indivisible") is the smallest particle still characterizing a chemical element.
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The molar mass constant, symbol Mu, is a physical constant which relates atomic weight and molar mass. Its value is defined to be 1×10–3 kg/mol.
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