Relative Atomic mass

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Introduction to fundamental concepts of chemistry
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Relative Atomic mass
Empirical formula and Molecular Formula
Combustion Analysis
Concept of mole
Avogadro’s number
Molar Volume
Stoichiometry
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Relative Atomic Mass
Empirical and Molecular Formula
Combustion Analysis
Concept of Mole
Avogadro's Number
Molar Volume
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Fundamental principles of organic chemistry
Chemistry of Hydrocarbons
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RELATIVE ATOMIC MASS
Relative atomic mass is the mass of an atom of an element as compared to the mass of an atom of carbon taken as 12.
Relative atomic masses are measured in atomic mass units.
1 a.m.u. is 1/12th part of mass of an atom of C-12.
1 a.m.u.= 1.661 x 10-27kg
= 1.661 10-24g
Examples: Na = 23 a.m.u.
Cl = 35.5 a.m.u

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