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Course Content
Introduction to fundamental concepts of chemistry
0/18
Relative Atomic mass
Empirical formula and Molecular Formula
Combustion Analysis
Concept of mole
Avogadro’s number
Molar Volume
Stoichiometry
Limiting reactant
Percentage yield
Relative Atomic Mass
Empirical and Molecular Formula
Combustion Analysis
Concept of Mole
Avogadro's Number
Molar Volume
Test
check
Biological Molecules
Atomic Structure
Gases
Liquids
Solids
Chemical Equilibrium
Reaction Kinetics
Thermo-chemistry and Energetics of chemical reactions
Electrochemistry
Chemical bonding
S and p block elements
Transition Elements
Fundamental principles of organic chemistry
Chemistry of Hydrocarbons
Alkyl halides
Alcohols & phenols
Aldehydes and Ketones
Carboxylic acid
Macromolecules
MDCAT Chemistry Mastery
About Lesson

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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