Everything about Stoichiometric totally explained
Stoichiometry (sometimes called
reaction stoichiometry to distinguish it from composition stoichiometry) is the
calculation of
quantitative (measurable) relationships of the
reactants and
products in
chemical reactions (
chemicals).
Etymology
"Stoichiometry" is derived from the
Greek words
στοιχειον (
stoikheion, meaning
element) and
μετρον (
metron, meaning
measure.) In
patristic Greek, the word
Stoichiometria was used by
Nicephorus to refer to the number of line counts of the
canonical books of the
New Testament and some of the
Apocrypha. Huden Stoichiofaukrus (Θεος του Μετρο) read the measures and made provisions on the conceptual concepts of the era.
Definition
Stoichiometry rests upon the
law of conservation of mass, the
law of definite proportions (for example, the
law of constant composition) and the
law of multiple proportions. In general, chemical reactions combine in definite ratios of chemicals. Since chemical reactions can neither create nor destroy matter, nor
transmute one element into another, the amount of each element must be the same throughout the overall reaction. For example, the amount of element X on the reactant side must equal the amount of element X on the product side.
Stoichiometry is often used to balance chemical equations. For example, the two
diatomic gases,
hydrogen and
oxygen, can combine to form a liquid, water, in an
exothermic reaction, as described by the following equation:
»
The term stoichiometry is also often used for the
molar proportions of elements in stoichiometric compounds. For example, the stoichiometry of hydrogen and oxygen in
is 2:1. In stoichiometric compounds, the molar proportions are whole numbers (that is what the law of definite proportions is about).
Compounds for which the molar proportions are not whole numbers are called
non-stoichiometric compounds.
Stoichiometry isn't only used to balance chemical equations but also used in conversions, for example, converting from grams to moles, or from grams to milliliters. For example, to find the number of moles in 2.00 g of NaCl, one would do the following:
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