Stoichiometry

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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 (chemical equations).

1 Etymology
2 Definition
3 Different stoichiometries in competing reactions
4 Stoichiometric air-fuel ratios of common fuels
5 See also
6 External links

[edit] Etymology

"Stoichiometry" derives from the Greek words stoikheion ("element") and metriā ("measure," from metron). 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.

[edit] Definition

Stoichiometry rests upon the law of conservation of mass, the law of definite proportions (i.e., the law of constant composition) and the law of multiple proportions. In general, chemical reactions will combine in definite ratios of chemicals. Since matter cannot be created or destroyed, 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 Equation A.

(A) H₂ + O₂ → H₂O

Equation A does not depict the proper stoichiometry of the reaction—that is, it does not reflect the relative proportions of the reactants and products.

(B) 2H₂ + O₂ → 2H₂O

Equation B does have proper stoichiometry and is therefore said to be a "balanced" equation, depicting the same number of atoms of each type on each side of the equation. There are four H on the reactant side and 4 H on the product side and there are 2 O on both sides as well; mass has been conserved.

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 H₂O is 2:1. In stoichiometric compounds, the molar proportions are whole numbers (that is what the law of multiple proportions is about).

Compounds for which the molar proportions are not whole numbers are called non-stoichiometric compounds.

Stoichiometry is used not only to balance chemical equations but also is used in conversions—i.e. converting from grams to moles, or from grams to milliliters. For example, if there were 2.00 g of NaCl, to find the number of moles, one would do the following:

$\rm{} \frac{2.00 \ g \ NaCl}{58.44 \ g \ NaCl \ mol^{-1}} = 0.034 \ mol$

In the above example, when written out in fraction form, the units of grams cancels out, leaving one with the amount of moles (the unit that was needed), as shown in the following equation:

$\rm{}\left(\frac{2.00 \ g \ NaCl}{1}\right)\left(\frac{1 \ mol \ NaCl}{58.44 \ g \ NaCl}\right) = .034223135\ mol$ Stoichiometry is also used to find the right amount of reactants to use in a chemical reaction. An example is shown below using the Thermite reaction:

Fe₂O₃ + 2Al → Al₂O₃ + 2Fe

So, to completely react with 85.0 grams of Iron (III) oxide, 28.7 grams of Aluminum are needed.

[edit] Different stoichiometries in competing reactions

Often, more than one reaction is possible given the same starting materials. The reactions may differ in their stoichiometry. For example, the methylation of benzene (C₆H₆) may produce singly-methylated (A), doubly-methylated (B), or still more highly-methylated products (C):

(A) C₆H₆ + CH₃Cl → C₆H₅CH₃ + HCl

(B) C₆H₆ + 2CH₃Cl → C₆H₄(CH₃)₂ + 2HCl