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Stoichiometry

Stoichiometry


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What is stoichiometry? Definition:

stoichiometry refers to the theory of calculating or calculating the relative mass composition of reactants (starting materials) and products (resulting substances) in chemical reactions. In other words, stoichiometry is used in chemistry to understand chemical reactions in relation to the real proportions of the substances involved in the chemical reaction. The term stoichiometry is borrowed from the two Greek terms 'stoicheion' (= basic material) and 'metrein' (= measuring).

Stoichiometric laws:

The stoichiometry is essentially based on three basic laws, which are presented below.
Law of Conservation of the Earth (Lomonosov-Lavoisier Law):
Core sentence: "After a chemical reaction, the mass of the products still corresponds to the mass of the educts." In a chemical reaction, there is only a rearrangement or rearrangement of the atoms. During the reaction, however, no atoms form / disappear, so the mass remains the same.
Law of Constant Proportions (Proust's Law):
Core sentence: "The mass ratio of the elements of a particular chemical compound is always the same." The simplest example is the chemical compound of the water. A water molecule always consists of one oxygen atom and two hydrogen atoms.
Law of Multiple Proportions (Dalton's Law):
Core sentence: "The mass ratio of the elements of chemical compounds is always in an integer relationship to each other." This law is based on the law of constant proportions. Therefore, back to the water molecule example: In a glass with water, the ratio of hydrogen to oxygen is always 2: 1, since every water molecule consists of two hydrogen atoms and one oxygen atom.



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