Definition of Stoichiometry and Types of Stoichiometry
Definition of Stoikimetri
Definition of Stoichiometry and Types of Stoichiometry - Stoichiometry is a branch of chemistry that deals with a quantitative relationship that exists between reactants and products in chemical reactions. A reactant is a substance that participates in a chemical reaction, and also a product is a substance obtained as a result of a chemical reaction.
Stoichiometry
That stoichiometry depends on the fact that elements behave in ways that can or can be predicted, and also matter that cannot be created or destroyed.
Therefore, when the elements are combined then produce a chemical reaction, something that is known and also specific that will occur and the results of the reaction can be predicted based on the elements and also the amount involved. Stoichiometry is the mathematics behind chemistry.
The stoichiometry calculation can find out how the elements and also the components which are diluted in a solution whose concentration is known, react under experimental conditions. The word "Stoichiometry" is derived from the Greek word "stoicheion", meaning "element" and also "metron" means "size".
Law governing Stoichiometry.
Stoichiometry relies on laws such as the law of fixed comparison, the law of double comparison and also the law of conservation of mass.
The law of conservation of mass
By using physical laws such as the law of conservation of mass, which suggests that the reactant mass is the same as the mass of the product, Stoichiometry is used to gather information about the amount of various elements used in a chemical reaction.
The law of comparison is fixed
This law states that these chemical compounds (substances consisting of 2 (two) or more elements) which always contain the same proportion of an element (compounds with one type of atom) with mass.
The law of multiple comparisons
This law is one of the basic laws of stoichiometry, besides the fixed comparative law. Sometimes also called Dalton's law. It is said that, if 2 (two) elements form more than 1 compound between them, then the mass ratio of a second element that joins the fixed mass of the first two elements will have a ratio of a small amount of the whole.
Explanation of Stoichiometry
Based on the above laws, chemical reactions can be combined in a definite chemical ratio. The amount of each element must be the same in all reactions. In a balanced chemical reaction, the relationship between the amount of reactants and products will usually form an integer ratio. For example, in a reaction that forms ammonia (NH3), exactly 1 (one) nitrogen molecule (N2) reacts with 3 (three) hydrogen (H2) molecules to produce 2 NH3 molecules. This can be described as follows
N2 + 3H2 ——-> 2NH3
Thus, the Stoichiometry can be used to be able to calculate the amount is like the amount of product that can be produced if given a reactant and also the percentage of reactants made into a known product.
Stoichiometry type
Stoichiometry Reaction
Stoichiometry is often used to balance the chemical equations that can be found in reaction stoichiometry. This illustrates that the quantitative relationship between substances is caused by their participation in chemical reactions.
Stoichiometry Composition
The stoichiometry of this composition explains the quantitative (mass) relationship between an element in a compound. For example, the stoichiometry of the composition depicts the (mass) nitrogen with hydrogen that combines and becomes a complex ammonia. which is 1 mole of nitrogen and also 3 moles of hydrogen in each of 2 moles of ammonia. Mol is a unit used in chemistry for the amount of substances.
Gas Stoichiometry
The type of stoichiometry is related to a reaction involving a gas, which gas is at a temperature, pressure and also a volume that is known and can also be considered an ideal gas. For gases, the ideal volume ratio is the same as the ideal gas law, but the ratio of the mass of the single reaction must be calculated from the molecular mass of the reactants as well as the product, where the molecular mass is the mass of 1 (one) molecule of the substance.
The ideal gas is a theoretical gas consisting of 1 (one) set of randomly moving, non-interacting particles that obeys an ideal gas law. The ideal gas law is an equation of the ideal gas state. The ideal gas law equation is as follows:
"PV = nRT, where P is pressure, V is volume and T is absolute temperature, n is gas mole and R is universal gas constant".
Definition of the stoichiometric ratio
A number of stoichiometry or reagent ratios (substances added to a system in order to create a chemical reaction) is the amount or also the ratio which, assuming that the results of a reaction are finished on the basis, among others are as follows:
All reagents consumed
There is no reagent deficit
There are no residual residues
The reaction will only occur or be created at a stoichiometric ratio