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	~~'''~~Stoichiometry~~''' is a branch of [[Chemistry\|chemistry]] that deals with the quantitative relationships that exist among the reactants and products in [[Chemical reactions\|chemical reactions]].~~		== Stoichiometry ==

	~~== Overview ==~~		[[File:Combustion_reaction_of_methane.jpg\|thumb\|right\|Combustion reaction of methane]]
	Stoichiometry is derived from the Greek words ''stoicheion'' meaning "element" and ''metron'' meaning "measure". It is a calculation used to determine the amount of reactants needed or products formed in a chemical reaction. It is based on the [[~~Law of Conservation of Mass~~\|~~law of conservation of mass]] and the [[Law of Definite Proportions~~\|~~law~~ of ~~definite proportions~~]].

	~~== Principles ==~~		'''Stoichiometry''' is a branch of [[chemistry]] that deals with the quantitative relationships between the amounts of reactants and products in a chemical reaction. It is based on the [[law of conservation of mass]], which states that matter is neither created nor destroyed in a chemical reaction. Stoichiometry allows chemists to predict the quantities of substances consumed and produced in a given reaction.
	Stoichiometry is based on ~~several principles:~~

	* '''[[Law of Conservation of Mass]]''': This law states that matter cannot be created or destroyed in a chemical reaction. Therefore, the total mass of the reactants must equal the total mass of the products.		== Basic Concepts ==

	* '''[[Law of Definite Proportions]]''': ~~This law states that a chemical compound always contains the same elements in the same proportions by mass.~~		Stoichiometry involves several key concepts, including:

	* '''[[Law of Multiple Proportions]]''': This law states that when two elements combine to form more than one compound, the ratios of the masses of the second element that combine with a fixed mass of the first element are small whole numbers.		=== Mole Concept ===

	~~== Applications ==~~		The [[mole (unit)\|mole]] is a fundamental unit in chemistry that represents a specific number of particles, usually atoms or molecules. One mole is defined as exactly 6.022 x 10^23 particles, known as [[Avogadro's number]]. The mole allows chemists to convert between the mass of a substance and the number of particles it contains.
	~~Stoichiometry~~ is ~~used~~ in ~~many areas~~ of ~~chemistry~~ and ~~chemical engineering~~. ~~Some of its applications include:~~

	* '''[[Chemical ~~synthesis]]''': Stoichiometry is used to determine the quantities of reactants needed to produce a desired amount of product.~~		=== Balanced Chemical Equations ===

	* '''[[~~Chemical analysis~~]]~~''': Stoichiometry is used to determine~~ the ~~composition~~ of ~~a sample by analyzing~~ the ~~amounts~~ of ~~its constituent elements~~.		A [[chemical equation]] represents a chemical reaction using symbols and formulas. A balanced chemical equation has the same number of each type of atom on both sides of the equation, reflecting the conservation of mass. Balancing chemical equations is a crucial step in stoichiometry.

	* '''[[Chemical reactions\|Reaction prediction]]''': Stoichiometry is used to predict the amounts of products that will be formed in a chemical reaction.		=== Molar Ratios ===

	== ~~See also~~ ==		Molar ratios are derived from the coefficients of a balanced chemical equation. They indicate the proportions of reactants and products involved in the reaction. These ratios are used to calculate the amounts of substances consumed or produced.

			== Stoichiometric Calculations ==

			Stoichiometric calculations involve using the balanced chemical equation to determine the quantities of reactants and products. The steps typically include:

			1. '''Writing and Balancing the Chemical Equation''': Ensure the chemical equation is balanced.
			2. '''Converting Mass to Moles''': Use the molar mass of substances to convert between mass and moles.
			3. '''Using Molar Ratios''': Apply the molar ratios from the balanced equation to find the moles of other substances.
			4. '''Converting Moles to Mass''': Convert moles back to mass if needed.

			== Example: Combustion of Methane ==

			The combustion of [[methane]] is a common example used to illustrate stoichiometry. The balanced chemical equation for the combustion of methane is:

			\[
			\text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O}
			\]

			In this reaction, one mole of methane reacts with two moles of oxygen to produce one mole of carbon dioxide and two moles of water. Using stoichiometry, one can calculate the amount of oxygen needed to completely combust a given amount of methane, or the amount of carbon dioxide produced.

			== Related Pages ==

			* [[Chemical reaction]]
			* [[Mole (unit)]]
			* [[Avogadro's number]]
	* [[Chemical equation]]		* [[Chemical equation]]
	* [[~~Mole (unit)]]~~		* [[Conservation of mass]]
	* [[Chemical formula]]
	* [[Chemical reaction]]
	* [[Chemical compound]]

	~~== References ==~~		{{Chemistry}}
	~~<references />~~

	[[Category:Chemistry]]		[[Category:Chemistry]]
	~~[[Category:Chemical reactions]]~~
	~~[[Category:Chemical engineering]]~~
	~~[[Category:Chemical synthesis]]~~
	~~[[Category:Chemical analysis]]~~

	~~{{stub}}~~

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'''Stoichiometry''' is a branch of [[Chemistry|chemistry]] that deals with the quantitative relationships that exist among the reactants and products in [[Chemical reactions|chemical reactions]].

== Overview ==
Stoichiometry is derived from the Greek words ''stoicheion'' meaning "element" and ''metron'' meaning "measure". It is a calculation used to determine the amount of reactants needed or products formed in a chemical reaction. It is based on the [[Law of Conservation of Mass|law of conservation of mass]] and the [[Law of Definite Proportions|law of definite proportions]].

== Principles ==
Stoichiometry is based on several principles:

* '''[[Law of Conservation of Mass]]''': This law states that matter cannot be created or destroyed in a chemical reaction. Therefore, the total mass of the reactants must equal the total mass of the products.

* '''[[Law of Definite Proportions]]''': This law states that a chemical compound always contains the same elements in the same proportions by mass.

* '''[[Law of Multiple Proportions]]''': This law states that when two elements combine to form more than one compound, the ratios of the masses of the second element that combine with a fixed mass of the first element are small whole numbers.

== Applications ==
Stoichiometry is used in many areas of chemistry and chemical engineering. Some of its applications include:

* '''[[Chemical synthesis]]''': Stoichiometry is used to determine the quantities of reactants needed to produce a desired amount of product.

* '''[[Chemical analysis]]''': Stoichiometry is used to determine the composition of a sample by analyzing the amounts of its constituent elements.

* '''[[Chemical reactions|Reaction prediction]]''': Stoichiometry is used to predict the amounts of products that will be formed in a chemical reaction.

== See also ==
* [[Chemical equation]]
* [[Mole (unit)]]
* [[Chemical formula]]
* [[Chemical reaction]]
* [[Chemical compound]]

== References ==
<references />

[[Category:Chemistry]]
[[Category:Chemical reactions]]
[[Category:Chemical engineering]]
[[Category:Chemical synthesis]]
[[Category:Chemical analysis]]

{{stub}}

Stoichiometry - Revision history

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