"Stoichiometry is the relationship between the quantities of reactants and products before, during, and following chemical reactions."
The quantitative relationships among the reactants and products in a chemical reaction.
Balancing Chemical Equations: This topic deals with the process of adjusting the coefficients in a chemical equation in order to ensure that the same number of atoms of each element is present on both sides of the equation.
Mole Concept: Mole concept deals with the relationship between masses and molar amounts of different substances. It is crucial for understanding how to use the stoichiometry of a reaction to calculate reaction products or reactants.
Limiting Reactants: This concept involves identifying the reactant in a chemical reaction that is entirely used up when the reaction is completed. It is essential for calculating the yield of products and understanding how much of each reactant is required to produce a given amount of product.
Percent Yield: Percent yield is a measure of the completeness of a chemical reaction. It is calculated by dividing the actual yield of a reaction by the theoretical yield and expressing this value as a percentage.
Stoichiometric Calculations: This involves using the principles of stoichiometry to calculate the amount of product formed or reactant consumed in a chemical reaction.
Gas Stoichiometry: This topic involves understanding how to use the concepts of stoichiometry to calculate the pressure, volume, or number of moles of a gas in a chemical reaction.
Solution Stoichiometry: This concept deals with the calculation of concentrations of reactants and products in a chemical reaction, often in the context of aqueous solutions.
Empirical and Molecular Formulas: These formulas are used to represent the chemical composition of a substance, with empirical formulas representing the simplest whole-number ratio of atoms in a compound, and molecular formulas representing the actual number of atoms in a compound.
Reaction Energy: This involves understanding the energy changes that occur during chemical reactions, including exothermic and endothermic reactions, as well as the principles of enthalpy and entropy.
Reaction Rates: This involves understanding the factors that influence the rate of a chemical reaction, including temperature, concentration, and catalysts. The principles of reaction kinetics are also important in this topic.
Combination Reactions: In a combination reaction, two or more reactants combine to form one product. The general form of a combination reaction is A + B → AB.
Decomposition Reactions: In a decomposition reaction, one reactant breaks down into two or more products. The general form of a decomposition reaction is AB → A + B.
Single Displacement Reactions: In a single displacement reaction, one element or ion in a compound is replaced by another element or ion. The general form of a single displacement reaction is A + BC → AC + B or B + AC → BC + A.
Double Displacement Reactions: In a double displacement reaction, two compounds exchange ions to form two new compounds. The general form of a double displacement reaction is AB + CD → AD + CB.
Combustion Reactions: In a combustion reaction, a substance reacts with oxygen to produce heat and light. The general form of a combustion reaction is fuel + oxygen → carbon dioxide + water + energy.
Redox Reactions: In a redox reaction, there is a transfer of electrons between species. Oxidation is the loss of electrons, and reduction is the gain of electrons.
Acid-Base Reactions: In an acid-base reaction, an acid reacts with a base to produce a salt and water. The general form of an acid-base reaction is acid + base → salt + water.
Precipitation Reactions: In a precipitation reaction, two aqueous solutions react to form a solid precipitate that falls out of solution. The general form of a precipitation reaction is A + B → AB (s).
"Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products, leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers."
"This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated."
"If one reactant has a known quantity and the quantity of the products can be empirically determined, then the amount of the other reactants can also be calculated."
"CH4 + 2 O2 → CO2 + 2 H2O"
"one molecule of methane reacts with two molecules of oxygen gas"
"This particular chemical equation is an example of complete combustion."
"Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry."
"Stoichiometry measures these quantitative relationships and is used to determine the amount of products and reactants that are produced or needed in a given reaction."
"Because of the well-known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry."
"Gas stoichiometry deals with reactions involving gases."
"Where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases."
"For gases, the volume ratio is ideally the same by the ideal gas law."
"But the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products."
"In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio."
Yes, stoichiometry can be applied to any chemical reaction, not only reactions involving gases.
"Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products."
"The main goal of stoichiometry is to determine the quantities of reactants and products involved in a chemical reaction."
"The relations among quantities of reactants and products typically form a ratio of positive integers."
"Stoichiometry measures these quantitative relationships and is used to determine the amount of products and reactants that are produced or needed in a given reaction."