"Stoichiometry is the relationship between the quantities of reactants and products before, during, and following chemical reactions."
This topic covers the quantitative study of reactions, including balancing chemical equations, mole ratios, and limiting reactants.
Mole concept: Understanding the concept of moles, Avogadro's number, and its significance in chemical calculations.
Chemical Equations: Understanding how to balance chemical equations, identifying reactants and products, and their stoichiometric coefficients.
Limiting Reagents: Understanding how to identify and work with the limiting reagent, calculating theoretical and actual yields, and percentage yield.
Molarity and concentration: Understanding how to calculate molarity and concentration of solutions, dilutions, and electrochemistry problems.
Gas stoichiometry: Understanding how to work with gases, gas laws and their applications, including ideal gas equation, Dalton's law of partial pressure, and the gas constant.
Thermochemistry: Understanding enthalpy, heat, and calorimetry, including the calculation of heat exchanged or absorbed, Hess's law, and standard enthalpy of formation and reaction.
Acid-base stoichiometry: Understanding how to work with acidic and basic solutions, identifying the acid and base, calculating pH, and balancing acid-base reactions.
Redox stoichiometry: Understanding how to work with oxidation-reduction reactions, balancing redox equations, and identifying oxidizing and reducing agents.
"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."