reaction stoichiometry

(noun)

Describes the quantitative relationship between reactants and products within a given chemical reaction.

Related Terms

Examples of reaction stoichiometry in the following topics:

  • Reaction Stoichiometry

    • Reaction stoichiometry studies the quantitative relationships between reactants and products within a given chemical reaction.
    • Stoichiometry is a branch of chemistry that deals with the relative quantities of reactants and products that are consumed/produced within a given chemical reaction.
    • From this brief description, we can see that stoichiometry has many important applications.
    • Stoichiometry can also be used to make useful determinations about limiting reactants, and to calculate the amount of excess reactant(s) left over after a given reaction has run to completion.
    • The science of stoichiometry is possible because it rests upon the law of conservation of mass.

  • Gas Stoichiometry

    • Stoichiometry is the quantitative study of the relative amounts of reactants and products in chemical reactions; gas stoichiometry involves chemical reactions that produce gases.
    • According to the above reaction, what volume of NO2(g) is produced from the combustion of 100 g of NH3(g), assuming the reaction takes place at standard temperature and pressure?
    • Because we are told that the reaction takes place at STP, we can relate volume, 22.4 L, to 1 mol NO2.
    • Shows how to use stoichiometry to convert from grams of a gas to liters of a gas.
    • Calculate volumes of gases consumed/produced in a reaction using gas stoichiometry.

  • Amount of Reactants and Products

    • Stoichiometry is the study of the relative quantities of reactants and products in chemical reactions and how to calculate those quantities.
    • Stoichiometry is the field of chemistry that is concerned with the relative quantities of reactants and products in chemical reactions.
    • In addition, stoichiometry can be used to find quantities such as the amount of products that can be produced with a given amount of reactants and percent yield.
    • Reaction stoichiometry describes the quantitative relationship among substances as they participate in various chemical reactions.
    • Reactions are balanced by adding coefficients so that there are the same number of atoms of each element on both sides of the reaction.

  • Solution Stoichiometry

    • Stoichiometry can be used to calculate the quantitative relationships between species in aqueous solution.
    • We can perform stoichiometric calculations for aqueous phase reactions just as we can for reactions in solid, liquid, or gas phases.
    • What is the mass of AgCl(s) formed in the precipitation reaction?
    • The next step, as in any calculation involving stoichiometry, is to determine our limiting reactant.
    • Stoichiometry deals with the relative quantities of reactants and products in chemical reactions.

  • Mole-to-Mole Conversions

    • A chemical equation is a visual representation of a chemical reaction.
    • To do this correctly, the reaction needs to be balanced.
    • The key is reaction stoichoimetry, which describes the quantitative relationship among the substances as they participate in the chemical reaction.
    • Each stoichiometric conversion factor is reaction-specific and requires that the reaction be balanced.
    • Therefore, each reaction must be balanced before starting calculations.

  • The Rate Law

    • The rate law for a chemical reaction relates the reaction rate with the concentrations or partial pressures of the reactants.
    • For the general reaction$aA + bB \rightarrow C$ with no intermediate steps in its reaction mechanism, meaning that it is an elementary reaction, the rate law is given by:
    • A smaller rate constant indicates a slower reaction, while a larger rate constant indicates a faster reaction.
    • What is the reaction order?
    • Note that the reaction order is unrelated to the stoichiometry of the reactions; it must be determined experimentally.

  • Overall Reaction Rate Laws

    • Rate laws for reactions are affected by the position of the rate-determining step in the overall reaction mechanism.
    • As discussed in the previous concept, if the first step in a reaction mechanism is the slow, rate-determining step, then the overall rate law for the reaction is easy to write, and simply follows the stoichiometry of the initial step.
    • Consider the following reaction:
    • At equilibrium, the rate of the forward reaction will equal the rate of the reverse reaction.
    • Combine elementary reaction rate constants to obtain equilibrium coefficients and construct overall reaction rate laws for reactions with both slow and fast initial steps

  • Strong Acid-Strong Base Titrations

    • Using the stoichiometry of the reaction, the unknown concentration can be determined.
    • It makes use of the neutralization reaction that occurs between acids and bases and the knowledge of how acids and bases will react if their formulas are known.
    • The other reactant of known concentration remains in a burette to be delivered during the reaction.
    • Neutralization is the reaction between an acid and a base, producing a salt and neutralized base.
    • Step 2: Use stoichiometry to figure out the moles of HCl in the analyte.

  • Limiting Reagents

    • From stoichiometry, the exact amount of reactant needed to react with another element can be calculated.
    • Then use stoichiometry to calculate the mass of the product that could be produced for each individual reactant.
    • STOICHIOMETRY - Limiting Reactant & Excess Reactant Stoichiometry & Moles - YouTube
    • A video showing two examples of how to solve limiting reactant stoichiometry problems.
    • The limiting reagent in a reaction is the first to be completely used up and prevents any further reaction from occurring.

  • Electrolysis Stoichiometry