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General Chemistry: Chemical Reactions and Stoichiometry

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이 집합의 용어 (20)

  • Empirical Formula

    The simplest whole-number ratio of atoms in a compound, derived from mass percentages using moles.

  • Molecular Formula

    Gives the actual number of atoms of each element in a compound, which is a multiple of the empirical formula.

  • Steps to Calculate Empirical Formula
    1. Write down mass or % of each element.
    2. Convert masses to grams (assume 100 g if % given).
    3. Convert grams to moles.
    4. Divide moles by smallest mole value.
    5. Adjust to whole numbers by rounding or multiplying.
  • Determining Molecular Formula
    1. Find empirical formula.
    2. Calculate empirical formula mass.
    3. Divide molar mass by empirical mass to find n-factor.
    4. Multiply empirical formula subscripts by n-factor.
  • Combustion Analysis Purpose

    Used to determine the empirical formula of compounds by burning them and analyzing the products CO2 and H2O.

  • Combustion Analysis Steps for Hydrocarbons
    1. Convert CO2 mass to C mass.
    2. Convert H2O mass to H mass.
    3. Subtract C and H masses from total to find O mass if present.
    4. Convert all masses to moles.
    5. Divide by smallest mole value and adjust to whole numbers.
  • Combustion Analysis for Non-Hydrocarbons

    Includes elements like N, S, halogens; products may include gases like NO, SO2, or halogen gases.

  • Balancing Chemical Equations

    Ensure the number of atoms of each element is equal on both sides using stoichiometric coefficients. Multiply to clear fractions.

  • Stoichiometry

    Quantitative relationship between reactants and products in a balanced chemical equation, used to calculate amounts of substances.

  • Limiting Reagent

    The reactant that is completely consumed first, limiting the amount of product formed.

  • Excess Reagent

    The reactant that remains after the limiting reagent is used up.

  • Theoretical Yield

    The maximum amount of product predicted from stoichiometric calculations assuming complete reaction.

  • Actual Yield

    The amount of product actually obtained from an experiment, usually less than theoretical yield.

  • Percent Yield Formula

    \(\text{Percent Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\%\)

  • Mass Percent Composition

    Percentage by mass of an element in a compound calculated as \(\frac{\text{mass of element}}{\text{mass of compound}} \times 100\%\).

  • Functional Group

    Part of a molecule responsible for its characteristic chemical reactions and properties.

  • Hydrocarbons

    Compounds containing only carbon and hydrogen atoms.

  • Functional Groups without Carbonyl

    Groups containing atoms like -OH, -NH2, -X (halogens), -SH but no carbonyl (C=O).

  • Functional Groups with Carbonyl

    Groups containing a carbonyl group (C=O), such as aldehydes, ketones, carboxylic acids, esters, and amides.

  • Combustion Apparatus Chambers
    • Chamber A: Vaporizes sample.
    • Chamber B: Converts H to H2O and nonmetals to gases.
    • Chamber C: Traps water.
    • Chamber D: Traps gases.