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    Balancing Chemical Equations

    Uploaded by

    cedrick
    This document provides examples of how to balance chemical equations by adjusting coefficients. It explains that coefficients can only be changed and subscripts cannot be altered when balancing equations. The examples show balancing equations for reactions involving nitrogen, hydrogen, oxygen, chlorine

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    © All Rights Reserved
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    Balancing Chemical Equations

    Uploaded by

    cedrick
    99 views18 pages
    This document provides examples of how to balance chemical equations by adjusting coefficients. It explains that coefficients can only be changed and subscripts cannot be altered when balancing equations. The examples show balancing equations for reactions involving nitrogen, hydrogen, oxygen, chlorine

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    Original Title

    5.-Balancing-Chemical-Equations

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    This document provides examples of how to balance chemical equations by adjusting coefficients. It explains that coefficients can only be changed and subscripts cannot be altered when balancing equations. The examples show balancing equations for reactions involving nitrogen, hydrogen, oxygen, chlorine

    Copyright:

    © All Rights Reserved
    Download as PPT, PDF, TXT or read online from Scribd
    Download as ppt, pdf, or txt
    99 views18 pages

    Balancing Chemical Equations

    Uploaded by

    cedrick
    This document provides examples of how to balance chemical equations by adjusting coefficients. It explains that coefficients can only be changed and subscripts cannot be altered when balancing equations. The examples show balancing equations for reactions involving nitrogen, hydrogen, oxygen, chlorine

    Copyright:

    © All Rights Reserved
    Download as PPT, PDF, TXT or read online from Scribd
    Download as ppt, pdf, or txt
    of 18

    Chemical equation - Describes a chemical change.

    Parts of an equation:

    Reactant Product

    2Ag + H2S Ag2S + H2

    Reaction symbol
    Reactant - The chemical(s) you start with before the
    reaction.
     Written on left side of equation.
    Product - The new chemical(s) formed by the
    reaction.
     Right side of equation.
    Subscript - shows how many atoms of an element
    are in a molecule.
     EX: H2O
    2 atoms of hydrogen (H)
    1 atom of oxygen (O)
    Coefficient - shows how many molecules there are
    of a particular chemical.
     EX: 3 H2O
    Means there are 3 water molecules.
    2H2 + O2  2H2O
    In a chem. rxn, matter is neither created nor
    destroyed.
     In other words, the number and type of atoms going
    INTO a rxn must be the same as the number and type of
    atoms coming OUT.
    If an equation obeys the Law of Conservation, it is
    balanced.
    CH4 + O2  CO2 + H2O

    Reactant Side Product Side

    1 carbon atom 1 carbon atom


    4 hydrogen atoms 2 hydrogen atoms
    2 oxygen atoms 3 oxygen atoms
    A Balanced Equation

    CH4 + 2O2  CO2 + 2H2O

    Reactant Side Product Side

    1 carbon atom 1 carbon atom


    4 hydrogen atoms 4 hydrogen atoms
    4 oxygen atoms 4 oxygen atoms
    1. Matter cannot be created or destroyed.
    2. Subscripts cannot be added, removed, or changed.
    3. You can only change coefficients.
    4. Coefficients can only go in front of chem.
    formulas...NEVER in the middle of a formula.
    A few extra tips:
    Try balancing big formulas first; save free elements for last.
    If the same polyatomic ion appears on both sides of the
    equation, it’s usually okay to treat it as one unit.
    There is no one particular way to balance equations. Some
    equations are harder to balance than others and might require
    some creativity to solve.
    Balance the following equation by adjusting
    coefficients.

    N2 + 3 H2  2NH3

    reactants products

    N 2 21
    H 6
    2 63
    Balance the following equation by adjusting
    coefficients.

    2 KClO3  2 KCl + 3O2


    reactants products

    K 1
    2 12
    Cl 1
    2 1
    2
    O 3
    6 2
    6
    Balance the following equation:
    2 C2H6 + 7O2  4CO2 + 6H2O
    Balance the following equation:
     4 Fe +3 O2  2 Fe2O3
    1. Synthesis or Combination
    Reaction
    2. Analysis or Decomposition
    Reactions
    3. Single Replacement Reactions
    4. Double Replacement Reactions
    1. Synthesis or
    Combination Reaction

    A+B AB
    1. Fe + S Fe S2
    Fe + 2 S Fe S2
    2. S + O 2 SO
    2 S + O2 2 SO
    AB A+ B
    Examples:
    Hg O Hg + O2
    2 Hg O 2 Hg + O2
    CaCo3 Ca O + Co2
    Identify what type of Chemical Reaction is present
    in each Equation and Balance it.
    1.Na + Cl2 Na Cl
    2.N2 + O2 NO
    3.KClO3 K Cl + O2
    4.H2O2 H2O + O2
    5.KNO3 KNO2 + O2

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