The Chemistry Book

Balancing equations involves understanding the law of conservation of matter. The law of the conservation of matter (or mass) is a law stating that the quantity of matter during an ordinary chemical change will remain constant ^[1]. In a chemical reaction, matter is neither created nor destroyed. Balancing Chemical Equations is the principle of balancing the atom which is conserves in a chemical reactions. Atoms are neither created nor destroyed, just arranged in a different manner. The same number of each atom is found among the reactants and the products. ^[2]

Chemical equations

Many chemical equations designate the conditions necessary (such as high temperature) for the reaction to occur. A chemical equation provides quantitative information about a chemical reaction, but only if it is balanced.^[3] The first step to making a balance equation is to identify reactants and products. When balancing equations the numbers must be placed carefully where the numbers belong. All of the equations and materials rework are produced by natural gas and oxygen gas are combined and burned. ^[4] Whenever a chemist thinks something is wrong a trial and error inspection come into place. The equations are unusually unbalanced on both sides on a row going side to side.

Coefficients are a major key to balancing any kind of equations. Without coefficients the process could not be accomplished. An example of the process would be, 2H(g) + O2(g) 2HO(1),in the example the same numbers of hydrogen and oxygen atoms are present and the numbers have simplified so the equation stays as shown. ^[5] The first step is to read the description then find the products, reactants and the states. In the unbalanced equation, sum up all the information from step 1. Figure out what coefficients are necessary to make the equation in the proper order, to make the equation balanced out.

Over Look

At the beginning, balancing euqations can be confusing if you don't know the step. So that's why you must first read the section or chapter about balancing equations. Then when you understand how to balance then you're ready to work on balancing equations. Most people look at an equation san say "Oh its too hard, I can't do this" when you haven't een tried it. Balancing equtions can be fun oncve y ou know the fundamentalks to balancing equations.Also remember that in order to do anything you must haverge eperiodic table memorized.It will be very helpful.

The first step in balancing an equation is to write a skeleton equation. This equation represents the reactants and products by chemical formulas and the states of matter.

Note. When balancing equations, you should keep in mind the 7 diatomic molecules we learned in class, in case you come across them. When you see one of these elements in an equation by themselves, you should write them out with a subscript 2. For example: Lithium Bromide should be written as LiBr₂

Example

(from class worksheet. BALANCING CHEMICAL EQUATIONS, pg. 58)

unbalanced equation: KClO₃ → KCl + O₂

balanced equation: 2KClO₃ → 2KCl + 3O₂
All you have to basically do is: make sure both sides have the same number of atoms.

Student Questions

What is a coefficient?

Coefficients are the numbers in front of a formula. In a chemical equation, the coefficients indicate the amount of the substance involved in the chemical reaction.

Is the state of matter in a chemical equation of any importance when balancing an equation?

No, it is not, the subscripts (the number of atoms) is everything that matters

Common Misconceptions

Students often try to change the entire chemical equation when balancing an equation, everything you have to do is change the coefficients, in order for both sides (the reactants and products) to be balanced.

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Balancing equations practice problems

See also

Definition: Chemical Reactions

Chemical reactions are a process in which one or more substances are changed into others. ^[6]

Evidence of a Chemical Reaction

Chemical reactions often give visual clues such as color changes, a solid forms, bubbles are produced, and a flame occurs. ^[7] Chemical reactions are not always visible but they sometimes give you signals by a change of temperature. If heat or a flame is produce or the heat is absorbed, that is a signal that a chemical reaction has occurred. There are many physical changes that can be confused with chemical changes. For example, boiling water or freezing water results in many changes in the properties of water, but those are physical changes, not chemical ones. But whether water is liquid, solid or a gas, it is still water, and that is why it is a physical rather than chemical change. The most common method is to use analytical chemical technique to verify the presence of the product molecules, or the disappearance of reactant molecules. ^[8]

 Ex. Rusty Nails: A chemical reaction between the iron in steel and oxygen in  the atmosphere causes rust.

Chemical Equations

A chemical equation is a representation of a chemical reaction in which the chemicals present before the reaction called reactants, shown on the left of an arrow and the chemicals formed by the reaction called the product, shown on the right of the arrow. ^[9]. The arrow indicates the direction of change

  Ex.  Al + O  →  AlO 
      Reactants  Product

The “+” is read as “reacts with” and the arrow means “produces”. ^[10]. Chemical equations also contain coefficients which are the whole numbers to the left of the element

Types of Chemical Reactions

• Single Dispalcement Reaction

In a single replacement reaction a single uncombined element replaces another in a compound. Two reactants yield two products. ^[11].

A + BC → AC + B

• Double Displacement Reaction

In a double replacement reaction parts of two compounds switch places to form two new compounds. Two reactants yield two products. ^[12].

AB + CD → AD + CB  

• Synthesis Reaction

In a synthesis reaction two or more simple substances combine to form a more complex substance. Two or more reactants yielding one product is another way to identify a synthesis reaction. ^[13]

A + B → AB

• Decomposition Reaction

In a decomposition reaction a more complex substance breaks down into its more simple parts. One reactant yields 2 or more products. Basically, synthesis and decomposition reactions are opposites. ^[14]

AB → A + B

• Combustion

A combustion reaction involves oxygen and produces heat so rapidly that a flame results. This reaction occurs between certain compounds, especially organic compounds, oxygen, and hydrocarbons, which are carbon and hydrogen attached. The products of this reaction include carbon dioxide and water. ^[15]

C(x)H(x)+O → 2H2O(g)+CO2(g)

Balancing Equations

The principle to understanding the balancing process of a chemical equation is that atoms are conserved in a chemical reaction. ^[16]. This principle means that an atom can neither be created or destroyed. When balancing chemical equations, the same number of the atom should be found in the reactants and the product. Subscripts in a chemical equation cannot be changed to make the equation equal on both sides, the coefficient is the only number that can be changed to make the reactants and product equal.

   Ex.  SnO₂ + H₂ → Sn + H₂O

See also

Physical changes are the changes in which the original substance hasn't been chemically altered. Physical changes pertain to changes of energy and states of matter; the substance has only changed form. ^[17] This change does not produce a new substance; it merely changes the distance between particles.

References

Popular Articles	Newest Articles	Latest Scientists
Periodic Table Elements Scientific Method History of Chemistry Classification of Matter Math Skills Chemical Bonds Polyatomics Bohr Model	Molality Learning chemistry Nuclear decay Photoelectric effect Acids Solute Specific heat Catalyst Duet rule Octet rule	Henry Moseley Jean Baptiste Perrin Evangelista Torricelli Antoine Lavoisier Clemens Winkler Henri Becquerel Friedrich Wöhler Henri Louis Le Chatelier Josiah Willard Gibbs Benjamin Thompson

Latest Article Edits on Wiki

Molar Mass Uncertainty Scientific notation Measurements Tools Lab safety Scientific Method Instructors SI Units Heiny SI Units Base Ellis Chemistry Labs Ellis Handouts Ellis Physics Labs Ellis Ellis Physics Course Outline Ellis Chemistry Course Outline Candle Activity Getting organized Composition book Labs Video Lab 001 Stockdale Course Syllabus Ellis Notebook Pages Chemistry Policies Learning chemistry Why learn chemistry Electron configurations Inorganic nomenclature

Further Reading

• http://richardbowles.tripod.com/chemistry/balance.htm
• http://www.webqc.org/balance.php
• http://www.visionlearning.com/library/module_viewer.php?mid=56
• http://library.thinkquest.org/10429/low/balequa/balequa.htm
• http://dwb4.unl.edu/calculators/activities/BalEqn.html
• http://www.educationsoft.net/chemical_equation_expert/index.html
• http://www.sky-web.net/science/balancing_chemical_equations.htm
• http://www.ehow.com/how_2222284_balance-chemical-equations-using-fun.html

References

Popular Articles	Newest Articles	Latest Scientists
Periodic Table Elements Scientific Method History of Chemistry Classification of Matter Math Skills Chemical Bonds Polyatomics Bohr Model	Molality Learning chemistry Nuclear decay Photoelectric effect Acids Solute Specific heat Catalyst Duet rule Octet rule	Henry Moseley Jean Baptiste Perrin Evangelista Torricelli Antoine Lavoisier Clemens Winkler Henri Becquerel Friedrich Wöhler Henri Louis Le Chatelier Josiah Willard Gibbs Benjamin Thompson

Latest Article Edits on Wiki

Molar Mass Uncertainty Scientific notation Measurements Tools Lab safety Scientific Method Instructors SI Units Heiny SI Units Base Ellis Chemistry Labs Ellis Handouts Ellis Physics Labs Ellis Ellis Physics Course Outline Ellis Chemistry Course Outline Candle Activity Getting organized Composition book Labs Video Lab 001 Stockdale Course Syllabus Ellis Notebook Pages Chemistry Policies Learning chemistry Why learn chemistry Electron configurations Inorganic nomenclature