A chemical equation is a symbolic representation of a chemical reaction. ^{[1]} The coefficients next to the symbols and formulae of entities are the absolute values of the stoichiometric numbers. The first chemical equation was diagrammed by Jean Beguin in 1615. For other uses, see Chemical reaction (disambiguation). ...
In a chemical reaction system the stoichiometric coefficient of the ith component is defined as or where Ni is the number of molecules of i and Î¾ is the progress variable or extent of reaction. ...
Jean Beguin (15501620) was an iatrochemist noted for his 1610 Tyrocinium Chymicum (Beginners Chemistry), which many consider to be one of the first chemistry textbooks. ...
Balancing chemical equations
In a chemical reaction, the quantity of each element does not change. Thus, each side of the equation must represent the same quantity of any particular element. Also in case of net ionic reactions the same charge must be present on both sides of the hiddly unbalanced equation, one may balance it by changing the scalar number for each molecular formula. For other uses, see Chemical reaction (disambiguation). ...
A chemical formula (also called molecular formula) is a concise way of expressing information about the atoms that constitute a particular chemical compound. ...
Simple chemical equations can be balanced by inspection, that is, by trial and error. Generally, it is best to balance the most complicated molecule first. Hydrogen and oxygen are usually balanced last. Ex #1. Na + O_{2} → Na_{2}O In order for this equation to be balanced, there must be an equal amount of Na on the left hand side as on the right hand side. As it stands now, there is 1 Na on the left but 2 Na's on the right. This problem is solved by putting a 2 in front of the Na on the left hand side:  2Na + O_{2} → Na_{2}O
In this there are 2 Na atoms on the left and 2 Na atoms on the right. In the next step the oxygen atoms are balanced as well. On the left hand side there are 2 O atoms and the right hand side only has one. This is still an unbalanced equation. To fix this a 2 is added in front of the Na_{2}O on the right hand side. Now the equation reads:  2Na + O_{2} → 2Na_{2}O
Notice that the 2 on the right hand side is "distributed" to both the Na_{2} and the O. Currently the left hand side of the equation has 2 Na atoms and 2 O atoms. The right hand side has 4 Na's total and 2 O's. Again, this is a problem, there must be an equal amount of each chemical on both sides. To fix this 2 more Na's are added on the left side. The equation will now look like this:  4Na + O_{2} → 2Na_{2}POOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOOO Stain
This equation is a balanced equation because there is an equal number of atoms of each element on the left and right hand sides of the equation. Ex #2. This equation is not balanced because there is an unequal amount of O's on both sides of the equation. The left hand side has 4 P's and the right hand side has 4 P's. So the P atoms are balanced. The left hand side has 2 O's and the right hand side has 10 O's.  P_{4} + O_{2} → 2P_{2}O_{5}
To fix this unbalanced equation a 5 in front of the O_{2} on the left hand side is added to make 10 O's on both sides resulting in  P_{4} + 5O_{2} → 2P_{2}O_{5}
The equation is now balanced because there is an equal amount of substances on the left and the right hand side of the equation. Ex #3. C_{2}H_{5}OH + O_{2} → CO_{2} + H_{2}O This equation is more complex than the previous examples and requires more steps. The most complicated molecule here is C_{2}H_{5}OH, so balancing begins by placing the coefficient 2 before the CO_{2} to balance the carbon atoms.  C_{2}H_{5}OH + O_{2} → 2CO_{2} + H_{2}O
Since C_{2}H_{5}OH contains 6 hydrogen atoms, the hydrogen atoms can be balanced by placing 3 before the H_{2}O:  C_{2}H_{5}OH + O_{2} → 2CO_{2} + 3H_{2}O
Finally the oxygen atoms must be balanced. Since there are 7 oxygen atoms on the right and only 3 on the left, a 3 is placed before O_{2}, to produce the balanced equation:  C_{2}H_{5}OH + 3O_{2} → 2CO_{2} + 3H_{2}O
Linear system balancing In reactions involving many compounds, equations may then be balanced using an algebraic method, based on solving set of linear equations. 1. Assign variables to each coefficient. (Coefficients represent both the basic unit and mole ratios in balanced equations.):  a K_{4}Fe(CN)_{6} + b H_{2}SO_{4} + c H_{2}O → d K_{2}SO_{4} + e FeSO_{4} + f (NH_{4})_{2}SO_{4} + g CO
2. There must be the same quantities of each atom on each side of the equation. So, for each element, count its atoms and let both sides be equal.  K: 4a = 2d
 Fe: 1a = 1e
 C: a = 6g
 N: a = 3f
 H: 2b+2c = 8f
 S: b = d+e+f
 O: 4b+c = 4d+4e+4f+g
3. Solve the system (Direct substitution is usually the best way.)  d=2a
 e=a
 g=6a
 f=3a
 b=6a
 c=6a
which means that all coefficients depend on a parameter a, just choose a=1 (a number that will make all of them small whole numbers), which gives:  a=1 b=6 c=6 d=2 e=1 f=3 g=6
4. And the balanced equation at last:  K_{4}Fe(CN)_{6} + 6 H_{2}SO_{4} + 6 H_{2}O → 2 K_{2}SO_{4} + FeSO_{4} + 3 (NH_{4})_{2}SO_{4} + 6 CO
To speed up the process, one can combine both methods to get a more practical algorithm: 1. Identify elements which occur in one compound in each member. (This is very usual.) 2. Start with the one among those which has a big index (this will help to keep working with integers), and assign a variable, such as a.  a K_{4}Fe(CN)_{6} + H_{2}SO_{4} + H_{2}O → K_{2}SO_{4} + FeSO_{4} + (NH_{4})_{2}SO_{4} + CO
3. K_{2}SO_{4} has to be 2a (because of K), and also, FeSO_{4} has to be 1a (because of Fe), CO has to be 6a (because of C) and (NH_{4})_{2}SO_{4} has to be 3a (because of N). This removes the first four equations of the system. It is already known that whatever the coefficients are, those proportions must hold:  a K_{4}Fe(CN)_{6} + H_{2}SO_{4} + H_{2}O → 2a K_{2}SO_{4} + a FeSO_{4} + 3a (NH_{4})_{2}SO_{4} + 6a CO
4. One can continue by writing the equations now (and having simpler problem to solve) or, in this particular case (although not so particular) one could continue by noticing that adding the Sulfurs yields 6a for H_{2}SO_{4} and finally by adding the hydrogens (or the oxygens) one can find the lasting 6a for H_{2}SO_{4}. 5. Again, having a convenient value for a (in this case 1 will do, but if a results in fractional values in the other coefficients, one would like to cancel the denominators) The result is  K_{4}Fe(CN)_{6} + 6 H_{2}SO_{4} + 6 H_{2}O → 2 K_{2}SO_{4} + FeSO_{4} + 3 (NH_{4})_{2}SO_{4} + 6 CO
Reading chemical equations When reading a chemical equation there are some points to consider.  Each side of an equation represents a mixture of chemicals. The mixture is written as a set of molecular formulas, separated by + symbols.
 Each formula is preceded by an optional scalar number (if no scalar number is written, it is implied that the number is 1). The scalar numbers indicate the relative quantity of molecules in the reaction. For instance, the string 2H_{2}O + 3CH_{4} represents a mixture containing 2 molecules of H_{2}O for every 3 molecules of CH_{4}.
 The two sides of the equation are separated by an arrow. If the reaction is nonreversible, a rightarrow (→) is used, indicating that the left side represents the mixture of chemicals before the reaction, and the right side indicates the mixture after the reaction. For a reversible reaction, a twoway arrow is used. For example the equation 4Na + O_{2} → 2Na_{2}O represents a nonreversible reaction. In this reaction, sodium (Na) and oxygen (O_{2}) are converted to a single molecule, Na_{2}O (containing 2 sodium atoms and 1 oxygen atom). We can also see that for every 4 sodium atoms at the beginning of the reaction, a single O_{2} molecule will participate, and 2 Na_{2}O molecules will result.
 A chemical equation does not imply that all reactants are consumed in a chemical process. For instance a limiting reagent determines how far a reaction can go.
 In an ionic equation balancing of charge also takes place. In a full equation all reactants are written as molecules.
A chemical formula (also called molecular formula) is a concise way of expressing information about the atoms that constitute a particular chemical compound. ...
A reversible reaction is a chemical reaction that may proceed in both the forward and reverse directions. ...
For sodium in the diet, see Salt. ...
This article is about the chemical element and its most stable form, or dioxygen. ...
In a scientific sense, a chemical process is a method or means of somehow changing one or more chemicals or chemical compounds. ...
In chemistry, the limiting reagent, or also called the limiting reactant, is the chemical that determines how far the reaction will go before the chemical in question gets used up, causing the reaction to stop. ...
An ionic equation is a chemical equation in which strong electrolytes are written as dissociated ions. ...
A molecular equation is a chemical equation written as if all components exist as molecules. ...
References  ^ IUPAC Compendium of Chemical Terminology
The International Union of Pure and Applied Chemistry (IUPAC) is an international nongovernmental organization devoted to the advancement of chemistry. ...
External links  Chemical Equation Balancer, balances chemical equations, including ReductionOxidation (redox) reactions and reactions with several distinct solutions. Also teaches how to balance an equation using matrices and linear algebra.
 Classic Chembalancer  Play Chembalancer, a free online game at FunBasedLearning.com, to learn how to balance equations by inspection
 Online calculator, determines of the coefficients of a chemical equation
 Free chemical equation balancer, solves chemical equation, works online, low bandwidth
 Chemical equation balancing program  works offline, calculates stoichiometry and limiting reagents, balances charge.
 Online Chemical Equation Balancer Balances equation of any chemical reaction (full or halfcell) in one click.
 Balance chemical equations Teaches how to balance chemical equations
edother usesreduction}} Illustration of a redox reaction Redox (shorthand for reduction/oxidation reaction) describes all chemical reactions in which atoms have their oxidation number (oxidation state) changed. ...
