CHEMISTRY: BALANCING EQUATIONS

There are 2 tricks to balancing equations.  First, spelling the technical word:
                       STOICHIOMETRY

Second, insuring that there are an equal number of atoms of each element on both sides of the equation, following the Law of Conservation of Mass.

The left side of a balanced equation is called the reactant(s).  The right side is called the product(s).

The number of atoms is determined by multiplying the coefficients and subscripts.

To balance a chemical equation, change only the coefficients.  This changes the number of elements or molecules used or produced without changing the element or molecular configuration itself.

Let’s balance an easy one...

We have 2 H’s on the left, so we need 2 on the right.

And now the 2 Cl’s on the right match the 2 on the left.  We’re in balance.

Here’s one with more steps:

Start with the most complicated configuration, maybe Pb3
on the right.   We need 3 Pb’s on the left.

 

That gives us 12 Cl’s on the left, so we need the same number on the right.

Now there are 12 Na’s on the right, so we need the same number of Na atoms on the left. 

TIP:  Because the PO4 on the right is held together with parentheses, keep the PO4 on the left as a single entity as well.

And counting up the PO4’s shows that we have 16 on both the left and the right.  We’re in balance.  Notice that we didn’t have to write the coefficient ‘1’ because it is implied.

TIP:  In the balancing act, it is easier to make the final adjustments if there is a reactant that stands alone, a single element.  Try to save these until last.

BALANCING with FRACTIONS

Sometimes when balancing an equation, you'll wind up with terms that can't be split up.  What if you have O2 on one side and O3 on the other?

Assume that O3 is the more complicated entry so we need to get 3 oxygens from the diatomic O2 on the left.  Think of fractions.  We need one and a half O2s or 3/2.

Even though this equation is technically "in balance," most teachers will want you to use only whole numbers as coefficients in chemical equations.  Think about what you would do in a simple Algebra equation to get rid of a fraction.  You'd multiply by a common denominator, so do the same here.  Multiply ALL terms on BOTH SIDES by the denominator 2 to yield

TIP:  The diatomic oxygen is so frequently involved in these fraction situations, that I try to "balance" the oxygens last.  

Although these examples seem simple, the concept itself is simple also, regardless of how complicated a balancing question may appear.  Just remember

MATTER CAN BE NEITHER CREATED NOR DESTROYED.