There are 2 tricks to balancing equations. First, spelling the technical word:
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).
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...
Here’s one with more steps:
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.
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
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