Balancing Chemical Equations in THREE easy steps: the Box Method
This balancing method provides a very visual way to count atoms, making balancing quick and straightforward. Students are often looking for quick and reliable ways to balance, which this method provides. Two rationales for balancing are also given at the end of the video.
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Balanced equations are written with smallest whole-number coefficients. If there is no coefficient before a chemical formula, the coefficient is 1.
The method of inspection can be outlined as putting a coefficient of 1 in front of the most complex chemical formula and putting the other coefficients before everything else such that both sides of the arrows have the same number of each atom. If any fractional coefficient exists, multiply every coefficient with the smallest number required to make them whole, typically the denominator of the fractional coefficient for a reaction with a single fractional coefficient.
As an example, seen in the above image, the burning of methane would be balanced by putting a coefficient of 1 before the CH4:
1 CH4 + O2 → CO2 + H2O
Since there is one carbon on each side of the arrow, the first atom (carbon) is balanced.
Looking at the next atom (hydrogen), the right-hand side has two atoms, while the left-hand side has four. To balance the hydrogens, 2 goes in front of the H2O, which yields:
1 CH4 + O2 → CO2 + 2 H2O
Inspection of the last atom to be balanced (oxygen) shows that the right-hand side has four atoms, while the left-hand side has two. It can be balanced by putting a 2 before O2, giving the balanced equation:
CH4 + 2 O2 → CO2 + 2 H2O
This equation does not have any coefficients in front of CH4 and CO2, since a coefficient of 1 is dropped.