Balancing Equations Notes:
Balancing Equations Notes:
Chemical equations must be balanced on both sides according to the Law of Conservation of Mass, which says that matter cannot be created or destroyed. Therefore, atoms that are present on one side of the equation must be present on the other side as well.
Example:
H2 + O2 ( H2O
Reactant Product
This equation is unbalanced. Count your atoms on each side!
Reactant side (left):
H = 2
O = 2
Product side (right):
H = 2
O = 1
*To balance an equation, you can ONLY change the coefficient (the big number) at the front of the compound!
We can add a coefficient of 2 in front of the H2O to get 2 O’s. It will look like this 2H2O
*The coefficient gets multiplied with the subscripts* so then we have 4 hydrogens.
Let’s recount our atoms again!
H2 + O2 ( 2H2O
Reactant side:
H = 2
O = 2
Product side:
H = 4
O = 2
The equation is still unbalanced. Remember we can ONLY change the coefficient.
How about add a coefficient of 2 in front of the H2.
*The coefficient gets multiplied with the subscripts* so you have 4 hydrogens.
Let’s recount our atoms again!
2H2 + O2 ( 2H2O
Reactant side:
H = 4
O = 2
Product side:
H = 4
O = 2
The new balanced equation: 2H2 + O2 ( 2H2O
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