1. Balancing Chemical Equations
By: Jason R. Steele

2. Law of Conservation of Matter
A natural law describing the fact that matter is neither created nor destroyed in any process
Simply means that:
The amount of matter that you start with has to equal to the amount of matter that you end with

3. For Chemical Reactions This Means That:
The amount of reactants has to equal the amount of products.
Matter cannot be created or destroyed through a chemical reaction.
Chemical equations have to be balanced.

4. Balancing Chemical Equations
Example:
HCl + NaOH NaCl + H2O
H= H=2
Cl=1 Cl=1
Na=1 Na=1
O=1 O=1
The equation is balanced because the number of atoms in the reactants are equal to the number of atoms in the products.

5. Balancing Chemical Equations Rules
Before beginning to balance an equation, check each formula to see that it is correct. NEVER change a formula during the balancing of an equation.
Balancing is done by placing coefficients in front of the formulas to insure the same number of atoms of each element on both sides of the arrow.

6. Balancing Chemical Equations
Example:
H2 + O H2O
H=2 O= H=2 O=1
H2 + O H2O
H=2 O= H= O=2
2H2 + O H2O
H=4 O= H=4 O=2

7. Balancing Chemical Equations
Example:
Cu + AgNO3 Cu(NO3)2 + Ag
Cu=1 Ag=1 N=1 O= Cu=1 Ag=1 N=2 O=6
Cu + 2AgNO3 Cu(NO3)2 + Ag
Cu=1 Ag=2 N=2 O= Cu=1 Ag=1 N=2 O=6
Cu + 2AgNO3 Cu(NO3)2 + 2Ag
Cu=1 Ag=2 N=2 O= Cu=1 Ag=2 N=2 O=6

8. Balancing Chemical Equations
Example:
Sodium bicarbonate + citric acid
carbon dioxide, water, and sodium citrate.
Empirical Formula:
NaHCO3 + H3C6H5O7
CO2 + H2O + Na3C6H5O7

9. Balancing Chemical Equations
Example:
NaHCO3 + H3C6H5O7 CO2 + H2O + Na3C6H5O7
Na=1 H=9 C=7 O= Na=3 H=7 C=7 O=10
3NaHCO3 + H3C6H5O7 CO2 + H2O + Na3C6H5O7
Na=3 H=11 C=9 O= Na=3 H=7 C=7 O=10
3NaHCO3 + H3C6H5O7 3CO2 + H2O + Na3C6H5O7
Na=3 H=11 C=9 O= Na=3 H=7 C=9 O=14
3NaHCO3 + H3C6H5O7 3CO2 + 3H2O + Na3C6H5O7
Na=3 H=11 C=9 O= Na=3 H=11 C=9 O=16

10. The End