1. Balancing Chemical Equations

2. The Balanced Equation Atoms can’t be created or destroyed.
All the atoms we start with we must end up with.
A balanced equation has the same number of each element on both sides of the equation.

3. The Balanced Equation
Balanced equations show how mass and atoms are conserved.

4. ® O + C C O O C + O2 ® CO This equation is NOT balanced.
There is one carbon atom on the left and one on the right.
There are two oxygen atoms on the left and only one on the right.

5. O + C C O O
C + O2 ® CO
We need one more oxygen atom in the products.
We can’t change the formula, because it describes what it is.

6. C O O + C O C O
In order to have two oxygen atoms, another CO must be produced.
But where did the other carbon come from?

7. C C O O + O C C O
We must have started with two carbon atoms.

8. C C O O + O C C O
The balanced chemical equation is
2 C + O2 ® 2 CO

9. Chemical Equations
Numbers and types of atoms must balance.

11. Rules for Balancing
Write the correct formulas for all the reactants and products.
Count the number of atoms of each type appearing on both sides.
Balance the elements one at a time by adding coefficients (the numbers in front).
Check to make sure it is balanced.

12. Never Never change a subscript to balance an equation.
If you change the formula you are describing a different reaction.

13. Never Never put a coefficient in the middle of a formula.
2 NaCl is okay; Na2Cl is not.

14. H2 + O2 ® H2O Example Make a table to keep track of where you
are in the balancing process.

15. Example ® H2 + O2 H2O Reactants Products 2 H 2 2 O 1
We need twice as much O in the product.

16. Example
H2 + O2 2
H2O
We need 2 oxygen atoms on the product side, so a coefficient of 2 should be placed in front of water.

17. Example
H2 + O2 2
H2O
We must recalculate the number of hydrogen and oxygen atoms on the right. Coefficients are used as multipliers. R P 2 H 2 4 2 O 1 2

18. Example
H2 + O2 2
H2O
Now we need 4 hydrogen atoms on the reactant side. R P 2 H 4 2 O 2

19. Example 2
H2 + O2 2
H2O
A coefficient of 2 should be placed in front of hydrogen gas. R P 4 2 H 4 2 O 2

20. Example 2
H2 + O2 2
H2O
The equation is balanced; it has the same number of each kind of atom on both sides! R P 4 H 4 2 O 2

21. Example R P 4 2 H 2 4 2 O 1 2 2 H2 + O2 ® 2 H2O This is the answer,
not this.

22. Balancing Hints metals nonmetals hydrogen oxygen
Balance elements in the following order:
metals
nonmetals
hydrogen
oxygen

23. Balancing Hints
If an atom appears more than once on a side, balance it last.
If you fix everything except one element, and it is even on one side and odd on the other, double the first number, then move on from there.

24. Problem CH4 + O2 ® CO2 + H2O CH4 + 2 O2 ® CO2 + 2 H2O
Balance the following equation.
CH4 + O2 ® CO2 + H2O
CH4 + 2 O2 ® CO2 + 2 H2O

25. Problem AgNO3 + Cu ® Cu(NO3)2 + Ag 2 AgNO3 + Cu ® Cu(NO3)2 + 2 Ag
Balance the following equation.
AgNO3 + Cu ® Cu(NO3)2 + Ag
2 AgNO3 + Cu ® Cu(NO3)2 + 2 Ag

26. Problem Mg + N2 ® Mg3N2 3 Mg + N2 ® Mg3N2
Balance the following equation.
Mg + N2 ® Mg3N2
3 Mg + N2 ® Mg3N2

27. Problem
Balance the following equation.
P + O2 ® P4O10
4 P + 5 O2 ® P4O10

28. Problem Na + H2O ® H2 + NaOH 2 Na + 2 H2O ® H2 + 2 NaOH
Balance the following equation.
Na + H2O ® H2 + NaOH
2 Na + 2 H2O ® H NaOH