Balancing Equations Balancing, Writing, and Naming Equations
Balancing Equations
Balancing Equations <ul><li>Law of Conservation of Matter: </li></ul><ul><ul><li>In a chemical reaction, matter can be nei...
Balancing Equations <ul><li>Paraphrase: </li></ul><ul><li>Law of Conservation of  Atoms : </li></ul><ul><ul><li>The number...
Balancing Equations <ul><li>Hydrogen and oxygen are diatomic elements. </li></ul><ul><li>Their subscripts cannot be change...
Balancing Equation <ul><li>Count the atoms on each side. </li></ul><ul><ul><li>Reactant side: 2 atoms H and 2 atoms O </li...
Balancing Equations <ul><li>H 2  +  O 2   H 2 O </li></ul><ul><li>If the subscripts cannot be altered, how can the atoms b...
Balancing Equations <ul><li>Reactants:  2 atoms of H and 2 atoms of O </li></ul><ul><li>Products:  4 atoms of H and 2 atom...
Balancing Equations <ul><li>Reactant side:  4 atoms of H and 2 atoms of O </li></ul><ul><li>Product side:  4 atoms of H an...
Balancing Equations <ul><li>Count atoms. </li></ul><ul><ul><li>Reactants:  2 atoms N and 2 atoms H </li></ul></ul><ul><ul>...
Balancing Equations <ul><li>Nothing is balanced. </li></ul><ul><li>Balance the nitrogen first by placing a coefficient of ...
Balancing Equations <ul><li>Hydrogen is not balanced. </li></ul><ul><li>Place a 3 in front of H 2. </li></ul><ul><li>React...
Balancing Equations <ul><li>Count atoms. </li></ul><ul><li>Reactants:  Ca – 3 atoms, P – 2 atoms, O – 8 atoms; H – atoms, ...
Balancing Equations <ul><li>Side note on Ca 3 (PO 4 ) 2 </li></ul><ul><li>The subscript after the phosphate indicates two ...
Balancing Equations <ul><li>Ca 3 (PO 4 ) 2   +  H 2 SO 4   CaSO 4  +  H 3 PO 4 </li></ul><ul><li>Count atoms in the produc...
Balancing Equations <ul><li>In this equation, the ion groups do not break up. </li></ul><ul><li>Instead of counting indivi...
Balancing Equations <ul><li>Ca 3 (PO 4 ) 2   +  H 2 SO 4   CaSO 4  +  H 3 PO 4 </li></ul><ul><li>Reactants:  Ca 2+  – 3, P...
Balancing Equations <ul><li>Balance the metal first by placing a coefficient of 3 in front of CaSO 4 . </li></ul><ul><li>P...
Balancing Equations <ul><li>Three sulfate groups are needed on the reactant side so place a coefficient of 3 in front of H...
Balancing Equations <ul><li>A coefficient of 2 placed in front of H 3 PO 4  which balances both hydrogen and phosphate. </...
Balancing Equations <ul><li>The sulfate group breaks up.  Each atom must be counted individually.  Ugh! </li></ul><ul><li>...
Balancing Equations <ul><li>Sulfur is not balanced. </li></ul><ul><li>Place a two in front of sulfuric acid. </li></ul><ul...
Balancing Equations <ul><li>Hydrogen needs to be balanced so place a 2 in front of the H 2 O.  </li></ul><ul><li>Count the...
Balancing Equations <ul><li>Reactants:  Cu – 1, H – 4, S – 2, O – 8 </li></ul><ul><li>Products:  Cu – 1, S – 1, O – 4, H –...
Balancing Equations <ul><li>Balancing hints: </li></ul><ul><ul><li>Balance the metals first. </li></ul></ul><ul><ul><li>Ba...
Balancing Equations <ul><li>This method of balancing equations is the inspection method. </li></ul><ul><li>The method is t...
Upcoming SlideShare
Loading in...5
×

Balancing Equations #1

2,264

Published on

How to balance chemical equations

Published in: Education, Technology, Business
0 Comments
1 Like
Statistics
Notes
  • Be the first to comment

No Downloads
Views
Total Views
2,264
On Slideshare
0
From Embeds
0
Number of Embeds
1
Actions
Shares
0
Downloads
154
Comments
0
Likes
1
Embeds 0
No embeds

No notes for slide

Balancing Equations #1

  1. 1. Balancing Equations Balancing, Writing, and Naming Equations
  2. 2. Balancing Equations
  3. 3. Balancing Equations <ul><li>Law of Conservation of Matter: </li></ul><ul><ul><li>In a chemical reaction, matter can be neither created nor destroyed. </li></ul></ul><ul><ul><li>In a chemical reaction, the amount of reactants equal the amount of products. </li></ul></ul>
  4. 4. Balancing Equations <ul><li>Paraphrase: </li></ul><ul><li>Law of Conservation of Atoms : </li></ul><ul><ul><li>The number of atoms of each type of element must be the same on each side of the equation. </li></ul></ul>
  5. 5. Balancing Equations <ul><li>Hydrogen and oxygen are diatomic elements. </li></ul><ul><li>Their subscripts cannot be changed. </li></ul><ul><li>The subscripts on water cannot be changed. </li></ul><ul><li>Hydrogen + oxygen water </li></ul><ul><li>H 2 + O 2 H 2 O </li></ul>
  6. 6. Balancing Equation <ul><li>Count the atoms on each side. </li></ul><ul><ul><li>Reactant side: 2 atoms H and 2 atoms O </li></ul></ul><ul><ul><li>Product side: 2 atoms H and 1 atom O </li></ul></ul><ul><li>H 2 + O 2 H 2 O </li></ul>
  7. 7. Balancing Equations <ul><li>H 2 + O 2 H 2 O </li></ul><ul><li>If the subscripts cannot be altered, how can the atoms be made equal? </li></ul><ul><li>Adjust the number of molecules by changing the coefficients . </li></ul>
  8. 8. Balancing Equations <ul><li>Reactants: 2 atoms of H and 2 atoms of O </li></ul><ul><li>Products: 4 atoms of H and 2 atoms of O </li></ul><ul><li>H is no longer balanced! </li></ul><ul><li>H 2 + O 2 2 H 2 O </li></ul>
  9. 9. Balancing Equations <ul><li>Reactant side: 4 atoms of H and 2 atoms of O </li></ul><ul><li>Product side: 4 atoms of H and 2 atoms of O </li></ul><ul><li>It’s Balanced! </li></ul><ul><li>2 H 2 + O 2 2 H 2 O </li></ul>
  10. 10. Balancing Equations <ul><li>Count atoms. </li></ul><ul><ul><li>Reactants: 2 atoms N and 2 atoms H </li></ul></ul><ul><ul><li>Products: 1 atom N and 3 atoms of NH 3 </li></ul></ul><ul><li>N 2 + H 2 NH 3 </li></ul><ul><li>Nitrogen + hydrogen ammonia </li></ul>
  11. 11. Balancing Equations <ul><li>Nothing is balanced. </li></ul><ul><li>Balance the nitrogen first by placing a coefficient of 2 in front of the NH 3 . </li></ul><ul><li>N 2 + H 2 2 NH 3 </li></ul>
  12. 12. Balancing Equations <ul><li>Hydrogen is not balanced. </li></ul><ul><li>Place a 3 in front of H 2. </li></ul><ul><li>Reactant side: 2 atoms N, 6 atoms H </li></ul><ul><li>Product side: 2 atoms N, 6 atoms H </li></ul><ul><li>N 2 + 3 H 2 2 NH 3 </li></ul>
  13. 13. Balancing Equations <ul><li>Count atoms. </li></ul><ul><li>Reactants: Ca – 3 atoms, P – 2 atoms, O – 8 atoms; H – atoms, S – 1 atom, O – 4 atoms </li></ul><ul><li>Ca 3 (PO 4 ) 2 + H 2 SO 4 CaSO 4 + H 3 PO 4 </li></ul>
  14. 14. Balancing Equations <ul><li>Side note on Ca 3 (PO 4 ) 2 </li></ul><ul><li>The subscript after the phosphate indicates two phosphate groups. </li></ul><ul><li>This means two PO 4 3- groups with two P and eight O atoms. </li></ul>
  15. 15. Balancing Equations <ul><li>Ca 3 (PO 4 ) 2 + H 2 SO 4 CaSO 4 + H 3 PO 4 </li></ul><ul><li>Count atoms in the product. </li></ul><ul><li>Ca atoms – 1, S atom – 1, O atoms – 4; H atoms – 3, P atom – 1, O atoms - 4 </li></ul>
  16. 16. Balancing Equations <ul><li>In this equation, the ion groups do not break up. </li></ul><ul><li>Instead of counting individual atoms, ion groups may be counted. </li></ul><ul><li>Ca 3 (PO 4 ) 2 + H 2 SO 4 CaSO 4 + H 3 PO 4 </li></ul>
  17. 17. Balancing Equations <ul><li>Ca 3 (PO 4 ) 2 + H 2 SO 4 CaSO 4 + H 3 PO 4 </li></ul><ul><li>Reactants: Ca 2+ – 3, PO 4 3- - 2, H + – 2, SO 4 2+ - 1 </li></ul><ul><li>Products: Ca 2+ - 1, SO 4 2- - 1, H + - 3, PO 4 3- - 1 </li></ul>
  18. 18. Balancing Equations <ul><li>Balance the metal first by placing a coefficient of 3 in front of CaSO 4 . </li></ul><ul><li>Products: Ca – 3 atoms, SO 4 2- - 3 groups </li></ul><ul><li>Ca 3 (PO 4 ) 2 + H 2 SO 4 3 CaSO 4 + H 3 PO 4 </li></ul>
  19. 19. Balancing Equations <ul><li>Three sulfate groups are needed on the reactant side so place a coefficient of 3 in front of H 2 SO 4 . </li></ul><ul><li>3H 2 SO 4 gives 6 H + and 3 SO 4 2- . </li></ul><ul><li>Neither phosphate nor calcium is balanced. </li></ul><ul><li>Ca 3 (PO 4 ) 2 + 3 H 2 SO 4 3 CaSO 4 + H 3 PO 4 </li></ul>
  20. 20. Balancing Equations <ul><li>A coefficient of 2 placed in front of H 3 PO 4 which balances both hydrogen and phosphate. </li></ul><ul><li>Ca 3 (PO 4 ) 2 + 3 H 2 SO 4 3 CaSO 4 + 2 H 3 PO 4 </li></ul>
  21. 21. Balancing Equations <ul><li>The sulfate group breaks up. Each atom must be counted individually. Ugh! </li></ul><ul><li>Reactants: Cu – 1, H – 2, S – 1, O – 4 </li></ul><ul><li>Products: Cu – 1, S – 1, O - 4, H – 2, O – 1, S – 1, O - 2 </li></ul><ul><li>Cu + H 2 SO 4 </li></ul><ul><li>CuSO 4 + H 2 O + SO 2 </li></ul>
  22. 22. Balancing Equations <ul><li>Sulfur is not balanced. </li></ul><ul><li>Place a two in front of sulfuric acid. </li></ul><ul><li>Count atoms: 2 H 2 SO 4 H – 4, S – 2, O - 8 </li></ul><ul><li>Cu + 2 H 2 SO 4 </li></ul><ul><li>CuSO 4 + H 2 O + SO 2 </li></ul>
  23. 23. Balancing Equations <ul><li>Hydrogen needs to be balanced so place a 2 in front of the H 2 O. </li></ul><ul><li>Count the number of atoms. </li></ul><ul><li>Cu + 2 H 2 SO 4 </li></ul><ul><li>CuSO 4 + 2 H 2 O + SO 2 </li></ul>
  24. 24. Balancing Equations <ul><li>Reactants: Cu – 1, H – 4, S – 2, O – 8 </li></ul><ul><li>Products: Cu – 1, S – 1, O – 4, H – 4, O – 2, S – 1, O – 2 = Cu – 1, S – 2, H – 4, O – 8 </li></ul><ul><li>It’s balanced! </li></ul><ul><li>Cu + 2 H 2 SO 4 </li></ul><ul><li>CuSO 4 + 2 H 2 O + SO 2 </li></ul>
  25. 25. Balancing Equations <ul><li>Balancing hints: </li></ul><ul><ul><li>Balance the metals first. </li></ul></ul><ul><ul><li>Balance the ion groups next. </li></ul></ul><ul><ul><li>Balance the other atoms. </li></ul></ul><ul><ul><li>Save the non ion group oxygen and hydrogen until the end. </li></ul></ul>
  26. 26. Balancing Equations <ul><li>This method of balancing equations is the inspection method. </li></ul><ul><li>The method is trial and error. </li></ul><ul><li>Practice. </li></ul>
  1. A particular slide catching your eye?

    Clipping is a handy way to collect important slides you want to go back to later.

×