1. Balancing Chemical Equations

2. Standards
SC2. Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions.
SC2a Identify and balance the following types of chemical equations:
• Synthesis
• Decomposition
• Single Replacement
• Double Replacement
• Combustion

3. Law of Conservation of Mass
In ordinary chemical reactions, the total mass of reacting substances is equal to the total mass of products
All atoms on the reactant side must appear on the product side, and in equal numbers
No new elements may appear
No elements may disappear

4. Types of Chemical Equations
Synthesis Reaction
A + X  AX
one product
Decomposition Reaction
AX  A + X
one reactant
Single Replacement Reaction
A + BX  B +AX
one element replaces another in a compound
Double Replacement Reaction
AX + BY  AY + BX
elements in a compound switch partners
Combustion Reaction
AB + O2  AO + BO
Compound burns in oxygen gas
Acid Base (Neutralization)Reaction
HA + XOH  XA + H2O
acid and base react to form a salt and water

5. Synthesis Reactions
1. ___CaO + ___H2O  ___Ca(OH)2 2. ___P4 + ___O2  ___P2O5 3. ___Ca + ___O2  ___CaO 4. ___Cu + ___S8  ___ CuS 5. ___CuO + ___H2O  ___Cu(OH)2 6. ___S8 + ___O2  ___SO2 7. ___H2 + ___N2  ___NH3 8. ___H2 + ___Cl2  ___HCl 9. ___Ag + ___S8  ___Ag2S 10. ___Cr + ___O2  ___Cr2O3

6. Decomposition Reactions
11. ___BaCO  ___BaO ___CO2
12. ___MgCO  ___MgO ___CO2
13. ___K2CO  ___K2O ___CO2
14. ___Zn(OH)  ___ZnO ___H2O
15. ___Fe(OH)  ___FeO ___H2O
16. ___Ni(ClO3)  ___NiCl ___O2
17. ___NaClO  ___NaCl ___O2
18. ___KClO  ___KCl ___O2
19. ___H2SO  ___H2O ___SO3
___H2CO  ___H2O ___CO2

7. Single Replacement Reactions
21. ___AgNO ___Ni  ___Ni(NO3) ___Ag
22. ___AlBr ___Cl  ___AlCl ___Br2
23. ___NaI ___Br  ___NaBr ___I2
24. ___Ca ___HCl  ___CaCl ___H2
25. ___Mg ___HNO3  ___Mg(NO3) ___H2
26. ___ Zn ___H2SO4  ___ZnSO ___H2
27. ___K ___H2O  ___KOH ___H2
28. ___Na ___H2O  ___NaOH ___H2

8. Double Replacement Reactions
29. ___AlI3 + ___HgCl2  ____AlCl3 + ____HgI2(ppt) 30. ___HCl + ___NaOH  ___NaCl + ___H2O 31. ___BaCl2 + ___H2SO4  ___BaSO4 + ___HCl 32. ___Al2(SO4)3 + ___Ca(OH)2  ___Al(OH)3 + ___CaSO4 33. ___AgNO3 + ___K3PO4  ___Ag3PO4 + ___KNO3 34. ___CuBr2 + ___AlCl3  ___CuCl2 + ___AlBr3 35. ___Ca(C2H3O2)2 + ___Na2CO3  ___CaCO3 + ___NaC2H3O2 36. ___NH4Cl + ___Hg2(C2H3O2)2  ___NH4 C2H3O2 + ___Hg2Cl2 37. ___Ca(NO3)2 + ___HCl  ___CaCl2 + ___HNO3 38. ___FeS + ___HCl  ___FeCl2 + ___H2S

9. Combustion Reactions
39. ___C2H6 + ___O2  ___CO2 + ___H2O 40. ___C3H8 + ___O2  ___CO2 + ___H2O 41. ___C4H10 + ___O2  ___CO2 + ___H2O 42. ___C5H12 + ___O2  ___CO2 + ___H2O 43. ___C6H14 + ___O2  ___CO2 + ___H2O 44. ___C2H4 + ___O2  ___CO2 + ___H2O 45. ___C2H2 + ___O2  ___CO2 + ___H2O 46. ___C6H6 + ___O2  ___CO2 + ___H2O

10. Acid Base (Neutralization)Reactions
___HCl+ ___ NaOH  ___ H2O + ___ NaCl
___ HF + ___ LiOH  ___ H2O + ___ LiF
___ H3PO4 + ___ LiOH  ___ H2O + ___ Li3PO4
___ Fe(OH)3 + ___ HNO3  ___ Fe(NO3) 3 + ___ H2O