1. Balancing Chemical Equations

2. CA Standards Students know how to describe chemical reactions by writing balanced equations.

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 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. Synthesis Reactions 1. ___CaO + ___H 2 O  ___Ca(OH) 2 2. ___P 4 + ___O 2  ___P 2 O 5 3. ___Ca + ___O 2  ___CaO 4. ___Cu + ___S 8  ___ CuS 5.___CaO + ___H 2 O  ___Ca(OH) 2 6. ___S 8 + ___O 2  ___SO 2 7.___H 2 + ___N 2  ___NH 3 8.___H 2 + ___Cl 2  ___HCl 9.___Ag + ___S 8  ___Ag 2 S 10.___Cr + ___O 2  ___Cr 2 O 3 11.___Al + ___Br 2  ___AlBr 3 12.___Na + ___I 2  ___NaI 13.___H 2 + ___O 2  ___H 2 O 14. ___Al + ___O 2  ___Al 2 O 3

5. Decomposition Reactions 15. ___BaCO 3  ___BaO + ___CO 2 16.___MgCO 3  ___MgO + ___CO 2 17.___K 2 CO 3  ___K 2 O + ___CO 2 18. ___Zn(OH) 2  ___ZnO + ___H 2 O 19. ___Fe(OH) 2  ___FeO + ___H 2 O 20. ___Ni(ClO 3 ) 2  ___NiCl 2 + ___O 2 21. ___NaClO 3  ___NaCl + ___O 2 22. ___KClO 3  ___KCl + ___O 2 23. ___H 2 SO 4  ___H 2 O + ___SO 3 24. ___H 2 CO 3  ___H 2 O + ___CO 2 25. ___Al 2 O 3  ___Al + ___O 2 26. ___Ag 2 O  ___Ag + ___O 2

6. Decomposition Reactions 15. ___BaCO 3  ___BaO + ___CO 2 16.___MgCO 3  ___MgO + ___CO 2 17.___K 2 CO 3  ___K 2 O + ___CO 2 18. ___Zn(OH) 2  ___ZnO + ___H 2 O 19. ___Fe(OH) 2  ___FeO + ___H 2 O 20. ___Ni(ClO 3 ) 2  ___NiCl 2 + ___O 2 21. ___NaClO 3  ___NaCl + ___O 2 22. ___KClO 3  ___KCl + ___O 2 23. ___H 2 SO 4  ___H 2 O + ___SO 3 24. ___H 2 CO 3  ___H 2 O + ___CO 2 25. ___Al 2 O 3  ___Al + ___O 2 26. ___Ag 2 O  ___Ag + ___O 2

7. Single Replacement Reactions 27. ___AgNO 3 + ___Ni  ___Ni(NO 3 ) 2 + ___Ag 28. ___AlBr 3 + ___Cl 2  ___AlCl 3 + ___Br 2 29. ___NaI + ___Br 2  ___NaBr + ___I 2 30. ___Ca + ___HCl  ___CaCl 2 + ___H 2 31. ___Mg + ___HNO 3  ___Mg(NO 3 ) 2 + ___H 2 32. ___ Zn + ___H 2 SO 4  ___ZnSO 4 + ___H 2 33. ___K + ___H 2 O  ___KOH + ___H 2 34. ___Na + ___H 2 O  ___NaOH + ___H 2

8. Double Replacement Reactions 35. ___AlI 3 + ___HgCl 2  ____AlCl 3 + ____HgI 2 (ppt) 36. ___HCl + ___NaOH  ___NaCl ___H 2 O 37. ___BaCl 2 + ___H 2 SO 4  ___BaSO 4 + ___HCl 38. ___Al 2 (SO 4 ) 3 + ___Ca(OH) 2  ___Al(OH) 3 + ___CaSO 4 39. ___AgNO 3 + ___K 3 PO 4  ___Ag 3 PO 4 + ___KNO 3 40. ___CuBr 2 + ___AlCl 3  ___CuCl 2 + ___AlBr 3 41. ___Ca(C 2 H 3 O 2 ) 2 + ___Na 2 CO 3  ___CaCO 3 + ___NaC 2 H 3 O 2 42. ___NH 4 Cl + ___Hg 2 (C 2 H 3 O 2 ) 2  ___NH 4 C 2 H 3 O 2 + ___Hg 2 Cl 2 43. ___Ca(NO 3 ) 2 + ___HCl  ___CaCl 2 + ___HNO 3 44. ___FeS + ___HCl  ___FeCl 2 + ___H 2 S 45. ___Cu(OH) 2 + ___HC 2 H 3 O 2  ___Cu(C 2 H 3 O 2 ) 2 + ___H 2 O 46. ___Ca(OH) 2 + ___H 3 PO 4  ___Ca 3 (PO 4 ) 2 + ___H 2 O 47. ___CaBr 2 + ___KOH  ___Ca(OH) 2 + ___KBr

9. Combustion Reactions 48. ___CH 4 + ___O 2  ___CO 2 + ___H 2 O 49. ___C 2 H 6 + ___O 2  ___CO 2 + ___H 2 O 50. ___C 3 H 8 + ___O 2  ___CO 2 + ___H 2 O 51. ___C 4 H 10 + ___O 2  ___CO 2 + ___H 2 O 52. ___C 5 H 12 + ___O 2  ___CO 2 + ___H 2 O 53. ___C 6 H 14 + ___O 2  ___CO 2 + ___H 2 O 54. ___C 2 H 4 + ___O 2  ___CO 2 + ___H 2 O 55. ___C 2 H 2 + ___O 2  ___CO 2 + ___H 2 O 56. ___C 6 H 6 + ___O 2  ___CO 2 + ___H 2 O