1. Journal #38 Balance the equations:
H2 (g) N2 (g) → NH3 (g)
2. KClO3 (s) → KCl(s) O2 (g)
Al (s) + CuCl2 (aq) → AlCl3 (aq) Cu(s)
Cu2S (s) → Cu (s) S (s)
5. Ba(NO3)2 aq) + Na2(SO4)(aq) → Ba(SO4)(s) + Na(NO3)(aq)
6. Al (s) N2 (g) → AlN (s)

2. Journal #38 Balance the equations:
H2 (g) N2 (g) → 2NH3 (g)
KClO3 (s) → KCl(s) O2 (g)
Al (s) CuCl2 (aq) → 2AlCl3 (aq) Cu(s)
Cu2S (s) → 2Cu (s) S (s)
5. Ba(NO3)2 aq) + Na2(SO4)(aq) → Ba(SO4)(s) + 2Na(NO3)(aq)
Al (s) N2 (g) → AlN (s)

3. Reaction Classification

4. Classifying Reactions
To classify a reaction we need to look at the reaction equation.
We are looking for:
specific reactants and products
states
relationship between reactants and products

5. Decomposition Reactions
Compound is broken into simpler pieces
2 HgO (s) → 2 Hg (l) + O2 (g)

6. Synthesis Reactions 4 Al(s) + 3O2(g) → 2Al2O3(s)
Two or more reactants combine to form one product
4 Al(s) + 3O2(g) → 2Al2O3(s)

7. Single Displacement Reactions
One element in a compound is kicked out and replaced by another
Zn(s) + 2HCl(aq) → ZnCl2 (aq) + H2(g)

8. Double Displacement Reactions
Ion swap
May form precipitate (use solubility table)
May form water
2 Na3PO4(aq) + 3 ZnSO4(aq) → 3 Na2SO4 (aq) Zn3(PO4)2(s)

9. Combustion Reactions Oxygen must be a reactant
Heat and flame are produced
CH4(g) + O2(g) → CO2(g) + 2H2O(g)

10. Lets practice… Reaction Types
Decomposition; Synthesis; Single Displacement
Double Displacement; Combustion
1. 3H2 (g) + N2 (g) → 2NH3 (g) Rxn type ____________
2. 2KClO3 (s) → 2 KCl(s) + 3O2 (g)
Rxn type ____________
Synthesis
Decomposition

11. Single Rep. Double Rep. Synthesis
3. 2Al (s) CuCl2 (aq) → 2AlCl3 (aq) Cu(s)
Rxn type ____________
4. Cu2S (s) → 2Cu (s) + S (s)
5. Ba(NO3)2 aq) + Na2(SO4)(aq) → Ba(SO4)(s) + 2Na(NO3)(aq)
6. 2Al (s) N2 (g) → AlN (s)
Single Rep.
Decomposition
Double Rep.
Synthesis