Journal #38 Balance the equations: 1. H2 (g) + N2 (g) → NH3 (g) 2. KClO3 (s) → 2 KCl(s) + O2 (g) 3. Al (s) + CuCl2 (aq) → AlCl3 (aq) + Cu(s) 4. 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)

Journal #38 Balance the equations: 1. 3H2 (g) + N2 (g) → 2NH3 (g) 2. 2KClO3 (s) → 2 KCl(s) + 3O2 (g) 3. 2Al (s) + 3CuCl2 (aq) → 2AlCl3 (aq) + 3Cu(s) 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) → 2AlN (s)

Reaction Classification

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

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

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)

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

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)

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

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

Single Rep. Double Rep. Synthesis 3. 2Al (s) + 3CuCl2 (aq) → 2AlCl3 (aq) + 3Cu(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) → 2AlN (s) Single Rep. Decomposition Double Rep. Synthesis