1. Write and balance the following reactions:
Aqueous solutions of silver nitrate and potassium iodide are mixed. Silver iodide and potassium nitrate are produced. Use your solubility chart to figure out which one is the precipitate.
silver nitrate(aq) + potassium iodide(aq)  silver iodide + potassium nitrate
AgNO3(aq) + KI(aq)  AgI(s) + KNO3(aq)

2. Write and balance the following reactions:
2. When nitrogen dioxide is bubbled through water it produces nitric acid and nitrogen monoxide. What are the states of matter of nitrogen dioxide, nitric acid and nitrogen monoxide?
Nitrogen dioxide + water(l)  nitric acid + nitrogen monoxide
Nitrogen dioxide(g) + water(l)  nitric acid(aq) + nitrogen monoxide(g)
NO2(g) + H2O(l)  HNO3(aq) + NO(g)
3 NO2(g) + H2O(l)  2 HNO3(aq) + NO(g)

3. Write balanced chemical equations for the following synthesis and decomposition chemical reactions.
Figure out what the states of matter should be at room temperature.
Predict products according to the type of reaction.

4. Synthesis:
carbon + oxygen 
2. gallium + oxygen 
3. nitrogen + hydrogen 

5. Synthesis:
carbon + oxygen 
C(s) + O2(g)  CO2(g)
or 2 C(s) + O2(g)  2 CO(g)
gallium + oxygen 
4 Ga(s) + 3 O2(g)  2 Ga2O3(s)
nitrogen + hydrogen 
N2(g) H2(g)  2 NH3(g)

6. Decomposition:
1. sodium oxide 
aluminum chloride 
3. calcium carbonate 
4. potassium chlorate 

7. Decomposition: sodium oxide  2 Na2O(s)  4 Na(s) + O2(g)
aluminum chloride 
2 AlCl3(s)  2 Al(s) + 3 Cl2(g) D D

8. Decomposition: 3. calcium carbonate  CaCO3(s)  CaO(s) + CO2(g) 4
Decomposition: 3. calcium carbonate  CaCO3(s)  CaO(s) + CO2(g) 4. potassium chlorate  2 KClO3(s)  2 KCl(s) + 3 O2(g) D D

9. The Activity Series a. Li(s) + Fe(NO3)3(aq)  _________
For each of the following reactants, use the activity series to determine whether the reaction would take place or not. If no reaction takes. If a reaction does take placeplace, write NR in the blank, write the formulas for the products of the reaction. (Hint: If an active metal replaces the hydrogen in water, the hydroxide of the active metal forms. H-OH)
a. Li(s) + Fe(NO3)3(aq)  _________
b. Au(s) + HCl(aq)  __________
c. Cl2(g) + KBr(aq)  ___________
d. Cu(s) + Al(NO3)3(aq)  ________
e. Ag(s) + HBr(aq)  _________
f. Ni(s) + SnCl2(aq)  ___________

10. The Activity Series a. 3 Li(s) + Fe(NO3)3(aq)  3 LiNO3(aq) + Fe(s)
For each of the following reactants, use the activity series to determine whether the reaction would take place or not. If no reaction takes place, write NR in the blank. If a reaction does take place, write the formulas for the products of the reaction. (Hint: If an active metal replaces the hydrogen in water, the hydroxide of the active metal forms.)
a. 3 Li(s) + Fe(NO3)3(aq)  3 LiNO3(aq) + Fe(s)
b. Au(s) + HCl(aq)  NR
c. Cl2(g) KBr(aq)  2 KCl(aq) + Br2(l)
d. Cu(s) + Al(NO3)3(aq)  NR
e. Ag(s) + HBr(aq)  NR
f. Ni(s) + SnCl2(aq)  Sn(s) + NiCl2(aq)

11. Use the activity series or solubility table to predict the product of the following reactions: Na(s) + SrBr2(aq)  CrI3(aq) + KCl(aq)  Zn(s) + H2SO3(aq)  K2CO3(aq) + HI(aq) 

12. Use the activity series or solubility table to predict the product of the following reactions: 2 Na(s) + SrBr2(aq)  NR CrI3(aq) + 3 KCl(aq)  CrCl3(s) + 3 KI(aq) (DR – ppt) Zn(s) + H2SO3(aq)  ZnSO3(aq) + H2(g) (SR – metal + acid) K2CO3(aq) + 2 HI(aq)  2 KI(aq) + H2CO3(aq) (DR – gas) H2O(l) + CO2(g)

13. Use the activity series or solubility table to predict the product of the following reactions: Na(s) + H2O(l)  HC2H3O2(aq) + (NH4)2S(aq)  Fe(s) + CuCl2(aq)  HBr(aq) + Ba(OH)2(aq) 

14. Use the activity series or solubility table to predict the product of the following reactions:
2 Na(s) + 2 H2O(l)  2 NaOH(aq) + H2(g) (SR – metal + H2O)
2 HC2H3O2(aq) +(NH4)2S(aq) H2S(g)+2 NH4C2H3O2(aq)(DR – gas)
Fe(s) + CuCl2(aq)  Cu(s) + FeCl2(aq) (SR – metal/metal)
2 HBr(aq) + Ba(OH)2(aq)  BaBr2(aq) + 2 H2O(l) (DR – acid-base neutralization)

15. Is # of H in hydrocarbon divisible by 4?
If yes, hydrocarbon coefficient = 1
if no, hydrocarbon coefficient = 2
Balance hydrogen
Balance carbon
Balance oxygen LAST
Balance the following complete combustion reactions:
___C3H8(g) + ___O2(g)  ___CO2(g) + ___H2O(g)
___C5H12(g) + ___O2(g)  ___CO2(g) + ___H2O(g)

16. Balance Combustion Reactions
Now balance the chemical reactions for the complete combustion of hexane(C6H14) and decane (C10H22): ___C6H14(g) + ___O2(g)  ___CO2(g) + ___H2O(g) ___C10H22(g) + ___O2(g)  ___CO2(g) + ___H2O(g)

17. Write balanced chemical equations for the complete combustion of
propane (C3H8)
C3H8(g) O2(g)  CO2(g) H2O(g) + heat
C3H8(g) O2(g)  CO2(g) H2O(g) + heat
C3H8(g) O2(g)  CO2(g) H2O(g) + heat
C3H8(g) O2(g)  CO2(g) H2O(g) + heat

18. Write balanced chemical equations for the complete combustion of decane (C10H22) C10H22(g) + O2(g)  CO2(g) + H2O(g) + heat 2 C10H22(g) + O2(g)  CO2(g) + 22 H2O(g) + heat 2 C10H22(g) + O2(g)  20 CO2(g) + 22 H2O(g) + heat 2 C10H22(g) + 31 O2(g)  20 CO2(g) + 22 H2O(g) + heat