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Honors Chemistry
REACTION PREDICTION
DIRECTIONS: FOR EACH OF THE FOLLOWING, STATE THE TYPE OF REACTION AND WRITE
THE BALANCED EQUATION. A FEW OF THE REACTIONS WILL NOT OCCUR ACCORDING TO
THE REACTIVITY SERIES. WRITE "NR" FOR THESE. IDENTIFY DRIVING FORCE AND LIST
SPECTATOR IONS.
Driving forces are Bolded and spectator ions are listed on the side.
1. magnesium plus zinc nitrate 
Mg(s) + Zn(NO3)2(aq)  Zn(s) + Mg(NO3)2(aq)
SI: Mg+2, (NO3)-1
2. fluorine plus potassium bromide 
F2(g) + 2 KBr(aq)  2 KF(aq) + Br2()
SI: K+1, F-1
3. sodium plus oxygen 
4 Na(s) + O2(g)  2 Na2O(s)
4. methane (CH4) plus oxygen 
CH4 + 2 O2 + spark  CO2(g) + 2 H2O(g)
5. aluminum plus hydrochloric acid 
2 Al(s) + 6 HCl(aq)  2 AlCl3(aq) + 3 H2(g)
SI: Al+3, Cl-1
6. calcium hydroxide plus nitric acid 
Ca(OH)2(aq) + 2 HNO3(aq)  Ca(NO3)2(aq) + 2 H(OH)()
SI: Ca+2, (NO3)-1
7. sodium bromide plus silver nitrate 
NaBr(aq) + AgNO3(aq)  AgBr(s) + NaNO3(aq)
SI: Na+1, (NO3)-1
8. zinc chloride plus hydrogen sulfide 
ZnCl2(aq) + H2S(aq)  2 HCl(aq) + ZnS(s)
SI: H+1, Cl-1
9. calcium phosphate plus aluminum sulfate 
Ca3(PO4)2(s) + Al2(SO4)3(aq)  Al(PO4)(s) + Ca(SO4)(aq)
SI: Ca+2, (SO4)-2
10. mercury (I) sulfate plus ammonium nitrate 
Hg2SO4(aq) + 2 NH4NO3(aq)  (NH4)2SO4(aq) + 2 HgNO3(aq)
No Reaction
11. potassium plus fluorine 
2 K(s) + F2(g)  2 KF(s)
12. silver plus barium nitrate
Ag(s) + Ba(NO3)2(s)  No Reaction (according to activity series)
13. iron (III) hydroxide plus phosphoric acid 
Fe(OH)3(s) + H3(PO4)(aq)  3 H(OH)() + FePO4(s)
14. sodium plus nitric acid 
2 Na(s) + 2 HNO3(aq)  2 NaNO3(aq) + H2(g)
SI: Na+1, (NO3)-1
15. silver nitrate plus magnesium chloride 
2 AgNO3(aq) + MgCl2(aq)  2 AgCl(s) + Mg(NO3)2(aq)
SI: Mg+2, (NO3)-1
16. sodium sulfate plus barium chloride 
Na2SO4(aq) + BaCl2(aq)  BaSO4(s) + 2 NaCl(aq)
SI: Na+1, Cl-1
17. ammonium phosphate plus lithium hydroxide 
(NH4)3PO4(aq) + 3 LiOH(aq)  Li3PO4(aq) + 3 NH4OH(aq)
No Reaction
18. hydrogen plus oxygen 
2 H2(g) + O2(g) + spark  2 H2O(g)
19. calcium carbonate plus lithium chloride 
CaCO3(s) + 2 LiCl(aq)  Li2CO3(aq) + CaCl2(aq)
No Reaction
20. mercury (I) sulfate plus hydrochloric acid 
Hg2SO4(aq) + 2 HCl(aq)  H2SO4(aq) + 2 HgCl(aq)
21. propane plus oxygen 
C3H8 + 5 O2 + spark  3 CO2(g) + 4 H2O(g)
22. sodium plus iodine
2 Na(s) + I2(s)  2 NaI(s)
No Reaction
23. chlorine plus magnesium
Cl2(g) + Mg(s)  MgCl2(s)
24. mercury (I) nitrate plus sodium carbonate
2 HgNO3(aq) + Na2CO3(aq)  2 NaNO3(aq) + Hg2CO3(s)
SI: Na+1, (NO3)-1
25. magnesium plus hydrochloric acid
Mg(s) + 2 HCl(aq)  MgCl2(aq) + H2(g)
SI: Mg+2, Cl-1
26. water (electrolyzed) 
2 H2O()  2 H2(g) + O2(g)
27. ammonium nitrite plus barium hydroxide
2 NH4NO3(aq) + Ba(OH)2(aq)  Ba(NO3)2(aq) + 2 NH4OH(aq)
No Reaction
28. ammonium sulfate plus calcium hydroxide
(NH4)2SO4(aq) + Ca(OH)2(aq)  CaSO4(s) + 2 NH4OH(aq)
SI: (NH4)+1, (OH)-1
29. mercury (II) oxide (heated) 
2 HgO(s)  2 Hg(s) + O2(g)
30. ammonium phosphate plus aluminum chloride
(NH4)3PO4(aq) + AlCl3(aq)  AlPO4(s) + 3 NH4Cl(aq)
SI: (NH4)+1, Cl-1
31. iron (III) hydroxide plus nitric acid
Fe(OH)3(s) + 3 HNO3(aq)  3 H(OH)() + Fe(NO3)3(s)
No Reaction
32. calcium plus phosphoric acid
3 Ca(s) + 2 H3PO4(aq)  Ca3(PO4)2(s) + 3 H2(g)
33. calcium chloride plus ammonium hydroxide
CaCl2(aq) + 2 NH4OH(aq)  2 NH4Cl(aq) + Ca(OH)2(aq)
No Reaction
34. aluminum sulfide plus hydrochloric acid
Al2S3(s) + 6 HCl(aq)  3 H2S(aq) + 2 AlCl3(aq)
No Reaction
35. magnesium plus sulfur
Mg(s) + S(s) + heat  MgS(s)
36. calcium plus aluminum chloride
3 Ca(s) + 2 AlCl3(aq)  3 CaCl2(aq) + 2 Al(s)
SI : Ca+2, Cl-1
37. sodium carbonate plus sulfuric acid
Na2CO3(aq) + H2SO4(aq)  H2CO3(aq) + Na2SO4(aq)
No Reaction
38. lithium plus bromine
2 Li(s) + Br2()  2 LiBr(s)
39. potassium sulfide plus iron (II) nitrate
K2S(aq) + Fe(NO3)2(aq)  FeS(s) + 2 KNO3(aq)
SI : K+1, (NO3)-1
40. sodium plus calcium
Na(s) + Ca(s)  No Reaction (both metals)
41. calcium carbonate plus hydrochloric acid
CaCO3(s) + 2 HCl(aq)  CaCl2(aq) + CO2(g) + H2O()
SI: Ca+2, Cl-1
42. Pentane plus oxygen
C5H12 + 8 O2(g) + spark  5 CO2(g) + 6 H2O(g)
43. ammonium acetate plus iron (II) chloride
2 NH4C2H3O2(aq) + FeCl2(aq)  Fe(C2H3O2)2(aq) + 2 NH4Cl(aq)
No Reaction
44. zinc plus sulfuric acid
Zn(s) + H2SO4(aq)  ZnSO4(aq) + H2(g)
45. neon plus potassium
Ne(g) + K(s)  No Reaction (Ne is a noble gas)
46. lead (II) hydroxide plus hydrochloric acid
Pb(OH)2(s) + 2 HCl(aq)  2 H(OH)() + PbCl2(s)
47. potassium iodide plus ammonium nitrate
SI: Zn+2, (SO4)-2
KI(aq) + NH4NO3(aq)  NH4I(aq) + KNO3(aq)
No Reaction
48. potassium plus sodium nitrate
K(s) + NaNO3(aq)  KNO3(aq) + Na(s)
SI: K+1, (NO3)-1
49. silver plus hydrochloric acid
2 Ag + 2 HCl(aq)  2 AgCl(s) + H2(g)
50. magnesium nitrate plus hydrochloric acid
Mg(NO3)(s) + 2 HCl(aq)  2 HNO3(aq) + MgCl2(aq)
No Reaction
51. zinc hydroxide plus sulfuric acid
Zn(OH)2(s) + H2SO4(aq)  2 H(OH)() + ZnSO4(aq)
SI: Zn+2, (SO4)-2
52. sodium plus chlorine
2 Na(s) + Cl2(g)  2 NaCl(s)
53. fluorine plus potassium bromide
F2(g) + 2 KBr(aq)  2 KF(aq) + Br2(g)
SI: K+1, F-1
54. ammonium hydroxide plus sulfuric acid
2 NH4OH(aq) + H2SO4(aq)  2 H(OH)() + (NH4)2SO4(aq)
SI: (NH4)+1, (SO4)-2
55. sodium chloride plus potassium nitrate
NaCl(aq) + KNO3(aq)  KCl(aq) + NaNO3(aq)
No Reaction
56. chlorine plus lithium bromide
Cl2(g) + 2 LiBr(aq)  2 LiCl(aq) + Br2()
SI: Li+1, Cl-1
57. lithium hydroxide plus phosphoric acid
3 LiOH(aq) + H3PO4(aq)  3 H(OH)() + Li3PO4(aq)
SI: Li+1, (PO4)-3
58. butane plus oxygen
2 C4H10 + 13 O2(g)  8 CO2(g) + 10 H2O(g)
59. potassium sulfite plus nitric acid
K2SO3(aq) + 2 HNO3(aq)  2 KNO3(aq) + H2SO3(aq)
60. ammonium chloride plus potassium hydroxide
No Reaction
NH4Cl(aq) + KOH(aq)  KCl(aq) + NH4OH(aq)
No Reaction
61. sodium hydroxide plus hydrochloric acid
NaOH(aq) + HCl(aq)  H(OH)() + NaCl(aq)
SI: Na+1, Cl-1
62. octane plus oxygen
2 C8H18 + 25 O2(g)  16 CO2(g) + 18 H2O(g)
ACTIVITY SERIES
Li
Rb
K
react with cold
water and
Elements higher on the char
Metal Reactivity
Ba
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Co
Ni
Sn
Pb
H2
Cu
Ag
Hg
Pt
Au
acids, replacing
hydrogen
react with acids or
steam, but usually not
liquid water, to
replace hydrogen
react with
acids, but not
water, to replace
hydrogen
react with O2
to form oxides
mostly
unreactive
Halogen Reactivity
F2 ………most reactive
Cl2
Br2
I2 …….…least reactive