7.A – Chemical Equations: Balancing and Mole Ratios
Instructions: Balance the following chemical equations. Remember this is a trial and error process. It takes practice. DO NOT WRITE “1”, leave blank.
1. _2_ H2
+ ___ O2

_2_ H2O
13. _4_ Si2H3
+ _17_ O2 
_8_ SiO2
+ _6_ H2O3
2.
___ N2
+_3_ H2

_2_ NH3
14. _2_ Al(OH)3
+ _3_ H2SO4 
_6_ H2O
3.
___ S8
+ _12_ O2

_8_ SO3
15. _4_ Fe
+ _3_ O2

_2_ Fe2O3
4.
_2_ N2
+ ___ O2

_2_ N2O
16. ___ Fe2(SO4)3 + _6_ KOH 
_3_ K2SO4
+ _2_ Fe(OH)3
5.
_2_ HgO

_2_ Hg
+ ___ O2
17. _2_ C7H6O2
+ _17_ O2

_14_ CO2
+ _6_ H2O
6.
_6_ CO2
+ _6_ H2O

_6_ O2
+ ___ C6H12O6
18. ___ H2SO4
+ _8_ HI

___ H2S
+ _4_ I2
7.
___ Zn
+ _2_ HCl

___ ZnCl2
+ ___ H2
19. _4_ FeS2
+ _11_ O2

_2_ Fe2O3
+ _8_ SO2
8.
___ SiCl4
+ _4_ H2O

___ H4SiO4 + _4_ HCl
20. _2_ Al
+ _3_ FeO

___ Al2O3
+ _3_ Fe
9.
_2_ Na
+ ___ H2O

_2_ NaOH + ___ H2
21. ___ Fe2O3
+ _3_ H2

_2_ Fe
+ _3_ H2O

___ H2O
+ ___ H4P2O7
22. ___ Na2CO3
+ _2_ HCl

_2_ NaCl
+ ___ H2O + ___ CO2
+ _8_ H2O
10. _2_ H3PO4
11. ___ C10H16
+ _8_ Cl2

_10_ C
+ _16_ HCl
23. ___ C7H16
+ _11_ O2

_7_ CO2
12. ___ CO2
+ _2_ NH3

___ H2O
+ ___ OC(NH2)2
24. ___ P4
+ _5_ O2

_2_ P2O5
+ ___ Al2(SO4)3
+ _4_ H2O
Instructions: Given the following chemical equations, balance them. Then ON A SEPARATE SHEET OF PAPER, use dimensional analysis to perform the following
conversions related to the mole ratios. You MUST use dimensional analysis to preform each conversion. Remember, Sig Figs, NW = NC, Boxed Answers and N3 (this
includes labeling and in your set-up!!!)
1 mol Na2CO3
25. _3_ (NH4)2CO3 + _2_ Al(NO3)3  _6_ NH4NO3 + ___ Al2(CO3)3
a. 50.5 mol (NH4)2CO3 → mole NH4NO3
50.5 mol (NH4)2CO3
NH4NO3
b. 50.5 mol (NH4)2CO3
50.5 mol (NH4)2CO3
Al(NO3)3
6 mol NH4NO3
b. 4.3 mol Na2SO4
4.3 mol Na2SO4
2 mol Al(NO3)3
b. 120 mol H2
120 mol Mg
b. 0.20 mol Cu
0.20 mol Cu
b. 0.06 mol Na2CO3
0.06 mol Na2CO3
b. 63.23 mol CO2
=
33.7
mol
= 2.48 mol H2O
62.23 mol CO2
2 mol NaOH
1 mol Na2SO4
2 mol HCl
1 mol Mg
= 8.6 mol NaOH
+ ___ H2
= 1648 mol HCl
1 mol MgCl2
1 mol Mg
1 mol Cu
1 mol Zn
= 120 mol MgCl2
+ ___ Cu
= 533 mol Cu
2 mol NaNO3
2 mol HNO3
= 0.20 mol CuSO4
+ ___ H2O + ___ CO2
=62.35mol NaNO3
0.23 mol O2
0.53 mol CO2
5.61 mol H2O
1 mol C3H6O3
3 mol H2O
400 mol C7H9O
= 308 mol CO2
= 62.23 mol H2O
+ _3_ H2O
=21.2 mol C3H6O3
→ mole O2
3 mol O2
3 mol H2O
2 mol H2O
6 mol O2
= 12.6 mol O2
+ _2_ H2O
= 0.077 mol H2O
→ mole O2
6 mol O2
5 mol CO2
14 mol CO2
2 mol C7O10
= 0.64 mol O2
+ _10_ H2O
= 0.02 mol CO2
→ mole C7H10
2 mol C7O10
10 mol H2O
34. _4_ C7H9O
+ _35_ O2
 _28_ CO2
a. 400 mol C7H9O
→ mole CO2
650 mol C7H9O
= 0.03 mol CO2
6 mol H2O
6 mol CO2
33. _2_ C7H10
+ _19_ O2
 _14_ CO2
a. 0.003 mol C7H10
→ mole CO2
0.003 mol C7O10
+ _6_ H2O
→ mole H2O
32. ___ C5H4
+ _6_ O2
 _5_ CO2
a. 0.23 mol O2
→ mole H2O
b. 650 mol C7H9O
→ mole CO2
1 mol CO2
12.6 mol H2O
b. 5.61 mol H2O
→ mole CuSO4
1 mol CuSO4
1 mol Cu
63.6 mol H2O
b. 0.53 mol CO2
→ mole MgCl2
6 mol CO2
1 mol C6H12
31. ___ C3H6O3
+ _3_ O2
 _3_ CO2
a. 63.6 mol H2O
→ mole C3H6O3
b. 12.6 mol H2O
→ mole NaOH
29. ___ Na2CO3
+ _2_ HNO3
 _2_ NaNO3
a. 62.35 mol HNO3
→ mole NaNO3
2.35 mol HNO3
51.3 mol C6H12
+ _2_ H2O
2 mol H2O
1 mol H2SO4
28. ___ Zn
+ ___ CuSO4  ___ ZnSO4
a. 533 mol Zn
→ mole Cu
533 mol Zn
mol
3 mol (NH4)2CO3
27. ___ Mg
+ _2_ HCl
 ___ MgCl2
a. 824.0 mol Mg
→ mole HCl
824.0 mol Mg
101
3 mol (NH4)2CO3
→ mole Al(NO3)3
26. _2_ NaOH
+___ H2SO4
 ___ Na2SO4
a. 1.24 mol H2SO4
→ mole H2O
1.24 mol H2SO4
=
30. ___ C6H12
+ _9_ O2
 _6_ CO2
a. 51.3 mol C6H12
→ mole CO2
28 mol CO2
4 mol C7H9O
= 1.12 mol C7H10
+ _18_ H2O
= 3000 mol CO2
→ mole H2O
18 mol H2O
4 mol C7H9O
= 2900 mol CO2
7.B – Chemical Equations: Solubility Rules , Types and Writing
1. Ammonium acetate
Soluble / Insoluble
NH4+ (aq)
C2H3O2− (aq)
9. Zinc Hydroxide
Soluble / Insoluble
Zn(OH)2 (s)
_______
2. Barium hydroxide
Soluble / Insoluble
Ba2+ (aq)
2 OH− (aq)
10. Zinc phosphate
Soluble / Insoluble
Zn3(PO4)2 (s)
_______
3. Iron (II) Carbonate
Soluble / Insoluble
FeCO3 (s)
_______
11. Silver Bromide
Soluble / Insoluble
AgBr (s)
_______
4. Sodium hydroxide
Soluble / Insoluble
Na+ (aq)
OH− (aq)
12. Potassium Nitrate
Soluble / Insoluble
K+ (aq)
NO3− (aq)
5. Rubidium nitrate
Soluble / Insoluble
Rb+ (aq)
NO3− (aq)
13. Aluminum Sulfide
Soluble / Insoluble
Al2S3 (s)
_______
6. Cesium Sulfate
Soluble / Insoluble
2 Cs+ (aq)
SO42− (aq)
14. Silver Acetate
Soluble / Insoluble
Ag+ (aq)
C2H3O2− (aq)
7. Magnesium sulfate
Soluble / Insoluble
Mg2+ (aq)
SO42− (aq)
15. Strontium chloride
Soluble / Insoluble
SrCl2 (s)
_______
8. Zinc chloride
Soluble / Insoluble
Zn2+ (aq)
2 Cl− (aq)
16. Aluminum phosphate
Soluble / Insoluble
AlPO4 (s)
_______
25. 2 NaCl(aq)
+
Pb(NO3)2 (aq)
 PbCl2 (s)
+
2 NaNO3 (aq)
26. Ba(NO3)2 (aq)
+
H2SO4 (aq)
 BaSO4 (s)
+
2 HNO3 (aq)
27. 2 AgNO3 (aq)
+
K2CrO4 (aq)
 Ag2CrO4 (s)
+
2 KNO3 (aq)
28. CaCO3 (s)
+
2 HCl (aq)
 CaCl2 (aq)
+
CO2 (g)
29. ZnCl2 (aq)
+
H2S (g)
 ZnS (s)
+
2 HCl (aq)
30. Mg(NO3)2 (aq)
+
2 KOH (aq)
 Mg(OH)2 (s)
+
2 KNO3 (aq)
31. Al(OH)3 (s)
+
3 HNO3 (aq)
 Al(NO3)3 (aq)
+
3 H2O (L)
32. Pb(NO3)4 (aq)
+
2 Na2SO4 (aq)
 Pb(SO4)2 (s)
+
4 NaNO3 (aq)
33. 2 NaOH (aq)
+
CO2 (g)
 Na2CO3 (aq)
+
H2O (L)
34. MgO (s)
+
2 HCl (aq)
 MgCl2 (s)
+
H2O (L)
35. Zn (s)
+
H2SO4 (aq)
 ZnSO4 (aq)
+
H2 (g)
36. Molecular:
Ions that Result =
Ionic:
Net Ionic:
2 NaCl(aq)
Na+ & Cl―
2 Na+ (aq)
2 Na+ (aq)
+
 2 NaF(aq)
Na+ & F―
+ F2(g)
+ F2(g)
+
37. Molecular:
Ions that Result =
Ionic:
Net Ionic:
Pb(OH)2(aq) + 2 HCl(aq)
Pb2+ & OH―
H+ & Cl ―
Pb2+ (aq)
+ 2 OH ― (aq)
Pb2+ (aq)
+ OH ― (aq)
 2 H2O(l)
―
+ 2 H+ (aq)
+ H+ (aq)
+
38. Molecular:
Ions that Result =
Ionic:
Net Ionic:
2 AlBr3 (aq)
Al3+ & Br―
2 Al3+ (aq)
2 Al3+ (aq)
+
 6 KBr (aq)
K+ & Br ―
+ 6 K+ (aq)
+ 6 K+ (aq)
+
39. Molecular:
Ions that Result =
Ionic:
Net Ionic:
FeCl3 (aq)
Fe3+ & Cl―
Fe3+ (aq)
Fe3+ (aq)
+
3 NaOH (aq)  Fe(OH)3(s)
Na+ & OH―
―
―
3 Cl (aq)
+ 3 Na + (aq)
―
3 Cl (aq)
+ 3 Na + (aq)
+
+
+
+
+
+
+
F2(g)
―
2 Cl ― (aq)
2 Cl ― (aq)
3 K2SO4 (aq)
K+ & SO42―
6 Br ― (aq)
6 Br ― (aq)
Cl2(g)
―
 2 Na+ (aq)
 2 Na+ (aq)
+
+
H2O (L)
+
+
2 F ― (aq)
2 F ― (aq)
+
+
Cl2(g)
Cl2(g)
 H2O(l)
 H2O(l)
+
Pb2+ (aq)
+ 2 Cl― (aq)
Al2(SO4)3(s)
―
3 SO42― (aq)
3 SO42― (aq)
 6 K + (aq)
 6 K + (aq)
+
+
6 Br― (aq)
6 Br― (aq)
+ Al2(SO4)3 (s)
+ Al2(SO4)3 (s)
3 NaCl(aq)
Na+ & Cl―
3 OH― (aq)
3 OH― (aq)
 Fe(OH)3 (s)
 Fe(OH)3 (s)
+
+
3 Na + (aq)
3 Na + (aq)
+
+
PbCl2 (aq)
Pb2+ & Cl―
+ 2 Cl ― (aq)
+ 2 Cl ― (aq)
+
+
+
(HAVE TO SIMPLIFY OR NOT BALANCED)+
3 Cl― (aq)
3 Cl― (aq)
40. Molecular:
Ions that Result =
Ionic:
Net Ionic:
2 Ag2O(s)
Ag+ & O2
2 Ag2O(s)
2 Ag2O(s)
 4 Ag(s)
―
 4 Ag(s)
 4 Ag(s)
41. Molecular:
Ions that Result =
Ionic:
Net Ionic:
2 K(s)
―
2 K(s)
2 K(s)
+
MgBr2 (aq)
Mg2+ & Br―
+
Mg2+ (aq)
+
Mg2+ (aq)
 2 KBr(aq)
K+ & Br―
+ 2 Br― (aq)
+ 2 Br― (aq)
+
42. Molecular:
Ions that Result =
Ionic:
Net Ionic:
2 HCl (aq)
H+ & Cl―
2 H+ (aq)
2 H+ (aq)
+
CaCO3 (s)
―
2 Cl― (aq)
2 Cl― (aq)
 CaCl2 (aq)
Ca2+ & Cl―
+ CaCO3 (s)
+ CaCO3 (s)
+
43. Molecular:
Ions that Result =
Ionic:
Net Ionic:
2 NaBr (aq)
Na+ & Br―
2 Na+ (aq)
2 Na+ (aq)
+
CaF2 (aq)
Ca2+ & F―
2 Br― (aq)
2 Br― (aq)
 2 NaF (aq)
Na+ & F―
+ Ca2+ (aq)
+ Ca2+ (aq)
+
44. Molecular:
Ions that Result =
Ionic:
Net Ionic:
H2SO4 (aq)
+ 2 NaNO2 (aq)  2 HNO2 (aq)
+ Na2SO4 (aq)
H+ & SO42―
Na+ & NO2―
H+ & NO2
Na+ & SO42―
2 H+ (aq) + SO42― (aq) + 2 Na+ (aq)
+ 2 NO2― (aq)
 2 H + (aq)
―
45. Molecular:
Ions that Result =
Ionic:
Net Ionic:
K3PO4 (aq)
+ FeCl3 (aq)
 FePO4 (s)
+
K+ & PO43―
Fe3+ & Cl―
―
3 K+ (aq) + PO43― (aq) + Fe3+ (aq)
+ 3 Cl― (aq)
3 K+ (aq) + PO43― (aq) + Fe3+ (aq)
+ 3 Cl― (aq)
+
+
+
+
7.C – Chemical Equations: Classifications and Writing
Balance the equation…
+ O2(g)
―
+ O2(g)
+ O2(g)
…and classify it.
Mg(s)
―
 2 K + (aq)
 2 K + (aq)
H2CO3 (aq)
H+ & CO32―
 Ca2+ (aq)
 Ca2+ (aq)
CaBr2 (s)
―
―
+ 2 F (aq)
+ 2 F― (aq)
+
+
2 Br― (aq)
2 Br― (aq)
+
+
Mg (s)
Mg (s)
+
+
2 Cl― (aq)
2 Cl― (aq)
+
+
2 H+ (aq)
2 H+ (aq)
+ 2 CO32― (aq)
+ 2 CO32― (aq)
 2 Na+ (aq)
 2 Na+ (aq)
+
+
2 F― (aq)
2 F― (aq)
+ 2 CaF2 (s)
+ 2 CaF2 (s)
3 KCl (aq)
K+ & Cl―
 FePO4 (s)
 FePO4 (s)
+ 2 NO2― (aq)
+ 3 K+ (aq)
+ 3 K+ (aq)
+ 2 Na+ (aq) + SO42― (aq)
+
+
3 Cl― (aq)
3 Cl― (aq)
Balance the equation…
…and classify it.
1. _2_ Sb + _3_ Cl2  _2_ SbCl3
_S_
19. ____ Na2CO3 + _2_ HCl  _2_ NaCl + ____ H2CO3
_DR_
2. _2_ Mg + ____O2  _2_ MgO
_S_
20. ____ NH4NO2  ____ N2 + _2_ H2O
_D_
3. ____ CH4 + _2_ O2  _2_ H2O + ____ CO2
_C_
21. _2_ N2 + _5_ O2  _2_ N2O5
_S_
4. _2_ NaClO3  _2_ NaCl + _3_ O2
_D_
22. ____ MgCO3  ____ MgO + ____ CO2
_D_
5. ____ Fe + _2_ HCl  ____ FeCl2 + ____ H2
_SR_
23. _2_ KBr + ____ Cl2  _2_ KCl + ____ Br2
_SR_
6. ____ CuO + ____ H2  ____ Cu + ____ H2O
_SR_
24. ____ C11H22O11 + _11_ O2  _11_ H2O + _11_ CO2
_C_
7. _2_ Al + _3_ H2SO4  ____ Al2(SO4)3 + _3_ H2
_SR_
25. ____ P4 + _3_ O2  ____ P4O6
_S_
8. ____ C6H8 + _8_ O2  _4_ H2O + _6_ CO2
_C_
26. ____ SrBr2 + ____ (NH4)2CO3  ____ SrCO3 + _2_ NH4Br
_DR_
9. ____ SnO2 + _2_ C  ____ Sn + _2_ CO
_SR_
27. _2_ AgNO3 + ____ (NH4)2CrO4  ____ Ag2CrO4 + _2_ NH4NO3
_DR_
10. ____ Pb(NO3)2 + ____ H2S  ____ PbS + _2_ HNO3
_DR_
28. _2_ K + _2_ H2O  _2_ KOH + ____ H2
_SR_
11. _2_ HgO  _2_ Hg + ____ O2
_D_
29. _2_ Al + _3_ Pb(NO3)2  _2_ Al(NO3)3 + _3_ Pb
_SR_
12. _2_ KClO3  _2_ KCl + _3_ O2
_D_
30. _3_ Fe + _2_ O2  ____ Fe3O4
_S_
13. ____ N2 + _3_ H2  _2_ NH3
_S_
31. _____ C3H2O + _3_ O2  ____ H2O + _3_ CO2
_C_
14. _2_ NaBr + ____ Cl2  _2_ NaCl + ____ Br2
_SR_
32. ____ ZnCl2 + _2_ KOH  ____ Zn(OH)2 + _2_ KCl
_DR_
15. ____ Zn + _2_ AgNO3  ____ Zn(NO3)2 + _2_ Ag
_SR_
33. ____ Fe3O4 + _4_ H2  _3_ Fe + _4_ H2O
_SR_
16. ____ Sn + _2_ Cl2  ____ SnCl4
_S_
34. ____ Pb(NO3)2  ____ Pb + _2_ NO2 + ____ O2
_D_
17. ____ C2H6O + _3_ O2  _3_ H2O + _2_ CO2
_C_
35. _2_ H2O  _2_ H2 + ____ O2
_D_
18. ____ Mg(OH)2 + _2_ HCl  ____ MgCl2 + _2_ H2O
_DR_
36. _3_ Mg + ____ N2  ____ Mg3N2
_S_
37. Fe (s)
+
SO2 (g)
 FeS (s)
+
O2 (aq)
38. Zn (s)
+
CuSO4 (aq)
 ZnSO4 (aq)
+
Cu (s)
39. AgNO3 (aq)
+
NaBr (aq)
 NaNO3 (aq)
+
AgBr (s)
40. 2 KClO3 (aq)

2 KCl (s)
+
3 O2 (g)
41. 2 H2O (L)

2 H2 (g)
+
O2 (g)
42. 2 HgO (s)

2 Hg (L)
+
O2 (g)
43. 2 KI (aq)
+
Pb(NO3)2 (aq)
 PbI2 (s)
+
2 KNO3 (aq)
44. 4 Al (s)
+
2 O2 (g)
 2 Al2O3 (s)
45. 2 Na2O2 (aq)
+
2 H2O (L)
 4 NaOH (aq)
+
O2 (g)
46. Fe2O3 (s)
+
3 C (s)
 2 Fe (s)
+
3 CO (aq)
47. Fe (s)
+
H2O (L)
 H2 (g)
+
Fe2O3 (s)
48. FeCl3 (aq)
+
3 KOH (aq)
 3 KCl (aq)
+
Fe(OH)3 (s)
49. 2 Al (s)
+
3 H2SO4 (aq)
 Al2(SO4)3 (aq) +
3 H2 (g)
50. Na2CO3 (aq)
+
Ca(OH)2 (aq)
 2 NaOH (aq)
CaCO3 (s)
51. CO2 (g)
+
H2O (L)
 H2CO3 (aq)
52. CaO (s)
+
H2O (L)
 Ca(OH)2 (aq)
+
7.D – Chemical Equations: Predicting Products
Instructions: ON A SEPARATE SHEET OF PAPER , transcribe and complete each equation by predicting the products using your “ORANGE SHEET” as a reference.
Check to make sure you have completed the equation correctly. Remember to indicated state and “THE 9 + H”. Then go back and balance each equation!!!!
1. Ag2O (s)
→
2 Ag(s)
+
O2 (g)
2.
3 S8 (g)
+
16 Fe(s)
→
8 Fe2S3 (g)
3.
CH3CH2CH3 (g)
+
5 O2 (g)
→
3 CO2 (g)
+
4 H2O (g)
4.
Pb(NO3)2 (aq)
+
2 NaCl(aq)
→
PbCl2 (s)
+
2 NaNO3(aq)
5.
2 CuBr(s)
→
2 Cu(s)
+
Br2 (l)
6.
3 Zn (s)
+
2 H3PO4 (aq)
→
Zn3(PO4)2
+
3 H2 (g)
7.
2 K (s)
+
2 H2O (l)
→
2 KOH (aq)
+
H2 (g)
8.
3 AgClO3 (aq)
+
AlI3 (aq)
→
Al (ClO3)3 (aq)
+
3 AgI (s)
9.
2 Fe(s)
+
3 Cl2 (g)
→
2 FeCl3 (s)
10. C12H22O11 (s)
+
12 O2 (g)
→
12 CO2 (g)
+
11 H2O (g)
11. Pb(C2H3O2)2 (aq)
+
Li2CrO4 (aq)
→
PbCrO4 (s)
+
2 LiC2H3O2 (aq)
12. F2 (g)
+
2 RbBr (s)
→
2 RbF(s)
+
Br2 (l)
→
8 Cu(s)
+
S8(s)
13. 8 CuS (s)
(s)
14. 2 HCl (aq)
+
Ca(s)
→
CaCl2 (aq)
+
H2 (g)
15. 3 H2SO4 (aq)
+
2 Cr(OH)3 (aq)
→
6 H2O (l)
+
Cr2(SO4)3 (aq)
16. 4 Co (s)
+
3 O2 (g)
→
3 Co2O3 (s)
17. 3 CuSO4 (aq)
+
2 Na3PO4 (aq)
→
3 Na2SO4 (aq)
+
Cu3(PO4)2 (s)
18. CH4 (g)
+
2 O2 (g)
→
CO2 (g)
+
2 H2O (g)
19. Sn(Cr2O7)2 (aq)
+
2 (NH4)2S
→
SnS2 (s)
+
2 (NH4)2Cr2O7 (aq)
→
3 Zn (s)
+
N2 (g)
20. Zn3N2 (s)
21. Sr (s)
+
2 HClO2 (aq)
→
Sr(ClO2)2 (aq)
+
H2 (g)
22. Al(OH)3 (s)
+
3 HNO3 (aq)
→
Al(NO3)3 (aq)
+
3 H2O (l)
23. 2 C2H6
+
7 O2 (g)
→
4 CO2 (g)
+
6 H2O (g)
24. Ti (s)
+
4 HNO2 (aq)
→
Ti(NO2)4 (aq)
+
2 H2 (g)
7.E – Chemical Equations: Predicting Products and Activity Series
Instructions: Complete each equation using your “Orange Sheet” to predict products and the activity series to determine if the reaction will occur. If a
reaction will not occur; you must write: “No Reaction”. DO NOT go back and balance each equation…..unless you need the practice.
1.
Mg + O2 →
MgO
2.
Al2(SO4)3 + Cu →
No Rxn
3.
HNO3 + Cu →
No Rxn
4.
HBr + F2 →
HF
5.
Cu + H2O(g) →
No Rxn
6.
Na + H2O(g) →
7.
+
Br2
NaOH
+
H2
CrBr3 + F2 →
CrF3
+
Br2
8.
Li + H2O(l) →
LiOH
+
H2
9.
KF + Cl2 →
No Rxn
10.
Pb(NO3)2 + Ni →
Ni(NO3)2 +
Pb
11.
HNO2 + Ca →
Ca(NO2)2 +
Ca
12.
Mn + H2O(g) →
No Rxn
13.
Zn + H2O(g) →
Zn(OH)2 +
Zn
14.
H2SO4 + Ni →
NiSO4
H2
15.
Mn + H2O(l) →
No Rxn (Has to be steam (g), to react with water)
16.
FeCl3 + H2 →
No Rxn
17.
Sr + HBr →
SrBr2
18.
Au + O2
19.
Rb + H2O(g) →
RbOH
20.
HCl + Pt →
No Rxn
21.
H2O(l) + K → KOH
+
22.
Al + H2O(l) →
No Rxn (Has to be steam (g), to react with water)
23.
Zn + H3PO4 →
Zn3(PO4)2+
H2
24.
Na + H2O(g) →
NaOH
H
→
+
+
H2
+
H2
No Rxn
H2
+