Practice Problems Basic Chemistry: Types of Reactions

7/27/2019 Practice Problems Basic Chemistry: Types of Reactions

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Practice Problems (Chapter 4): Types of Reactions

CHEM 1A

Identify the type(s) of reaction in the following equations.

1. 2 SO2 + O2 2 SO3 ___________________________

2. 4 Al + 3 MnO2 3 Mn + 2 Al2O3 ___________________________

3. Bi2S3 + 6 HCl 2 BiCl3 + 3 H2S ___________________________

4. 2 PbO2 2 PbO + O2 ___________________________

5. 3 H2SO4 + 2 Al(OH)3 6 H2O + Al2(SO4)3 ___________________________

6. C3H8 + 5 O2 3 CO2 + 4 H2O ___________________________

Predict the products for the following combination reactions and balance them (show your check).

The product of each reaction is a charge neutral ionic compound.

7. ___ Mg(s) + ___ O2(g)

8. ___ Al(s) + ___ Br2(l)

Predict the products for the following single replacement reactions

and balance them (show your check). If no reaction occurs, write

no reaction on the product side of the arrow.

9. ___ Cu(s) + ___ FeCl3(aq)

10. ___ Al(s) + ___ HBr(aq)

11. ___ H2(g) + ___ Al2O3(aq)

12. ___ Cl2(g) + ___ HBr(aq)

13. ___ I2(s) + ___ HCl(aq)

KEY

no reaction

no reaction

no reaction

___ AlBr3 + ___ H262 2 3

___ HCl + ___ Br22 2

Check:Al 2

H 6

Br 6

charge 0

Check:Cl 2 H 2

Br 2

charge 0

combination, redox

___ AlBr332 2Check:

Al 2

Br 6

charge 0

___ MgO2

Check:Mg 2

O 2

charge 0

12

Activity Series:

Metals Non-Meta(and Hydrogen) (Halogens)

form cations form anion

K F2

Ca Cl2

Na Br2Mg I2

Al

ZnFeNi

Sn

PbH

CuAg

HgAu

increasing

activit

11

single displacement, redox

double displacement

decomposition, redox

acid-base neutralization, double displacement

combustion, redox


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Predict the products for the following double replacement reactions and balance them (show your

check). Use the solubility rules to determine if a precipitate (solid) will form. Label the phase of

insoluble products as solid and soluble products as aqueous.

14. ___ Cu(NO3)2(aq) + ___ FeCl3(aq)

15. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq)

16. ___ KCl(aq) + ___ Pb(NO3)2(aq)

17. ___ Na2CO3(aq) + ___ CaBr2(aq)

18. ___ CaCl2(aq) + ___ AgNO3(aq)

Complete the following combustion reactions (in air) and balance them (show your check).

19. ___ C2H2(g) + ___ ______(g)

20. ___ C3H8(g) + ___ ______(g)

21. ___ C2H5OH(l) + ___ ______(g)

Predict the products for the following acid-base neutralization reactions and balance them (show

your check).

22. ___ HBr(aq) + ___ Al(OH)3(s)

23. ___ HCl(aq) + ___ CaCO3(s)

24. ___ H2SO4(aq) + ___ KOH(aq)

25. ___ H3PO4(aq) + ___ Ba(OH)2(aq)

___ BaSO4(s) + ___ NH4C2H3O2(aq)11 1 2

___ NaBr(aq) + ___ CaCO3(s)1 2

Check (#17 Na 2

C 1

O 3

Ca 1

Br 2

charge 0

11

Check (#19):C 4 H 4

O 10

charge 0

___ H2O + ___ CO2 + ___ CaCl212 1 1

3

Check (#22):H 6

Br 3

Al 1

O 3 charge 0

Check (#25H 12

P 2

O 14Ba 2

charge 0

2

___ CuCl2(aq) + ___ Fe(NO3)3(aq)3 2

Check (#14):Cu 3

N 6

O 18 Fe 2 Cl 6

charge 0

3 2Check (#15

Ba 1

C 4

H 14

O 8N 2

S 1

charge 0

___ KNO3(aq) + ___ PbCl2(s)2 12 1

Check (#16):K 2

Cl 2 Pb 1

N 2

O 6 charge 0

___ Ca(NO3)2(aq) + ___ AgCl(s)1

Check (#18):Ca 1

Cl 2

Ag 2

N 2 O 6

charge 0

21 2

___ CO2 + ___ H2O4 2O22 5

___ CO2 + ___ H2O3 4O21 5

___ CO2 + ___ H2O2 3O21 3

Check (#20 C 3

H 8

O 10charge 0

Check (#21):C 2 H 6

O 7

charge 0

___ H2O + ___ AlBr33 13 1

1

Check (#23H 2Cl 2

Ca 1

C 1O 3

charge 0Check (#24):

H 4

S 1 O 6

K 2

charge 0

___ H2O + ___ K2SO42 121

___ H2O + ___ Ba3(PO4)26 1


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Balance the following redox reactions using the reaction method.

26. CH3OH(aq) + Cr2O72-(aq) CH2O(aq) + Cr3+(aq)

27. Zn(s) + HCl(aq) Zn2+(aq) + H2(g) + Cl(aq)

2 +6 0 +3

Red. Agent Ox. Agent

3 CH3OH 3 CH2O + 6 H+ + 6 e

+20 0+1

Red.

Agent

Ox.

Agent

Zn Zn + + 2 e

Note: HCl exists as H+

+ Cl

in aqueous

solution. The Cl

is a spectator ion and

doesnt need to be included.

Balanced Redox Equation:

CH3OH CH2O

+ 2 H+

+ 2 e

x 3

Check:

C 3

H 20

O 10

Cr 2

charge 6+

Cr2O7 2 Cr +

+ 7 H2O

+ 14 H+

+ 6 e

x 1

Cr2O7+ 14 H

++ 6 e

2 Cr ++ 7 H2O

Oxidation Reaction: Reduction Reaction:

8

3 CH3OH + Cr2O72 + 8 H

+ 3 CH2O + 2 Cr3+ + 7 H2O

3 CH3OH + Cr2O7+ 14 H

++ 6 e

3 CH2O + 6 H+ + 6 e + 2 Cr ++ 7 H2O

Oxidation Reaction:

Zn Zn ++ 2 e

x 1

Check:

Zn 1

H 2

charge 2+

2 H+ H2

+ 2 e

x 1

2 H+

+ 2 e H2

Reduction Reaction:

Zn + 2 H+ Zn2+ + H2

Zn + 2 H+

+ 2 e Zn + + 2 e + H2



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Note: This is a disproportionation reaction

(the same element is being reduced and oxidized)28. Cl2(g) ClO

-(aq) + Cl

-(aq)

(Occurring in a basic solution)

Write and balance the formula equation, the complete ionic equation, and the net ionic equation

for the following reaction. Include the phases in the formula equation, and circle the spectator

ions in the complete ionic equation.

29. The acid-base neutralization reaction between aqueous phosphoric acid and aqueous sodiumhydroxide

Formula Eqn.:

H3PO4 (aq) + 3 NaOH (aq) 3 H2O (l) + Na3PO4 (aq)

Check:H 6

P 1 O 7

Na 3

charge 0 weak

acid

strong

base

molecular

compound

soluble

salt

Complete Ionic Eqn.:

H3PO4 + 3 Na+ + 3 OH 3 H2O + 3 Na

+ + PO43

Net Ionic Eqn.:

H3PO4 + 3 OH 3 H2O + PO4

3

1+10

Oxidation Reaction:

Cl2 2 ClO

+ 2 H2O

+ 2 e

x 1

Cl2 2 Cl

+ 2 e

x 1

Reduction Reaction:

+ 4 H+

+ 4 OH

4 H2O2

Cl2 + 2 e 2 ClCl2 + 4 OH 2 ClO + 2 H2O + 2 e

+ 4 OH

Check:

Cl 2

O 2

H 2

charge 2

Cl2 + 2 OH ClO + H2O + Cl

reduce by 22 Cl2 + 4 OH

+ 2 e

2 ClO + 2 H2O + 2 e + 2 Cl


Practice Problems Basic Chemistry: Types of Reactions

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