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Classification of Chemical Reactions

Total questions: 47

Worksheet time: 24mins

Name
Class
Date
1.

Identify the oxidation number of the underlined element: Na2S2O3

a)

0

b)

+1

c)

+2

d)

+3

2.

Identify the oxidation number of the underlined element: C2O4-2

a)

0

b)

+1

c)

+2

d)

+3

3.

Identify the oxidation number of the underlined element: CuCl

a)

0

b)

+1

c)

+2

d)

+3

4.

Identify the oxidation number of the underlined element: I2

a)

0

b)

+1

c)

+2

d)

+3

5.

What is the product of a synthesis reaction between solid potassium (K) and chlorine gas (Cl2)?

a)

KCl

b)

K2Cl

c)

PCl2

6.

As shown, a student added a small amount of sodium carbonate solution to a test tube containing calcium chloride solution. A white solid immediately appeared. What conclusion can be made from this experiment?

a)

The chemical reaction requires energy to occur.

b)

A precipitate was formed during the reaction.

c)

Heat is generated by the chemical reaction.

d)

Sodium carbonate is less soluble than calcium chloride.

7.

Which of the following chemical reactions will produce a precipitate?

a)

Na2CO3 + CaCl2  CaCO3 + 2NaCl

b)

3KBr + AlPO4  K3PO4 + AlBr3

c)

NH4OH + KCl   KOH + NH4Cl

d)

ZnCl2 + MgSO4  ZnSO4 + MgCl2

8.

Which is not an example of a redox reaction?

a)

2Mg(s) + O2(g) 2MgO(s)

b)

2HgO(aq) + Cl2(g) 2HgCl(aq) + O2(g)

c)

CH4(g) + 2O2(g) CO2(g) + 2H2O(g)

d)

CuCl2(aq) + H2S(aq) CuS(s) + 2HCl(aq)

9.

What are the coefficients that balance the following equation?

___ PbO2 ___ PbO + ___ O2

a)

4, 3, 2

b)

2, 2, 1

c)

3, 4, 2

d)

2, 1, 1

10.

What type of reaction is the following?

___ PbO2 ___ PbO + ___ O2

a)

Decomposition

b)

single replacement

c)

combustion

d)

Synthesis

11.

Consider this chemical reaction:

2AgBr(s) + energy 2Ag(s) + Br2(l)

Which is true about the reaction?

a)

Silver is reduced.

b)

Bromine is reduced.

c)

Silver loses electrons.

d)

Bromine gains electrons.

12.

Which chemical equation supports the Law of Conservation of Mass?

a)

Al4C3(aq) + H2O(l) CH4(g) + Al(OH)3(s)

b)

2H2O(l) H2(g) + O2(g)

c)

CH4(g) + 2O2(g) CO2(g) + 2H2O(g)

d)

Zn(s) + HCl(aq) ZnCl2(aq) + H2(g)

13.

Which equation represents a single replacement reaction that can occur?

a)

Li(s) + KCl(aq) LiCl(aq) + K(s)

b)

Zn(s) + 2NaF(aq) ZnF2(aq) + 2Na(s)

c)

K(s) + LiCl(aq) KCl(aq) + Li(s)

d)

Cu(s) + 2NaCl(aq) CuCl2(aq) + 2Na(s)

14.

Which diagram best demonstrates the law of conservation of mass?

a)
b)
c)
d)
15.

Cu + 2AgNO3 Cu(NO3)2 + 2Ag

This redox reaction above can also be classified as _____.

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

16.

Cu + 2AgNO3 Cu(NO3)2 + 2Ag

From the equation above, identify the correct reduction half-reaction.

a)

Cu2+ + 2e- Cu

b)

2Ag1+ + 2e- 2Ag

c)

2Ag 2Ag1+ + 2e-

d)

Cu Cu2+ + 2e-

17.

Cu + 2AgNO3 Cu(NO3)2 + 2Ag

From the equation above, identify the correct oxidation half-reaction.

a)

2Ag 2Ag1+ + 2e-

b)

Cu2+ + 2e- Cu

c)

Cu Cu2+ + 2e-

d)

2Ag1+ + 2e- 2Ag

18.

What are the coefficients that balance the following equation?____ RbNO3 + ____ BeF2 ____ Be(NO3)2 + ____ RbF

a)

1,2,1,2

b)

2,2,1,2

c)

1,2,2,1

d)

2,1,1,2

19.

What is the balanced chemical equation for the reaction shown in the image?

a)

Fe(s) + Cl(g) FeCl(s)

b)

Fe(s) + Cl2(g) FeCl3(s)

c)

2Fe(s) + 3Cl2(g) 2FeCl3(s)

d)

2Fe(s) + 6Cl(g) 2FeCl3(s)

20.

The redox reaction shown can also be classified as _____.

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

21.

Given the following balanced equation representing a redox reaction, which statement is true? 2Al + 3Cu2+ 2Al3+ + 3Cu

a)

Each Al loses 2e- and each Cu2+ gains 3e-.

b)

Each Al loses 3e- and each Cu2+ gains 2e-.

c)

Each Al3+ gains 2e- and each Cu loses 3e-.

d)

Each Al3+ gains 3e- and each Cu loses 2e-.

22.

The oxidation state of chlorine in the following reaction changes from:

2KClO3(s) 2KCl(s) + 3O2(g)

a)

+1 to -1

b)

-1 to +1

c)

+5 to -1

d)

-1 to +5

23.

Joe is classifying reactions as acid-base reactions, precipitation reactions, or oxidation-reduction reactions. What must be true of the reactions he classifies as oxidation-reduction reactions?

a)

Electrons are transferred from one substance to another.

b)

The element oxygen is in at least one reactant and one product.

c)

A substance reacts with oxygen to form water and carbon dioxide.

d)

Hydroxide ions and hydrogen ions combine to form water.

24.

H2(g) + 2AgCl(aq) 2Ag(s) + 2HCl(aq)

Using the above equation, which substance is the spectator ion?

a)

Cl1-

b)

Ag1+

c)

H20

d)

HCl

25.

H2(g) + 2AgCl(aq) 2Ag(s) + 2HCl(aq)

Using the above equation, which substance is oxidized?

a)

H20

b)

Ag1+

c)

HCl

d)

Cl1-

26.

Which choice is the correct chemical equation for the following word equation:

aqueous silver nitrate and aqueous sodium chloride react to produce which of the following products?

a)

AgNO3(aq) + NaCl(aq) ® NaNO3(s) + AgCl(s)

b)

AgNO2(aq) + NaCl(aq) ® NaAg(aq) + ClNO2(s)

c)

AgNO3(aq) + NaCl(aq) ® NaNO2(aq) + AgCl(aq)

d)

AgNO3(aq) + NaCl(aq) ® NaNO3(aq) + AgCl(s)

27.

Given the following reaction, what is the net ionic equation?

SrS(aq) + (NH4)2SO4(aq) (NH4)2S(aq) + SrSO4(s)

a)

Sr+2(aq) + 2NH4+1(aq) Sr(NH4)2(s)

b)

S-2(aq) + SO4-2(aq) SSO4(s)

c)

Sr+2(aq) + SO4-2(aq) SrSO4(s)

d)

2NH4+1(aq) + S-2(aq) (NH4)2S(s)

28.
a)

gains electrons

b)

loses electrons

c)

gains protons

d)

loses protons

29.

Identify the precipitate (insoluble substance) in the following reaction:

Pb(NO3)2 + NaI → PbI2 + NaNO3

a)

PbI2

b)

NaNO3

c)

NaI

d)

Pb(NO3)2

30.

Which is not an example of a redox reaction?

a)

2HgO + Cl2 2HgCl + O2

b)

CuCl2 + H2S CuS + 2HCl

c)

CH4 + 2O2 CO2  + 2H2O

d)

2Mg + O2 2MgO

31.

2Mg + O2  2MgO

Using the above equation, the oxidation state of oxygen changes from _____.

a)

+1 to -1

b)

-2 to 0

c)

0 to -2

d)

-1 to +1

32.

2Mg + O2  2MgO

In the above equation, oxygen is _____.

a)

oxidized

b)

reduced

33.

Which coefficients balance the following equation?

____ Br2 + ____ NaI  ____ I2 + ____ NaBr

a)

1,2,1,2

b)

1,1,1,1

c)

2,1,2,1

d)

2,2,2,2

34.

2AgBr(s) 2Ag(s) + Br2(l)

The redox reaction above can also be classified as _____.

a)

synthesis

b)

single replacement

c)

decomposition

d)

double replacement

35.

Which chemical equation supports the Law of Conservation of Mass?

a)

2H2O 2H2 + O2

b)

CH4 + 2O2 2CO2 + 2H2O

c)

Zn + HCl ZnCl2 + H2

36.

The image represents which type of chemical reaction?

a)

Decomposition

b)

Single repalcement

c)

Synthesis

d)

Double replacement

37.

Which metal is more active than Ni and less active than Zn?

a)

Mg

b)

Fe

c)

Cu

d)

Pb

38.

Consider the equation Ca(s) + O2(g) 2CaO(s). In this reaction, calcium is oxidized because it _____.

a)

becomes part of a compound.

b)

gains electrons.

c)

loses electrons.

39.

Which of the following compounds is solid in solution?

a)

NaCl

b)

AgCl

c)

Ca(NO3)2

d)

NH4Br

40.

H2(g) + 2AgCl(aq) 2Ag(s) + 2HCl(aq)

Using the above equation, which substance is reduced?

a)

H20

b)

Ag1+

c)

HCl

d)

Cl1-

41.

H2(g) + 2AgCl(aq) 2Ag(s) + 2HCl(aq)

The redox reaction above can also be classified as _____.

a)

synthesis

b)

single replacement

c)

combustion

d)

double replacement

42.

Balance the following chemical equation:

___ Ag2O  ___ Ag + ___ O2

a)

Ag2O  Ag + 2 O2

b)

2 Ag2O  4 Ag + O2

c)

Ag2O  2 Ag + O2

d)

4 Ag2O  8 Ag + O2

43.

What type of reaction does this image represent?

a)

Decomposition

b)

Synthesis

c)

Single replacement

d)

Double replacement

44.

Consider the reaction: NH4Cl(s) NH3(g) + HCl(g)

Which type of reaction does this equation represent?

a)

Single replacement

b)

Combustion

c)

Synthesis

d)

Decomposition

45.

Which of the following is an example of a combustion reaction?

a)

C2H4 + 3O2 →\rightarrow 2CO2 + 2H2O 

b)

BaCl2 + Na2SO4 →\rightarrow 2NaCl + BaSO4

c)

2HgO →\rightarrow 2Hg + O2

d)

Cl2 + 2NaBr →\rightarrow 2NaCl + Br2

46.

What type of reaction is shown?

a)

Decomposition

b)

Synthesis

c)

Single replacement

d)

Combustion

47.

Which of the following represents a double displacement reaction?

a)

ABC → AB + C

b)

A + B → AB

c)

AB + CD → AD + CB

d)

A + BC → AC + B

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