Question 1

Which of the following reactions is a redox single replacement reaction?

Accepted Answer

A)  Zn + H2SO4 $\rightarrow$ H2 + ZnSO4 
B)  2 KClO3 $\rightarrow$ 2 KCl + O2 
C)  2 NO2 + H2O2 $\rightarrow$ 2 HNO3 
D)  SO3 + H2O $\rightarrow$ H2SO4 
A)  Zn + H2SO4 $\rightarrow$ H2 + ZnSO4 
B)  2 KClO3 $\rightarrow$ 2 KCl + O2 
C)  2 NO2 + H2O2 $\rightarrow$ 2 HNO3 
D)  SO3 + H2O $\rightarrow$ H2SO4

Question 2

In which of the following compounds does Cl have an oxidation number of +7?

Accepted Answer

A)  LiClO3 
B)  Al(ClO4)3 
C)  Ca(ClO3)2 
D)  NaClO2 
A)  LiClO3 
B)  Al(ClO4)3 
C)  Ca(ClO3)2 
D)  NaClO2

Question 3

Which of the following formula unit or net ionic equations represents a disproportionation reaction?

Accepted Answer

A)  Fe + 3 Ag+ $\rightarrow$ Fe3+ + 3 Ag 
B)  2 HNO3 + SO2 $\rightarrow$H2SO4 + 2 NO2 
C)  ClO- + Cl- + 2 H+ $\rightarrow$ Cl2 + H2O 
D)  CH4 + 2 O2 $\rightarrow$ CO2 + H2O 
A)  Fe + 3 Ag+ $\rightarrow$ Fe3+ + 3 Ag 
B)  2 HNO3 + SO2 $\rightarrow$H2SO4 + 2 NO2 
C)  ClO- + Cl- + 2 H+ $\rightarrow$ Cl2 + H2O 
D)  CH4 + 2 O2 $\rightarrow$ CO2 + H2O

Question 4

Which is the balanced half reaction in basic solution for the reaction below?
Cr(OH)4-$\rightarrow$ CrO42-

Accepted Answer

A)  3 e- + Cr(OH)4- + 2 OH- $\rightarrow$ Cr(OH)4- + 2 H2O 
B)  4 OH- + Cr(OH)4- $\rightarrow$CrO42- + 3e- + 4 H2O 
C)  2 OH- + Cr(OH)4-  $\rightarrow$ CrO42- + 6 e- + 3 H2O 
D)  Cr(OH)4- $\rightarrow$ CrO42- + 4 H2O + 2 e- 
A)  3 e- + Cr(OH)4- + 2 OH- $\rightarrow$ Cr(OH)4- + 2 H2O 
B)  4 OH- + Cr(OH)4- $\rightarrow$CrO42- + 3e- + 4 H2O 
C)  2 OH- + Cr(OH)4-  $\rightarrow$ CrO42- + 6 e- + 3 H2O 
D)  Cr(OH)4- $\rightarrow$ CrO42- + 4 H2O + 2 e-

Question 5

In which of the following compounds does nitrogen have an oxidation number of +4?

Accepted Answer

A)  HNO3 
B)  NO2 
C)  N2O 
D)  NH4Cl 
A)  HNO3 
B)  NO2 
C)  N2O 
D)  NH4Cl

Question 6

Which statement is incorrect?

Accepted Answer

A)  Reduction occurs at the anode in an electrolytic cell. 
B)  Electroplating is the deposition of a thin layer of metal on an object. 
C)  During recharging the lead storage battery is functioning as an electrolytic cell. 
D)  Electrolysis is a process in which electrical energy is used to cause a nonspontaneous reaction to occur. 
A)  Reduction occurs at the anode in an electrolytic cell. 
B)  Electroplating is the deposition of a thin layer of metal on an object. 
C)  During recharging the lead storage battery is functioning as an electrolytic cell. 
D)  Electrolysis is a process in which electrical energy is used to cause a nonspontaneous reaction to occur.

Question 7

The following reactions are classified first as redox or nonredox. They are further classified as synthesis, decomposition, single replacement, or double displacement reactions. Which of the following reactions is incorrectly classified as to redox/nonredox or as to synthesis, decomposition, single-replacement, or double-displacement (precipitation) reactions?

Accepted Answer

A)  HNO3(aq) + LiOH(aq) $\rightarrow$ LiNO3 (aq) + H2O(l) non-redox / double-displacement 
B)  Pb(NO3)2(aq) + 2 Na(s) $\rightarrow$ Pb(s) + NaNO3(aq) redox / single-replacement 
C)  2 H2O2(l) $\rightarrow$ 2 H2O(l) + O2(g) non-redox / decomposition 
D)  AgNO3(aq) + KOH(aq) $\rightarrow$ KNO3(aq) + AgOH(s) non-redox / precipitation 
A)  HNO3(aq) + LiOH(aq) $\rightarrow$ LiNO3 (aq) + H2O(l) non-redox / double-displacement 
B)  Pb(NO3)2(aq) + 2 Na(s) $\rightarrow$ Pb(s) + NaNO3(aq) redox / single-replacement 
C)  2 H2O2(l) $\rightarrow$ 2 H2O(l) + O2(g) non-redox / decomposition 
D)  AgNO3(aq) + KOH(aq) $\rightarrow$ KNO3(aq) + AgOH(s) non-redox / precipitation

Question 8

Indicate whether each of the following formula unit or net ionic equations is or is not a redox reaction by writing the word
-NH4+(aq) + CN-(aq) $\rightarrow$ HCN(aq) + NH3(aq) ____________________

Accepted Answer

A)  non-redox 
B)  redox 
A)  non-redox 
B)  redox

Question 9

Which response represents the balanced half reaction for oxidation for the reaction given below?
HCl (aq) + Fe (s) $\rightarrow$ FeCl3 (aq) + H2 (g)

Accepted Answer

A)  6 e- + 6 H+ $\rightarrow$ 3 H2 
B)  2 Fe $\rightarrow$ 2 Fe3+ + 6 e- 
C)  3 Fe $\rightarrow$ Fe3+ + 3 e- 
D)  Fe + 3 e- $\rightarrow$Fe3+ 
A)  6 e- + 6 H+ $\rightarrow$ 3 H2 
B)  2 Fe $\rightarrow$ 2 Fe3+ + 6 e- 
C)  3 Fe $\rightarrow$ Fe3+ + 3 e- 
D)  Fe + 3 e- $\rightarrow$Fe3+

Question 10

The oxidation number of C in BaC2O4 is ________.

Accepted Answer

A)  -3 
B) -2 
C)  +2 
D)  +3 
A)  -3 
B) -2 
C)  +2 
D)  +3

Question 11

In which of the following sequences of sulfur-containing species are the species arranged in order of decreasing oxidation number for S?

Accepted Answer

A)  SO32-, SO42-, S2- 
B)  SO42-, S2O32-, S2- 
C)  S2O32-, SO32-, S2- 
D)  SO42-, S2-, S2O32- 
A)  SO32-, SO42-, S2- 
B)  SO42-, S2O32-, S2- 
C)  S2O32-, SO32-, S2- 
D)  SO42-, S2-, S2O32-

Question 12

In the following reaction, which species is the reducing agent?
3 Cu (s) + 6 H+ (aq) + 2 HNO3 (aq) $\rightarrow$ 3 Cu+2 (aq) + 2 NO (g) + 4 H2O (l)

Accepted Answer

A)  H+ 
B)  Cu 
C)  N in NO 
D)  Cu+2 
A)  H+ 
B)  Cu 
C)  N in NO 
D)  Cu+2

Question 13

When the redox reaction: Zn + As2O3 $\rightarrow$ AsH3 + Zn2+ (acidic solution) is balanced, the correct coefficients for H2O, H+ and AsH3 are, respectively, ________.

Accepted Answer

A)  6, 6 and 3 
B)  6, 3 and 12 
C)  3, 12 and 2 
D)  4, 8 and 3 
A)  6, 6 and 3 
B)  6, 3 and 12 
C)  3, 12 and 2 
D)  4, 8 and 3

Question 14

Which substance is serving as the reducing agent in the following reaction?
14H+ + Cr2O7-2 + 3 Ni $\rightarrow$ 3 Ni2+ + 2 Cr+3 + 7 H2O

Accepted Answer

A)  Ni 
B)  H+ 
C)  Cr2O7-2 
D)  H2O 
A)  Ni 
B)  H+ 
C)  Cr2O7-2 
D)  H2O

Question 15

In balancing the equation for a disproportionation reaction, using the oxidation number method, the substance undergoing disproportionation is ________.

Accepted Answer

A)  initially written twice on the reactant side of the equation 
B)  initially written twice on the product side of the equation 
C)  initially written on both the reactant and product sides of the equation 
D)  always assigned an oxidation number of zero 
A)  initially written twice on the reactant side of the equation 
B)  initially written twice on the product side of the equation 
C)  initially written on both the reactant and product sides of the equation 
D)  always assigned an oxidation number of zero

Question 16

Balance the following net ionic equation using the half reaction method (in acidic solution). What is the coefficient for MnO4-?
H+ + Fe2+ + MnO4- $\rightarrow$Fe3+ + Mn2+ + H2O

Accepted Answer

A)  8 
B)  5 
C)  1 
D)  14 
A)  8 
B)  5 
C)  1 
D)  14

Question 17

Which of the following is not correct for both acidic and alkaline dry cells?

Accepted Answer

A)  As the name implies, the electrolyte is a dry material. 
B)  The anode reaction involves Zn. 
C)  The cathode reaction involves MnO2. 
D)  The cathode is an inert material. 
A)  As the name implies, the electrolyte is a dry material. 
B)  The anode reaction involves Zn. 
C)  The cathode reaction involves MnO2. 
D)  The cathode is an inert material.

Question 18

Which of the following reactions is a disproportionation reaction?

Accepted Answer

A)  2 H2O $\rightarrow$ 2 H2 + O2 
B)  H2SO3 $\rightarrow$ H2O + SO2 
C)  HNO2 $\rightarrow$ NO + NO3- 
D)  Mg + H2SO4 $\rightarrow$ MgSO4 + H2 
A)  2 H2O $\rightarrow$ 2 H2 + O2 
B)  H2SO3 $\rightarrow$ H2O + SO2 
C)  HNO2 $\rightarrow$ NO + NO3- 
D)  Mg + H2SO4 $\rightarrow$ MgSO4 + H2

Question 19

Which of the following accurately represents the oxidation of the Co+2 ion?

Accepted Answer

A)  Co+2 + 2 e- $\rightarrow$Co 
B)  Co+2 $\rightarrow$Co+3 + e- 
C)  Co $\rightarrow$Co+2 + 2 e- 
D)  Co+3 + e- $\rightarrow$ Co+2 
A)  Co+2 + 2 e- $\rightarrow$Co 
B)  Co+2 $\rightarrow$Co+3 + e- 
C)  Co $\rightarrow$Co+2 + 2 e- 
D)  Co+3 + e- $\rightarrow$ Co+2

Question 20

Which response represents the balanced half reaction for reduction for the reaction given below?
Fe (s) + CuSO4 (aq)$\rightarrow$ Fe2(SO4)3 (aq) + Cu (s)

Accepted Answer

A)  2 Cu2+ + 3 e- $\rightarrow$ 2 Cu 
B)  Fe + 3 e- $\rightarrow$ Fe3+ 
C)  3 Cu2+ + 6 e-$\rightarrow$ 3 Cu 
D)  2 Fe $\rightarrow$ 2 Fe3+ + 6e- 
A)  2 Cu2+ + 3 e- $\rightarrow$ 2 Cu 
B)  Fe + 3 e- $\rightarrow$ Fe3+ 
C)  3 Cu2+ + 6 e-$\rightarrow$ 3 Cu 
D)  2 Fe $\rightarrow$ 2 Fe3+ + 6e-

Which of the following reactions is a redox single replacement reaction?

In which of the following compounds does Cl have an oxidation number of +7?

Which of the following formula unit or net ionic equations represents a disproportionation reaction?

Which is the balanced half reaction in basic solution for the reaction below? Cr(OH)₄^- $\rightarrow$ CrO₄^2-

In which of the following compounds does nitrogen have an oxidation number of +4?

Which statement is incorrect?

Indicate whether each of the following formula unit or net ionic equations is or is not a redox reaction by writing the word -NH₄⁺(aq) + CN^-(aq) $\rightarrow$ HCN(aq) + NH₃(aq) ____________________

Which response represents the balanced half reaction for oxidation for the reaction given below? HCl (aq) + Fe (s) $\rightarrow$ FeCl₃(aq) + H₂ (g)

The oxidation number of C in BaC₂O₄ is ________.

In which of the following sequences of sulfur-containing species are the species arranged in order of decreasing oxidation number for S?

In the following reaction, which species is the reducing agent? 3 Cu (s) + 6 H⁺ (aq) + 2 HNO₃ (aq) $\rightarrow$ 3 Cu⁺² (aq) + 2 NO (g) + 4 H₂O (l)

When the redox reaction: Zn + As₂O₃ $\rightarrow$ AsH₃ + Zn²⁺ (acidic solution) is balanced, the correct coefficients for H₂O, H⁺ and AsH₃ are, respectively, ________.

Which substance is serving as the reducing agent in the following reaction? 14H⁺ + Cr₂O₇^-2 + 3 Ni $\rightarrow$ 3 Ni²⁺ + 2 Cr⁺³ + 7 H₂O

In balancing the equation for a disproportionation reaction, using the oxidation number method, the substance undergoing disproportionation is ________.

Balance the following net ionic equation using the half reaction method (in acidic solution). What is the coefficient for MnO₄^-? H⁺ + Fe²⁺ + MnO₄^- $\rightarrow$ Fe³⁺ + Mn²⁺ + H₂O

Which of the following is not correct for both acidic and alkaline dry cells?

Which of the following reactions is a disproportionation reaction?

Which of the following accurately represents the oxidation of the Co⁺² ion?

Which response represents the balanced half reaction for reduction for the reaction given below? Fe (s) + CuSO₄(aq) $\rightarrow$ Fe₂(SO₄)₃(aq) + Cu (s)

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Exam 15: Oxidation and Reduction

Which of the following reactions is a redox single replacement reaction?

In which of the following compounds does Cl have an oxidation number of +7?

Which of the following formula unit or net ionic equations represents a disproportionation reaction?

Which is the balanced half reaction in basic solution for the reaction below? Cr(OH)4- →\rightarrow→ CrO42-

In which of the following compounds does nitrogen have an oxidation number of +4?

Which statement is incorrect?

Indicate whether each of the following formula unit or net ionic equations is or is not a redox reaction by writing the word -NH4+(aq) + CN-(aq) →\rightarrow→ HCN(aq) + NH3(aq) ____________________

Which response represents the balanced half reaction for oxidation for the reaction given below? HCl (aq) + Fe (s) →\rightarrow→ FeCl3 (aq) + H2 (g)

The oxidation number of C in BaC2O4 is ________.

In which of the following sequences of sulfur-containing species are the species arranged in order of decreasing oxidation number for S?

In the following reaction, which species is the reducing agent? 3 Cu (s) + 6 H+ (aq) + 2 HNO3 (aq) →\rightarrow→ 3 Cu+2 (aq) + 2 NO (g) + 4 H2O (l)

When the redox reaction: Zn + As2O3 →\rightarrow→ AsH3 + Zn2+ (acidic solution) is balanced, the correct coefficients for H2O, H+ and AsH3 are, respectively, ________.

Which substance is serving as the reducing agent in the following reaction? 14H+ + Cr2O7-2 + 3 Ni →\rightarrow→ 3 Ni2+ + 2 Cr+3 + 7 H2O

In balancing the equation for a disproportionation reaction, using the oxidation number method, the substance undergoing disproportionation is ________.

Balance the following net ionic equation using the half reaction method (in acidic solution). What is the coefficient for MnO4-? H+ + Fe2+ + MnO4- →\rightarrow→ Fe3+ + Mn2+ + H2O

Which of the following is not correct for both acidic and alkaline dry cells?

Which of the following reactions is a disproportionation reaction?

Which of the following accurately represents the oxidation of the Co+2 ion?

Which response represents the balanced half reaction for reduction for the reaction given below? Fe (s) + CuSO4 (aq) →\rightarrow→ Fe2(SO4)3 (aq) + Cu (s)

The Science of Chemistry

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Chemical Nomenclature

Chemical Calculations: the Mole Concept and Chemical Formulas

Chemical Calculations Involving Chemical Equations

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Acids, Bases and Salts

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Which is the balanced half reaction in basic solution for the reaction below? Cr(OH)₄^- $\rightarrow$ CrO₄^2-

Indicate whether each of the following formula unit or net ionic equations is or is not a redox reaction by writing the word -NH₄⁺(aq) + CN^-(aq) $\rightarrow$ HCN(aq) + NH₃(aq) ____________________

Which response represents the balanced half reaction for oxidation for the reaction given below? HCl (aq) + Fe (s) $\rightarrow$ FeCl₃(aq) + H₂ (g)

The oxidation number of C in BaC₂O₄ is ________.

In the following reaction, which species is the reducing agent? 3 Cu (s) + 6 H⁺ (aq) + 2 HNO₃ (aq) $\rightarrow$ 3 Cu⁺² (aq) + 2 NO (g) + 4 H₂O (l)

When the redox reaction: Zn + As₂O₃ $\rightarrow$ AsH₃ + Zn²⁺ (acidic solution) is balanced, the correct coefficients for H₂O, H⁺ and AsH₃ are, respectively, ________.

Which substance is serving as the reducing agent in the following reaction? 14H⁺ + Cr₂O₇^-2 + 3 Ni $\rightarrow$ 3 Ni²⁺ + 2 Cr⁺³ + 7 H₂O

Balance the following net ionic equation using the half reaction method (in acidic solution). What is the coefficient for MnO₄^-? H⁺ + Fe²⁺ + MnO₄^- $\rightarrow$ Fe³⁺ + Mn²⁺ + H₂O

Which of the following accurately represents the oxidation of the Co⁺² ion?

Which response represents the balanced half reaction for reduction for the reaction given below? Fe (s) + CuSO₄(aq) $\rightarrow$ Fe₂(SO₄)₃(aq) + Cu (s)