Question

Indicate the elements oxidized/reduced, as well as their oxidation states before and after the reaction. Determine...

Indicate the elements oxidized/reduced, as well as their oxidation states before and after the reaction. Determine which species is the oxidizing agent and which is the reducing agent.

  2 AgNO3(aq) + Cu(s) ……> Cu(NO3)2(aq) + 2 Ag(s)

A.

Cu 0 à 2+; oxidized, Cu oxidizing agent;

Ag + à 1-, reduced, AgNO3 reducing agent

B.

Cu 0 à 2+; oxidized, Cu oxidizing agent;

Ag + à 0, reduced, AgNO3 reducing agent

C.

Cu 0 à 2+; oxidized, Cu reducing agent;

Ag + à 1-, reduced, AgNO3 oxidizing agent

D.

Cu 0 à 2+; reduced, Cu oxidizing agent;

Ag + à 1-, oxidized, AgNO3 reducing agent

E.

Cu 0 à 2+; reduced, Cu oxidizing agent;

Ag + à 0, oxidized, AgNO3 reducing agent

F.

Cu 0 à 2+; oxidized, Cu reducing agent;

Ag + à 0, reduced, AgNO3 oxidizing agent

G.

Cu 0 à 2+; reduced, Cu reducing agent;

Ag + à 0, oxidized, AgNO3 oxidizing agent

H.

Cu 0 à 2+; reduced, Cu reducing agent;

Ag + à 1-, oxidized, AgNO3 oxidizing agent

Indicate the elements oxidized/reduced, as well as their oxidation states before and after the reaction. Determine which species is the oxidizing agent and which is the reducing agent.

Cu(s) + 4 HNO3(aq) …….> Cu(NO3)2(aq) + 2 H2O(l) + 2 NO2 (g)

A.

Cu 0 à 2+; oxidized, Cu reducing agent;

N 5+ à 4-, reduced, HNO3 oxidizing agent

B.

Cu 0 à 2+; oxidized, Cu reducing agent;

N 5+ à 4+, reduced, HNO3 oxidizing agent

C.

Cu 0 à 2+; oxidized, Cu oxidizing agent;

N 5+ à 4+, reduced, HNO3 reducing agent

D.

Cu 0 à 2+; reduced, Cu reducing agent;

N 5+ à 4-, oxidized, HNO3 oxidizing agent

E.

Cu 0 à 2+; reduced, Cu reducing agent;

N 5+ à 4+, oxidized, HNO3 oxidizing agent

F.

Cu 0 à 2+; reduced, Cu oxidizing agent;

N 5+ à 4+, oxidized, HNO3 reducing agent

G.

Cu 0 à 2+; reduced, Cu oxidizing agent;

N 5+ à 4-, oxidized, HNO3 reducing agent

H.

Cu 0 à 2+; oxidized, Cu oxidizing agent;

N 5+ à 4-, reduced, HNO3 reducing agent

Indicate the elements oxidized/reduced, as well as their oxidation states before and after the reaction. Determine which species is the oxidizing agent and which is the reducing agent.

2 Na(s) + FeCl2(aq) ……> 2 NaCl(aq) + Fe(s)

A.

Na 0 à 1+; oxidized, Na reducing agent;

Fe 2+ à 1-, reduced, FeCl2 oxidizing agent

B.

Na 0 à 1+; oxidized, Na oxidizing agent;

Fe 2+ à 0, reduced, FeCl2 reducing agent

C.

Na 0 à 1+; oxidized, Na reducing agent;

Fe 2+ à 0, reduced, FeCl2 oxidizing agent

D.

Na 0 à 1+; reduced, Na oxidizing agent;

Fe 2+ à 1-, oxidized, FeCl2 reducing agent

E.

Na 0 à 1+; reduced, Na reducing agent;

Fe 2+ à 1-, oxidized, FeCl2 oxidizing agent

F.

Na 0 à 1+; reduced, Na reducing agent;

Fe 2+ à 0, oxidized, FeCl2 oxidizing agent

G.

Na 0 à 1+; oxidized, Na oxidizing agent;

Fe 2+ à 1-, reduced, FeCl2 reducing agent

H.

Na 0 à 1+; reduced, Na oxidizing agent;

Fe 2+ à 0, oxidized, FeCl2 reducing agent

Balance the following redox reaction in acidic solution:

            Cr2O72-(aq) + Fe2+(aq) ……> Cr3+(aq) + Fe3+(aq)

A.

10H+ + Cr2O72- + 3 Fe2+ à 3 Fe3+ + 2 Cr3+ + 5H2O

B.

14H+ + Cr2O72- + 3 Fe2+ à 3 Fe3+ + 2 Cr3+ + 7H2O

C.

10H+ + Cr2O72- + 6 Fe2+ à 6 Fe3+ + 2 Cr3+ + 5H2O

D.

10H+ + Cr2O72- + 4 Fe2+ à 4 Fe3+ + 2 Cr3+ + 5H2O

E.

14H+ + Cr2O72- + 6 Fe2+ à 6 Fe3+ + 2 Cr3+ + 7H2O

F.

14H+ + Cr2O72- + Fe2+ à Fe3+ + 2 Cr3+ + 7H2O

G.

14H+ + Cr2O72- + 5 Fe2+ à 5 Fe3+ + 2 Cr3+ + 7H2O

H.

10H+ + Cr2O72- + 5 Fe2+ à 5 Fe3+ + 2 Cr3+ + 5H2O

Write the balanced equation for the reaction of iron (II) sulfate with potassium permanganate to form iron (III) sulfate in the presence of sulfuric acid.

A.

5 FeSO4(aq) + 4 H2SO4(aq) + 2 KMnO4(aq) à 5Fe2(SO4)3(aq) + 2 MnSO4(aq) + 4H2O(l) + K2SO4(aq)

B.

5 FeSO4(aq) + 10 H2SO4(aq) + 2 KMnO4(aq) à 5Fe2(SO4)3(aq) + 2 MnSO4(aq) + 10H2O(l) + K2SO4(aq)

C.

10FeSO4(aq) + 4 H2SO4(aq) + KMnO4(aq) à 5Fe2(SO4)3(aq) + MnSO4(aq) + 8H2O(l) + K2SO4(aq)

D.

5 FeSO4(aq) + 4 H2SO4(aq) + KMnO4(aq) à 5Fe2(SO4)3(aq) + MnSO4(aq) + 4 H2O(l) + K2SO4(aq)

E.

10FeSO4(aq) + 4 H2SO4(aq) + 2 KMnO4(aq) à 5Fe2(SO4)3(aq) + 2 MnSO4(aq) + 4H2O(l) + K2SO4(aq)

F.

5 FeSO4(aq) + 8 H2SO4(aq) + 2 KMnO4(aq) à 5Fe2(SO4)3(aq) + 2 MnSO4(aq) + 8H2O(l) + K2SO4(aq)

G.

10FeSO4(aq) + 8 H2SO4(aq) + 2 KMnO4(aq) à5Fe2(SO4)3(aq) + 2 MnSO4(aq) + 8H2O(l) + K2SO4(aq)

H.

10FeSO4(aq) + 10 H2SO4(aq) + 2 KMnO4(aq) à 5Fe2(SO4)3(aq) + 2 MnSO4(aq) + 10H2O(l) + K2SO4(aq)

Write the balanced equation for the reaction of tin (II) chloride with potassium dichromate in aqueous hydrochloric acid to form Chromium (III) chloride and tin (IV) chloride as major products.

A.

SnCl2(aq) + 8HCl(aq) + K2Cr2O7(aq) à SnCl4(aq) + 2 KCl(aq) + 2 CrCl3(aq) + 4 H2O(l)

B.

3 SnCl2(aq) + 8 HCl(aq) + K2Cr2O7(aq) à 3 SnCl4(aq) + 2 KCl(aq) + 2 CrCl3(aq) + 4 H2O(l)

C.

SnCl2(aq) + 12HCl(aq) + K2Cr2O7(aq) à SnCl4(aq) + 2 KCl(aq) + 2 CrCl3(aq) + 6 H2O(l)

D.

3 SnCl2(aq) + 12 HCl(aq) + K2Cr2O7(aq) à 3 SnCl4(aq) + 2 KCl(aq) + 2 CrCl3(aq) + 6 H2O(l)

E.

SnCl2(aq) + 14HCl(aq) + K2Cr2O7(aq) à SnCl4(aq) + 2 KCl(aq) + 2 CrCl3(aq) + 7 H2O(l)

F.

3 SnCl2(aq) + 14HCl(aq) + K2Cr2O7(aq) à 3 SnCl4(aq) + 2 KCl(aq) + 2 CrCl3(aq) + 7 H2O(l)

G.

SnCl2(aq) + 12HCl(aq) + K2Cr2O7(aq) à SnCl4(aq) + 2 KCl(aq) + CrCl3(aq) + 6 H2O(l)

H.

3 SnCl2(aq) + 10HCl(aq) + K2Cr2O7(aq) à 3 SnCl4(aq) + 2 KCl(aq) + 2 CrCl3(aq) + 5 H2O(l)
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Homework Answers

Answer #1

1) Answer F

Cu 0 à 2+; oxidized, Cu reducing agent;

Ag + à 0, reduced, AgNO3 oxidizing agent

2) Answer B

Cu 0 à 2+; oxidized, Cu reducing agent;

N 5+ à 4+, reduced, HNO3 oxidizing agent

3) Answer C

Na 0 à 1+; oxidized, Na reducing agent;

Fe 2+ à 0, reduced, FeCl2 oxidizing agent

4) Answer B

14H+ + Cr2O72- + 3 Fe2+ --------> à 3 Fe3+ + 2 Cr3+ + 7H2O

5) Answer G

10FeSO4(aq) + 8 H2SO4(aq) + 2 KMnO4(aq) ----> à5Fe2(SO4)3(aq) + 2 MnSO4(aq) + 8H2O(l) + K2SO4(aq)

6) Answer F

3 SnCl2(aq) + 14HCl(aq) + K2Cr2O7(aq) ----> à 3 SnCl4(aq) + 2 KCl(aq) + 2 CrCl3(aq) + 7 H2O(l)

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