Question 1

Calculate ΔG° for the oxidation of 3 moles of copper by nitric acid. Cu2+(aq)  + 2e-
  2+(aq)  + 2e-     Cu(s)  E° = 0.34 V NO3-(aq)  + 4H+(aq)  + 3e-     NO(g)  + 2H2O(l)  E° = 0.957 V A)  -120 kJ B)  -180 kJ C)  -240 kJ D)  -300 kJ E)  -360 kJ" class="answers-bank-image d-inline" rel="preload" > Cu(s)  E° = 0.34 V
NO3-(aq)  + 4H+(aq)  + 3e-
  2+(aq)  + 2e-     Cu(s)  E° = 0.34 V NO3-(aq)  + 4H+(aq)  + 3e-     NO(g)  + 2H2O(l)  E° = 0.957 V A)  -120 kJ B)  -180 kJ C)  -240 kJ D)  -300 kJ E)  -360 kJ" class="answers-bank-image d-inline" rel="preload" > NO(g)  + 2H2O(l)  E° = 0.957 V

Accepted Answer

A)   -120 kJ
B)   -180 kJ
C)   -240 kJ
D)   -300 kJ
E)   -360 kJF) A) and C)
G) A) and D)

Question 2

A solution is prepared by dissolving 32.0 g of NiSO4 in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Accepted Answer

A)   1.1 A
B)   2.2 A
C)   3.3 A
D)   4.4 A
E)   5.5 AF) A) and C)
G) B) and D)

Question 3

A buried iron pipe can be protected against corrosion by connecting it to a rod of magnesium.

Accepted Answer

A) True 
 B)False

Question 4

What is the E°cell for the cell represented by the combination of the following half-reactions? 2Hg2+(aq)  + 2e- cell for the cell represented by the combination of the following half-reactions? 2Hg2+(aq)  + 2e-   Hg22+(aq)  E° = 0.92 V Cr3+(aq)  + 3e-   Cr(s)  E° = -0.74 V A)  -0.18 V B)  0.18 V C)  1.28 V D)  1.66 V E)  2.12 V" class="answers-bank-image d-inline" rel="preload" > Hg22+(aq)  E° = 0.92 V
Cr3+(aq)  + 3e- cell for the cell represented by the combination of the following half-reactions? 2Hg2+(aq)  + 2e-   Hg22+(aq)  E° = 0.92 V Cr3+(aq)  + 3e-   Cr(s)  E° = -0.74 V A)  -0.18 V B)  0.18 V C)  1.28 V D)  1.66 V E)  2.12 V" class="answers-bank-image d-inline" rel="preload" > Cr(s)  E° = -0.74 V

Accepted Answer

A)   -0.18 V
B)   0.18 V
C)   1.28 V
D)   1.66 V
E)   2.12 VF) A) and C)
G) B) and E)

Question 5

Electrolytic cells utilize electrical energy to drive nonspontaneous redox reactions.

Accepted Answer

A) True 
 B)False

Question 6

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq)  + e-
  3+(aq)  + e-     Co2+(aq)  E° = 1.82 V MnO4-(aq)  + 2H2O(l)  + 3e- MnO2(s)  + 4OH-(aq)  E° = 0.59 V Overall reaction: MnO4-(aq)  + 2H2O(l)  + 3Co2+(aq)  → MnO2(s)  + 3Co3+(aq)  + 4OH-(aq)  A)  E° cell = -1.23 V, spontaneous B)  E° cell = -1.23 V, nonspontaneous C)  E° cell = 1.23 V, spontaneous D)  E° cell = 1.23 V, nonspontaneous E)  E° cell = -0.05 V, nonspontaneous" class="answers-bank-image d-inline" rel="preload" > Co2+(aq)  E° = 1.82 V
MnO4-(aq)  + 2H2O(l)  + 3e- MnO2(s)  + 4OH-(aq)  E° = 0.59 V
Overall reaction:
MnO4-(aq)  + 2H2O(l)  + 3Co2+(aq)  → MnO2(s)  + 3Co3+(aq)  + 4OH-(aq)

Accepted Answer

A)   E° cell = -1.23 V, spontaneous
B)   E° cell = -1.23 V, nonspontaneous
C)   E° cell = 1.23 V, spontaneous
D)   E° cell = 1.23 V, nonspontaneous
E)   E° cell = -0.05 V, nonspontaneousF) C) and E)
G) A) and B)

Question 7

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

Accepted Answer

A)   sodium from Na3PO4(aq) 
B)   sulfur from K2SO4(aq) 
C)   oxygen from H2SO4(aq) 
D)   potassium from KCl(aq) 
E)   nitrogen from AgNO3(aq) F) None of the above
G) C) and E)

Question 8

A battery is considered "dead" when

Accepted Answer

A)    1. 
D)     = K. 
E)     /K = 0." class="answers-bank-image d-inline" rel="preload" > 
B)    1. 
D)     = K. 
E)     /K = 0." class="answers-bank-image d-inline" rel="preload" > = 1.
C)    1. 
D)     = K. 
E)     /K = 0." class="answers-bank-image d-inline" rel="preload" > > 1.
D)    1. 
D)     = K. 
E)     /K = 0." class="answers-bank-image d-inline" rel="preload" > = K.
E)    1. 
D)     = K. 
E)     /K = 0." class="answers-bank-image d-inline" rel="preload" > /K = 0.F) None of the above
G) B) and D)

Question 9

What is the value of the equilibrium constant for the cell reaction below at 25°C? E° cell = 0.30 V Sn2+(aq)  + Fe(s)   cell = 0.30 V Sn2+(aq)  + Fe(s)    Sn(s)  + Fe2+(aq)  A)  1.2 × 105 B)  1.4 × 1010 C)  8.6 × 10-6 D)  7.1 × 10-11 E)  2.3 × 1023" class="answers-bank-image d-inline" rel="preload" > Sn(s)  + Fe2+(aq)

Accepted Answer

A)   1.2 × 105
B)   1.4 × 1010
C)   8.6 × 10-6
D)   7.1 × 10-11
E)   2.3 × 1023F) A) and E)
G) D) and E)

Question 10

Calculate E° cell for the reaction of nickel(II)  ions with cadmium metal at 25°C. K = 1.17 × 105 Ni2+(aq)  + Cd(s)  → Cd2+(aq)  + Ni(s)

Accepted Answer

A)   0.075 V
B)   0.10 V
C)   0.12 V
D)   0.15 V
E)   0.30 VF) A) and E)
G) C) and D)

Question 11

The value of the equilibrium constant for the reaction of nickel(II)  ions with cadmium metal is 1.17 × 105. Calculate ΔG° for the reaction at 25°C.

Accepted Answer

A)   -12.6 kJ
B)   -28.9 kJ
C)   12.6 kJ
D)   28.9 kJ
E)   None of these choices are correct.F) A) and D)
G) B) and E)

Question 12

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s)  | Cu2+(aq)  || Ag+(aq)  | Ag(s) 
Which of the following processes occurs at the cathode?

Accepted Answer

A)   Cu(s)  → Cu2+(aq)  + 2e-
B)   Cu2+(aq)  + 2e- → Cu(s) 
C)   Ag(s)  → Ag+(aq)  + e-
D)   Ag+(aq)  + e- → Ag(s) 
E)   Cu(s)  + 2Ag+(aq)  → Cu2+(aq)  + 2Ag(s) F) A) and E)
G) A) and B)

Question 13

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) 3-will be Bi(OH) 3(s)  + Sn(OH) 3(aq)  → Sn(OH) 62-(aq)  + Bi(s)  (basic solution)

Accepted Answer

A)   1.
B)   2.
C)   3.
D)   6.
E)   None of these choices are correct.F) A) and C)
G) A) and E)

Question 14

Which of the following elements can be isolated by electrolysis of the aqueous salt shown?

Accepted Answer

A)   phosphorus from K3PO4(aq) 
B)   sodium from NaBr(aq) 
C)   aluminum from AlCl3(aq) 
D)   fluorine from KF(aq) 
E)   iodine from NaI(aq) F) B) and C)
G) A) and E)

Question 15

Consider the reaction CuO(s)  + H2(g)  → Cu(s)  + H2O(l) 
In this reaction, which substances are the oxidant and reductant, respectively?

Accepted Answer

A)   CuO and H2
B)   H2 and CuO
C)   CuO and Cu
D)   H2O and H2
E)   None of these choices are correct.F) A) and E)
G) A) and C)

Question 16

What is the value of the equilibrium constant for the cell reaction below at 25°C? E° cell = 0.61 V 2Cr(s)  + 3Pb2+(aq)   cell = 0.61 V 2Cr(s)  + 3Pb2+(aq)    3Pb(s)  + 2Cr3+(aq)  A)  4.1 × 1020 B)  8.2 × 1030 C)  3.3 × 1051 D)  7.4 × 1061 E)  > 9.9 × 1099" class="answers-bank-image d-inline" rel="preload" > 3Pb(s)  + 2Cr3+(aq)

Accepted Answer

A)   4.1 × 1020
B)   8.2 × 1030
C)   3.3 × 1051
D)   7.4 × 1061
E)   > 9.9 × 1099F) B) and C)
G) A) and E)

Question 17

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr4(aq)  + 3e-
  4(aq)  + 3e-     Au(s)  + 4Br-(aq)  E° = 0.854 V Mn2+(aq)  + 2e-     Mn(s)  E° = -1.185 V K+(aq)  + e-     K(s)  E° = -2.931 V F2O(aq)  + 2H+(aq)  + 4e-     2F-(aq)  + H2O(l)  E° = 2.153 V A)  AuBr4-(aq)  B)  Mn2+(aq)  C)  K+(aq)  D)  F2O(aq)  E)  H+(aq) " class="answers-bank-image d-inline" rel="preload" > Au(s)  + 4Br-(aq)  E° = 0.854 V
Mn2+(aq)  + 2e-
  4(aq)  + 3e-     Au(s)  + 4Br-(aq)  E° = 0.854 V Mn2+(aq)  + 2e-     Mn(s)  E° = -1.185 V K+(aq)  + e-     K(s)  E° = -2.931 V F2O(aq)  + 2H+(aq)  + 4e-     2F-(aq)  + H2O(l)  E° = 2.153 V A)  AuBr4-(aq)  B)  Mn2+(aq)  C)  K+(aq)  D)  F2O(aq)  E)  H+(aq) " class="answers-bank-image d-inline" rel="preload" > Mn(s)  E° = -1.185 V
K+(aq)  + e-
  4(aq)  + 3e-     Au(s)  + 4Br-(aq)  E° = 0.854 V Mn2+(aq)  + 2e-     Mn(s)  E° = -1.185 V K+(aq)  + e-     K(s)  E° = -2.931 V F2O(aq)  + 2H+(aq)  + 4e-     2F-(aq)  + H2O(l)  E° = 2.153 V A)  AuBr4-(aq)  B)  Mn2+(aq)  C)  K+(aq)  D)  F2O(aq)  E)  H+(aq) " class="answers-bank-image d-inline" rel="preload" > K(s)  E° = -2.931 V
F2O(aq)  + 2H+(aq)  + 4e-
  4(aq)  + 3e-     Au(s)  + 4Br-(aq)  E° = 0.854 V Mn2+(aq)  + 2e-     Mn(s)  E° = -1.185 V K+(aq)  + e-     K(s)  E° = -2.931 V F2O(aq)  + 2H+(aq)  + 4e-     2F-(aq)  + H2O(l)  E° = 2.153 V A)  AuBr4-(aq)  B)  Mn2+(aq)  C)  K+(aq)  D)  F2O(aq)  E)  H+(aq) " class="answers-bank-image d-inline" rel="preload" > 2F-(aq)  + H2O(l)  E° = 2.153 V

Accepted Answer

A)   AuBr4-(aq) 
B)   Mn2+(aq) 
C)   K+(aq) 
D)   F2O(aq) 
E)   H+(aq) F) A) and C)
G) A) and B)

Question 18

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be--. I2(s)  + HNO3(aq)  → HIO3(aq)  + NO2(g)  + H2O(l)

Accepted Answer

A)   1
B)   2
C)   4
D)   10
E)   None of these choices are correct.F) C) and E)
G) B) and C)

Question 19

A voltaic cell can be prepared from copper and tin. What is the E°cell for the cell that forms from the following half-reactions? Cu2+(aq)  + 2e- cell for the cell that forms from the following half-reactions? Cu2+(aq)  + 2e-   Cu(s)  E° = 0.34 V Sn4+(aq)  + 2e-   Sn2+(aq)  E° = 0.13 V A)  0.47 V B)  0.21 V C)  -0.21 V D)  -0.47 V E)  0.42 V" class="answers-bank-image d-inline" rel="preload" > Cu(s)  E° = 0.34 V
Sn4+(aq)  + 2e- cell for the cell that forms from the following half-reactions? Cu2+(aq)  + 2e-   Cu(s)  E° = 0.34 V Sn4+(aq)  + 2e-   Sn2+(aq)  E° = 0.13 V A)  0.47 V B)  0.21 V C)  -0.21 V D)  -0.47 V E)  0.42 V" class="answers-bank-image d-inline" rel="preload" > Sn2+(aq)  E° = 0.13 V

Accepted Answer

A)   0.47 V
B)   0.21 V
C)   -0.21 V
D)   -0.47 V
E)   0.42 VF) D) and E)
G) A) and E)

Question 20

Consider the following redox equation Mn(OH) 2(s)  + MnO4(aq)  → MnO42-(aq)  (basic solution) 
When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH-(aq)  and on which side of the equation is OH-(aq)  present?

Accepted Answer

A)   4, reactant side
B)   4, product side
C)   6, reactant side
D)   6, product side
E)   None of these choices are correct.F) None of the above
G) C) and D)

Exam 21: Electrochemistry Chemical Change and Electrical Work

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which of the following processes occurs at the cathode?

Correct Answer
verified

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.30 V Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq)

Correct Answer
verified

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.61 V 2Cr(s) + 3Pb²⁺(aq) 3Pb(s) + 2Cr³⁺(aq)

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) 3-will be Bi(OH) ₃(s) + Sn(OH) ₃(aq) → Sn(OH) ₆^2-(aq) + Bi(s) (basic solution)

Correct Answer
verified

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 10⁵. Calculate ΔG° for the reaction at 25°C.

Correct Answer
verified

Consider the following redox equation Mn(OH) ₂(s) + MnO₄(aq) → MnO₄^2-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH^-(aq) and on which side of the equation is OH^-(aq) present?

Correct Answer
verified

A buried iron pipe can be protected against corrosion by connecting it to a rod of magnesium.

Correct Answer
verified

Calculate E°_cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 10⁵ Ni²⁺(aq) + Cd(s) → Cd²⁺(aq) + Ni(s)

Correct Answer
verified

What is the E°_cell for the cell represented by the combination of the following half-reactions? 2Hg²⁺(aq) + 2e- Hg₂²⁺(aq) E° = 0.92 V Cr³⁺(aq) + 3e- Cr(s) E° = -0.74 V

Correct Answer
verified

A solution is prepared by dissolving 32.0 g of NiSO₄ in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be--. I₂(s) + HNO₃(aq) → HIO₃(aq) + NO₂(g) + H₂O(l)

Correct Answer
verified

Consider the reaction CuO(s) + H₂(g) → Cu(s) + H₂O(l) In this reaction, which substances are the oxidant and reductant, respectively?

Correct Answer
verified

Correct Answer
verified

A battery is considered "dead" when

Correct Answer
verified

Calculate ΔG° for the oxidation of 3 moles of copper by nitric acid. Cu²⁺(aq) + 2e^- Cu(s) E° = 0.34 V NO₃^-(aq) + 4H⁺(aq) + 3e^- NO(g) + 2H²O(l) E° = 0.957 V

Correct Answer
verified

A voltaic cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e- Cu(s) E° = 0.34 V Sn⁴⁺(aq) + 2e- Sn²⁺(aq) E° = 0.13 V

Correct Answer
verified

Which of the following elements can be isolated by electrolysis of the aqueous salt shown?

Correct Answer
verified

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr₄(aq) + 3e^- Au(s) + 4Br^-(aq) E° = 0.854 V Mn²⁺(aq) + 2e^- Mn(s) E° = -1.185 V K⁺(aq) + e^- K(s) E° = -2.931 V F₂O(aq) + 2H⁺(aq) + 4e^- 2F^-(aq) + H₂O(l) E° = 2.153 V

Correct Answer
verified

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

Correct Answer
verified

Electrolytic cells utilize electrical energy to drive nonspontaneous redox reactions.

Correct Answer
verified

Exam 21: Electrochemistry Chemical Change and Electrical Work

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode?

Correct AnswerverifiedShow Answer

What is the value of the equilibrium constant for the cell reaction below at 25°C? E° cell = 0.30 V Sn2+(aq) + Fe(s) Sn(s) + Fe2+(aq)

Correct AnswerverifiedShow Answer

What is the value of the equilibrium constant for the cell reaction below at 25°C? E° cell = 0.61 V 2Cr(s) + 3Pb2+(aq) 3Pb(s) + 2Cr3+(aq)

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) 3-will be Bi(OH) 3(s) + Sn(OH) 3(aq) → Sn(OH) 62-(aq) + Bi(s) (basic solution)

Correct AnswerverifiedShow Answer

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 105. Calculate ΔG° for the reaction at 25°C.

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Consider the following redox equation Mn(OH) 2(s) + MnO4(aq) → MnO42-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH-(aq) and on which side of the equation is OH-(aq) present?

Correct AnswerverifiedShow Answer

A buried iron pipe can be protected against corrosion by connecting it to a rod of magnesium.

Correct AnswerverifiedShow Answer

Calculate E° cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 105 Ni2+(aq) + Cd(s) → Cd2+(aq) + Ni(s)

Correct AnswerverifiedShow Answer

What is the E°cell for the cell represented by the combination of the following half-reactions? 2Hg2+(aq) + 2e- Hg22+(aq) E° = 0.92 V Cr3+(aq) + 3e- Cr(s) E° = -0.74 V

Correct AnswerverifiedShow Answer

A solution is prepared by dissolving 32.0 g of NiSO4 in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be--. I2(s) + HNO3(aq) → HIO3(aq) + NO2(g) + H2O(l)

Correct AnswerverifiedShow Answer

Consider the reaction CuO(s) + H2(g) → Cu(s) + H2O(l) In this reaction, which substances are the oxidant and reductant, respectively?

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Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq) + e- Co2+(aq) E° = 1.82 V MnO4-(aq) + 2H2O(l) + 3e- MnO2(s) + 4OH-(aq) E° = 0.59 V Overall reaction: MnO4-(aq) + 2H2O(l) + 3Co2+(aq) → MnO2(s) + 3Co3+(aq) + 4OH-(aq)

Correct AnswerverifiedShow Answer

A battery is considered "dead" when

Correct AnswerverifiedShow Answer

Calculate ΔG° for the oxidation of 3 moles of copper by nitric acid. Cu2+(aq) + 2e- Cu(s) E° = 0.34 V NO3-(aq) + 4H+(aq) + 3e- NO(g) + 2H2O(l) E° = 0.957 V

Correct AnswerverifiedShow Answer

A voltaic cell can be prepared from copper and tin. What is the E°cell for the cell that forms from the following half-reactions? Cu2+(aq) + 2e- Cu(s) E° = 0.34 V Sn4+(aq) + 2e- Sn2+(aq) E° = 0.13 V

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Which of the following elements can be isolated by electrolysis of the aqueous salt shown?

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Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr4(aq) + 3e- Au(s) + 4Br-(aq) E° = 0.854 V Mn2+(aq) + 2e- Mn(s) E° = -1.185 V K+(aq) + e- K(s) E° = -2.931 V F2O(aq) + 2H+(aq) + 4e- 2F-(aq) + H2O(l) E° = 2.153 V

Correct AnswerverifiedShow Answer

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

Correct AnswerverifiedShow Answer

Electrolytic cells utilize electrical energy to drive nonspontaneous redox reactions.

Correct AnswerverifiedShow Answer

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which of the following processes occurs at the cathode?

Correct Answer
verified

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.30 V Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq)

Correct Answer
verified

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.61 V 2Cr(s) + 3Pb²⁺(aq) 3Pb(s) + 2Cr³⁺(aq)

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) 3-will be Bi(OH) ₃(s) + Sn(OH) ₃(aq) → Sn(OH) ₆^2-(aq) + Bi(s) (basic solution)

Correct Answer
verified

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 10⁵. Calculate ΔG° for the reaction at 25°C.

Correct Answer
verified

Consider the following redox equation Mn(OH) ₂(s) + MnO₄(aq) → MnO₄^2-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH^-(aq) and on which side of the equation is OH^-(aq) present?

Correct Answer
verified

Correct Answer
verified

Calculate E°_cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 10⁵ Ni²⁺(aq) + Cd(s) → Cd²⁺(aq) + Ni(s)

Correct Answer
verified

What is the E°_cell for the cell represented by the combination of the following half-reactions? 2Hg²⁺(aq) + 2e- Hg₂²⁺(aq) E° = 0.92 V Cr³⁺(aq) + 3e- Cr(s) E° = -0.74 V

Correct Answer
verified

A solution is prepared by dissolving 32.0 g of NiSO₄ in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be--. I₂(s) + HNO₃(aq) → HIO₃(aq) + NO₂(g) + H₂O(l)

Correct Answer
verified

Consider the reaction CuO(s) + H₂(g) → Cu(s) + H₂O(l) In this reaction, which substances are the oxidant and reductant, respectively?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate ΔG° for the oxidation of 3 moles of copper by nitric acid. Cu²⁺(aq) + 2e^- Cu(s) E° = 0.34 V NO₃^-(aq) + 4H⁺(aq) + 3e^- NO(g) + 2H²O(l) E° = 0.957 V

Correct Answer
verified

A voltaic cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e- Cu(s) E° = 0.34 V Sn⁴⁺(aq) + 2e- Sn²⁺(aq) E° = 0.13 V

Correct Answer
verified

Correct Answer
verified

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr₄(aq) + 3e^- Au(s) + 4Br^-(aq) E° = 0.854 V Mn²⁺(aq) + 2e^- Mn(s) E° = -1.185 V K⁺(aq) + e^- K(s) E° = -2.931 V F₂O(aq) + 2H⁺(aq) + 4e^- 2F^-(aq) + H₂O(l) E° = 2.153 V

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified