Question 1

Which of the following metals will dissolve in HCl?

Accepted Answer

A)  Au; E°(Au3+/Au) = +1.50V 
B)  Ag; E°(Ag+/Ag) = +0.80V 
C)  Cu; E°(Cu2+/Cu) = +0.34V 
D)  Al; E°(Al3+/Al) = -1.66V 
E)  Pt; E°(Pt2+/Pt) = +1.19V 
A)  Au; E°(Au3+/Au) = +1.50V 
B)  Ag; E°(Ag+/Ag) = +0.80V 
C)  Cu; E°(Cu2+/Cu) = +0.34V 
D)  Al; E°(Al3+/Al) = -1.66V 
E)  Pt; E°(Pt2+/Pt) = +1.19V D

Question 2

Which of the following is the strongest oxidizing agent?

Accepted Answer

A)  Cl2(g) 
B)  Au+3(aq) 
C)  F2(g) 
D)  O2(g) 
E)  Fe(s) 
A)  Cl2(g) 
B)  Au+3(aq) 
C)  F2(g) 
D)  O2(g) 
E)  Fe(s) C

Question 3

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Fe(s) ∣ Fe3+(aq, 0.0011 mol L-1)   Fe3+(aq, 2.33 mol L-1) ∣ Fe(s)
E°(Fe3+/Fe) = -0.036 V

Accepted Answer

A)  +0.066 V 
B)  -0.036 V 
C)  0.00 V 
D)  -0.099 V 
E)  +0.20 V 
A)  +0.066 V 
B)  -0.036 V 
C)  0.00 V 
D)  -0.099 V 
E)  +0.20 V A

Question 4

A voltaic cell is constructed with two silver-silver chloride electrodes, where the half-reaction is AgCl(s) +   → Ag(s) +   (aq) E° = +0.222 V
The concentrations of chloride ion in the two compartments are 0.0557 mol L-1 and 5.31 mol L-1, respectively. The cell emf is ________ V.

Accepted Answer

A)  0.00557 
B)  0.531 
C)  53.1 
D)  0.234 
E)  0.117 
A)  0.00557 
B)  0.531 
C)  53.1 
D)  0.234 
E)  0.117

Question 5

Match the following.
-Q < K

Accepted Answer

A) Ecell = E°cell B) Ecell > 0 C) Ecell = 0 D) E°cell > 0 E) E°cell cell < 0 A) Ecell = E°cell B) Ecell > 0 C) Ecell = 0 D) E°cell > 0 E) E°cell cell < 0

Question 6

What is the shorthand notation that represents the following galvanic cell reaction? 2 Sn2+(aq) + Cl2(g) → 2 Sn3+(aq) + 2 Cl-(aq)

Accepted Answer

A)  Sn2+(aq) ∣ Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) 
B)  Sn(s) ∣ Sn2+(aq) ∣∣ Sn4+(aq) Cl2(g) ∣ Cl-(aq) ∣ C(s) 
C)  Pt(s) ∣ Sn4+(aq), Sn2+(aq), Cl2(g) ∣∣ Cl-(aq) ∣ C(s) 
D)  Pt(s) ∣ Sn2+(aq), Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s) 
A)  Sn2+(aq) ∣ Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) 
B)  Sn(s) ∣ Sn2+(aq) ∣∣ Sn4+(aq) Cl2(g) ∣ Cl-(aq) ∣ C(s) 
C)  Pt(s) ∣ Sn4+(aq), Sn2+(aq), Cl2(g) ∣∣ Cl-(aq) ∣ C(s) 
D)  Pt(s) ∣ Sn2+(aq), Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s)

Question 7

Match the following.
-Q = 1

Accepted Answer

A) Ecell = E°cell B) Ecell > 0 C) Ecell = 0 D) E°cell > 0 E) E°cell cell < 0 A) Ecell = E°cell B) Ecell > 0 C) Ecell = 0 D) E°cell > 0 E) E°cell cell < 0

Question 8

Using the following standard reduction potentials, Fe3+(aq) + e- →Fe2+(aq) E° = +0. 77 V
Ni2+(aq) + 2 e- →Ni(s) E° = -0.23 V
Calculate the standard cell potential for the galvanic cell reaction given below and determine whether or not this reaction is spontaneous under standard conditions.
Ni2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Ni(s)

Accepted Answer

A)  E° = -1.00 V, nonspontaneous 
B)  E° = -1.00 V, spontaneous 
C)  E° = +1.00 V, nonspontaneous 
D)  E° = +1.00 V, spontaneous 
A)  E° = -1.00 V, nonspontaneous 
B)  E° = -1.00 V, spontaneous 
C)  E° = +1.00 V, nonspontaneous 
D)  E° = +1.00 V, spontaneous

Question 9

What is electrolysis?

Accepted Answer

An electrical curren

Question 10

Predict the species that will be reduced first if a mixture of molten salts containing the following ions undergoes electrolysis: Zn2+, Mn2+, Na+, Al3+, Li+

Accepted Answer

A)  Na+ 
B)  Zn2+ 
C)  Mn2+ 
D)  Al3+ 
E)  Li+ 
A)  Na+ 
B)  Zn2+ 
C)  Mn2+ 
D)  Al3+ 
E)  Li+

Question 11

Match the following.
-ΔrG° < 0

Accepted Answer

A) Ecell = E°cell B) Ecell > 0 C) Ecell = 0 D) E°cell > 0 E) E°cell cell < 0 A) Ecell = E°cell B) Ecell > 0 C) Ecell = 0 D) E°cell > 0 E) E°cell cell < 0

Question 12

Identify the metal if during a 1.000 hour long 2 electron electrolysis reaction 8.388 g of metal is deposited using a constant current of 4.000 A.

Accepted Answer

A)  Al 
B)  Mn 
C)  Cd 
D)  Au 
E)  Ag 
A)  Al 
B)  Mn 
C)  Cd 
D)  Au 
E)  Ag

Question 13

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s) ∣ Sn2+(aq, 0.010 mol L-1)   Ag+(aq, 1.00 mol L-1) ∣ Ag(s)
E°(Sn2+/Sn) = -0.14 V and E°(Ag+/Ag) = +0.80 V

Accepted Answer

A)  +1.18 V 
B)  -1.18 V 
C)  +1.00 V 
D)  +0.94 V 
E)  -0.94 V 
A)  +1.18 V 
B)  -1.18 V 
C)  +1.00 V 
D)  +0.94 V 
E)  -0.94 V

Question 14

Predict the species that will be oxidized first if a mixture of molten salts containing the following ions undergoes electrolysis: Cu2+, Mg2+, Cl⁻, Br⁻, F⁻

Accepted Answer

A)  Cl⁻ 
B)  F⁻ 
C)  Cu2+ 
D)  Mg2+ 
E)  Br⁻ 
A)  Cl⁻ 
B)  F⁻ 
C)  Cu2+ 
D)  Mg2+ 
E)  Br⁻

Question 15

What is undergoing oxidation in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe3+(aq)   Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)

Accepted Answer

A)  Fe(s) 
B)  Fe3+(aq) 
C)  Cl2(g) 
D)  Cl⁻(aq) 
E)  Pt(s) 
A)  Fe(s) 
B)  Fe3+(aq) 
C)  Cl2(g) 
D)  Cl⁻(aq) 
E)  Pt(s)

Question 16

The gas OF2 can be produced from the electrolysis of an aqueous solution of KF, as shown in the equation below: OF2(g) + 2H+(aq) + 4 e- → H2O(l) + 2F-(aq) E° = +2.15 V
Using the given standard reduction potential, calculate the amount of OF2 that is produced, and the electrode at which the OF2 is produced, upon the passage of 0. 480 faradays through an aqueous KF solution.

Accepted Answer

A)  6.48 g of OF2 at the anode 
B)  26.0 g of OF2 at the anode 
C)  6.48 g of OF2 at the cathode 
D)  26.0 g of OF2 at the cathode 
A)  6.48 g of OF2 at the anode 
B)  26.0 g of OF2 at the anode 
C)  6.48 g of OF2 at the cathode 
D)  26.0 g of OF2 at the cathode

Question 17

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I2(s) + Fe(s) → Fe3+(aq) + I⁻(aq)

Accepted Answer

A)  1 
B)  2 
C)  6 
D)  3 
E)  4 
A)  1 
B)  2 
C)  6 
D)  3 
E)  4

Question 18

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Mg(s) ∣ Mg2+(aq, 2.74 mol L-1)   Cu2+(aq, 0.0033 mol L-1) ∣ Cu(s)
E°(Mg2+/Mg) = -2.37 V and E°(Cu2+/Cu) = +0.34 V

Accepted Answer

A)  -2.80 V 
B)  +2.62 V 
C)  +2.71 V 
D)  +2.12 V 
E)  -1.94 V 
A)  -2.80 V 
B)  +2.62 V 
C)  +2.71 V 
D)  +2.12 V 
E)  -1.94 V

Question 19

Which of the following is the strongest oxidizing agent?

Accepted Answer

A)  H2O2(aq) 
B)  Fe3+(aq) 
C)  ClO2(g) 
D)  I2(s) 
E)  Fe(s) 
A)  H2O2(aq) 
B)  Fe3+(aq) 
C)  ClO2(g) 
D)  I2(s) 
E)  Fe(s)

Question 20

Identify the characteristics of a spontaneous reaction.

Accepted Answer

A)  ΔrG° > 0 
B)  ΔE°cell cell > 0 
E)  K = 0 
A)  ΔrG° > 0 
B)  ΔE°cell cell > 0 
E)  K = 0

Exam 18: Electrochemistry

Which of the following metals will dissolve in HCl?

Which of the following is the strongest oxidizing agent?

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Fe(s) ∣ Fe3+(aq, 0.0011 mol L-1) Fe3+(aq, 2.33 mol L-1) ∣ Fe(s) E°(Fe3+/Fe) = -0.036 V

A voltaic cell is constructed with two silver-silver chloride electrodes, where the half-reaction is AgCl(s) + → Ag(s) + (aq) E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0557 mol L-1 and 5.31 mol L-1, respectively. The cell emf is ________ V.

Match the following. -Q < K

What is the shorthand notation that represents the following galvanic cell reaction? 2 Sn2+(aq) + Cl2(g) → 2 Sn3+(aq) + 2 Cl-(aq)

Match the following. -Q = 1

What is electrolysis?

Predict the species that will be reduced first if a mixture of molten salts containing the following ions undergoes electrolysis: Zn2+, Mn2+, Na+, Al3+, Li+

Match the following. -ΔrG° < 0

Identify the metal if during a 1.000 hour long 2 electron electrolysis reaction 8.388 g of metal is deposited using a constant current of 4.000 A.

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s) ∣ Sn2+(aq, 0.010 mol L-1) Ag+(aq, 1.00 mol L-1) ∣ Ag(s) E°(Sn2+/Sn) = -0.14 V and E°(Ag+/Ag) = +0.80 V

Predict the species that will be oxidized first if a mixture of molten salts containing the following ions undergoes electrolysis: Cu2+, Mg2+, Cl⁻, Br⁻, F⁻

What is undergoing oxidation in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe3+(aq) Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I2(s) + Fe(s) → Fe3+(aq) + I⁻(aq)

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Mg(s) ∣ Mg2+(aq, 2.74 mol L-1) Cu2+(aq, 0.0033 mol L-1) ∣ Cu(s) E°(Mg2+/Mg) = -2.37 V and E°(Cu2+/Cu) = +0.34 V

Which of the following is the strongest oxidizing agent?

Identify the characteristics of a spontaneous reaction.

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Fe(s) ∣ Fe³⁺(aq, 0.0011 mol L^-1) Fe³⁺(aq, 2.33 mol L^-1) ∣ Fe(s) E°(Fe³⁺/Fe) = -0.036 V

A voltaic cell is constructed with two silver-silver chloride electrodes, where the half-reaction is AgCl(s) + → Ag(s) + (aq) E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0557 mol L^-1 and 5.31 mol L^-1, respectively. The cell emf is ________ V.

What is the shorthand notation that represents the following galvanic cell reaction? 2 Sn²⁺(aq) + Cl₂(g) → 2 Sn³⁺(aq) + 2 Cl^-(aq)

Predict the species that will be reduced first if a mixture of molten salts containing the following ions undergoes electrolysis: Zn²⁺, Mn²⁺, Na⁺, Al³⁺, Li⁺

Match the following. -Δ_rG° < 0

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s) ∣ Sn²⁺(aq, 0.010 mol L^-1) Ag⁺(aq, 1.00 mol L^-¹) ∣ Ag(s) E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

Predict the species that will be oxidized first if a mixture of molten salts containing the following ions undergoes electrolysis: Cu²⁺, Mg²⁺, Cl⁻, Br⁻, F⁻

What is undergoing oxidation in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe³⁺(aq) Cl₂(g) ∣ Cl⁻(aq) ∣ Pt(s)

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I₂(s) + Fe(s) → Fe³⁺(aq) + I⁻(aq)

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Mg(s) ∣ Mg²⁺(aq, 2.74 mol L^-1) Cu²⁺(aq, 0.0033 mol L^-1) ∣ Cu(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Cu²⁺/Cu) = +0.34 V