Question 1

A primary battery is recharged by passing electricity through the battery.

Accepted Answer

A) True 
 B)False

Question 2

The following galvanic cell has a measured cell potential E°cell = 0.646 V.
Pt(s)∣ Sn4+(aq),Sn2+(aq)   Ag+(aq)∣ Ag(s)
Given that the standard reduction potential for the reduction of Ag+(aq)to Ag(s)is +0.800 V,what is the standard reduction potential for the Sn4+/Sn2+ half-reaction?

Accepted Answer

A) +0.154 V 
B) -0.154 V 
C) +1.45 V 
D) -1.45 V 
E) +0.308 V 
A) +0.154 V 
B) -0.154 V 
C) +1.45 V 
D) -1.45 V 
E) +0.308 V

Question 3

In a galvanic cell,oxidation occurs at the:

Accepted Answer

A) anode 
B) cathode 
C) salt bridge 
D) electrolyte 
E) in cathodic space 
A) anode 
B) cathode 
C) salt bridge 
D) electrolyte 
E) in cathodic space

Question 4

Calculate the Ksp of lead iodide from the following standard electrode potentials,at 25 °C:
2 e- + PbI2(S)→ Pb(s)+ 2 I-(aq)E° = -0.365 V
2 e- + Pb2+(aq)→ Pb(s)E° = -0.126 V

Accepted Answer

A) 8 × 10-9  
B) 9 × 10-5  
C) 2 × 10-17  
D) 5 × 10-13  
E) 6 × 10-5  
A) 8 × 10-9  
B) 9 × 10-5  
C) 2 × 10-17  
D) 5 × 10-13  
E) 6 × 10-5

Question 5

Determine Ecell at 25 °C for the following reaction at 25 °C:
Al(s)∣ Al3+(0.435 M)   Sn2+(2.12 × 10-3 M)∣ Sn(s)
3 Sn2+(aq)+ 2 Al(s)→ 2 Al3+(aq)+ 3 Sn(s)
Al3+(aq)+ 3 e- → Al(s)E° = -1.676 V
Sn2+(aq)+ 2 e- → Sn(s)E° = -0.137 V

Accepted Answer

A) 1.227 V 
B) 1.611 V 
C) 1.562 V 
D) 1.487 V 
E) 1.467 V 
A) 1.227 V 
B) 1.611 V 
C) 1.562 V 
D) 1.487 V 
E) 1.467 V

Question 6

What is ΔG° at 25 °C for the reaction (not balanced): C3H8(g)+ O2(g)→ CO2(g)+ H2O(l)if the standard cell potential is 1.092 V?

Accepted Answer

A) -105 kJ 
B) -211 kJ 
C) 105 kJ 
D) -2107 kJ 
E) 211 kJ 
A) -105 kJ 
B) -211 kJ 
C) 105 kJ 
D) -2107 kJ 
E) 211 kJ

Question 7

Determine E°cell for the reaction: 2 Ag+(aq)+ Mg(s)→ 2 Ag(s)+ Mg2+(aq).The half reactions are:
Mg2+(aq)+ 2 e- → Mg(s)E° = -2.356 V
Ag+(aq)+ e- → Ag(s)E° = 0.800 V

Accepted Answer

A) 0.756 V 
B) -0.756 V 
C) 3.156 V 
D) -1.556 V 
E) 1.556 V 
A) 0.756 V 
B) -0.756 V 
C) 3.156 V 
D) -1.556 V 
E) 1.556 V

Question 8

Cathodic protection is attaching a more active metal to the protected metal.

Accepted Answer

A) True 
 B)False

Question 9

Choose the correct statement based on the following oxidation potentials.
Mg/Mg2+ +2.37 v Fe/Fe2+ +0.44 v Cu/Cu2+ -0.34 v
Zn/Zn2+ +0.76 v Sn/Sn2+ +0.14 v Ag/Ag+ -0.80 v

Accepted Answer

A) Mg will not displace Zn2+ from solution 
B) Cu will displace Sn2+ from solution 
C) Fe will displace Zn2+ from solution 
D) Fe will displace H+ from solution 
E) Sn will displace Fe2+ from solution 
A) Mg will not displace Zn2+ from solution 
B) Cu will displace Sn2+ from solution 
C) Fe will displace Zn2+ from solution 
D) Fe will displace H+ from solution 
E) Sn will displace Fe2+ from solution

Question 10

What is the Ecell for the following concentration cell at 25 °C:
Pt(s)∣ H2(g,0.025 atm)∣ H+ (0.012 M)   H+ (aq,1 M)∣ H2(g,1 atm)∣ Pt(s)
2 H+(aq)+ 2 e- → H2(g)E° = 0.V

Accepted Answer

A) -0.16 V 
B) +0.066 V 
C) -0.132 V 
D) 0.16 V 
E) -0.066 V 
A) -0.16 V 
B) +0.066 V 
C) -0.132 V 
D) 0.16 V 
E) -0.066 V

Question 11

What is the [H+] in a concentration cell at 25 °C if the cell potential is 0.0451 V and cell diagram:
Pt(s)∣ H2 (g,1 atm)∣ H+(?)   H+ (aq,1 M)∣ H2(g,1 atm)
2 H+(aq)+ 2 e- → H2(g)E° = 0.V

Accepted Answer

A) 0.51 M 
B) 0.42 M 
C) 0.030 M 
D) 0.17 M 
E) 5.7 M 
A) 0.51 M 
B) 0.42 M 
C) 0.030 M 
D) 0.17 M 
E) 5.7 M

Question 12

Consider the galvanic cell,  
Which one of the following changes to the cell would cause the cell potential to increase (i.e. ,become more positive)?

Accepted Answer

A) increase the [Zn2+] concentration 
B) increase the [Pb2+] concentration 
C) increase the mass of Zn(s) 
D) decrease the mass of Zn(s) 
A) increase the [Zn2+] concentration 
B) increase the [Pb2+] concentration 
C) increase the mass of Zn(s) 
D) decrease the mass of Zn(s)

Question 13

Choose the INCORRECT statement.

Accepted Answer

A) The work available in a cell = -zFEcell. 
B) ΔG ° = -zFE°cell  
C) When Ecell cell = 0,the reaction is at equilibrium. 
E) Reversing a cell reaction changes the sign of Ecell. 
A) The work available in a cell = -zFEcell. 
B) ΔG ° = -zFE°cell  
C) When Ecell cell = 0,the reaction is at equilibrium. 
E) Reversing a cell reaction changes the sign of Ecell.

Question 14

Determine E°cell for the reaction: Cl2(g)+ 2 F-(aq)→ 2 Cl-(aq)+ F2(g).The half reactions are:
F2(g)+ 2 e- → 2 F-(aq)E° = +2.866 V
Cl2(g)+ 2 e- → 2 Cl-(aq)E° = 1.358 V

Accepted Answer

A) 3.016 V 
B) -4.224 V 
C) 1.508 V 
D) 4.224 V 
E) -1.508 V 
A) 3.016 V 
B) -4.224 V 
C) 1.508 V 
D) 4.224 V 
E) -1.508 V

Question 15

What mass of aluminum can be deposited by the passage of a constant current of 5.00 A through a Al(NO3)3(aq)solution for 2.00 hours?

Accepted Answer

A) 3.36 g 
B) 1.12 g 
C) 0.0559 g 
D) 0.672 g 
E) 0.125 g 
A) 3.36 g 
B) 1.12 g 
C) 0.0559 g 
D) 0.672 g 
E) 0.125 g

Question 16

What is the cell diagram for the spontaneous cell involving the Cl2(g)∣ Cl-(aq)(1.358 V)and the Sn2+(aq)∣ Sn(s)(-0.137V)half cells?

Accepted Answer

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

Question 17

Determine E°cell at 25 °C for the following reaction:
3 Sn2+(aq)+ 2 Al(s)→ 2 Al3+(aq)+ 3 Sn(s)
Al3+(aq)+ 3 e- → Al(s)E° = -1.676 V
Sn2+(aq)+ 2 e- → Sn(s)E° = -0.137 V

Accepted Answer

A) 2.941 V 
B) -1.813 V 
C) 1.813 V 
D) -1.539 V 
E) 1.539 V 
A) 2.941 V 
B) -1.813 V 
C) 1.813 V 
D) -1.539 V 
E) 1.539 V

Question 18

What is the cell diagram for the spontaneous cell involving the Fe3+(aq)∣ Fe2+(aq)∣ Pt(s)(0.771V)half cell and the Zn2+(aq)∣ Zn(s)(-0.763 V)half cell?

Accepted Answer

A) Fe2+(aq)∣ Fe3+(aq)   Zn2+(aq)∣ Zn(s) 
B) Pt(s)∣ Fe2+(aq),Fe3+(aq)   Zn2+(aq)∣ Zn(s) 
C) Zn(s)∣ Zn2+(aq)   Fe3+(aq)∣ Fe2+(aq)∣ Pt(s) 
D) Zn(s)∣ Zn2+(aq)   Fe3+(aq)∣ Fe2+(aq) 
E) Zn(s)∣ Zn2+(aq)   Fe3+(aq)∣ Fe2+(aq)∣ Zn(s) 
A) Fe2+(aq)∣ Fe3+(aq)   Zn2+(aq)∣ Zn(s) 
B) Pt(s)∣ Fe2+(aq),Fe3+(aq)   Zn2+(aq)∣ Zn(s) 
C) Zn(s)∣ Zn2+(aq)   Fe3+(aq)∣ Fe2+(aq)∣ Pt(s) 
D) Zn(s)∣ Zn2+(aq)   Fe3+(aq)∣ Fe2+(aq) 
E) Zn(s)∣ Zn2+(aq)   Fe3+(aq)∣ Fe2+(aq)∣ Zn(s)

Question 19

Determine the Ksp at 25 °C of AgCl(s).The half-reactions are:
Ag+(aq)+ 1 e- → Ag(s)E° = +0.771 V
AgCl(s)+ 1 e- → Ag(s)+ Cl-(aq) E° = +0.222 V

Accepted Answer

A) 1 × 10-2  
B) 0.771 
C) 4 × 1011  
D) 5 × 10-10 
E) 4 × 10-11  
A) 1 × 10-2  
B) 0.771 
C) 4 × 1011  
D) 5 × 10-10 
E) 4 × 10-11

Question 20

Determine E°cell for the reaction: 2 Ag(s)+ Mg2+(aq)→ 2 Ag+(aq)+ Mg.(s)The half reactions are:
Mg2+(aq)+ 2 e- → Mg(s)E° = -2.356 V
Ag+(aq)+ e- → Ag(s)E° = 0.800 V

Accepted Answer

A) 0.756 V 
B) -0.756 V 
C) 3.156 V 
D) -3.156 V 
E) 1.556 V 
A) 0.756 V 
B) -0.756 V 
C) 3.156 V 
D) -3.156 V 
E) 1.556 V

Exam 19: Electrochemistry

A primary battery is recharged by passing electricity through the battery.

The following galvanic cell has a measured cell potential E°cell = 0.646 V. Pt(s)∣ Sn4+(aq),Sn2+(aq) Ag+(aq)∣ Ag(s) Given that the standard reduction potential for the reduction of Ag+(aq)to Ag(s)is +0.800 V,what is the standard reduction potential for the Sn4+/Sn2+ half-reaction?

In a galvanic cell,oxidation occurs at the:

Calculate the Ksp of lead iodide from the following standard electrode potentials,at 25 °C: 2 e- + PbI2(S)→ Pb(s)+ 2 I-(aq)E° = -0.365 V 2 e- + Pb2+(aq)→ Pb(s)E° = -0.126 V

Determine Ecell at 25 °C for the following reaction at 25 °C: Al(s)∣ Al3+(0.435 M) Sn2+(2.12 × 10-3 M)∣ Sn(s) 3 Sn2+(aq)+ 2 Al(s)→ 2 Al3+(aq)+ 3 Sn(s) Al3+(aq)+ 3 e- → Al(s)E° = -1.676 V Sn2+(aq)+ 2 e- → Sn(s)E° = -0.137 V

What is ΔG° at 25 °C for the reaction (not balanced): C3H8(g)+ O2(g)→ CO2(g)+ H2O(l)if the standard cell potential is 1.092 V?

Determine E°cell for the reaction: 2 Ag+(aq)+ Mg(s)→ 2 Ag(s)+ Mg2+(aq).The half reactions are: Mg2+(aq)+ 2 e- → Mg(s)E° = -2.356 V Ag+(aq)+ e- → Ag(s)E° = 0.800 V

Cathodic protection is attaching a more active metal to the protected metal.

Choose the correct statement based on the following oxidation potentials. Mg/Mg2+ +2.37 v Fe/Fe2+ +0.44 v Cu/Cu2+ -0.34 v Zn/Zn2+ +0.76 v Sn/Sn2+ +0.14 v Ag/Ag+ -0.80 v

What is the Ecell for the following concentration cell at 25 °C: Pt(s)∣ H2(g,0.025 atm)∣ H+ (0.012 M) H+ (aq,1 M)∣ H2(g,1 atm)∣ Pt(s) 2 H+(aq)+ 2 e- → H2(g)E° = 0.V

What is the [H+] in a concentration cell at 25 °C if the cell potential is 0.0451 V and cell diagram: Pt(s)∣ H2 (g,1 atm)∣ H+(?) H+ (aq,1 M)∣ H2(g,1 atm) 2 H+(aq)+ 2 e- → H2(g)E° = 0.V

Consider the galvanic cell, Which one of the following changes to the cell would cause the cell potential to increase (i.e. ,become more positive)?

Choose the INCORRECT statement.

Determine E°cell for the reaction: Cl2(g)+ 2 F-(aq)→ 2 Cl-(aq)+ F2(g).The half reactions are: F2(g)+ 2 e- → 2 F-(aq)E° = +2.866 V Cl2(g)+ 2 e- → 2 Cl-(aq)E° = 1.358 V

What mass of aluminum can be deposited by the passage of a constant current of 5.00 A through a Al(NO3)3(aq)solution for 2.00 hours?

What is the cell diagram for the spontaneous cell involving the Cl2(g)∣ Cl-(aq)(1.358 V)and the Sn2+(aq)∣ Sn(s)(-0.137V)half cells?

Determine E°cell at 25 °C for the following reaction: 3 Sn2+(aq)+ 2 Al(s)→ 2 Al3+(aq)+ 3 Sn(s) Al3+(aq)+ 3 e- → Al(s)E° = -1.676 V Sn2+(aq)+ 2 e- → Sn(s)E° = -0.137 V

What is the cell diagram for the spontaneous cell involving the Fe3+(aq)∣ Fe2+(aq)∣ Pt(s)(0.771V)half cell and the Zn2+(aq)∣ Zn(s)(-0.763 V)half cell?

Determine the Ksp at 25 °C of AgCl(s).The half-reactions are: Ag+(aq)+ 1 e- → Ag(s)E° = +0.771 V AgCl(s)+ 1 e- → Ag(s)+ Cl-(aq) E° = +0.222 V

Determine E°cell for the reaction: 2 Ag(s)+ Mg2+(aq)→ 2 Ag+(aq)+ Mg.(s)The half reactions are: Mg2+(aq)+ 2 e- → Mg(s)E° = -2.356 V Ag+(aq)+ e- → Ag(s)E° = 0.800 V

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

Calculate the K_sp of lead iodide from the following standard electrode potentials,at 25 °C: 2 e^- + PbI₂(S)→ Pb(s)+ 2 I^-(aq)E° = -0.365 V 2 e^- + Pb²⁺(aq)→ Pb(s)E° = -0.126 V

Determine E_cell at 25 °C for the following reaction at 25 °C: Al(s)∣ Al³⁺(0.435 M) Sn²⁺(2.12 × 10^-3 M)∣ Sn(s) 3 Sn²⁺(aq)+ 2 Al(s)→ 2 Al³⁺(aq)+ 3 Sn(s) Al³⁺(aq)+ 3 e^- → Al(s)E° = -1.676 V Sn²⁺(aq)+ 2 e^- → Sn(s)E° = -0.137 V

What is ΔG° at 25 °C for the reaction (not balanced): C₃H₈(g)+ O₂(g)→ CO₂(g)+ H₂O(l)if the standard cell potential is 1.092 V?

Determine E°_cell for the reaction: 2 Ag⁺(aq)+ Mg(s)→ 2 Ag(s)+ Mg²⁺(aq).The half reactions are: Mg²⁺(aq)+ 2 e^- → Mg(s)E° = -2.356 V Ag⁺(aq)+ e^- → Ag(s)E° = 0.800 V

Choose the correct statement based on the following oxidation potentials. Mg/Mg²⁺ +2.37 v Fe/Fe²⁺ +0.44 v Cu/Cu²⁺ -0.34 v Zn/Zn²⁺ +0.76 v Sn/Sn²⁺ +0.14 v Ag/Ag⁺ -0.80 v

What is the E_cell for the following concentration cell at 25 °C: Pt(s)∣ H₂(g,0.025 atm)∣ H⁺ (0.012 M) H⁺ (aq,1 M)∣ H₂(g,1 atm)∣ Pt(s) 2 H⁺(aq)+ 2 e^- → H₂(g)E° = 0.V

What is the [H⁺] in a concentration cell at 25 °C if the cell potential is 0.0451 V and cell diagram: Pt(s)∣ H₂ (g,1 atm)∣ H⁺(?) H⁺ (aq,1 M)∣ H₂(g,1 atm) 2 H⁺(aq)+ 2 e^- → H₂(g)E° = 0.V

Determine E°_cell for the reaction: Cl₂(g)+ 2 F^-(aq)→ 2 Cl^-(aq)+ F₂(g).The half reactions are: F₂(g)+ 2 e^- → 2 F^-(aq)E° = +2.866 V Cl₂(g)+ 2 e^- → 2 Cl^-(aq)E° = 1.358 V

What mass of aluminum can be deposited by the passage of a constant current of 5.00 A through a Al(NO₃)₃(aq)solution for 2.00 hours?

What is the cell diagram for the spontaneous cell involving the Cl₂(g)∣ Cl-(aq)(1.358 V)and the Sn²⁺(aq)∣ Sn(s)(-0.137V)half cells?

Determine E°_cell at 25 °C for the following reaction: 3 Sn²⁺(aq)+ 2 Al(s)→ 2 Al³⁺(aq)+ 3 Sn(s) Al³⁺(aq)+ 3 e^- → Al(s)E° = -1.676 V Sn²⁺(aq)+ 2 e^- → Sn(s)E° = -0.137 V

What is the cell diagram for the spontaneous cell involving the Fe³⁺(aq)∣ Fe²⁺(aq)∣ Pt(s)(0.771V)half cell and the Zn²⁺(aq)∣ Zn(s)(-0.763 V)half cell?

Determine the K_spat 25 °C of AgCl(s).The half-reactions are: Ag⁺(aq)+ 1 e^- → Ag(s)E° = +0.771 V AgCl(s)+ 1 e^- → Ag(s)+ Cl^-(aq) E° = +0.222 V

Determine E°_cell for the reaction: 2 Ag(s)+ Mg²⁺(aq)→ 2 Ag⁺(aq)+ Mg.(s)The half reactions are: Mg²⁺(aq)+ 2 e^- → Mg(s)E° = -2.356 V Ag⁺(aq)+ e^- → Ag(s)E° = 0.800 V