Question 1

For the reaction 2 Al(s)+ 3 Co2+(aq)→ 2 Al3+(aq)+ 3 Co(s),ΔG° is -799 kJ.What is E° for a standard cell based on this reaction?

Accepted Answer

A) +1.38 V 
B) +2.76 V 
C) +4.14 V 
D) +8.28 V 
A) +1.38 V 
B) +2.76 V 
C) +4.14 V 
D) +8.28 V A

Question 2

Based on the half-reactions and their respective standard reduction potentials below,what is the standard cell potential for the reaction that is expected to occur?
Fe3+(aq)+ e- → Fe2+(aq)0.77 V
Sn4+(aq)+ 2 e- → Sn2+(aq)0.15 V
Pb2+(aq)+ 2 e- → Pb(s)-0.13 V

Accepted Answer

A) 0)28 V 
B) 0)64 V 
C) 0)90 V 
D) 1)03 V 
A) 0)28 V 
B) 0)64 V 
C) 0)90 V 
D) 1)03 V C

Question 3

-Use Table 17.1 to calculate the standard potential for the reaction
O2(g)+ 4 H+(aq)+ 2 Cu(s)→ 2 Cu2+(aq)+ 2 H2O(l).

Accepted Answer

A) -1.57 V 
B) -0.89 V 
C) +0.89 V 
D) +1.57 V 
A) -1.57 V 
B) -0.89 V 
C) +0.89 V 
D) +1.57 V C

Question 4

An electrolytic cell is

Accepted Answer

A) a battery. 
B) a cell in which the cell reaction is spontaneous. 
C) a cell in which an electric current drives a nonspontaneous reaction. 
D) a cell in which reactants are continuously supplied to the cell. 
A) a battery. 
B) a cell in which the cell reaction is spontaneous. 
C) a cell in which an electric current drives a nonspontaneous reaction. 
D) a cell in which reactants are continuously supplied to the cell.

Question 5

Based on the half-reactions and their respective standard reduction potentials below,the strongest reducing agent is ________,and the strongest oxidizing agent is ________.
Fe3+(aq)+ 3 e- → Fe2+(aq)0.77 V
Sn4+(aq)+ 2 e- → Sn2+(aq)0.15 V
Pb2+(aq)+ 2 e- → Pb(s)-0.13 V

Accepted Answer

Question 6

Which requires the most electricity (in terms of faradays of charge transferred)per gram of useful product formed?

Accepted Answer

A) electrolysis of aqueous NaCl (chlor-alkali industry) 
B) electrolysis of molten NaCl/CaCl2 in a Downs cell 
C) electrorefining copper metal 
D) production of aluminum in the Hall-Heroult process 
A) electrolysis of aqueous NaCl (chlor-alkali industry) 
B) electrolysis of molten NaCl/CaCl2 in a Downs cell 
C) electrorefining copper metal 
D) production of aluminum in the Hall-Heroult process

Question 7

A constant current is passed through a solution containing Cu2+(aq)resulting in the deposition of 4.40 g of Cu at the cathode.Assuming a current efficiency of 100%,if this same current is passed through a solution of TcO4- for the same amount of time,how many grams of Tc would form at the cathode?

Accepted Answer

A) 0)969 g 
B) 1)94 g 
C) 6)78 g 
D) 13.6 g 
A) 0)969 g 
B) 1)94 g 
C) 6)78 g 
D) 13.6 g

Question 8

Calculate the value of the reaction quotient,Q,for the galvanic cell expressed using shorthand notation below.Use the balanced chemical equation that has the smallest whole number stoichiometric coefficients.
Zn(s)∣ Zn2+(aq,0.0100 M)∣∣ Ag+(aq,1.25 M)∣ Ag(s)

Accepted Answer

A) 156 
B) 125 
C) 8)00 × 10-3 
D) 6)40 × 10-3 
A) 156 
B) 125 
C) 8)00 × 10-3 
D) 6)40 × 10-3

Question 9

The nickel-cadmium battery cell has a standard potential of +1.20 V.The cell reaction is
2 NiO(OH)(s)+ Cd(s)+ 2 H2O(l)→ 2 Ni(OH)2(s)+ Cd(OH)2(s).
What is the standard free energy change for this reaction?

Accepted Answer

A) -38.7 kJ 
B) -116 kJ 
C) -232 kJ 
D) -463 kJ 
A) -38.7 kJ 
B) -116 kJ 
C) -232 kJ 
D) -463 kJ

Question 10

Given: Ag+(aq)+ e- → Ag(s)E° = +0.799 V
AgI(s)+ e- → Ag(s)+ I-(aq)E° = -0.152 V
Ni2+(aq)+ 2 e- → Ni(s)E° = -0.267 V
Which of the following reactions should be spontaneous under standard conditions?
I.2 AgI(s)+ Ni(s)→ 2 Ag(s)+ 2 I-(aq)+ Ni2+(aq)
II.Ag+(aq)+ I-(aq)→ AgI(s)

Accepted Answer

A) I and II are both nonspontaneous. 
B) I is nonspontaneous and II is spontaneous. 
C) I is spontaneous and II is nonspontaneous. 
D) I and II are both spontaneous. 
A) I and II are both nonspontaneous. 
B) I is nonspontaneous and II is spontaneous. 
C) I is spontaneous and II is nonspontaneous. 
D) I and II are both spontaneous.

Question 11

Based on the following information,
F2(g)+ 2 e- → 2 F-(aq)E° = +2.87 V
Mg2+(aq)+ 2 e- → 2 Mg(s)E° = -2.37 V
Which of the following chemical species is the strongest reducing agent?

Accepted Answer

A) F2(g) 
B) Mg2+(aq) 
C) F-(aq) 
D) Mg(s) 
A) F2(g) 
B) Mg2+(aq) 
C) F-(aq) 
D) Mg(s)

Question 12

Which statement is true?

Accepted Answer

A) The cathode is positive for a galvanic cell and negative for an electrolytic cell. 
B) Electrons flow through the external circuit to the cathode in a galvanic cell and to the anode in an electrolytic cell. 
C) Oxidation occurs at the anode in a galvanic cell and at the cathode in an electrolytic cell. 
D) Oxidation occurs at the cathode in a galvanic cell and at the anode in an electrolytic cell. 
A) The cathode is positive for a galvanic cell and negative for an electrolytic cell. 
B) Electrons flow through the external circuit to the cathode in a galvanic cell and to the anode in an electrolytic cell. 
C) Oxidation occurs at the anode in a galvanic cell and at the cathode in an electrolytic cell. 
D) Oxidation occurs at the cathode in a galvanic cell and at the anode in an electrolytic cell.

Question 13

A steel pipe can be protected from corrosion by attaching the pipe to a piece of magnesium because

Accepted Answer

A) magnesium forms a tight oxide coating. 
B) magnesium is more easily oxidized than iron. 
C) magnesium is inert. 
D) magnesium and steel form a corrosion resistant alloy. 
A) magnesium forms a tight oxide coating. 
B) magnesium is more easily oxidized than iron. 
C) magnesium is inert. 
D) magnesium and steel form a corrosion resistant alloy.

Question 14

A galvanic cell employs the reaction
Mg2+(aq)+ Cu(s)→ Mg(s)+ Cu2+(aq)
And NaNO3 is the salt used in the salt bridge.During the course of the reaction

Accepted Answer

A) Na+ leaves the salt bridge and enters the anode compartment. 
B) NaNO3 leaves the salt bridge and enters the anode compartment. 
C) Na+ leaves the salt bridge and enters the cathode compartment. 
D) NaNO3 leaves the salt bridge and enters the cathode compartment. 
A) Na+ leaves the salt bridge and enters the anode compartment. 
B) NaNO3 leaves the salt bridge and enters the anode compartment. 
C) Na+ leaves the salt bridge and enters the cathode compartment. 
D) NaNO3 leaves the salt bridge and enters the cathode compartment.

Question 15

In the galvanic cell represented by the shorthand notation
Al(s)|Al3+(aq)||Fe3+(aq)|Fe(s)
the anode is ________ and the cathode is ________.

Accepted Answer

Question 16

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the anode?
Mg(s)∣ Mg2+(aq)∣∣ Cd2+(aq)∣Cd(s)

Accepted Answer

A) Mg(s)→ Mg2+(aq)+ 2 e- 
B) Mg2+(aq)+ 2 e- → Mg(s) 
C) Cd(s)→ Cd2+(aq)+ 2 e- 
D) Cd2+(aq)+ 2 e- → Cd(s) 
A) Mg(s)→ Mg2+(aq)+ 2 e- 
B) Mg2+(aq)+ 2 e- → Mg(s) 
C) Cd(s)→ Cd2+(aq)+ 2 e- 
D) Cd2+(aq)+ 2 e- → Cd(s)

Question 17

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NICl2 for 60.0 minutes?

Accepted Answer

A) 10.9 g 
B) 16.4 g 
C) 32.8 g 
D) 36.3 g 
A) 10.9 g 
B) 16.4 g 
C) 32.8 g 
D) 36.3 g

Question 18

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below?
Pt(s)|Sn2+(aq)|Sn4+(aq)∣∣Br2(l)|Br-(aq)|Pt(s)

Accepted Answer

A) Sn2+(aq)+ Br2(l)→ Sn4+(aq)+ 2 Br-(aq) 
B) Sn2+(aq)+ 2 Br-(aq)→ Sn4+(aq)+ Br2(l) 
C) Sn4+(aq)+ Br2(l)→ Sn2+(aq)+ 2 Br-(aq) 
D) Sn4+(aq)+ 2 Br-(aq)→ Sn2+(aq)+ Br2(l) 
A) Sn2+(aq)+ Br2(l)→ Sn4+(aq)+ 2 Br-(aq) 
B) Sn2+(aq)+ 2 Br-(aq)→ Sn4+(aq)+ Br2(l) 
C) Sn4+(aq)+ Br2(l)→ Sn2+(aq)+ 2 Br-(aq) 
D) Sn4+(aq)+ 2 Br-(aq)→ Sn2+(aq)+ Br2(l)

Question 19

In the shorthand notation for a galvanic cell,a double vertical line (∣∣)represents

Accepted Answer

A) a double phase boundary 
B) an inert electrode 
C) a phase boundary 
D) a salt bridge 
A) a double phase boundary 
B) an inert electrode 
C) a phase boundary 
D) a salt bridge

Question 20

How many moles of electrons,n,are transferred in the following reduction-oxidation reaction?
2 MnO4-(aq)+ 16 H+(aq)+ 10 Cl-(aq)→ 2 Mn2+(aq)+ 5 Cl2(g)+ 8 H2O(l)

Accepted Answer

A) 2 
B) 4 
C) 5 
D) 10 
A) 2 
B) 4 
C) 5 
D) 10

Exam 17: Electrochemistry

For the reaction 2 Al(s)+ 3 Co2+(aq)→ 2 Al3+(aq)+ 3 Co(s),ΔG° is -799 kJ.What is E° for a standard cell based on this reaction?

Based on the half-reactions and their respective standard reduction potentials below,what is the standard cell potential for the reaction that is expected to occur? Fe3+(aq)+ e- → Fe2+(aq)0.77 V Sn4+(aq)+ 2 e- → Sn2+(aq)0.15 V Pb2+(aq)+ 2 e- → Pb(s)-0.13 V

-Use Table 17.1 to calculate the standard potential for the reaction O2(g)+ 4 H+(aq)+ 2 Cu(s)→ 2 Cu2+(aq)+ 2 H2O(l).

An electrolytic cell is

Based on the half-reactions and their respective standard reduction potentials below,the strongest reducing agent is ________,and the strongest oxidizing agent is ________. Fe3+(aq)+ 3 e- → Fe2+(aq)0.77 V Sn4+(aq)+ 2 e- → Sn2+(aq)0.15 V Pb2+(aq)+ 2 e- → Pb(s)-0.13 V

Which requires the most electricity (in terms of faradays of charge transferred)per gram of useful product formed?

A constant current is passed through a solution containing Cu2+(aq)resulting in the deposition of 4.40 g of Cu at the cathode.Assuming a current efficiency of 100%,if this same current is passed through a solution of TcO4- for the same amount of time,how many grams of Tc would form at the cathode?

Calculate the value of the reaction quotient,Q,for the galvanic cell expressed using shorthand notation below.Use the balanced chemical equation that has the smallest whole number stoichiometric coefficients. Zn(s)∣ Zn2+(aq,0.0100 M)∣∣ Ag+(aq,1.25 M)∣ Ag(s)

The nickel-cadmium battery cell has a standard potential of +1.20 V.The cell reaction is 2 NiO(OH)(s)+ Cd(s)+ 2 H2O(l)→ 2 Ni(OH)2(s)+ Cd(OH)2(s). What is the standard free energy change for this reaction?

Given: Ag+(aq)+ e- → Ag(s)E° = +0.799 V AgI(s)+ e- → Ag(s)+ I-(aq)E° = -0.152 V Ni2+(aq)+ 2 e- → Ni(s)E° = -0.267 V Which of the following reactions should be spontaneous under standard conditions? I.2 AgI(s)+ Ni(s)→ 2 Ag(s)+ 2 I-(aq)+ Ni2+(aq) II.Ag+(aq)+ I-(aq)→ AgI(s)

Based on the following information, F2(g)+ 2 e- → 2 F-(aq)E° = +2.87 V Mg2+(aq)+ 2 e- → 2 Mg(s)E° = -2.37 V Which of the following chemical species is the strongest reducing agent?

Which statement is true?

A steel pipe can be protected from corrosion by attaching the pipe to a piece of magnesium because

A galvanic cell employs the reaction Mg2+(aq)+ Cu(s)→ Mg(s)+ Cu2+(aq) And NaNO3 is the salt used in the salt bridge.During the course of the reaction

In the galvanic cell represented by the shorthand notation Al(s)|Al3+(aq)||Fe3+(aq)|Fe(s) the anode is ________ and the cathode is ________.

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the anode? Mg(s)∣ Mg2+(aq)∣∣ Cd2+(aq)∣Cd(s)

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NICl2 for 60.0 minutes?

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Pt(s)|Sn2+(aq)|Sn4+(aq)∣∣Br2(l)|Br-(aq)|Pt(s)

In the shorthand notation for a galvanic cell,a double vertical line (∣∣)represents

How many moles of electrons,n,are transferred in the following reduction-oxidation reaction? 2 MnO4-(aq)+ 16 H+(aq)+ 10 Cl-(aq)→ 2 Mn2+(aq)+ 5 Cl2(g)+ 8 H2O(l)

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For the reaction 2 Al(s)+ 3 Co²⁺(aq)→ 2 Al³⁺(aq)+ 3 Co(s),ΔG° is -799 kJ.What is E° for a standard cell based on this reaction?

Based on the half-reactions and their respective standard reduction potentials below,what is the standard cell potential for the reaction that is expected to occur? Fe³⁺(aq)+ e^- → Fe²⁺(aq)0.77 V Sn⁴⁺(aq)+ 2 e^- → Sn²⁺(aq)0.15 V Pb²⁺(aq)+ 2 e^- → Pb(s)-0.13 V

-Use Table 17.1 to calculate the standard potential for the reaction O₂(g)+ 4 H⁺(aq)+ 2 Cu(s)→ 2 Cu²⁺(aq)+ 2 H₂O(l).

Based on the half-reactions and their respective standard reduction potentials below,the strongest reducing agent is ,and the strongest oxidizing agent is . Fe³⁺(aq)+ 3 e^- → Fe²⁺(aq)0.77 V Sn⁴⁺(aq)+ 2 e^- → Sn²⁺(aq)0.15 V Pb²⁺(aq)+ 2 e^- → Pb(s)-0.13 V

Calculate the value of the reaction quotient,Q,for the galvanic cell expressed using shorthand notation below.Use the balanced chemical equation that has the smallest whole number stoichiometric coefficients. Zn(s)∣ Zn²⁺(aq,0.0100 M)∣∣ Ag+(aq,1.25 M)∣ Ag(s)

The nickel-cadmium battery cell has a standard potential of +1.20 V.The cell reaction is 2 NiO(OH)(s)+ Cd(s)+ 2 H₂O(l)→ 2 Ni(OH)₂(s)+ Cd(OH)₂(s). What is the standard free energy change for this reaction?

Given: Ag⁺(aq)+ e^- → Ag(s)E° = +0.799 V AgI(s)+ e^- → Ag(s)+ I^-(aq)E° = -0.152 V Ni²⁺(aq)+ 2 e^- → Ni(s)E° = -0.267 V Which of the following reactions should be spontaneous under standard conditions? I.2 AgI(s)+ Ni(s)→ 2 Ag(s)+ 2 I^-(aq)+ Ni²⁺(aq) II.Ag+(aq)+ I^-(aq)→ AgI(s)

Based on the following information, F₂(g)+ 2 e^- → 2 F^-(aq)E° = +2.87 V Mg²⁺(aq)+ 2 e^- → 2 Mg(s)E° = -2.37 V Which of the following chemical species is the strongest reducing agent?

A galvanic cell employs the reaction Mg²⁺(aq)+ Cu(s)→ Mg(s)+ Cu²⁺(aq) And NaNO₃ is the salt used in the salt bridge.During the course of the reaction

In the galvanic cell represented by the shorthand notation Al(s)|Al³⁺(aq)||Fe³⁺(aq)|Fe(s) the anode is and the cathode is .

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the anode? Mg(s)∣ Mg²⁺(aq)∣∣ Cd²⁺(aq)∣Cd(s)

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NICl₂ for 60.0 minutes?

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Pt(s)|Sn²⁺(aq)|Sn⁴⁺(aq)∣∣Br₂(l)|Br^-(aq)|Pt(s)

How many moles of electrons,n,are transferred in the following reduction-oxidation reaction? 2 MnO₄^-(aq)+ 16 H⁺(aq)+ 10 Cl^-(aq)→ 2 Mn²⁺(aq)+ 5 Cl₂(g)+ 8 H₂O(l)