Question 1

A concentration cell is based on the aqueous reaction
Cu2+(1.00 M) F1F1F1S1F1F1F10 Cu2+(0.0100 M)
Calculate the potential of this cell if it operates at 25.0°C.

Accepted Answer

Question 2

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction)  potential for the anode is - 0.22 V, what is the standard electrode potential for the cathode?

Accepted Answer

A)   0.96 V
B)   0.52 V
C)   -0.52 V
D)   -0.96 V
E)   Need to know the cell reaction in order to calculate the answer.F) A) and B)
G) A) and C)

Question 3

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°Fe = -0.44 V; all E° values refer to the M2+/M half-cell reactions.

Accepted Answer

A)   copper, Cu, E° = 0.15 V
B)   cobalt, Co, E° = -0.28 V
C)   chromium, Cr, E° = -0.74 V
D)   tin, Sn, E° = -0.14 V
E)   None of these metals would be capable of acting as a sacrificial anode with iron.F) C) and D)
G) B) and E)

Question 4

A much-studied cell in electrochemistry has the following cell notation:
Ag(s) F1F1F1S1F1F1F10 AgCl(s) F1F1F1S1F1F1F10 HCl(aq) F1F1F1S1F1F1F10 H2(g) F1F1F1S1F1F1F10 Pt(s)
Bearing in mind that HCl(aq) consists of H+(aq) and Cl-(aq), and that this solution is in contact with both electrodes (there is no salt bridge), write down balanced equations for
a. the anode half-reaction.
b. the cathode half-reaction.
c. the cell reaction.

Accepted Answer

a. Ag(s) + Cl^-(aq) F1F...

Question 5

What product forms at the cathode during the electrolysis of molten lithium iodide?

Accepted Answer

A)   Li+(l) 
B)   Li(l) 
C)   I-(l) 
D)   I2(g) 
E)   I3-(l) F) A) and E)
G) B) and D)

Question 6

A voltaic cell prepared using aluminum and nickel has the following cell notation. 
Al(s)  | Al3+(aq)  || Ni2+(aq)  | Ni(s) 
Which of the following reactions occurs at the anode?

Accepted Answer

A)   Al(s)   Al3+(aq)  + 3e-
B)   Al3+(aq)  + 3e  Al(s) 
C)   Ni(s)   Ni2+(aq)  + 2e-
D)   Ni2+(aq)  + 2e-  Ni(s) 
E)   none of the aboveF) B) and C)
G) None of the above

Question 7

A voltaic cell consists of a Mn/Mn2+ electrode (E° = -1.18 V)  and a Fe/Fe2+ electrode (E° = -0.44 V) . Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25°C.

Accepted Answer

A)   0.040 M
B)   0.24 M
C)   1.1 M
D)   1.8 M
E)   none of the aboveF) A) and D)
G) C) and D)

Question 8

In the absence of oxygen, iron will rust as long as moisture is present.

Accepted Answer

A) True 
 B)False

Question 9

Oxidation occurs at the cathode of a galvanic cell, but at the anode of an electrolytic cell.

Accepted Answer

A) True 
 B)False

Question 10

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 D)
G) B) and C)

Question 11

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 the aboveF) B) and C)
G) A) and D)

Question 12

A battery is considered "dead" when

Accepted Answer

A)   Q 
B)   Q = 1.
C)   Q > 1.
D)   Q = K.
E)   Q/K = 0.F) A) and B)
G) B) and C)

Question 13

A secondary cell (battery) can operate either as a galvanic or an electrolytic cell.

Accepted Answer

A) True 
 B)False

Question 14

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

Accepted Answer

A) True 
 B)False

Question 15

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Accepted Answer

A) True 
 B)False

Question 16

When metal A is placed in a solution of metal ions B2+, a reaction occurs between A and B2+, and metal ions A2+ appear in the solution. When metal B is placed in acid solution, gas bubbles form on its surface. When metal A is placed in a solution of metal ions C2+, no reaction occurs. Which of the following reactions would not occur spontaneously?

Accepted Answer

A)   C(s)  + 2H+(aq)   H2(g)  + C2+(aq) 
B)   C(s)  + A2+(aq)   A(s)  + C2+(aq) 
C)   B(s)  + C2+(aq)   C(s)  + B2+(aq) 
D)   A(s)  + 2H+(aq)   H2(g)  + A2+(aq) 
E)   B(s)  + 2H+(aq)   H2(g)  + B2+(aq) F) A) and B)
G) None of the above

Question 17

The line notation, Pt | H2(g)  | H+(aq)  || Cu2+(aq)  | Cu(s) , indicates that

Accepted Answer

A)   copper metal is a product of the cell reaction.
B)   hydrogen gas (H2)  is a product of the cell reaction.
C)   Cu is the anode.
D)   Pt is the cathode.
E)   Cu2+ is the reducing agent.F) C) and D)
G) A) and E)

Question 18

In one or two short sentences each, explain what is meant by the following terms.
a. galvanic or voltaic cell
b. electrolytic cell
c. salt bridge
d. secondary battery or cell
e. primary battery or cell
f. glass electrode

Accepted Answer

a. A galvanic (voltaic) cell is one in w...

Question 19

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

Accepted Answer

A)   sodium and sulfur
B)   hydrogen and sulfur
C)   oxygen and sulfur
D)   oxygen and sulfuric acid
E)   hydrogen and oxygenF) B) and C)
G) C) and D)

Question 20

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E°Fe = -0.44 V; all E° values refer to the M2+/M half-cell reactions.

Accepted Answer

A)   manganese, Mn, E° = -1.18 V
B)   cadmium, Cd, E° = -0.40 V
C)   magnesium, Mg, E° = -2.37 V
D)   zinc, Zn, E° = -0.76 V
E)   All of these metals are capable of acting as sacrificial anodes with iron.F) A) and E)
G) A) and D)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M)  Cu²⁺(0.0100 M) Calculate the potential of this cell if it operates at 25.0°C.

Correct Answer
verified

In one or two short sentences each, explain what is meant by the following terms. a. galvanic or voltaic cell b. electrolytic cell c. salt bridge d. secondary battery or cell e. primary battery or cell f. glass electrode

Correct Answer
verified
a. A galvanic (voltaic) cell is one in w...
View Answer

Oxidation occurs at the cathode of a galvanic cell, but at the anode of an electrolytic cell.

Correct Answer
verified

Correct Answer
verified
a. Ag(s) + Cl^-(aq) F1F...
View Answer

In the absence of oxygen, iron will rust as long as moisture is present.

Correct Answer
verified

What product forms at the cathode during the electrolysis of molten lithium iodide?

Correct Answer
verified

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

Correct Answer
verified

Correct Answer
verified

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is - 0.22 V, what is the standard electrode potential for the cathode?

Correct Answer
verified

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

Correct Answer
verified

A battery is considered "dead" when

Correct Answer
verified

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s) , indicates that

Correct Answer
verified

A voltaic cell consists of a Mn/Mn²⁺ electrode (E°= -1.18 V) and a Fe/Fe²⁺ electrode (E°= -0.44 V) . Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25°C.

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

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following reactions occurs at the anode?

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 secondary cell (battery) can operate either as a galvanic or an electrolytic cell.

Correct Answer
verified

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

Correct Answer
verified

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Correct Answer
verified

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

Correct Answer
verified

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A concentration cell is based on the aqueous reaction Cu2+(1.00 M)  Cu2+(0.0100 M) Calculate the potential of this cell if it operates at 25.0°C.

Correct AnswerverifiedShow Answer

In one or two short sentences each, explain what is meant by the following terms. a. galvanic or voltaic cell b. electrolytic cell c. salt bridge d. secondary battery or cell e. primary battery or cell f. glass electrode

Correct Answerverifieda. A galvanic (voltaic) cell is one in w...View AnswerShow Answer

Oxidation occurs at the cathode of a galvanic cell, but at the anode of an electrolytic cell.

Correct AnswerverifiedShow Answer

Correct Answerverifieda. Ag(s) + Cl-(aq) F1F...View AnswerShow Answer

In the absence of oxygen, iron will rust as long as moisture is present.

Correct AnswerverifiedShow Answer

What product forms at the cathode during the electrolysis of molten lithium iodide?

Correct AnswerverifiedShow Answer

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E°Fe = -0.44 V; all E° values refer to the M2+/M half-cell reactions.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is - 0.22 V, what is the standard electrode potential for the cathode?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

A battery is considered "dead" when

Correct AnswerverifiedShow Answer

The line notation, Pt | H2(g) | H+(aq) || Cu2+(aq) | Cu(s) , indicates that

Correct AnswerverifiedShow Answer

A voltaic cell consists of a Mn/Mn2+ electrode (E° = -1.18 V) and a Fe/Fe2+ electrode (E° = -0.44 V) . Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25°C.

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

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following reactions occurs at the anode?

Correct AnswerverifiedShow Answer

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 secondary cell (battery) can operate either as a galvanic or an electrolytic cell.

Correct AnswerverifiedShow Answer

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°Fe = -0.44 V; all E° values refer to the M2+/M half-cell reactions.

Correct AnswerverifiedShow Answer

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Correct AnswerverifiedShow Answer

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

Correct AnswerverifiedShow Answer

A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M)  Cu²⁺(0.0100 M) Calculate the potential of this cell if it operates at 25.0°C.

Correct Answer
verified

Correct Answer
verified
a. A galvanic (voltaic) cell is one in w...
View Answer

Correct Answer
verified

Correct Answer
verified
a. Ag(s) + Cl^-(aq) F1F...
View Answer

Correct Answer
verified

Correct Answer
verified

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s) , indicates that

Correct Answer
verified

A voltaic cell consists of a Mn/Mn²⁺ electrode (E°= -1.18 V) and a Fe/Fe²⁺ electrode (E°= -0.44 V) . Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25°C.

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

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following reactions occurs at the anode?

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

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified