Question 1

Consider the following electrochemical cell: U | U3+(aq)|| Cl-(aq),Cl2(g)| Pt
If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium?

Accepted Answer

A) -3.16 V 
B) +3.16 V 
C) -1.80 V 
D) +1.80 V 
E) +1.36 V 
A) -3.16 V 
B) +3.16 V 
C) -1.80 V 
D) +1.80 V 
E) +1.36 V

Question 2

How many coulombs of charge are required to cause reduction of 0.20 mole of Cr3+ to Cr?

Accepted Answer

A) 0.60 C 
B) 3.0 C 
C) 2.9 $\times$ 104 C 
D) 5.8 $\times$ 104 C 
E) 9.65 $\times$ 104 C 
A) 0.60 C 
B) 3.0 C 
C) 2.9 $\times$ 104 C 
D) 5.8 $\times$ 104 C 
E) 9.65 $\times$ 104 C

Question 3

Consider the following reaction: 2Fe2+(aq)+ Cu2+ $\to$ 2Fe3+(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

Accepted Answer

A) 0.43 V 
B) 1.11 V 
C) 0.78 V 
D) -0.43 V 
E) 0 V 
A) 0.43 V 
B) 1.11 V 
C) 0.78 V 
D) -0.43 V 
E) 0 V

Question 4

Predict the products of the electrolysis of aqueous aluminum bromide AlBr3(aq). (Balancing is not required.)

Accepted Answer

A) Al + Br2 
B) Al + O2 + H+ 
C) H2 + OH-  + Br2 
D) H2 + O2 
A) Al + Br2 
B) Al + O2 + H+ 
C) H2 + OH-  + Br2 
D) H2 + O2

Question 5

An electrochemical cell based on the following reaction has a standard cell voltage (E°cell)of 0.48 V: Sn(s)+ Cu2+(aq)$\to$ Sn2+(aq)+ Cu(s)
What is the standard reduction potential of tin(II)? (E°(Cu2+/Cu)= 0.34 V)

Accepted Answer

A) -0.14 V 
B) 0.14 V 
C) -0.82 V 
D) 0.82 V 
E) none of these 
A) -0.14 V 
B) 0.14 V 
C) -0.82 V 
D) 0.82 V 
E) none of these

Question 6

When an aqueous solution of AgNO3 is electrolyzed, a gas is observed to form at the anode. The gas is

Accepted Answer

A) H2. 
B) O2. 
C) NO. 
D) NO2. 
A) H2. 
B) O2. 
C) NO. 
D) NO2.

Question 7

Aluminum does not corrode as does iron, because

Accepted Answer

A) Al does not react with O2. 
B) A protective layer of Al2O3 forms on the metal surface. 
C) Al is harder to oxidize than is Fe. 
D) Fe gives cathodic protection to Al. 
E) The electrical circuit cannot be completed on an Al surface. 
A) Al does not react with O2. 
B) A protective layer of Al2O3 forms on the metal surface. 
C) Al is harder to oxidize than is Fe. 
D) Fe gives cathodic protection to Al. 
E) The electrical circuit cannot be completed on an Al surface.

Question 8

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl3 electrolyte. Calculate the number of moles of gold deposited in 3.0 min by a constant current of 10.A.

Accepted Answer

A) 6.2 $\times$ 10-3 mol 
B) 9.3 $\times$ 10-3 mol 
C) 1.8 $\times$ 10-2 mol 
D) 3.5 $\times$ 10-5 mol 
E) 160 mol 
A) 6.2 $\times$ 10-3 mol 
B) 9.3 $\times$ 10-3 mol 
C) 1.8 $\times$ 10-2 mol 
D) 3.5 $\times$ 10-5 mol 
E) 160 mol

Question 9

How many faradays are transferred in an electrolytic cell when a current of 2.0 amperes flows for 12 hours?

Accepted Answer

A) 24 F 
B) 8.6 $\times$ 104 F 
C) 0.90 F 
D) 6.2 $\times$ 10 -3 F 
E) 1.1 F 
A) 24 F 
B) 8.6 $\times$ 104 F 
C) 0.90 F 
D) 6.2 $\times$ 10 -3 F 
E) 1.1 F

Question 10

Which one of the following reactions will occur spontaneously at standard-state conditions and 25°C?

Accepted Answer

A) Mg2+ + Ca $\to$Mg + Ca2+ 
B) Au + 3K+$\to$ Au3+ + 3K 
C) 2Al3+ + 3Fe $\to$ 2Al + 3Fe2+ 
D) Cu + 2H+ $\to$ Cu2+ + H2 
A) Mg2+ + Ca $\to$Mg + Ca2+ 
B) Au + 3K+$\to$ Au3+ + 3K 
C) 2Al3+ + 3Fe $\to$ 2Al + 3Fe2+ 
D) Cu + 2H+ $\to$ Cu2+ + H2

Question 11

Consider a voltaic cell based on the following cell reaction: Ni(s)+ At2(s)$\to$ Ni2+(aq)+ 2At- (aq)
Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E°(Ni2+/Ni)= -0.25 V]

Accepted Answer

A) 0.80 V 
B) 0.30 V 
C) -0.30 V 
D) -0.80 V 
E) 0.43 V 
A) 0.80 V 
B) 0.30 V 
C) -0.30 V 
D) -0.80 V 
E) 0.43 V

Question 12

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Bi(OH)3 + SnO22- $\to$ Bi + SnO32- (basic solution)

Accepted Answer

A) 32 
B) 25 
C) 16 
D) 13 
E) None of these. 
A) 32 
B) 25 
C) 16 
D) 13 
E) None of these.

Question 13

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. • an Al(s)electrode in 0.5 M Al2(SO4)3 solution
• a Pb(s)electrode in 1.0 M Pb(NO3)2 solution
Which electrode is the anode?

Accepted Answer

A) Al 
B) Pb 
C) Neither 
A) Al 
B) Pb 
C) Neither

Question 14

Consider the following standard reduction potentials in acid solution:   The strongest reducing agent listed above is

Accepted Answer

A) Cr3+. 
B) Cr. 
C) Mn2+. 
D) Co. 
E) MnO4-. 
A) Cr3+. 
B) Cr. 
C) Mn2+. 
D) Co. 
E) MnO4-.

Question 15

Complete and balance the following redox reaction under acidic conditions:
ClO2-(aq)$\to$  ClO2(g)+ Cl-(aq)

Accepted Answer

5ClO₂^-(a

Question 16

The electrochemical cell that utilizes the reaction Zn + Cu2+ (1 M)$\to$ Zn2+ (1 M)+ Cu will have a lower cell emf when the concentrations of Zn2+ and Cu2+ ions are decreased to 0.1 M.

Accepted Answer

A) True 
 B)False

Question 17

Determine the equilibrium constant for the following reaction at 298 K.
2Fe3+(aq)+ H2O2(aq)   2H+(aq)+ O2(g)+ 2Fe2+(aq).

Accepted Answer

The answer of Determine the equilibrium constant for the following...

Question 18

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. • a Fe electrode in 1.0 M FeCl2 solution
• a Ni electrode in 1.0 M Ni(NO3)2 solution
When the cell is running spontaneously, which choice includes only true statements and no false ones?

Accepted Answer

A) The nickel electrode loses mass and the nickel electrode is the cathode. 
B) The nickel electrode gains mass and the nickel electrode is the cathode. 
C) The iron electrode gains mass and the iron electrode is the anode. 
D) The iron electrode loses mass and the iron electrode is the cathode. 
A) The nickel electrode loses mass and the nickel electrode is the cathode. 
B) The nickel electrode gains mass and the nickel electrode is the cathode. 
C) The iron electrode gains mass and the iron electrode is the anode. 
D) The iron electrode loses mass and the iron electrode is the cathode.

Question 19

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl3 for 45.0 min?

Accepted Answer

A) 9.3 $\times$ 10-4 g 
B) 0.042 g 
C) 2.5 g 
D) 24 g 
E) 2.3 $\times$1010 g 
A) 9.3 $\times$ 10-4 g 
B) 0.042 g 
C) 2.5 g 
D) 24 g 
E) 2.3 $\times$1010 g

Question 20

Complete and balance the following redox equation. What is the coefficient of H2S when the equation is balanced using the set of smallest whole-number coefficients? H2S + MnO4- $\to$ Mn2+ + SO42- (acidic solution)

Accepted Answer

A) 1 
B) 2 
C) 4 
D) 5 
E) None of these. 
A) 1 
B) 2 
C) 4 
D) 5 
E) None of these.

Exam 19: Electrochemistry

Consider the following electrochemical cell: U | U3+(aq)|| Cl-(aq),Cl2(g)| Pt If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium?

How many coulombs of charge are required to cause reduction of 0.20 mole of Cr3+ to Cr?

Consider the following reaction: 2Fe2+(aq)+ Cu2+ →\to→ 2Fe3+(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

Predict the products of the electrolysis of aqueous aluminum bromide AlBr3(aq). (Balancing is not required.)

An electrochemical cell based on the following reaction has a standard cell voltage (E°cell)of 0.48 V: Sn(s)+ Cu2+(aq) →\to→ Sn2+(aq)+ Cu(s) What is the standard reduction potential of tin(II)? (E°(Cu2+/Cu)= 0.34 V)

When an aqueous solution of AgNO3 is electrolyzed, a gas is observed to form at the anode. The gas is

Aluminum does not corrode as does iron, because

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl3 electrolyte. Calculate the number of moles of gold deposited in 3.0 min by a constant current of 10.A.

How many faradays are transferred in an electrolytic cell when a current of 2.0 amperes flows for 12 hours?

Which one of the following reactions will occur spontaneously at standard-state conditions and 25°C?

Consider a voltaic cell based on the following cell reaction: Ni(s)+ At2(s) →\to→ Ni2+(aq)+ 2At- (aq) Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E°(Ni2+/Ni)= -0.25 V]

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Bi(OH)3 + SnO22- →\to→ Bi + SnO32- (basic solution)

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. • an Al(s)electrode in 0.5 M Al2(SO4)3 solution • a Pb(s)electrode in 1.0 M Pb(NO3)2 solution Which electrode is the anode?

Consider the following standard reduction potentials in acid solution: The strongest reducing agent listed above is

Complete and balance the following redox reaction under acidic conditions: ClO2-(aq) →\to→ ClO2(g)+ Cl-(aq)

The electrochemical cell that utilizes the reaction Zn + Cu2+ (1 M) →\to→ Zn2+ (1 M)+ Cu will have a lower cell emf when the concentrations of Zn2+ and Cu2+ ions are decreased to 0.1 M.

Determine the equilibrium constant for the following reaction at 298 K. 2Fe3+(aq)+ H2O2(aq) 2H+(aq)+ O2(g)+ 2Fe2+(aq).

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. • a Fe electrode in 1.0 M FeCl2 solution • a Ni electrode in 1.0 M Ni(NO3)2 solution When the cell is running spontaneously, which choice includes only true statements and no false ones?

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl3 for 45.0 min?

Complete and balance the following redox equation. What is the coefficient of H2S when the equation is balanced using the set of smallest whole-number coefficients? H2S + MnO4- →\to→ Mn2+ + SO42- (acidic solution)

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Consider the following electrochemical cell: U | U³⁺(aq)|| Cl^-(aq),Cl₂(g)| Pt If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium?

How many coulombs of charge are required to cause reduction of 0.20 mole of Cr³⁺ to Cr?

Consider the following reaction: 2Fe²⁺(aq)+ Cu²⁺ $\to$ 2Fe³⁺(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

Predict the products of the electrolysis of aqueous aluminum bromide AlBr₃(aq). (Balancing is not required.)

An electrochemical cell based on the following reaction has a standard cell voltage (E°_cell)of 0.48 V: Sn(s)+ Cu²⁺(aq) $\to$ Sn²⁺(aq)+ Cu(s) What is the standard reduction potential of tin(II)? (E°(Cu²⁺/Cu)= 0.34 V)

When an aqueous solution of AgNO₃ is electrolyzed, a gas is observed to form at the anode. The gas is

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl₃ electrolyte. Calculate the number of moles of gold deposited in 3.0 min by a constant current of 10.A.

Consider a voltaic cell based on the following cell reaction: Ni(s)+ At₂(s) $\to$ Ni²⁺(aq)+ 2At^-(aq) Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E°(Ni²⁺/Ni)= -0.25 V]

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Bi(OH)₃ + SnO₂^2- $\to$ Bi + SnO₃^2- (basic solution)

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. • an Al(s)electrode in 0.5 M Al₂(SO₄)₃ solution • a Pb(s)electrode in 1.0 M Pb(NO₃)₂ solution Which electrode is the anode?

Complete and balance the following redox reaction under acidic conditions: ClO₂^-(aq) $\to$ ClO₂(g)+ Cl^-(aq)

The electrochemical cell that utilizes the reaction Zn + Cu²⁺(1 M) $\to$ Zn²⁺(1 M)+ Cu will have a lower cell emf when the concentrations of Zn²⁺ and Cu²⁺ ions are decreased to 0.1 M.

Determine the equilibrium constant for the following reaction at 298 K. 2Fe³⁺(aq)+ H₂O₂(aq) 2H⁺(aq)+ O₂(g)+ 2Fe²⁺(aq).

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl₃ for 45.0 min?

Complete and balance the following redox equation. What is the coefficient of H₂S when the equation is balanced using the set of smallest whole-number coefficients? H₂S + MnO₄^- $\to$ Mn²⁺ + SO₄^2- (acidic solution)