Question 1

How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten   (l)with an electrical current of 12.0 A?

Accepted Answer

A) 27.0 
B) 9.00 
C) 1.19 × 103 
D) 2.90 ×   
E) 3.57 ×   
A) 27.0 
B) 9.00 
C) 1.19 × 103 
D) 2.90 ×   
E) 3.57 ×   E

Question 2

Using the following reduction half-reactions and their respective standard reduction potentials at 25 °C,draw a diagram of a galvanic cell.
Cr2O72-(aq)+ 14 H+(aq)+ 6e- → 2 Cr3+(aq)+ 7 H2O(l)E° = +1.33 V
Zn2+(aq)+ 2 e- → Zn(s)E° = -0.763 V

Accepted Answer

A) Zn2+(aq)∣ Zn(s),H+(aq)   Cr2O72-(aq),Cr(s)∣ Cr3+(aq) 
B) Zn(s)∣ Zn2+(aq)   H+(aq),Cr3+(aq)∣ Cr(s) 
C) Cr(s)∣ Cr3+(aq),H+(aq),Cr2O72-(aq)   Zn(S)∣ Zn2+(aq) 
D) Zn(s)∣ Zn2+(aq)   Cr2O72-(aq),H+(aq),Cr3+(aq)∣ Pt(s) 
E) Pt(s)∣ Cr3+(aq),Cr2O72-(aq),H+(aq)   Zn2+(aq)∣ Zn(s) 
A) Zn2+(aq)∣ Zn(s),H+(aq)   Cr2O72-(aq),Cr(s)∣ Cr3+(aq) 
B) Zn(s)∣ Zn2+(aq)   H+(aq),Cr3+(aq)∣ Cr(s) 
C) Cr(s)∣ Cr3+(aq),H+(aq),Cr2O72-(aq)   Zn(S)∣ Zn2+(aq) 
D) Zn(s)∣ Zn2+(aq)   Cr2O72-(aq),H+(aq),Cr3+(aq)∣ Pt(s) 
E) Pt(s)∣ Cr3+(aq),Cr2O72-(aq),H+(aq)   Zn2+(aq)∣ Zn(s) D

Question 3

Determine E°cell for the reaction: I2(s)+ Cu(s)→ 2 I-(aq)+ Cu2+(aq).The half reactions are:
I2(s)+ 2 e- → 2 I-(aq)E° = +0.535 V
Cu2+(aq)+ 2 e- → Cu(s)E° = 0.340 V

Accepted Answer

A) 0.730 V 
B) -0.875 V 
C) 0.875 V 
D) 0.195 V 
E) -0.195 V 
A) 0.730 V 
B) -0.875 V 
C) 0.875 V 
D) 0.195 V 
E) -0.195 V D

Question 4

What is the reduction half-reaction for the following overall galvanic cell reaction?
Co2+(aq)+ 2Ag(s)→ Co(s)+ 2 Ag+(aq)

Accepted Answer

A) Ag(s)+ e- → Ag+(aq) 
B) Ag+(aq)+ e- → Ag(s) 
C) Co2+(aq)+ 2 e- → Co(s) 
D) Co2+(aq)+ e- → Co(s) 
A) Ag(s)+ e- → Ag+(aq) 
B) Ag+(aq)+ e- → Ag(s) 
C) Co2+(aq)+ 2 e- → Co(s) 
D) Co2+(aq)+ e- → Co(s)

Question 5

When Ecell < 0,the reaction is spontaneous.

Accepted Answer

A) True 
 B)False

Question 6

How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu2+ ions to produce 5.00 moles of copper metal?

Accepted Answer

A) 0.187 hours 
B) 0.373 hours 
C) 2.68 hours 
D) 5.36 hours 
A) 0.187 hours 
B) 0.373 hours 
C) 2.68 hours 
D) 5.36 hours

Question 7

What is E° of the spontaneous cell made from Ag+(aq)/Ag(s)(0.80 V)and Cl2(g)/Cl-(aq)(1.36 V)half cells?

Accepted Answer

A) 2.16 V 
B) -2.16 V 
C) -0.56 V 
D) 0.56 V 
E) 1.36 V 
A) 2.16 V 
B) -2.16 V 
C) -0.56 V 
D) 0.56 V 
E) 1.36 V

Question 8

Write the net redox reaction that occurs in the galvanic cell.
Zn(s)∣ Zn+2(aq)   Pb+2(aq)∣ Pb(s)

Accepted Answer

A) Pb(s)+ Zn(s)→ Pb+2(aq)+ Zn+2(aq)+ 4 e-  
B) Pb(s)+ Zn+2(aq)→ Pb+2(aq)+ Zn(s) 
C) Pb+2(s)+ Zn+2(s)→ Pb(s)+ Zn(s)+ 4 e-  
D) Pb+2(aq)+ Zn(s)→ Zn+2(aq)+ Pb(s) 
E) Pb(s)+ Zn(s)+ 4 e- → Pb+2(aq)+ Zn+2(aq) 
A) Pb(s)+ Zn(s)→ Pb+2(aq)+ Zn+2(aq)+ 4 e-  
B) Pb(s)+ Zn+2(aq)→ Pb+2(aq)+ Zn(s) 
C) Pb+2(s)+ Zn+2(s)→ Pb(s)+ Zn(s)+ 4 e-  
D) Pb+2(aq)+ Zn(s)→ Zn+2(aq)+ Pb(s) 
E) Pb(s)+ Zn(s)+ 4 e- → Pb+2(aq)+ Zn+2(aq)

Question 9

What is the cell reaction of the spontaneous cell made from the Zn2+(aq)/Zn(s)(-0.76 V)and Br2(l)/2 Br-(aq)(1.07 V)half cells?

Accepted Answer

A) 2Br-(aq)+ Zn2+(aq)→ Zn + Br2(l)  
B) Br2(l)+ Zn → Zn2+(aq)+ 2Br-(aq)  
C) 2Br-(aq)+ Zn → Br2(l)+ Zn2+(aq) 
D) Br2(l)+ Zn → Zn2+(aq)+ Br-(aq)  
E) Br2(l)+ Zn2+(aq)→ Zn + 2Br-(aq)  
A) 2Br-(aq)+ Zn2+(aq)→ Zn + Br2(l)  
B) Br2(l)+ Zn → Zn2+(aq)+ 2Br-(aq)  
C) 2Br-(aq)+ Zn → Br2(l)+ Zn2+(aq) 
D) Br2(l)+ Zn → Zn2+(aq)+ Br-(aq)  
E) Br2(l)+ Zn2+(aq)→ Zn + 2Br-(aq)

Question 10

3.53 L of 0.362 M CuCl2(aq)solution are electrolyzed for 55.6 minutes with a current of 14.0-amperes.What is [CuCl2] when the electrolysis ends?

Accepted Answer

A) 0.361 M 
B) 0.328 M 
C) 0.120 M 
D) 0.171 M 
E) 0.293 M 
A) 0.361 M 
B) 0.328 M 
C) 0.120 M 
D) 0.171 M 
E) 0.293 M

Question 11

E°cell is the standard cell potential.

Accepted Answer

A) True 
 B)False

Question 12

Accepted Answer

A) I and V 
B) II and IV 
C) I and IV 
D) II and III 
E) I and III 
A) I and V 
B) II and IV 
C) I and IV 
D) II and III 
E) I and III

Question 13

A galvanic cell consists of a Ni2+(aq)/Ni(s)half-cell and a standard hydrogen electrode.If the Ni2+/Ni half-cell standard cell functions as the anode,and the standard cell potential is 0.26 V,what is the standard reduction potential for the Ni2+(aq)/Ni(s)half-cell?

Accepted Answer

A) -0.26 V 
B) -0.13 V 
C) +0.13 V 
D) +0.26 V 
A) -0.26 V 
B) -0.13 V 
C) +0.13 V 
D) +0.26 V

Question 14

For a galvanic cell that uses the following two half-reactions,
Cr2O72-(aq)+ 14 H+(aq)+ 6 e- → 2 Cr3+(aq)+ 7 H2O(l)
Pb(s)→ Pb2+(aq)+ 2 e-
How many moles of Pb(s)are oxidized by three moles of Cr2O72-(aq)?

Accepted Answer

A) 3 
B) 6 
C) 9 
D) 18 
A) 3 
B) 6 
C) 9 
D) 18

Question 15

What is the cell potential for the following cell at 25 °C?
Al(s)∣ Al3+(0.00212 M)   Sn2+(0.435 M)∣ 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) 1.517 V 
B) 1.668 V 
C) 1.410 V 
D) 1.497 V 
E) 1.581 V 
A) 1.517 V 
B) 1.668 V 
C) 1.410 V 
D) 1.497 V 
E) 1.581 V

Question 16

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 17

What is the concentration of Al3+(aq)in the following cell at 25 °C if the cell voltage is 1.486 V?
Al(s)∣ Al3+(aq,?)   Sn2+(aq,3.21 × 10-4 M)∣ 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) 2.8 × 10-3 M 
B) 1.6 × 10-5 M 
C) 4.5 × 10-5 M 
D) 2.4 × 10-2 M 
E) 7.8 × 10-6 M 
A) 2.8 × 10-3 M 
B) 1.6 × 10-5 M 
C) 4.5 × 10-5 M 
D) 2.4 × 10-2 M 
E) 7.8 × 10-6 M

Question 18

How many coulombs would be needed to deposit all of the Ag+(aq)ion from 600 mL of a solution 0.250 M in Ag+(aq)?

Accepted Answer

A) 1.45 × 107 C 
B) 1.56 × 106 C 
C) 1.45 × 104 C 
D) 2.41 × 104 C 
E) 1.56 × 104 C 
A) 1.45 × 107 C 
B) 1.56 × 106 C 
C) 1.45 × 104 C 
D) 2.41 × 104 C 
E) 1.56 × 104 C

Question 19

For the reaction: Mg(s)+ 2 AgNO3(aq)→ 2 Ag(s)+ Mg(NO3)2(aq)
Write a voltaic diagram for the reaction.

Accepted Answer

A) Ag(s)| Ag(aq)   Mg2+(aq)| Mg(s) 
B) Mg(s)∣ Mg2+   Ag+ (aq)∣ Ag (s) 
C) Mg(s)∣ Mg2+   Ag(s)∣ Ag+ (aq) 
D) Ag(aq)∣ Ag(s)   Mg(s)∣ Mg2+ (aq) 
E) Ag(s)∣ Mg2+ (aq)   Ag+ (aq)∣ Mg(s) 
A) Ag(s)| Ag(aq)   Mg2+(aq)| Mg(s) 
B) Mg(s)∣ Mg2+   Ag+ (aq)∣ Ag (s) 
C) Mg(s)∣ Mg2+   Ag(s)∣ Ag+ (aq) 
D) Ag(aq)∣ Ag(s)   Mg(s)∣ Mg2+ (aq) 
E) Ag(s)∣ Mg2+ (aq)   Ag+ (aq)∣ Mg(s)

Question 20

What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below?
Al(s)∣ Al3+(aq)∣∣ Fe2+(aq)∣ Fe(s)

Accepted Answer

A) 2 Al(s)+ 3 Fe2+(aq)→ 2 Al3+(aq)+ 3Fe(s) 
B) 3 Al(s)+ 2 Fe2+(aq)→ 3 Al3+(aq)+ 2 Fe(s) 
C) 2 Fe(s)+ 3 Al3+(aq)→ 2 Fe2+(aq)+ 3 Al(s) 
D) 3 Fe(s)+ 2 Al3+(aq)→ 3 Fe2+(aq)+ 2 Al(s) 
A) 2 Al(s)+ 3 Fe2+(aq)→ 2 Al3+(aq)+ 3Fe(s) 
B) 3 Al(s)+ 2 Fe2+(aq)→ 3 Al3+(aq)+ 2 Fe(s) 
C) 2 Fe(s)+ 3 Al3+(aq)→ 2 Fe2+(aq)+ 3 Al(s) 
D) 3 Fe(s)+ 2 Al3+(aq)→ 3 Fe2+(aq)+ 2 Al(s)

Exam 19: Electrochemistry

How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten (l)with an electrical current of 12.0 A?

Using the following reduction half-reactions and their respective standard reduction potentials at 25 °C,draw a diagram of a galvanic cell. Cr2O72-(aq)+ 14 H+(aq)+ 6e- → 2 Cr3+(aq)+ 7 H2O(l)E° = +1.33 V Zn2+(aq)+ 2 e- → Zn(s)E° = -0.763 V

Determine E°cell for the reaction: I2(s)+ Cu(s)→ 2 I-(aq)+ Cu2+(aq).The half reactions are: I2(s)+ 2 e- → 2 I-(aq)E° = +0.535 V Cu2+(aq)+ 2 e- → Cu(s)E° = 0.340 V

What is the reduction half-reaction for the following overall galvanic cell reaction? Co2+(aq)+ 2Ag(s)→ Co(s)+ 2 Ag+(aq)

When Ecell < 0,the reaction is spontaneous.

How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu2+ ions to produce 5.00 moles of copper metal?

What is E° of the spontaneous cell made from Ag+(aq)/Ag(s)(0.80 V)and Cl2(g)/Cl-(aq)(1.36 V)half cells?

Write the net redox reaction that occurs in the galvanic cell. Zn(s)∣ Zn+2(aq) Pb+2(aq)∣ Pb(s)

What is the cell reaction of the spontaneous cell made from the Zn2+(aq)/Zn(s)(-0.76 V)and Br2(l)/2 Br-(aq)(1.07 V)half cells?

3.53 L of 0.362 M CuCl2(aq)solution are electrolyzed for 55.6 minutes with a current of 14.0-amperes.What is [CuCl2] when the electrolysis ends?

E°cell is the standard cell potential.

Which of the following are commonly used as alternate standard electrodes: I.Ag(s)| AgCl(s)| Cl- ((aq,1.0 M) II.Hg(l)| HgCl2(s)| Cl- (aq,1.0 M) III.Ag(s)| AgCl(s)| Cl- ((aq,1.0 M) IV.Hg(l)| Hg2Cl2(s)| Cl- (aq,1.0 M) V.Hg(s)| Hg2Cl2(s)| Cl- (aq,1.0 M)

A galvanic cell consists of a Ni2+(aq)/Ni(s)half-cell and a standard hydrogen electrode.If the Ni2+/Ni half-cell standard cell functions as the anode,and the standard cell potential is 0.26 V,what is the standard reduction potential for the Ni2+(aq)/Ni(s)half-cell?

For a galvanic cell that uses the following two half-reactions, Cr2O72-(aq)+ 14 H+(aq)+ 6 e- → 2 Cr3+(aq)+ 7 H2O(l) Pb(s)→ Pb2+(aq)+ 2 e- How many moles of Pb(s)are oxidized by three moles of Cr2O72-(aq)?

What is the cell potential for the following cell at 25 °C? Al(s)∣ Al3+(0.00212 M) Sn2+(0.435 M)∣ 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 concentration of Al3+(aq)in the following cell at 25 °C if the cell voltage is 1.486 V? Al(s)∣ Al3+(aq,?) Sn2+(aq,3.21 × 10-4 M)∣ Sn(s) Al3+(aq)+ 3 e- → Al(s)E° = -1.676 V Sn2+(aq)+ 2 e- → Sn(s)E° = -0.137 V

How many coulombs would be needed to deposit all of the Ag+(aq)ion from 600 mL of a solution 0.250 M in Ag+(aq)?

For the reaction: Mg(s)+ 2 AgNO3(aq)→ 2 Ag(s)+ Mg(NO3)2(aq) Write a voltaic diagram for the reaction.

What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below? Al(s)∣ Al3+(aq)∣∣ Fe2+(aq)∣ Fe(s)

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Using the following reduction half-reactions and their respective standard reduction potentials at 25 °C,draw a diagram of a galvanic cell. Cr₂O₇^2-(aq)+ 14 H⁺(aq)+ 6e^- → 2 Cr³⁺(aq)+ 7 H₂O(l)E° = +1.33 V Zn²+(aq)+ 2 e^- → Zn(s)E° = -0.763 V

Determine E°_cell for the reaction: I₂(s)+ Cu(s)→ 2 I^-(aq)+ Cu²⁺(aq).The half reactions are: I₂(s)+ 2 e^- → 2 I^-(aq)E° = +0.535 V Cu²⁺(aq)+ 2 e^- → Cu(s)E° = 0.340 V

What is the reduction half-reaction for the following overall galvanic cell reaction? Co²⁺(aq)+ 2Ag(s)→ Co(s)+ 2 Ag⁺(aq)

When E_cell < 0,the reaction is spontaneous.

How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu²⁺ ions to produce 5.00 moles of copper metal?

What is E° of the spontaneous cell made from Ag⁺(aq)/Ag(s)(0.80 V)and Cl₂(g)/Cl^-(aq)(1.36 V)half cells?

Write the net redox reaction that occurs in the galvanic cell. Zn(s)∣ Zn⁺²(aq) Pb⁺²(aq)∣ Pb(s)

What is the cell reaction of the spontaneous cell made from the Zn²⁺(aq)^/Zn(s)(-0.76 V)and Br₂(l)/2 Br^-(aq)(1.07 V)half cells?

3.53 L of 0.362 M CuCl₂(aq)solution are electrolyzed for 55.6 minutes with a current of 14.0-amperes.What is [CuCl₂] when the electrolysis ends?

E°_cell is the standard cell potential.

Which of the following are commonly used as alternate standard electrodes: I.Ag(s)| AgCl(s)| Cl^- ((aq,1.0 M) II.Hg(l)| HgCl₂(s)| Cl^- (aq,1.0 M) III.Ag(s)| AgCl(s)| Cl^- ((aq,1.0 M) IV.Hg(l)| Hg₂Cl₂(s)| Cl^- (aq,1.0 M) V.Hg(s)| Hg₂Cl₂(s)| Cl^- (aq,1.0 M)

A galvanic cell consists of a Ni²⁺(aq)/Ni(s)half-cell and a standard hydrogen electrode.If the Ni²⁺/Ni half-cell standard cell functions as the anode,and the standard cell potential is 0.26 V,what is the standard reduction potential for the Ni²⁺(aq)/Ni(s)half-cell?

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq)+ 14 H⁺(aq)+ 6 e^- → 2 Cr³⁺(aq)+ 7 H₂O(l) Pb(s)→ Pb²⁺(aq)+ 2 e^- How many moles of Pb(s)are oxidized by three moles of Cr₂O₇^2-(aq)?

What is the cell potential for the following cell at 25 °C? Al(s)∣ Al³⁺(0.00212 M) Sn²⁺(0.435 M)∣ 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 concentration of Al³⁺(aq)in the following cell at 25 °C if the cell voltage is 1.486 V? Al(s)∣ Al³⁺(aq,?) Sn²⁺(aq,3.21 × 10^-4 M)∣ Sn(s) Al³⁺(aq)+ 3 e^- → Al(s)E° = -1.676 V Sn²⁺(aq)+ 2 e^- → Sn(s)E° = -0.137 V

How many coulombs would be needed to deposit all of the Ag⁺(aq)ion from 600 mL of a solution 0.250 M in Ag⁺(aq)?

For the reaction: Mg(s)+ 2 AgNO₃(aq)→ 2 Ag(s)+ Mg(NO₃)₂(aq) Write a voltaic diagram for the reaction.

What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below? Al(s)∣ Al³⁺(aq)∣∣ Fe²⁺(aq)∣ Fe(s)