Question 1

A common car battery consists of six identical cells each of which carries out the reaction: Pb + PbO2 + 2HSO4- + 2H+  →	o→  2PbSO4 + 2H2O
Suppose that in starting a car on a cold morning a current of 125 amperes is drawn for 18.4 seconds from a cell of the type described above.How many grams of Pb would be consumed? (The atomic weight of Pb is 207.19. )

Accepted Answer

A)  4.94 g
B)  2.47 g
C)   2 + 2HSO4- + 2H+  	o  2PbSO4 + 2H2O Suppose that in starting a car on a cold morning a current of 125 amperes is drawn for 18.4 seconds from a cell of the type described above.How many grams of Pb would be consumed? (The atomic weight of Pb is 207.19. )  
A)  4.94 g 
B)  2.47 g 
C)      g 
D)      g 
E)      g " class="answers-bank-image d-inline" rel="preload" >  g
D)   2 + 2HSO4- + 2H+  	o  2PbSO4 + 2H2O Suppose that in starting a car on a cold morning a current of 125 amperes is drawn for 18.4 seconds from a cell of the type described above.How many grams of Pb would be consumed? (The atomic weight of Pb is 207.19. )  
A)  4.94 g 
B)  2.47 g 
C)      g 
D)      g 
E)      g " class="answers-bank-image d-inline" rel="preload" >  g
E)   2 + 2HSO4- + 2H+  	o  2PbSO4 + 2H2O Suppose that in starting a car on a cold morning a current of 125 amperes is drawn for 18.4 seconds from a cell of the type described above.How many grams of Pb would be consumed? (The atomic weight of Pb is 207.19. )  
A)  4.94 g 
B)  2.47 g 
C)      g 
D)      g 
E)      g " class="answers-bank-image d-inline" rel="preload" >  g

Question 2

Balance the following equation: Zn + As2O3 $\to$ AsH3 + Zn2+ (acid)

Accepted Answer

12H⁺ + 6Zn + As₂O<...

Question 3

Copper is electroplated from CuSO4 solution.A constant current of 3.19 amp is applied by an external power supply.How long will it take to deposit 1.00  ×	imes×  102 g of Cu? The atomic mass of copper is 63.546.

Accepted Answer

A)  26.4 h
B)  13.2 min
C)  2.03 days
D)  9.57 s
E)  3.78 h

Question 4

How many seconds would it take to deposit 18.2 g of Ag (atomic mass = 107.87) from a solution of AgNO3 using a current of 10.00 amp?

Accepted Answer

A)   3 using a current of 10.00 amp? 
A)     s 
B)     s 
C)     s 
D)     s 
E)     s" class="answers-bank-image d-inline" rel="preload" > s
B)   3 using a current of 10.00 amp? 
A)     s 
B)     s 
C)     s 
D)     s 
E)     s" class="answers-bank-image d-inline" rel="preload" > s
C)   3 using a current of 10.00 amp? 
A)     s 
B)     s 
C)     s 
D)     s 
E)     s" class="answers-bank-image d-inline" rel="preload" > s
D)   3 using a current of 10.00 amp? 
A)     s 
B)     s 
C)     s 
D)     s 
E)     s" class="answers-bank-image d-inline" rel="preload" > s
E)   3 using a current of 10.00 amp? 
A)     s 
B)     s 
C)     s 
D)     s 
E)     s" class="answers-bank-image d-inline" rel="preload" > s

Question 5

The following question refers to the following system: 3Ag(s) + NO3-(aq) + 4H+(aq)  →	o→ 3Ag+(aq) + NO(g) + 2H2O(l) 
Anode reaction:
Ag  →	o→  Ag+(aq) + e-
 ε\varepsilonε  ∘\circ∘  = -0.7990 V
Cathode reaction:
NO3-(aq) + 4H+(aq) + 3e-  →	o→  NO(g) + 2H2O(l) 
 ε\varepsilonε  ∘\circ∘  = 0.9644 V
Determine the standard cell potential.

Accepted Answer

A)  -1.7634 V
B)  0.1654 V
C)  2.0942 V
D)  3.5268 V
E)  0.5878 V

Question 6

If an electrolysis plant operates its electrolytic cells at a total current of 1.8  ×	imes× 106 amp,how long will it take to produce one metric ton (one million grams) of Mg(s) from seawater containing Mg2+? (1 faraday = 96,485 coulombs)

Accepted Answer

A)  1.2 h
B)  1.2 days
C)  37 min
D)  0.61 h
E)  0.31 year

Question 7

An unknown metal (M) is electrolyzed.It took 74.1 s for a current of 2.00 amp to plate 0.107 g of the metal from a solution containing M(NO3) 3.Identify the metal.

Accepted Answer

A)  La
B)  Bi
C)  Ga
D)  Cu
E)  Rh

Question 8

A concentration cell is constructed with copper electrodes and Cu2+ in each compartment.In one compartment,the [Cu2+] = 1.0  ×	imes×  10-3 M and in the other compartment,the [Cu2+] = 2.0 M.Calculate the potential for this cell at 25°C.The standard reduction potential for Cu2+ is +0.34 V.

Accepted Answer

A)  0.44 V
B)  -0.44 V
C)  0.098 V
D)  -0.098 V
E)  0.78 V

Question 9

Which energy conversion shown below takes place in a galvanic cell?

Accepted Answer

A)  electrical to chemical
B)  chemical to electrical
C)  mechanical to chemical
D)  chemical to mechanical
E)  mechanical to electrical

Question 10

What is the oxidation state of Hg in Hg2Cl2?

Accepted Answer

A)  +2
B)  -1
C)  -2
D)  +1
E)  0

Question 11

Which of the following species cannot function as an oxidizing agent?

Accepted Answer

A)  S(s) 
B)  NO3-(aq) 
C)  Cr2O72-(aq) 
D)  I-(aq) 
E)  MnO4-(aq)

Question 12

A concentration cell is constructed using two Ni electrodes with Ni2+ concentrations of 1.0 M and 1.00  ×	imes× 10-4 M in the two half-cells.The reduction potential of Ni2+ is -0.23 V.Calculate the potential of the cell at 25°C.

Accepted Answer

A)  -0.368 V
B)  +0.132 V
C)  -0.132 V
D)  +0.118 V
E)  +0.0592 V

Question 13

Which of the following used to be more precious than gold or silver,due to difficulties refining it?

Accepted Answer

A)  copper
B)  aluminum
C)  tin
D)  zinc
E)  iron

Question 14

The following question refers to a galvanic cell that utilizes the following reaction (unbalanced) : (AuCl4) -(aq) + Cu(s)  →	o→  Au(s) + Cl-(aq) + Cu2+(aq) 
Given the following information,determine the standard cell potential:
Species
Standard Reduction Potential (V) 
Au3+(aq) 
1.4980
Cu2+(aq)  4) -(aq) + Cu(s)  	o  Au(s) + Cl-(aq) + Cu2+(aq)  Given the following information,determine the standard cell potential: Species Standard Reduction Potential (V)  Au3+(aq)  1.4980 Cu2+(aq)    A) 1.1590 V B) 1.8370 V C) 3.8160 V D) 0.8200 V E) 4.1550 V " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  1.1590 V
B)  1.8370 V
C)  3.8160 V
D)  0.8200 V
E)  4.1550 V

Question 15

Consider the galvanic cell shown below (the contents of each half-cell are written beneath each compartment) : 2 0.20 M Cr3+ 0.10 M Br- The standard reduction potentials are as follows: Cr3+(aq) + 3e-  	o  Cr(s)   \varepsilon  \circ  =-0.73 V Br2(aq) + 2e-  	o  2Br-(aq)   \varepsilon  \circ  = +1.09 V Which of the following statements about this cell is false? A) This is a galvanic cell. B) Electrons flow from the Pt electrode to the Cr electrode. C) Reduction occurs at the Pt electrode. D) The cell is not at standard conditions. E) To complete the circuit,cations migrate into the left half-cell and anions migrate into the right half-cell from the salt bridge. " class="answers-bank-image d-inline" rel="preload" > 0.50 M Br2 0.20 M Cr3+ 0.10 M Br-
The standard reduction potentials are as follows:
Cr3+(aq) + 3e-  →	o→  Cr(s)   ε\varepsilonε  ∘\circ∘  =-0.73 V
Br2(aq) + 2e-  →	o→  2Br-(aq)   ε\varepsilonε  ∘\circ∘  = +1.09 V
Which of the following statements about this cell is false?

Accepted Answer

A)  This is a galvanic cell.
B)  Electrons flow from the Pt electrode to the Cr electrode.
C)  Reduction occurs at the Pt electrode.
D)  The cell is not at standard conditions.
E)  To complete the circuit,cations migrate into the left half-cell and anions migrate into the right half-cell from the salt bridge.

Question 16

Which of the following statements is true about a voltaic cell for which  ε\varepsilonε °cell = 1.00 V?

Accepted Answer

A)  It has  Δ\DeltaΔ G° > 0.
B)  The system is at equilibrium.
C)  It has K = 1.
D)  The cathode is at a higher energy than the anode.
E)  The reaction is spontaneous.

Question 17

Which of the following statements about batteries is false?

Accepted Answer

A)  A battery is a group of galvanic cells connected in series.
B)  Lead storage batteries contain lead at the anode and lead coated with lead dioxide at the cathode.
C)  The alkaline dry cell battery can last longer than a nickel-cadmium battery.
D)  A fuel cell is a galvanic cell for which the reactants are continuously supplied.
E)  Dry cell batteries are used in tape players and portable radios.

Question 18

If a constant current of 5.0 amperes is passed through a cell containing Cr3+ for 1.0 hour,how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996. )

Accepted Answer

A)  9.7 g
B)   3+ for 1.0 hour,how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996. )  
A)  9.7 g 
B)      g 
C)  3.2 g 
D)  29 g 
E)      g" class="answers-bank-image d-inline" rel="preload" >  g
C)  3.2 g
D)  29 g
E)   3+ for 1.0 hour,how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996. )  
A)  9.7 g 
B)      g 
C)  3.2 g 
D)  29 g 
E)      g" class="answers-bank-image d-inline" rel="preload" >  g

Question 19

When the following reaction is balanced in acidic solution,what is the coefficient of I2? IO3- + I-  →	o→  I2

Accepted Answer

A)  1
B)  2
C)  3
D)  4
E)  none of these

Question 20

A cell is set up with copper and lead electrodes in contact with CuSO4(aq) and Pb(NO3) 2(aq) ,respectively,at 25°C.The standard reduction potentials are: Pb2+ + 2e-  →	o→  Pb  ε\varepsilonε  ∘\circ∘  = -0.13 V
Cu2+ + 2e-  →	o→  Cu  ε\varepsilonε  ∘\circ∘  = +0.34 V
If the Pb2+ and Cu2+ are each 1.0 M,the potential of the cell,in volts,is:

Accepted Answer

A)  0.47 V
B)  0.92 V
C)  0.22 V
D)  0.58 V
E)  none of these

Exam 18: Electrochemistry

Which of the following used to be more precious than gold or silver,due to difficulties refining it?

Correct Answer
verified

Copper is electroplated from CuSO₄ solution.A constant current of 3.19 amp is applied by an external power supply.How long will it take to deposit 1.00 $\times$ 10² g of Cu? The atomic mass of copper is 63.546.

Correct Answer
verified

Which of the following statements about batteries is false?

Correct Answer
verified

Which energy conversion shown below takes place in a galvanic cell?

Correct Answer
verified

When the following reaction is balanced in acidic solution,what is the coefficient of I₂? IO₃^- + I^- $\to$ I₂

Correct Answer
verified

If an electrolysis plant operates its electrolytic cells at a total current of 1.8 $\times$ 10⁶amp,how long will it take to produce one metric ton (one million grams) of Mg(s) from seawater containing Mg²⁺? (1 faraday = 96,485 coulombs)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Which of the following species cannot function as an oxidizing agent?

Correct Answer
verified

What is the oxidation state of Hg in Hg₂Cl₂?

Correct Answer
verified

Correct Answer
verified

If a constant current of 5.0 amperes is passed through a cell containing Cr³⁺ for 1.0 hour,how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996. )

Correct Answer
verified

Correct Answer
verified

Balance the following equation: Zn + As₂O₃ $\to$ AsH₃ + Zn²⁺ (acid)

Correct Answer
verified
12H⁺ + 6Zn + As₂O<...
View Answer

Correct Answer
verified

Correct Answer
verified

An unknown metal (M) is electrolyzed.It took 74.1 s for a current of 2.00 amp to plate 0.107 g of the metal from a solution containing M(NO₃) ₃.Identify the metal.

Correct Answer
verified

Which of the following statements is true about a voltaic cell for which $\varepsilon$ °_cell = 1.00 V?

Correct Answer
verified

A concentration cell is constructed using two Ni electrodes with Ni²⁺ concentrations of 1.0 M and 1.00 $\times$ 10^-⁴ M in the two half-cells.The reduction potential of Ni²⁺ is -0.23 V.Calculate the potential of the cell at 25°C.

Correct Answer
verified

How many seconds would it take to deposit 18.2 g of Ag (atomic mass = 107.87) from a solution of AgNO₃ using a current of 10.00 amp?

Correct Answer
verified

Exam 18: Electrochemistry

Which of the following used to be more precious than gold or silver,due to difficulties refining it?

Correct AnswerverifiedShow Answer

Copper is electroplated from CuSO4 solution.A constant current of 3.19 amp is applied by an external power supply.How long will it take to deposit 1.00 ×\times× 102 g of Cu? The atomic mass of copper is 63.546.

Correct AnswerverifiedShow Answer

Which of the following statements about batteries is false?

Correct AnswerverifiedShow Answer

Which energy conversion shown below takes place in a galvanic cell?

Correct AnswerverifiedShow Answer

When the following reaction is balanced in acidic solution,what is the coefficient of I2? IO3- + I- →\to→ I2

Correct AnswerverifiedShow Answer

If an electrolysis plant operates its electrolytic cells at a total current of 1.8 ×\times× 106 amp,how long will it take to produce one metric ton (one million grams) of Mg(s) from seawater containing Mg2+? (1 faraday = 96,485 coulombs)

Correct AnswerverifiedShow Answer

A concentration cell is constructed with copper electrodes and Cu2+ in each compartment.In one compartment,the [Cu2+] = 1.0 ×\times× 10-3 M and in the other compartment,the [Cu2+] = 2.0 M.Calculate the potential for this cell at 25°C.The standard reduction potential for Cu2+ is +0.34 V.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which of the following species cannot function as an oxidizing agent?

Correct AnswerverifiedShow Answer

What is the oxidation state of Hg in Hg2Cl2?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

If a constant current of 5.0 amperes is passed through a cell containing Cr3+ for 1.0 hour,how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996. )

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Balance the following equation: Zn + As2O3 →\to→ AsH3 + Zn2+ (acid)

Correct Answerverified12H+ + 6Zn + As2O<...View AnswerShow Answer

Correct AnswerverifiedShow Answer

The following question refers to a galvanic cell that utilizes the following reaction (unbalanced) : (AuCl4) -(aq) + Cu(s) →\to→ Au(s) + Cl-(aq) + Cu2+(aq) Given the following information,determine the standard cell potential: Species Standard Reduction Potential (V) Au3+(aq) 1.4980 Cu2+(aq)

Correct AnswerverifiedShow Answer

An unknown metal (M) is electrolyzed.It took 74.1 s for a current of 2.00 amp to plate 0.107 g of the metal from a solution containing M(NO3) 3.Identify the metal.

Correct AnswerverifiedShow Answer

Which of the following statements is true about a voltaic cell for which ε\varepsilonε °cell = 1.00 V?

Correct AnswerverifiedShow Answer

A concentration cell is constructed using two Ni electrodes with Ni2+ concentrations of 1.0 M and 1.00 ×\times× 10-4 M in the two half-cells.The reduction potential of Ni2+ is -0.23 V.Calculate the potential of the cell at 25°C.

Correct AnswerverifiedShow Answer

How many seconds would it take to deposit 18.2 g of Ag (atomic mass = 107.87) from a solution of AgNO3 using a current of 10.00 amp?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Copper is electroplated from CuSO₄ solution.A constant current of 3.19 amp is applied by an external power supply.How long will it take to deposit 1.00 $\times$ 10² g of Cu? The atomic mass of copper is 63.546.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

When the following reaction is balanced in acidic solution,what is the coefficient of I₂? IO₃^- + I^- $\to$ I₂

Correct Answer
verified

If an electrolysis plant operates its electrolytic cells at a total current of 1.8 $\times$ 10⁶amp,how long will it take to produce one metric ton (one million grams) of Mg(s) from seawater containing Mg²⁺? (1 faraday = 96,485 coulombs)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the oxidation state of Hg in Hg₂Cl₂?

Correct Answer
verified

Correct Answer
verified

If a constant current of 5.0 amperes is passed through a cell containing Cr³⁺ for 1.0 hour,how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996. )

Correct Answer
verified

Correct Answer
verified

Balance the following equation: Zn + As₂O₃ $\to$ AsH₃ + Zn²⁺ (acid)

Correct Answer
verified
12H⁺ + 6Zn + As₂O<...
View Answer

Correct Answer
verified

Correct Answer
verified

An unknown metal (M) is electrolyzed.It took 74.1 s for a current of 2.00 amp to plate 0.107 g of the metal from a solution containing M(NO₃) ₃.Identify the metal.

Correct Answer
verified

Which of the following statements is true about a voltaic cell for which $\varepsilon$ °_cell = 1.00 V?

Correct Answer
verified

A concentration cell is constructed using two Ni electrodes with Ni²⁺ concentrations of 1.0 M and 1.00 $\times$ 10^-⁴ M in the two half-cells.The reduction potential of Ni²⁺ is -0.23 V.Calculate the potential of the cell at 25°C.

Correct Answer
verified

How many seconds would it take to deposit 18.2 g of Ag (atomic mass = 107.87) from a solution of AgNO₃ using a current of 10.00 amp?

Correct Answer
verified