Question 1

Ammonium metavanadate reacts with sulfur dioxide in acidic solution as follows (hydrogen ions and H2O omitted) :
XVO3- + ySO2 → xVO2+ + ySO42-
The ratio x : y is

Accepted Answer

A)   1 : 3
B)   1 : 2
C)   2 : 1
D)   3 : 1
E)   1 : 1

Question 2

An excess of finely divided iron is stirred up with a solution that contains Cu2+ ion, and the system is allowed to come to equilibrium. The solid materials are then filtered off, and electrodes of solid copper and solid iron are inserted into the remaining solution. What potential develops between these two electrodes at 25°C?

Accepted Answer

A)   0
B)   0.592 V
C)   0.296 V
D)   -0.78 V
E)   Not enough information is given.

Question 3

The reaction below occurs in basic solution. In the balanced equation, what is the sum of the coefficients?
Zn + NO3- → Zn(OH) 42- + NH3

Accepted Answer

A)   27
B)   19
C)   23
D)   12
E)   15

Question 4

Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment) .  The standard reduction potentials are as follows: 
-What is the cell potential at 25°C as read on the digital voltmeter?

Accepted Answer

A)   0.18 V
B)   2.58 V
C)   0.59 V
D)   0.10 V
E)   0.26 V

Question 5

Gold is produced electrochemically from an aqueous solution of Au(CN) 2- containing an excess of CN-. Gold metal and oxygen gas are produced at the electrodes. How many moles of O2 will be produced during the production of 1.00 mol of gold?

Accepted Answer

A)   4.00 mol
B)   3.56 mol
C)   0.50 mol
D)   1.00 mol
E)   0.25 mol

Question 6

Why is aluminum protected from corrosion? (Note: The standard reduction potential for Al3+ is -1.66 V.)

Accepted Answer

A)   Oxygen and aluminum have no affinity for one another.
B)   The oxidation of aluminum is not a favored process, as seen by the standard reduction potential for Al3+.
C)   Aluminum forms a protective oxide coating.
D)   At least two of these are correct.
E)   Aluminum is not protected from corrosion.

Question 7

Consider an electrochemical cell with a copper electrode immersed in 1.0 M Cu2+ and a silver electrode immersed in 1.0 M Ag+. 2+ and a silver electrode immersed in 1.0 M Ag+.   -Which of the electrodes is the anode?  A)  the silver electrode B)  the copper electrode " class="answers-bank-image d-inline" rel="preload" >
-Which of the electrodes is the anode?

Accepted Answer

A)   the silver electrode
B)   the copper electrode

Question 8

In a common car battery, six identical cells each carry out the following reaction:
Pb + PbO2 + 2HSO4- + 2H+ → 2PbSO4 + 2H2O
​
Suppose that to start a car on a cold morning, 138 amperes is drawn for 12.0 seconds from such a cell. How many grams of Pb are consumed? (The atomic mass of Pb is 207.19 g/mol.)

Accepted Answer

A)   0.562 g
B)   7.11 g
C)   1.78 g
D)   0.01235 g
E)   3.56 g

Question 9

A solution of MnO42- is electrolytically reduced to Mn3+. A current of 8.46 amp is passed through the solution for 15.0 minutes. What is the number of moles of Mn3+ produced in this process? (1 faraday = 96,485 coulombs)

Accepted Answer

A)   0.000438 mol
B)   0.0197 mol
C)   0.0789 mol
D)   0.0395 mol
E)   0.0263 mol

Question 10

Nickel is electroplated from a NiSO4 solution. A constant current of 5.72 amp is applied by an external power supply. How long will it take to deposit 2.08 × 102 g of Ni? (The atomic mass of Ni is 58.69 g/mol.)

Accepted Answer

A)   16.6 h
B)   33.2 h
C)   1.51 h
D)   19.9 min
E)   49.8 h

Question 11

What quantity of charge is required to reduce 32.6 g of CrCl3 to chromium metal? (1 faraday = 96,485 coulombs)

Accepted Answer

A)   3.97 × 104 C
B)   7.95 × 104 C
C)   5.96 × 104 C
D)   1.81 × 105 C
E)   1.99 × 104 C

Question 12

Consider the galvanic cell shown below (the contents of each half-cell are written beneath each compartment) .  The standard reduction potentials are as follows: 
What is the value of E for this cell at 25°C?

Accepted Answer

A)   1.88 V
B)   2.12 V
C)   1.76 V
D)   2.21 V
E)   0.59 V

Question 13

A strip of copper is placed in a 1 M solution of copper nitrate, and a strip of silver is placed in a 1 M solution of silver nitrate. The two metal strips are connected to a voltmeter by wires, and a salt bridge connects the solutions. The following standard reduction potentials apply:  When the voltmeter is removed and the two electrodes are connected by a wire, which of the following does not take place?

Accepted Answer

A)   Negative ions pass through the salt bridge from the silver half-cell to the copper half-cell.
B)   The silver electrode increases in mass as the cell operates.
C)   Electrons flow in the external circuit from the copper electrode to the silver electrode.
D)   Some positive copper ions pass through the salt bridge from the copper half-cell to the silver half-cell.
E)   There is a net general movement of silver ions through the salt bridge to the copper half-cell.

Question 14

The reaction Cr(s)  + NO3-(aq)  → Cr3+(aq)  + NO(g)  takes place in acidic solution.
-What is the coefficient of H2O(l)  in the balanced equation?

Accepted Answer

A)   3
B)   5
C)   4
D)   2
E)   1

Question 15

​Which of the following statements is/are true of metal plating?
1)  Metals that readily co​rrode can be protected by the application of a thin coating of a metal that resists corrosion.
2)  An object can be plated with metal by making it the cathode in a tank containing ions of the plating metal.
3)  An object can be plated with metal by making it the anode in a tank containing ions of the plating metal.

Accepted Answer

A)   2 only
B)   3 only
C)   1 only
D)   1 and 2
E)   1 and 3

Question 16

If a constant current of 5.2 amperes is passed through a cell containing Cr3+ for 2.1 hour, how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996 g/mol.)

Accepted Answer

A)   0.12 g
B)   1.1 g
C)   64 g
D)   21 g
E)   7.1 g

Question 17

​Which of the following statements is/are true of the electrolysis of brine?
1)  Chlorine is produced at the anode of the cell during the electrolysis of brine.
2)  Under normal circumstances, sodium is produced at the cathode of the cell during the electrolysis of brine.
3)  Hydrogen is produced at the cathode of the cell during the electrolysis of brine.

Accepted Answer

A)   ​1 only
B)   ​2 only
C)   ​3 only
D)   ​1 and 2
E)   ​1 and 3

Question 18

Use the following data to calculate the Ksp value at 25°C for PbSO4(s) . sp value at 25°C for PbSO4(s) .   A)  3.89 × 10-105 B)  2.57 × 10105 C)  1.7 × 10-8 D)  5.9 × 107 E)  None of these is within 5% of the correct answer. " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   3.89 × 10-105
B)   2.57 × 10105
C)   1.7 × 10-8
D)   5.9 × 107
E)   None of these is within 5% of the correct answer.

Question 19

Consider an electrochemical cell with a copper electrode immersed in 1.0 M Cu2+ and a silver electrode immersed in 1.0 M Ag+. 2+ and a silver electrode immersed in 1.0 M Ag+.   ​ If [Cu2+]0 is 0.0038 M and [Ag+]0 is 0.27 M, calculate E. A)  0.41 V B)  0.50 V C)  0.42 V D)  0.51 V E)  0.59 V" class="answers-bank-image d-inline" rel="preload" > ​
If [Cu2+]0 is 0.0038 M and [Ag+]0 is 0.27 M, calculate E.

Accepted Answer

A)   0.41 V
B)   0.50 V
C)   0.42 V
D)   0.51 V
E)   0.59 V

Question 20

In the following equation
ΔG = ΔG° + RT  nK

Accepted Answer

A)   K = 1
B)   ΔG° = 0
C)   ΔG = ΔG°
D)   ΔG = 0
E)   All of the above

Exam 11: Electrochemistry

Why is aluminum protected from corrosion? (Note: The standard reduction potential for Al³⁺ is -1.66 V.)

Correct Answer
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Correct Answer
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Gold is produced electrochemically from an aqueous solution of Au(CN) ₂^- containing an excess of CN^-. Gold metal and oxygen gas are produced at the electrodes. How many moles of O₂ will be produced during the production of 1.00 mol of gold?

Correct Answer
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Nickel is electroplated from a NiSO₄ solution. A constant current of 5.72 amp is applied by an external power supply. How long will it take to deposit 2.08 × 10² g of Ni? (The atomic mass of Ni is 58.69 g/mol.)

Correct Answer
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Correct Answer
verified

Correct Answer
verified

In the following equation ΔG = ΔG° + RT nK

Correct Answer
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Consider an electrochemical cell with a copper electrode immersed in 1.0 M Cu²⁺ and a silver electrode immersed in 1.0 M Ag⁺. -Which of the electrodes is the anode?

Correct Answer
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Ammonium metavanadate reacts with sulfur dioxide in acidic solution as follows (hydrogen ions and H₂O omitted) : XVO₃^- + ySO₂ → xVO²⁺ + ySO₄^2- The ratio x : y is

Correct Answer
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Use the following data to calculate the K_sp value at 25°C for PbSO₄(s) .

Correct Answer
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Correct Answer
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The reaction Cr(s) + NO₃^-(aq) → Cr³⁺(aq) + NO(g) takes place in acidic solution. -What is the coefficient of H₂O(l) in the balanced equation?

Correct Answer
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Consider the galvanic cell shown below (the contents of each half-cell are written beneath each compartment) . The standard reduction potentials are as follows: What is the value of E for this cell at 25°C?

Correct Answer
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If a constant current of 5.2 amperes is passed through a cell containing Cr³⁺ for 2.1 hour, how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996 g/mol.)

Correct Answer
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What quantity of charge is required to reduce 32.6 g of CrCl₃ to chromium metal? (1 faraday = 96,485 coulombs)

Correct Answer
verified

Correct Answer
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A solution of MnO₄^2- is electrolytically reduced to Mn³⁺. A current of 8.46 amp is passed through the solution for 15.0 minutes. What is the number of moles of Mn³⁺ produced in this process? (1 faraday = 96,485 coulombs)

Correct Answer
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Consider an electrochemical cell with a copper electrode immersed in 1.0 M Cu²⁺ and a silver electrode immersed in 1.0 M Ag⁺. If [Cu²⁺]₀ is 0.0038 M and [Ag⁺]₀ is 0.27 M, calculate E.

Correct Answer
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Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment) . The standard reduction potentials are as follows: -What is the cell potential at 25°C as read on the digital voltmeter?

Correct Answer
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The reaction below occurs in basic solution. In the balanced equation, what is the sum of the coefficients? Zn + NO₃^- → Zn(OH) ₄^2- + NH₃

Correct Answer
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Exam 11: Electrochemistry

Why is aluminum protected from corrosion? (Note: The standard reduction potential for Al3+ is -1.66 V.)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Gold is produced electrochemically from an aqueous solution of Au(CN) 2- containing an excess of CN-. Gold metal and oxygen gas are produced at the electrodes. How many moles of O2 will be produced during the production of 1.00 mol of gold?

Correct AnswerverifiedShow Answer

Nickel is electroplated from a NiSO4 solution. A constant current of 5.72 amp is applied by an external power supply. How long will it take to deposit 2.08 × 102 g of Ni? (The atomic mass of Ni is 58.69 g/mol.)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

In the following equation ΔG = ΔG° + RT nK

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Consider an electrochemical cell with a copper electrode immersed in 1.0 M Cu2+ and a silver electrode immersed in 1.0 M Ag+. -Which of the electrodes is the anode?

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Ammonium metavanadate reacts with sulfur dioxide in acidic solution as follows (hydrogen ions and H2O omitted) : XVO3- + ySO2 → xVO2+ + ySO42- The ratio x : y is

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Use the following data to calculate the Ksp value at 25°C for PbSO4(s) .

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The reaction Cr(s) + NO3-(aq) → Cr3+(aq) + NO(g) takes place in acidic solution. -What is the coefficient of H2O(l) in the balanced equation?

Correct AnswerverifiedShow Answer

Consider the galvanic cell shown below (the contents of each half-cell are written beneath each compartment) . The standard reduction potentials are as follows: What is the value of E for this cell at 25°C?

Correct AnswerverifiedShow Answer

If a constant current of 5.2 amperes is passed through a cell containing Cr3+ for 2.1 hour, how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996 g/mol.)

Correct AnswerverifiedShow Answer

What quantity of charge is required to reduce 32.6 g of CrCl3 to chromium metal? (1 faraday = 96,485 coulombs)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A solution of MnO42- is electrolytically reduced to Mn3+. A current of 8.46 amp is passed through the solution for 15.0 minutes. What is the number of moles of Mn3+ produced in this process? (1 faraday = 96,485 coulombs)

Correct AnswerverifiedShow Answer

Consider an electrochemical cell with a copper electrode immersed in 1.0 M Cu2+ and a silver electrode immersed in 1.0 M Ag+. ​ If [Cu2+]0 is 0.0038 M and [Ag+]0 is 0.27 M, calculate E.

Correct AnswerverifiedShow Answer

Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment) . The standard reduction potentials are as follows: -What is the cell potential at 25°C as read on the digital voltmeter?

Correct AnswerverifiedShow Answer

The reaction below occurs in basic solution. In the balanced equation, what is the sum of the coefficients? Zn + NO3- → Zn(OH) 42- + NH3

Correct AnswerverifiedShow Answer

Why is aluminum protected from corrosion? (Note: The standard reduction potential for Al³⁺ is -1.66 V.)

Correct Answer
verified

Correct Answer
verified

Gold is produced electrochemically from an aqueous solution of Au(CN) ₂^- containing an excess of CN^-. Gold metal and oxygen gas are produced at the electrodes. How many moles of O₂ will be produced during the production of 1.00 mol of gold?

Correct Answer
verified

Nickel is electroplated from a NiSO₄ solution. A constant current of 5.72 amp is applied by an external power supply. How long will it take to deposit 2.08 × 10² g of Ni? (The atomic mass of Ni is 58.69 g/mol.)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Consider an electrochemical cell with a copper electrode immersed in 1.0 M Cu²⁺ and a silver electrode immersed in 1.0 M Ag⁺. -Which of the electrodes is the anode?

Correct Answer
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Ammonium metavanadate reacts with sulfur dioxide in acidic solution as follows (hydrogen ions and H₂O omitted) : XVO₃^- + ySO₂ → xVO²⁺ + ySO₄^2- The ratio x : y is

Correct Answer
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Use the following data to calculate the K_sp value at 25°C for PbSO₄(s) .

Correct Answer
verified

Correct Answer
verified

The reaction Cr(s) + NO₃^-(aq) → Cr³⁺(aq) + NO(g) takes place in acidic solution. -What is the coefficient of H₂O(l) in the balanced equation?

Correct Answer
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Correct Answer
verified

If a constant current of 5.2 amperes is passed through a cell containing Cr³⁺ for 2.1 hour, how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996 g/mol.)

Correct Answer
verified

What quantity of charge is required to reduce 32.6 g of CrCl₃ to chromium metal? (1 faraday = 96,485 coulombs)

Correct Answer
verified

Correct Answer
verified

A solution of MnO₄^2- is electrolytically reduced to Mn³⁺. A current of 8.46 amp is passed through the solution for 15.0 minutes. What is the number of moles of Mn³⁺ produced in this process? (1 faraday = 96,485 coulombs)

Correct Answer
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Consider an electrochemical cell with a copper electrode immersed in 1.0 M Cu²⁺ and a silver electrode immersed in 1.0 M Ag⁺. If [Cu²⁺]₀ is 0.0038 M and [Ag⁺]₀ is 0.27 M, calculate E.

Correct Answer
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Correct Answer
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The reaction below occurs in basic solution. In the balanced equation, what is the sum of the coefficients? Zn + NO₃^- → Zn(OH) ₄^2- + NH₃

Correct Answer
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