Question 1

A concentration cell consists of two Zn/Zn2+ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO3) 2 and in compartment B is 0.60 M Zn(NO3) 2. What is the voltage of the cell at 25°C?

Accepted Answer

A)   0.010 V
B)   0.020 V
C)   0.023 V
D)   0.046 V
E)   none of the aboveF) None of the above
G) B) and D) C

Question 2

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu2+(aq)  + 2e-  Cu(s)  and Ag+(aq)  + e-  Ag(s) 
For every 1.00 g of copper produced in the first process, how many grams of silver will be produced in the second one?

Accepted Answer

A)   0.294 g
B)   0.588 g
C)   0.850 g
D)   1.70 g
E)   3.40 gF) C) and E)
G) B) and E)

Question 3

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be _____.
 I2(s)  + HNO3(aq)   HIO3(aq)  + NO2(g)  + H2O(l)

Accepted Answer

A)   1
B)   2
C)   4
D)   10
E)   none of the aboveF) B) and C)
G) A) and B)

Question 4

A battery that cannot be recharged is a

Accepted Answer

A)   fuel cell.
B)   primary battery.
C)   secondary battery.
D)   simple battery.
E)   flow battery.F) B) and E)
G) A) and E)

Question 5

a. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of molten KCl.
b. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of aqueous KCl.
c. Clearly explain why the products of the two processes are not the same.

Accepted Answer

a. 2KCl(l)  2K(l) + Cl₂(g...

Question 6

A concentration cell is based on the aqueous reaction
Cu2+(1.00 M) F1F1F1S1F1F1F10 Cu2+(0.0100 M)
The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Draw a neat diagram to represent this cell, showing and labeling all necessary components including: anode, cathode, electron flow, cation flow, and anion flow.

Accepted Answer

Question 7

Electrolytic cells utilize electrical energy to drive non-spontaneous redox reactions.

Accepted Answer

A) True 
 B)False

Question 8

The lead-acid battery is an example of a secondary battery.

Accepted Answer

A) True 
 B)False

Question 9

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

Accepted Answer

A)   sodium from Na3PO4(aq) 
B)   sulfur from K2SO4(aq) 
C)   oxygen from H2SO4(aq) 
D)   potassium from KCl(aq) 
E)   nitrogen from AgNO3(aq) F) B) and E)
G) C) and D)

Question 10

A primary battery is one which can be recharged.

Accepted Answer

A) True 
 B)False  False

Question 11

Predict the products of the cell reaction when a molten salt mixture of sodium bromide and calcium fluoride is electrolyzed (spectator ions are not considered to be products) .

Accepted Answer

A)   calcium and bromine
B)   sodium and fluorine
C)   calcium bromide
D)   calcium and fluorine
E)   sodium and bromineF) All of the above
G) None of the above

Question 12

A concentration cell is based on the aqueous reaction
Cu2+(1.00 M) F1F1F1S1F1F1F10 Cu2+(0.0100 M)
The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

Accepted Answer

Cu(s) <font face="symbol">F1F1F...

Question 13

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____. I-(aq)  + NO3-(aq)   NO(g)  + I2(s)  (acidic solution)

Accepted Answer

A)   2
B)   3
C)   6
D)   8
E)   none of the aboveF) C) and D)
G) None of the above

Question 14

Which of the following statements about voltaic and electrolytic cells is correct?

Accepted Answer

A)   The anode will definitely gain weight in a voltaic cell.
B)   Oxidation occurs at the cathode of both cells.
C)   The free energy change, G, is negative for the voltaic cell.
D)   The electrons in the external wire flow from cathode to anode in an electrolytic cell.
E)   None of the above statements is correct.F) C) and D)
G) B) and E)

Question 15

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. 
°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.     reaction: 2Cr(s)  + 3I2(s)   2Cr3+(aq)  + (aq)  + 6I-(aq)  A)  E°cell = -1.27 V, spontaneous B)  E°cell = -1.27 V, nonspontaneous C)  E°cell = 1.27 V, spontaneous D)  E°cell = 1.27 V, nonspontaneous E)  E°cell = 1.54 V, spontaneous" class="answers-bank-image d-inline" rel="preload" >
 reaction: 2Cr(s)  + 3I2(s)   2Cr3+(aq)  + (aq)  + 6I-(aq)

Accepted Answer

A)   E°cell = -1.27 V, spontaneous
B)   E°cell = -1.27 V, nonspontaneous
C)   E°cell = 1.27 V, spontaneous
D)   E°cell = 1.27 V, nonspontaneous
E)   E°cell = 1.54 V, spontaneousF) A) and B)
G) D) and E)

Question 16

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states) ?

Accepted Answer

A)   HCl and Cl-
B)   H+ and OH-
C)   H2O and H+
D)   Fe3+ and Fe2O3
E)   MnO2 and Mn2+F) B) and E)
G) B) and D)

Question 17

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____. Zn(s)  + ReO4-(aq)   Re(s)  + Zn2+(aq)  (acidic solution)

Accepted Answer

A)   2
B)   7
C)   8
D)   16
E)   none of the aboveF) All of the above
G) A) and B)

Question 18

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.61 V 2Cr(s)  + 3Pb2+(aq)  cell = 0.61 V 2Cr(s)  + 3Pb2+(aq)    3Pb(s)  + 2Cr3+(aq)  A)  4.1 × 1020 B)  8.2 × 1030 C)  3.3 × 1051 D)  7.4 × 1061 E)  > 9.9 × 1099" class="answers-bank-image d-inline" rel="preload" > 3Pb(s)  + 2Cr3+(aq)

Accepted Answer

A)   4.1 × 1020
B)   8.2 × 1030
C)   3.3 × 1051
D)   7.4 × 1061
E)   > 9.9 × 1099F) A) and C)
G) A) and B)

Question 19

In a fuel cell, an external source of electrical power is used to drive a non-spontaneous reaction in which a fuel is produced.

Accepted Answer

A) True 
 B)False  False

Question 20

Examine the following half-reactions and select the strongest reducing agent among the species listed. 
4-(aq)  E)  Zn(OH) 2(s) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Hg(l) 
B)   Zn(s) 
C)   Ag(s) 
D)   BH4-(aq) 
E)   Zn(OH) 2(s) F) All of the above
G) B) and E)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A concentration cell consists of two Zn/Zn²⁺ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO₃) ₂and in compartment B is 0.60 M Zn(NO₃) ₂. What is the voltage of the cell at 25°C?

Correct Answer
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C

Correct Answer
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When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be _____. I₂(s) + HNO₃(aq)  HIO₃(aq) + NO₂(g) + H₂O(l)

Correct Answer
verified

A battery that cannot be recharged is a

Correct Answer
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Correct Answer
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a. 2KCl(l)  2K(l) + Cl₂(g...
View Answer

Correct Answer
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Electrolytic cells utilize electrical energy to drive non-spontaneous redox reactions.

Correct Answer
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The lead-acid battery is an example of a secondary battery.

Correct Answer
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Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

Correct Answer
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A primary battery is one which can be recharged.

Correct Answer
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False

Predict the products of the cell reaction when a molten salt mixture of sodium bromide and calcium fluoride is electrolyzed (spectator ions are not considered to be products) .

Correct Answer
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A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M)  Cu²⁺(0.0100 M) The cell consists of copper electrodes dipping into solutions of Cu²⁺ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

Correct Answer
verified
Cu(s) F1F1F...
View Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____. I^-(aq) + NO₃^-(aq)  NO(g) + I₂(s) (acidic solution)

Correct Answer
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Which of the following statements about voltaic and electrolytic cells is correct?

Correct Answer
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Calculate E^°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. reaction: 2Cr(s) + 3I₂(s)  2Cr³⁺(aq) + (aq) + 6I^-(aq)

Correct Answer
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Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states) ?

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____. Zn(s) + ReO₄^-(aq)  Re(s) + Zn²⁺(aq) (acidic solution)

Correct Answer
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What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.61 V 2Cr(s) + 3Pb²⁺(aq) 3Pb(s) + 2Cr³⁺(aq)

Correct Answer
verified

In a fuel cell, an external source of electrical power is used to drive a non-spontaneous reaction in which a fuel is produced.

Correct Answer
verified
False

Examine the following half-reactions and select the strongest reducing agent among the species listed.

Correct Answer
verified

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A concentration cell consists of two Zn/Zn2+ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO3) 2 and in compartment B is 0.60 M Zn(NO3) 2. What is the voltage of the cell at 25°C?

Correct AnswerverifiedC

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be _____. I2(s) + HNO3(aq)  HIO3(aq) + NO2(g) + H2O(l)

Correct AnswerverifiedShow Answer

A battery that cannot be recharged is a

Correct AnswerverifiedShow Answer

Correct Answerverifieda. 2KCl(l)  2K(l) + Cl2(g...View AnswerShow Answer

Correct AnswerverifiedShow Answer

Electrolytic cells utilize electrical energy to drive non-spontaneous redox reactions.

Correct AnswerverifiedShow Answer

The lead-acid battery is an example of a secondary battery.

Correct AnswerverifiedShow Answer

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

Correct AnswerverifiedShow Answer

A primary battery is one which can be recharged.

Correct AnswerverifiedFalse

Predict the products of the cell reaction when a molten salt mixture of sodium bromide and calcium fluoride is electrolyzed (spectator ions are not considered to be products) .

Correct AnswerverifiedShow Answer

A concentration cell is based on the aqueous reaction Cu2+(1.00 M)  Cu2+(0.0100 M) The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

Correct AnswerverifiedCu(s) F1F1F...View AnswerShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____. I-(aq) + NO3-(aq)  NO(g) + I2(s) (acidic solution)

Correct AnswerverifiedShow Answer

Which of the following statements about voltaic and electrolytic cells is correct?

Correct AnswerverifiedShow Answer

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. reaction: 2Cr(s) + 3I2(s)  2Cr3+(aq) + (aq) + 6I-(aq)

Correct AnswerverifiedShow Answer

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states) ?

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____. Zn(s) + ReO4-(aq)  Re(s) + Zn2+(aq) (acidic solution)

Correct AnswerverifiedShow Answer

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.61 V 2Cr(s) + 3Pb2+(aq) 3Pb(s) + 2Cr3+(aq)

Correct AnswerverifiedShow Answer

In a fuel cell, an external source of electrical power is used to drive a non-spontaneous reaction in which a fuel is produced.

Correct AnswerverifiedFalse

Examine the following half-reactions and select the strongest reducing agent among the species listed.

Correct AnswerverifiedShow Answer

A concentration cell consists of two Zn/Zn²⁺ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO₃) ₂and in compartment B is 0.60 M Zn(NO₃) ₂. What is the voltage of the cell at 25°C?

Correct Answer
verified
C

Correct Answer
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When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be _____. I₂(s) + HNO₃(aq)  HIO₃(aq) + NO₂(g) + H₂O(l)

Correct Answer
verified

Correct Answer
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Correct Answer
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a. 2KCl(l)  2K(l) + Cl₂(g...
View Answer

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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False

Correct Answer
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A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M)  Cu²⁺(0.0100 M) The cell consists of copper electrodes dipping into solutions of Cu²⁺ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

Correct Answer
verified
Cu(s) F1F1F...
View Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____. I^-(aq) + NO₃^-(aq)  NO(g) + I₂(s) (acidic solution)

Correct Answer
verified

Correct Answer
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Calculate E^°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. reaction: 2Cr(s) + 3I₂(s)  2Cr³⁺(aq) + (aq) + 6I^-(aq)

Correct Answer
verified

Correct Answer
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When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____. Zn(s) + ReO₄^-(aq)  Re(s) + Zn²⁺(aq) (acidic solution)

Correct Answer
verified

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.61 V 2Cr(s) + 3Pb²⁺(aq) 3Pb(s) + 2Cr³⁺(aq)

Correct Answer
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Correct Answer
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False

Correct Answer
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