Question 1

A voltaic cell prepared using aluminum and nickel has the following cell notation. 2+(aq)  + Al(s)   \rightarrow  Al3+(aq)  + Ni(s)  B)  3Ni2+(aq)  + 2Al(s)   \rightarrow  2Al3+(aq)  + 3Ni(s)  C)  Ni(s)  + Al3+(aq)   \rightarrow Ni2+(aq)  + Al(s)  D)  3Ni(s)  + 2Al3+(aq)   \rightarrow  3Ni2+(aq)  + 2Al(s)  E)  None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" > Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

Accepted Answer

A)   Ni2+(aq)  + Al(s)   →\rightarrow→  Al3+(aq)  + Ni(s) 
B)   3Ni2+(aq)  + 2Al(s)   →\rightarrow→  2Al3+(aq)  + 3Ni(s) 
C)   Ni(s)  + Al3+(aq)   →\rightarrow→ Ni2+(aq)  + Al(s) 
D)   3Ni(s)  + 2Al3+(aq)   →\rightarrow→  3Ni2+(aq)  + 2Al(s) 
E)   None of these choices is correct. F) C) and D)
G) A) and D)

Question 2

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. 2+(aq)  B)  Fe(s)  C)  Fe2+(aq)  D)  Sr2+(aq)  E)  Co2+(aq) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Cr2+(aq) 
B)   Fe(s) 
C)   Fe2+(aq) 
D)   Sr2+(aq) 
E)   Co2+(aq) F) A) 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 _____.

Accepted Answer

A)   1
B)   2
C)   4
D)   10
E)   None of these choices is correct.F) A) and D)
G) C) and D)

Question 4

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction)  potential for the anode is -0.22 V, what is the standard electrode potential for the cathode?

Accepted Answer

A)   0.96 V
B)   0.52 V
C)   -0.52 V
D)   -0.96 V
E)   Need to know the cell reaction in order to calculate the answer.F) A) and B)
G) D) and E)

Question 5

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

Accepted Answer

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

Question 6

A voltaic cell prepared using aluminum and nickel has the following cell notation. 3+(aq)  + 3e¯ B)  Al3+(aq)  + 3e  \rightarrow  Al(s)  C)  Ni(s)   \rightarrow Ni2+(aq)  + 2e¯ D)  Ni2+(aq)  + 2e¯  \rightarrow  Ni(s)  E)  None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" > Which of the following reactions occurs at the anode?

Accepted Answer

A)   Al(s)   →\rightarrow→  Al3+(aq)  + 3e¯
B)   Al3+(aq)  + 3e  →\rightarrow→  Al(s) 
C)   Ni(s)   →\rightarrow→ Ni2+(aq)  + 2e¯
D)   Ni2+(aq)  + 2e¯  →\rightarrow→  Ni(s) 
E)   None of these choices is correct. F) A) and B)
G) A) and E)

Question 7

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn2+(aq)  + 2H2O(l)   →\rightarrow→ MnO2(s)  + 4H+(aq)  + 2e¯
What mass of MnO2 is deposited at this anode?

Accepted Answer

A)   19.5 kg
B)   12.9 kg
C)   4.87 kg
D)   2.43 kg
E)   None of these choices is correct. F) A) and B)
G) C) and D)

Question 8

Consider the following redox equation  When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH¯(aq)  and on which side of the equation is OH¯(aq)  present?

Accepted Answer

A)   4, reactant side
B)   4, product side
C)   6, reactant side
D)   6, product side
E)   None of these choices is correct.F) C) and D)
G) B) and D)

Question 9

Calculate E °\degree° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.   Overall reaction:   A)  E \degree cell = -2.891 V, nonspontaneous B)  E \degree cell = -2.891 V, spontaneous C)  E \degree cell = 2.891 V, nonspontaneous D)  E \degree cell = 2.891 V, spontaneous E)  Spontaneous, but none of the values of E \degree cell is correct. " class="answers-bank-image d-inline" rel="preload" > Overall reaction: cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.   Overall reaction:   A)  E \degree cell = -2.891 V, nonspontaneous B)  E \degree cell = -2.891 V, spontaneous C)  E \degree cell = 2.891 V, nonspontaneous D)  E \degree cell = 2.891 V, spontaneous E)  Spontaneous, but none of the values of E \degree cell is correct. " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   E °\degree° cell = -2.891 V, nonspontaneous
B)   E °\degree° cell = -2.891 V, spontaneous
C)   E °\degree° cell = 2.891 V, nonspontaneous
D)   E °\degree° cell = 2.891 V, spontaneous
E)   Spontaneous, but none of the values of E °\degree° cell is correct. F) A) and B)
G) B) and E)

Question 10

The value of the equilibrium constant for the reaction of nickel(II)  ions with cadmium metal is 1.17 * 105. Calculate  Δ\DeltaΔ G °\degree° or the reaction at 25 °\degree° C.

Accepted Answer

A)   -12.6 kJ
B)   -28.9 kJ
C)   12.6 kJ
D)   28.9 kJ
E)   None of these choices is correct. F) A) and E)
G) C) and E)

Question 11

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

Accepted Answer

A)   zinc
B)   graphite
C)   copper
D)   iron
E)   sodiumF) A) and C)
G) A) and D)

Question 12

A primary battery is one which can be recharged.

Accepted Answer

A) True 
 B)False

Question 13

Calculate Δ\DeltaΔ G °\degree° for the oxidation of 3 moles of copper by nitric acid.

Accepted Answer

A)   -120 kJ
B)   -180 kJ
C)   -240 kJ
D)   -300 kJ
E)   -360 kJ F) A) and B)
G) A) and C)

Question 14

In the absence of oxygen, iron will rust as long as moisture is present.

Accepted Answer

A) True 
 B)False

Question 15

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. 11ec9252_7630_6847_b435_a1c5fb864bb4_...

Question 16

Which one of the following statements about electrochemical cells is correct?

Accepted Answer

A)   In a salt bridge, current is carried by cations moving toward the anode, and anions toward the cathode.
B)   In the external wire, electrons travel from cathode to anode.
C)   The anode of a voltaic cell is labeled minus (-) .
D)   Oxidation occurs at the cathode, in an electrolytic cell.
E)   None of these choices is correct.F) A) and E)
G) B) and E)

Question 17

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. 2+(aq)  + 2e¯ B)  Cu2+(aq)  + 2e¯  \rightarrow  Cu(s)  C)  Ag(s)   \rightarrow  Ag+(aq)  + e¯ D)  Ag+(aq)  + e¯  \rightarrow  Ag(s)  E)  Cu(s)  + 2Ag+(aq)   \rightarrow  Cu2+(aq)  + 2Ag(s)  " class="answers-bank-image d-inline" rel="preload" > Which of the following processes occurs at the cathode?

Accepted Answer

A)   Cu(s)   →\rightarrow→ Cu2+(aq)  + 2e¯
B)   Cu2+(aq)  + 2e¯  →\rightarrow→  Cu(s) 
C)   Ag(s)   →\rightarrow→  Ag+(aq)  + e¯
D)   Ag+(aq)  + e¯  →\rightarrow→  Ag(s) 
E)   Cu(s)  + 2Ag+(aq)   →\rightarrow→  Cu2+(aq)  + 2Ag(s)  F) A) and E)
G) B) and D)

Question 18

In the electrolysis of aqueous potassium nitrate using inert electrodes, which one of the following species is oxidized?

Accepted Answer

A)   potassium ion
B)   nitrate ion
C)   water
D)   oxygen
E)   hydronium ionF) None of the above
G) B) and C)

Question 19

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

Accepted Answer

A)   sodium and sulfur
B)   hydrogen and sulfur
C)   oxygen and sulfur
D)   oxygen and sulfuric acid
E)   hydrogen and oxygenF) All of the above
G) B) and D)

Question 20

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) 3¯ will be _____. 3¯ will be _____.   A)  1 B)  2 C)  3 D)  6 E)  None of these choices is correct." class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   1
B)   2
C)   3
D)   6
E)   None of these choices is correct.F) A) and C)
G) A) and D)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

In the electrolysis of aqueous potassium nitrate using inert electrodes, which one of the following species is oxidized?

Correct Answer
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When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) ₃¯ will be _____.

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

Correct Answer
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Correct Answer
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Examine the following half-reactions and select the strongest oxidizing agent among the species listed.

Correct Answer
verified

Which one of the following statements about electrochemical cells is correct?

Correct Answer
verified

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

Correct Answer
verified

Calculate $\Delta$ G $\degree$ for the oxidation of 3 moles of copper by nitric acid. $Calculate \Delta G \degree for the oxidation of 3 moles of copper by nitric acid. A) -120 kJ B) -180 kJ C) -240 kJ D) -300 kJ E) -360 kJ$

Correct Answer
verified

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

Correct Answer
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A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is -0.22 V, what is the standard electrode potential for the cathode?

Correct Answer
verified

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 * 10⁵. Calculate $\Delta$ G $\degree$ or the reaction at 25 $\degree$ C.

Correct Answer
verified

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be _____.

Correct Answer
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Correct Answer
verified

In the absence of oxygen, iron will rust as long as moisture is present.

Correct Answer
verified

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn²⁺(aq) + 2H₂O(l) $\rightarrow$ MnO₂(s) + 4H⁺(aq) + 2e¯ What mass of MnO₂ is deposited at this anode?

Correct Answer
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Correct Answer
verified
a. 11ec9252_7630_6847_b435_a1c5fb864bb4_...
View Answer

Consider the following redox equation When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH¯(aq) and on which side of the equation is OH¯(aq) present?

Correct Answer
verified

Correct Answer
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Exam 21: Electrochemistry: Chemical Change and Electrical Work

In the electrolysis of aqueous potassium nitrate using inert electrodes, which one of the following species is oxidized?

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) 3¯ will be _____.

Correct AnswerverifiedShow Answer

A voltaic cell prepared using aluminum and nickel has the following cell notation. Which of the following reactions occurs at the anode?

Correct AnswerverifiedShow Answer

A primary battery is one which can be recharged.

Correct AnswerverifiedShow Answer

Calculate E °\degree° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction: 2Cr(s) + 3I2(s) →\rightarrow→ 2Cr3+(aq) + (aq) + 6I¯(aq)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Which one of the following statements about electrochemical cells is correct?

Correct AnswerverifiedShow Answer

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

Correct AnswerverifiedShow Answer

Calculate Δ\DeltaΔ G °\degree° for the oxidation of 3 moles of copper by nitric acid.

Correct AnswerverifiedShow Answer

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

Correct AnswerverifiedShow Answer

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is -0.22 V, what is the standard electrode potential for the cathode?

Correct AnswerverifiedShow Answer

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 * 105. Calculate Δ\DeltaΔ G °\degree° or the reaction at 25 °\degree° C.

Correct AnswerverifiedShow Answer

Calculate E °\degree° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction:

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be _____.

Correct AnswerverifiedShow Answer

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Which of the following processes occurs at the cathode?

Correct AnswerverifiedShow Answer

In the absence of oxygen, iron will rust as long as moisture is present.

Correct AnswerverifiedShow Answer

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn2+(aq) + 2H2O(l) →\rightarrow→ MnO2(s) + 4H+(aq) + 2e¯ What mass of MnO2 is deposited at this anode?

Correct AnswerverifiedShow Answer

Correct Answerverifieda. 11ec9252_7630_6847_b435_a1c5fb864bb4_...View AnswerShow Answer

Consider the following redox equation When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH¯(aq) and on which side of the equation is OH¯(aq) present?

Correct AnswerverifiedShow Answer

A voltaic cell prepared using aluminum and nickel has the following cell notation. Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

Correct AnswerverifiedShow Answer

Correct Answer
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When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) ₃¯ will be _____.

Correct Answer
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Correct Answer
verified

Correct Answer
verified

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Calculate $\Delta$ G $\degree$ for the oxidation of 3 moles of copper by nitric acid. $Calculate \Delta G \degree for the oxidation of 3 moles of copper by nitric acid. A) -120 kJ B) -180 kJ C) -240 kJ D) -300 kJ E) -360 kJ$

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 * 10⁵. Calculate $\Delta$ G $\degree$ or the reaction at 25 $\degree$ C.

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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A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn²⁺(aq) + 2H₂O(l) $\rightarrow$ MnO₂(s) + 4H⁺(aq) + 2e¯ What mass of MnO₂ is deposited at this anode?

Correct Answer
verified

Correct Answer
verified
a. 11ec9252_7630_6847_b435_a1c5fb864bb4_...
View Answer

Correct Answer
verified

Correct Answer
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