Question 1

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Accepted Answer

A)   0.419 g
B)   6.29 g
C)   12.6 g
D)   25.2 g
E)   33.4 gF) C) and E)
G) None of the above

Question 2

A voltaic cell consists of a Hg/Hg22+ electrode (E °\degree°  = 0.85 V)  and a Sn/Sn2+ electrode (E °\degree°  = -0.14 V) . Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25 °\degree° C.

Accepted Answer

A)   0.0001 M
B)   0.0007 M
C)   0.005 M
D)   0.03 M
E)   0.05 M F) D) and E)
G) A) and B)

Question 3

Consider the following balanced redox reaction 
Mn2+(aq)  + S2O82¯(aq)  + 2H2O(l)   →\rightarrow→  MnO2(s)  + 4H+(aq)  + 2SO42¯(aq) 
Which of the following statements is true?

Accepted Answer

A)   Mn2+(aq)  is the oxidizing agent and is reduced.
B)   Mn2+(aq)  is the oxidizing agent and is oxidized.
C)   Mn2+(aq)  is the reducing agent and is oxidized.
D)   Mn2+(aq)  is the reducing agent and is reduced.
E)   Manganese does not change its oxidation number in this reaction. F) C) and D)
G) A) and B)

Question 4

A solution is prepared by dissolving 32.0 g of NiSO4 in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Accepted Answer

A)   1.1 A
B)   2.2 A
C)   3.3 A
D)   4.4 A
E)   5.5 AF) B) and D)
G) C) and D)

Question 5

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu2+(aq)  + 2e¯  →\rightarrow→  Cu(s)  and Ag+(aq)  + e¯  →\rightarrow→  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 g F) None of the above
G) B) and C)

Question 6

What is the value of the equilibrium constant for the cell reaction below at 25 °\degree° C?
 E °\degree° 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 *1099 F) A) and E)
G) C) and D)

Question 7

Consider the reaction of iodine with manganese dioxide: 
3I2(s)  + 2MnO2(s)  + 8OH¯(aq)  2(s)  + 2MnO2(s)  + 8OH¯(aq)    6I¯(aq)  + 2MnO4¯(aq)  + 4H2O(l)  The equilibrium constant for the overall reaction is 8.30* 10¯7. Calculate  \Delta G \degree  for the reaction at 25 \degree C. A)  -15.1 kJ B)  -34.7 kJ C)  15.1 kJ D)  34.7 kJ E)  None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" > 6I¯(aq)  + 2MnO4¯(aq)  + 4H2O(l) 
The equilibrium constant for the overall reaction is 8.30* 10¯7. Calculate  Δ\DeltaΔ G °\degree°  for the reaction at 25 °\degree° C.

Accepted Answer

A)   -15.1 kJ
B)   -34.7 kJ
C)   15.1 kJ
D)   34.7 kJ
E)   None of these choices is correct. F) A) and B)
G) C) and E)

Question 8

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

Accepted Answer

A)   16.2 g
B)   33.4 g
C)   40.6 g
D)   81.3 g
E)   163 gF) A) and E)
G) A) and B)

Question 9

Examine the following half-reactions and select the strongest oxidizing agent among the substances. 4]2¯(aq)  B)  RuO4(s)  C)  HFeO4¯(aq)  D)  H4XeO6(aq)  E)  Cl¯(aq) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   [PtCl4]2¯(aq) 
B)   RuO4(s) 
C)   HFeO4¯(aq) 
D)   H4XeO6(aq) 
E)   Cl¯(aq) F) A) and D)
G) B) and E)

Question 10

Consider the following balanced redox reaction 
3CuO(s)  + 2NH3(aq)   →\rightarrow→  N2(g)  + 3H2O(l)  + 3Cu(s) 
Which of the following statements is true?

Accepted Answer

A)   CuO(s)  is the oxidizing agent and copper is reduced.
B)   CuO(s)  is the oxidizing agent and copper is oxidized.
C)   CuO(s)  is the reducing agent and copper is oxidized.
D)   CuO(s)  is the reducing agent and copper is reduced.
E)   CuO(s)  is the oxidizing agent and N2(g)  is the reducing agent. F) C) and E)
G) A) and B)

Question 11

A concentration cell consists of two Al/Al3+ electrodes. The electrolyte in compartment A is 0.050 M Al(NO3) 3 and in compartment B is 1.25 M Al(NO3) 3. What is the voltage of the cell at 25 °\degree° C?

Accepted Answer

A)   0.083 V
B)   0.062 V
C)   0.041V
D)   0.028 V
E)   None of these choices is correct. F) A) and E)
G) C) and D)

Question 12

Calculate E °\degree° cell for the reaction of nickel(II)  ions with cadmium metal at 25 °\degree° C. K = 1.17 *105. Ni2+(aq)  + Cd(s)   →\rightarrow→  Cd2+(aq)  + Ni(s)

Accepted Answer

A)   0.075 V
B)   0.10 V
C)   0.12 V
D)   0.15 V
E)   0.30 V F) C) and D)
G) C) and E)

Question 13

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics. If E °\degree° cell = 1.587 V and E °\degree° of the cathode half-cell is 0.536 V, what is E °\degree°  of the anode half-cell? cell = 1.587 V and E \degree of the cathode half-cell is 0.536 V, what is E \degree  of the anode half-cell?   A)  -1.051 V B)  -2.123 V C)  1.051 V D)  2.123 V E)  None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -1.051 V
B)   -2.123 V
C)   1.051 V
D)   2.123 V
E)   None of these choices is correct. F) B) and E)
G) B) and D)

Question 14

Examine the following half-reactions and select the weakest reducing agent among the substances. 2+(aq)  D)  Hg(l)  E)  OH¯(aq) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Cr(s) 
B)   Sn(s) 
C)   Mn2+(aq) 
D)   Hg(l) 
E)   OH¯(aq) F) A) and E)
G) D) and E)

Question 15

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) All of the above

Question 16

What is the E °\degree° cell for the cell represented by the combination of the following half-reactions? cell for the cell represented by the combination of the following half-reactions?   A)  -0.18 V B)  0.18 V C)  1.28 V D)  1.66 V E)  2.12 V " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -0.18 V
B)   0.18 V
C)   1.28 V
D)   1.66 V
E)   2.12 V F) A) and C)
G) D) and E)

Question 17

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

Accepted Answer

A)   Pb(s) 
B)   Ca(s) 
C)   Pt(s) 
D)   Br¯(aq) 
E)   Pt2+(aq) F) A) and B)
G) A) and E)

Question 18

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

Question 19

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

Accepted Answer

A)   2
B)   3
C)   6
D)   8
E)   None of these choices is correct.F) C) and D)
G) A) and B)

Question 20

Consider the non-aqueous cell reaction cell = 2.35 V at 200 \degree C.  \Delta G \degree at this temperature is A)  453 kJ. B)  -453 kJ. C)  907 kJ. D)  -907 kJ. E)  None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" > for which E °\degree° cell = 2.35 V at 200 °\degree° C.  Δ\DeltaΔ G °\degree° at this temperature is

Accepted Answer

A)   453 kJ.
B)   -453 kJ.
C)   907 kJ.
D)   -907 kJ.
E)   None of these choices is correct. F) D) and E)
G) A) and E)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

Correct Answer
verified

Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈²¯(aq) + 2H₂O(l) $\rightarrow$ MnO₂(s) + 4H⁺(aq) + 2SO₄²¯(aq) Which of the following statements is true?

Correct Answer
verified

Correct Answer
verified

A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E $\degree$ = 0.85 V) and a Sn/Sn²⁺ electrode (E $\degree$ = -0.14 V) . Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25 $\degree$ C.

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

Correct Answer
verified

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

Correct Answer
verified

A solution is prepared by dissolving 32.0 g of NiSO₄ in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Correct Answer
verified

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) $\rightarrow$ N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Correct Answer
verified

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

Correct Answer
verified

A battery that cannot be recharged is a

Correct Answer
verified

Examine the following half-reactions and select the weakest reducing agent among the substances.

Correct Answer
verified

What is the E $\degree$ _cell for the cell represented by the combination of the following half-reactions? $What is the E \degree <sub>cell</sub> for the cell represented by the combination of the following half-reactions? A) -0.18 V B) 0.18 V C) 1.28 V D) 1.66 V E) 2.12 V$

Correct Answer
verified

Calculate E $\degree$ _cell for the reaction of nickel(II) ions with cadmium metal at 25 $\degree$ C. K = 1.17 *10⁵. Ni²⁺(aq) + Cd(s) $\rightarrow$ Cd²⁺(aq) + Ni(s)

Correct Answer
verified

Correct Answer
verified

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Correct Answer
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Correct Answer
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Correct Answer
verified

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

Correct Answer
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A concentration cell consists of two Al/Al³⁺ electrodes. The electrolyte in compartment A is 0.050 M Al(NO₃) ₃ and in compartment B is 1.25 M Al(NO₃) ₃. What is the voltage of the cell at 25 $\degree$ C?

Correct Answer
verified

Exam 21: Electrochemistry: Chemical Change and Electrical Work

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

Correct AnswerverifiedShow Answer

Consider the following balanced redox reaction Mn2+(aq) + S2O82¯(aq) + 2H2O(l) →\rightarrow→ MnO2(s) + 4H+(aq) + 2SO42¯(aq) Which of the following statements is true?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A voltaic cell consists of a Hg/Hg22+ electrode (E °\degree° = 0.85 V) and a Sn/Sn2+ electrode (E °\degree° = -0.14 V) . Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25 °\degree° C.

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 AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

A solution is prepared by dissolving 32.0 g of NiSO4 in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Correct AnswerverifiedShow Answer

Consider the following balanced redox reaction 3CuO(s) + 2NH3(aq) →\rightarrow→ N2(g) + 3H2O(l) + 3Cu(s) Which of the following statements is true?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

A battery that cannot be recharged is a

Correct AnswerverifiedShow Answer

Examine the following half-reactions and select the weakest reducing agent among the substances.

Correct AnswerverifiedShow Answer

What is the E °\degree° cell for the cell represented by the combination of the following half-reactions?

Correct AnswerverifiedShow Answer

Calculate E °\degree° cell for the reaction of nickel(II) ions with cadmium metal at 25 °\degree° C. K = 1.17 *105. Ni2+(aq) + Cd(s) →\rightarrow→ Cd2+(aq) + Ni(s)

Correct AnswerverifiedShow Answer

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics. If E °\degree° cell = 1.587 V and E °\degree° of the cathode half-cell is 0.536 V, what is E °\degree° of the anode half-cell?

Correct AnswerverifiedShow Answer

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Correct AnswerverifiedShow Answer

Consider the reaction of iodine with manganese dioxide: 3I2(s) + 2MnO2(s) + 8OH¯(aq) 6I¯(aq) + 2MnO4¯(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30* 10¯7. Calculate Δ\DeltaΔ G °\degree° for the reaction at 25 °\degree° C.

Correct AnswerverifiedShow Answer

Consider the non-aqueous cell reaction for which E °\degree° cell = 2.35 V at 200 °\degree° C. Δ\DeltaΔ G °\degree° at this temperature is

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

A concentration cell consists of two Al/Al3+ electrodes. The electrolyte in compartment A is 0.050 M Al(NO3) 3 and in compartment B is 1.25 M Al(NO3) 3. What is the voltage of the cell at 25 °\degree° C?

Correct AnswerverifiedShow Answer

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

Correct Answer
verified

Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈²¯(aq) + 2H₂O(l) $\rightarrow$ MnO₂(s) + 4H⁺(aq) + 2SO₄²¯(aq) Which of the following statements is true?

Correct Answer
verified

Correct Answer
verified

A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E $\degree$ = 0.85 V) and a Sn/Sn²⁺ electrode (E $\degree$ = -0.14 V) . Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V 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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A solution is prepared by dissolving 32.0 g of NiSO₄ in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Correct Answer
verified

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) $\rightarrow$ N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
verified

What is the E $\degree$ _cell for the cell represented by the combination of the following half-reactions? $What is the E \degree <sub>cell</sub> for the cell represented by the combination of the following half-reactions? A) -0.18 V B) 0.18 V C) 1.28 V D) 1.66 V E) 2.12 V$

Correct Answer
verified

Calculate E $\degree$ _cell for the reaction of nickel(II) ions with cadmium metal at 25 $\degree$ C. K = 1.17 *10⁵. Ni²⁺(aq) + Cd(s) $\rightarrow$ Cd²⁺(aq) + Ni(s)

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
verified

A concentration cell consists of two Al/Al³⁺ electrodes. The electrolyte in compartment A is 0.050 M Al(NO₃) ₃ and in compartment B is 1.25 M Al(NO₃) ₃. What is the voltage of the cell at 25 $\degree$ C?

Correct Answer
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