Question 1

The balanced equation for a spontaneous reaction which involves the tin and zinc redox couple using the following standard reduction potentials in acid solution is: $\begin{array}{ll}
\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightarrow 2 \mathrm{H}_{2} \mathrm{O} & \mathrm{E}^{\circ}=+1.23 \mathrm{~V} \
\mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}^{2+} & \mathrm{E}^{\circ}=+0.13 \mathrm{~V} \
\mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(\mathrm{~s}) & \mathrm{E}^{\circ}=-0.76 \mathrm{~V}
\end{array}$ Zn + Sn4+ $\rarr$ Zn2+ + Sn2+

Accepted Answer

A) True 
 B)False

Question 2

The half-reaction that occurs at the cathode during electrolysis of an aqueous sodium iodide solution is

Accepted Answer

A)  Na+ + e-  →\rarr→  Na.
B)  Na  →\rarr→  Na+ + e-.
C)  2H2O + 2e-  →\rarr→  H2 + 2OH-.
D)  I2 + 2e-  →\rarr→  2I-.
E)  ( →\rarr→ 2I-  →\rarr→ I2 + 2e-) . F) A) and E)
G) A) and C)

Question 3

Calculate the cell emf for the following reaction at 25 ∘\circ∘ C: Ni(s)  + 2Cu2+(0.010 M)   →\rarr→  Ni2+(0.0010 M)  + 2Cu+(1.0 M)

Accepted Answer

A)   0.40 V
B)   -0.43 V
C)   0.43 V
D)   0.34 V
E)   0.37 V F) A) and B)
G) A) and E)

Question 4

Determine the equilibrium constant for the following reaction at 25 ∘\circ∘ C.2I- (aq)  + Br2(l)   ⇋\leftrightharpoons⇋  I2(s)  + 2Br-(aq) .

Accepted Answer

A)   1.8 * 1018
B)   2.8 * 1018
C)   3.8 * 1018
D)   4.8 * 1018
E)   None of the above F) A) and B)
G) A) and C)

Question 5

Consider an electrochemical cell based on the spontaneous reaction 
2AgCl(s)  + Zn(s)   →\rarr→  2Ag(s)  + 2Cl- + Zn2+.
If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Accepted Answer

A)   increase by 0.06 V.
B)   increase by 0.18 V.
C)   decrease by 0.06 V.
D)   decrease by 0.18 V.
E)   increase by 0.35 V. F) None of the above
G) A) and B)

Question 6

Calculate E ∘\circ∘ cell for the following electrochemical cell: Ni(s)  | Ni2+(aq)  || Hg22+(aq)  | Hg(l)  | Pt(s)

Accepted Answer

A)   1.10 V
B)   1.00 V
C)   0.90 V
D)   0.80 V
E)   None of the above F) C) and D)
G) All of the above

Question 7

What is the total number of moles (n)  of electrons exchanged between the oxidizing agent and the reducing agent in the overall redox equation: 5 Ag+(aq)  + Mn2+(aq)  + 4H2O(l)   →\rarr→  5Ag(s)  + MnO4-(aq)  + 8H+(aq)

Accepted Answer

A)   1
B)   2
C)   3
D)   5
E)   7 F) None of the above
G) A) and D)

Question 8

H2(g) will form when Ag is placed in 1.0 M HCl.

Accepted Answer

A) True 
 B)False

Question 9

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min

Accepted Answer

A)   0.20 g
B)   0.40 g
C)   12 g
D)   24 g
E)   47 gF) All of the above
G) A) and B)

Question 10

H2(g) will form when Fe is placed in 1.0 M HCl.

Accepted Answer

A) True 
 B)False

Question 11

Calculate the cell emf for the following reaction: Cu2+(0.10 M)  + H2(1 atm)   →\rarr→  Cu(s)  + 2H+(pH = 3.00)

Accepted Answer

A)   0.49 V
B)   0.19 V
C)   0.15 V
D)   0.40 V
E)   -0.34 V F) None of the above
G) B) and D)

Question 12

Many different ways have been proposed to make batteries. One cell is set up with copper and lead electrodes in contact with CuSO4(aq)  and Pb(NO3) 2 (aq) , respectively. If the Pb2+ and Cu2+ concentrations are each 1.0 M, what is the overall cell potential  Pb2++2e−→PbE∘=−0.22 VCu2++2e−→CuE∘=+0.34 V\begin{array}{ll}\mathrm{Pb}^{2+}+2 \mathrm{e}^{-} ightarrow \mathrm{Pb} & \mathrm{E}^{\circ}=-0.22 \mathrm{~V} \\mathrm{Cu}^{2+}+2 \mathrm{e}^{-} ightarrow \mathrm{Cu} & \mathrm{E}^{\circ}=+0.34 \mathrm{~V}\end{array}Pb2++2e−→PbCu2++2e−→Cu​E∘=−0.22 VE∘=+0.34 V​

Accepted Answer

A)   0.16 V
B)   0.36 V
C)   0.56 V
D)   0.76 V
E)   None of the above F) A) and E)
G) B) and E)

Question 13

Find the emf of the cell described by the cell diagram Ni | Ni2+ (0.750 M)  || Cu2+ (0.0500 M)  | Cu.

Accepted Answer

A)   0.62 V
B)   0.52 V
C)   0.59 V
D)   0.66 V
E)   0.56 VF) A) and E)
G) A) and D)

Question 14

Given the following cell diagram, Al(s)  | Al3+(aq)  || Cd2+(aq)  | Cd (s) 
What is the balanced overall (net)  cell reaction

Accepted Answer

A)  Al(s)  + Cd2+(aq)   →\rarr→  Al3+(aq)  + Cd (s) 
B)  Al3+(aq)  + Cd (s)   →\rarr→  Al(s)  + Cd2+(aq) 
C)  2Al(s)  + 3Cd2+(aq)   →\rarr→  2Al3+(aq)  + 3Cd (s) 
D)  2Al3+(aq)  + 3Cd (s)   →\rarr→  2Al(s)  + 3Cd2+(aq) 
E)  3Al3+(aq)  + 2Cd (s)   →\rarr→  3Al(s)  + 2Cd2+(aq)  F) A) and D)
G) A) and E)

Question 15

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn2+ is 2.0 M, what is the concentration of Cu2+

Accepted Answer

A)   1.5 * 10-8 M
B)   1.5 * 10-9 M
C)   1.5 * 10-10 M
D)   1.5 * 10-11 M
E)   None of the aboveF) C) and D)
G) A) and B)

Question 16

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl3 electrolyte. Calculate the number of moles of gold deposited in 3.0 min by a constant current of 10.A.

Accepted Answer

A)   6.2 * 10-3 mol
B)   9.3 * 10-3 mol
C)   1.8 * 10-2 mol
D)   3.5 * 10-5 mol
E)   160 molF) C) and D)
G) B) and C)

Question 17

Consider the reaction Fe + Sn2+(1 * 10-3 M)   →\rarr→ Fe2+(1.0 M)  + Sn. Calculate the voltage theoretically generated by the cell.

Accepted Answer

A)   0.10 V
B)   0.30 V
C)   0.50 V
D)   0.70 V
E)   None of the above F) B) and E)
G) All of the above

Question 18

The half-reaction that occurs at the cathode during electrolysis of an aqueous CuCl2 solution is

Accepted Answer

A)  Cu+ + e-  →\rarr→  Cu.
B)  Cu2+ + e-  →\rarr→  Cu+.
C)  2H2O + 2e-  →\rarr→  H2 + 2OH-.
D)  Cl2 + 2e-  →\rarr→  2Cl-.
E)  2Cl-  →\rarr→  Cl2 + 2e-. F) B) and D)
G) A) and B)

Question 19

Which element is associated with the term "galvanized"

Accepted Answer

A)   Ga
B)   Zn
C)   Cd
D)   Hg
E)   PbF) D) and E)
G) All of the above

Question 20

Which one of the following reagents is capable of reducing Cu2+(1 M)  to Cu(s)

Accepted Answer

A)   I- (1 M) 
B)   Ni(s) 
C)   Al3+ (1 M) 
D)   F- (1 M) 
E)   Ag(s) F) B) and E)
G) None of the above

Exam 18: Electrochemistry

H₂(g) will form when Ag is placed in 1.0 M HCl.

Correct Answer
verified

Correct Answer
verified

The half-reaction that occurs at the cathode during electrolysis of an aqueous sodium iodide solution is

Correct Answer
verified

Calculate the cell emf for the following reaction at 25^$\circ$C: Ni(s) + 2Cu²⁺(0.010 M) $\rarr$ Ni²⁺(0.0010 M) + 2Cu⁺(1.0 M)

Correct Answer
verified

Given the following cell diagram, Al(s) | Al³⁺(aq) || Cd²⁺(aq) | Cd (s) What is the balanced overall (net) cell reaction

Correct Answer
verified

Correct Answer
verified

The half-reaction that occurs at the cathode during electrolysis of an aqueous CuCl₂ solution is

Correct Answer
verified

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M) $\rarr$ Fe²⁺(1.0 M) + Sn. Calculate the voltage theoretically generated by the cell.

Correct Answer
verified

Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s) $\rarr$ 2Ag(s) + 2Cl^- + Zn²⁺. If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Correct Answer
verified

Calculate the cell emf for the following reaction: Cu²⁺(0.10 M) + H₂(1 atm) $\rarr$ Cu(s) + 2H⁺(pH = 3.00)

Correct Answer
verified

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO₄ for 90.0 min

Correct Answer
verified

Find the emf of the cell described by the cell diagram Ni | Ni²⁺ (0.750 M) || Cu²⁺ (0.0500 M) | Cu.

Correct Answer
verified

Determine the equilibrium constant for the following reaction at 25^$\circ$C.2I^- (aq) + Br₂(l) $\leftrightharpoons$ I₂(s) + 2Br^-(aq) .

Correct Answer
verified

What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the overall redox equation: 5 Ag⁺(aq) + Mn²⁺(aq) + 4H₂O(l) $\rarr$ 5Ag(s) + MnO₄^-(aq) + 8H⁺(aq)

Correct Answer
verified

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl₃ electrolyte. Calculate the number of moles of gold deposited in 3.0 min by a constant current of 10.A.

Correct Answer
verified

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn²⁺ is 2.0 M, what is the concentration of Cu²⁺

Correct Answer
verified

Calculate E^$\circ$_cell for the following electrochemical cell: Ni(s) | Ni²⁺(aq) || Hg₂²⁺(aq) | Hg(l) | Pt(s)

Correct Answer
verified

H₂(g) will form when Fe is placed in 1.0 M HCl.

Correct Answer
verified

Which element is associated with the term "galvanized"

Correct Answer
verified

Which one of the following reagents is capable of reducing Cu²⁺(1 M) to Cu(s)

Correct Answer
verified

Exam 18: Electrochemistry

H2(g) will form when Ag is placed in 1.0 M HCl.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The half-reaction that occurs at the cathode during electrolysis of an aqueous sodium iodide solution is

Correct AnswerverifiedShow Answer

Calculate the cell emf for the following reaction at 25 ∘\circ∘ C: Ni(s) + 2Cu2+(0.010 M) →\rarr→ Ni2+(0.0010 M) + 2Cu+(1.0 M)

Correct AnswerverifiedShow Answer

Given the following cell diagram, Al(s) | Al3+(aq) || Cd2+(aq) | Cd (s) What is the balanced overall (net) cell reaction

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The half-reaction that occurs at the cathode during electrolysis of an aqueous CuCl2 solution is

Correct AnswerverifiedShow Answer

Consider the reaction Fe + Sn2+(1 * 10-3 M) →\rarr→ Fe2+(1.0 M) + Sn. Calculate the voltage theoretically generated by the cell.

Correct AnswerverifiedShow Answer

Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s) →\rarr→ 2Ag(s) + 2Cl- + Zn2+. If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Correct AnswerverifiedShow Answer

Calculate the cell emf for the following reaction: Cu2+(0.10 M) + H2(1 atm) →\rarr→ Cu(s) + 2H+(pH = 3.00)

Correct AnswerverifiedShow Answer

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min

Correct AnswerverifiedShow Answer

Find the emf of the cell described by the cell diagram Ni | Ni2+ (0.750 M) || Cu2+ (0.0500 M) | Cu.

Correct AnswerverifiedShow Answer

Determine the equilibrium constant for the following reaction at 25 ∘\circ∘ C.2I- (aq) + Br2(l) ⇋\leftrightharpoons⇋ I2(s) + 2Br-(aq) .

Correct AnswerverifiedShow Answer

What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the overall redox equation: 5 Ag+(aq) + Mn2+(aq) + 4H2O(l) →\rarr→ 5Ag(s) + MnO4-(aq) + 8H+(aq)

Correct AnswerverifiedShow Answer

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl3 electrolyte. Calculate the number of moles of gold deposited in 3.0 min by a constant current of 10.A.

Correct AnswerverifiedShow Answer

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn2+ is 2.0 M, what is the concentration of Cu2+

Correct AnswerverifiedShow Answer

Calculate E ∘\circ∘ cell for the following electrochemical cell: Ni(s) | Ni2+(aq) || Hg22+(aq) | Hg(l) | Pt(s)

Correct AnswerverifiedShow Answer

H2(g) will form when Fe is placed in 1.0 M HCl.

Correct AnswerverifiedShow Answer

Which element is associated with the term "galvanized"

Correct AnswerverifiedShow Answer

Which one of the following reagents is capable of reducing Cu2+(1 M) to Cu(s)

Correct AnswerverifiedShow Answer

H₂(g) will form when Ag is placed in 1.0 M HCl.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate the cell emf for the following reaction at 25^$\circ$C: Ni(s) + 2Cu²⁺(0.010 M) $\rarr$ Ni²⁺(0.0010 M) + 2Cu⁺(1.0 M)

Correct Answer
verified

Given the following cell diagram, Al(s) | Al³⁺(aq) || Cd²⁺(aq) | Cd (s) What is the balanced overall (net) cell reaction

Correct Answer
verified

Correct Answer
verified

The half-reaction that occurs at the cathode during electrolysis of an aqueous CuCl₂ solution is

Correct Answer
verified

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M) $\rarr$ Fe²⁺(1.0 M) + Sn. Calculate the voltage theoretically generated by the cell.

Correct Answer
verified

Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s) $\rarr$ 2Ag(s) + 2Cl^- + Zn²⁺. If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Correct Answer
verified

Calculate the cell emf for the following reaction: Cu²⁺(0.10 M) + H₂(1 atm) $\rarr$ Cu(s) + 2H⁺(pH = 3.00)

Correct Answer
verified

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO₄ for 90.0 min

Correct Answer
verified

Find the emf of the cell described by the cell diagram Ni | Ni²⁺ (0.750 M) || Cu²⁺ (0.0500 M) | Cu.

Correct Answer
verified

Determine the equilibrium constant for the following reaction at 25^$\circ$C.2I^- (aq) + Br₂(l) $\leftrightharpoons$ I₂(s) + 2Br^-(aq) .

Correct Answer
verified

What is the total number of moles (n) of electrons exchanged between the oxidizing agent and the reducing agent in the overall redox equation: 5 Ag⁺(aq) + Mn²⁺(aq) + 4H₂O(l) $\rarr$ 5Ag(s) + MnO₄^-(aq) + 8H⁺(aq)

Correct Answer
verified

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl₃ electrolyte. Calculate the number of moles of gold deposited in 3.0 min by a constant current of 10.A.

Correct Answer
verified

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn²⁺ is 2.0 M, what is the concentration of Cu²⁺

Correct Answer
verified

Calculate E^$\circ$_cell for the following electrochemical cell: Ni(s) | Ni²⁺(aq) || Hg₂²⁺(aq) | Hg(l) | Pt(s)

Correct Answer
verified

H₂(g) will form when Fe is placed in 1.0 M HCl.

Correct Answer
verified

Correct Answer
verified

Which one of the following reagents is capable of reducing Cu²⁺(1 M) to Cu(s)

Correct Answer
verified