Question 1

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

Question 2

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 
A)  1.10 V 
B)  1.00 V 
C)  0.90 V 
D)  0.80 V 
E)  None of the above

Question 3

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

Question 4

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 
A)  1 
B)  2 
C)  3 
D)  5 
E)  7

Question 5

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-). 
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-).

Question 6

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 g 
A)  0.20 g 
B)  0.40 g 
C)  12 g 
D)  24 g 
E)  47 g

Question 7

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) 
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)

Question 8

Which element is associated with the term "galvanized"

Accepted Answer

A)  Ga 
B)  Zn 
C)  Cd 
D)  Hg 
E)  Pb 
A)  Ga 
B)  Zn 
C)  Cd 
D)  Hg 
E)  Pb

Question 9

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) 
A)  I- (1 M) 
B)  Ni(s) 
C)  Al3+ (1 M) 
D)  F- (1 M) 
E)  Ag(s)

Question 10

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 
A)  0.10 V 
B)  0.30 V 
C)  0.50 V 
D)  0.70 V 
E)  None of the above

Question 11

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

Accepted Answer

A) True 
 B)False

Question 12

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-. 
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-.

Question 13

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 $\begin{array}{ll}
\mathrm{Pb}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Pb} & \mathrm{E}^{\circ}=-0.22 \mathrm{~V} \
\mathrm{Cu}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu} & \mathrm{E}^{\circ}=+0.34 \mathrm{~V}
\end{array}$

Accepted Answer

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

Question 14

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 15

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 
A)  0.49 V 
B)  0.19 V 
C)  0.15 V 
D)  0.40 V 
E)  -0.34 V

Question 16

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

Question 17

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

Accepted Answer

A) True 
 B)False

Question 18

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 above 
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 above

Question 19

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. 
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.

Question 20

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 mol 
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 mol

Exam 18: Electrochemistry

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

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

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

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)

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

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

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

Which element is associated with the term "galvanized"

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

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

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

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

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 +2\rightarrow =-0.22 +2\rightarrow =+0.34

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: +4+4\rightarrow2 =+1.23 +2\rightarrow =+0.13 +2\rightarrow() =-0.76 Zn + Sn4+ →\rarr→ Zn2+ + Sn2+

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

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)

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

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+

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

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.

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

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

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

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

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)

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

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

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

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

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

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

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: +4+4\rightarrow2 =+1.23 +2\rightarrow =+0.13 +2\rightarrow() =-0.76 Zn + Sn⁴⁺ $\rarr$ Zn²⁺ + Sn²⁺

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

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)

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

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⁺

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

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.