Question 1

The following has a potential of 0.34 V. $\mathrm { Cu } ^ { 2 + } ( \mathrm { aq } ) + \mathrm { H } _ { 2 } ( \mathrm {~g} ) \rightarrow 2 \mathrm { H } ^ { + } ( \mathrm { aq } ) + \mathrm { Cu } ( \mathrm { s } )$ If the concentrations of each of the ions is 1.0 M and the pressure of H2 is 1.0 atm, then E° for the half-reaction $\mathrm { Cu } ^ { 2 + } ( \mathrm { aq } ) + 2 e ^ { - } \rightarrow \mathrm { Cu } ( \mathrm { s } )$ is _____.

Accepted Answer

A)  0.17 V 
B)  -0.17 V 
C)  0.34 V 
D)  -0.34 V 
E)  None of these

Question 2

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. 
Cu(s) | Cu2+(aq) || Mn2+(aq) | Mn(s)

Accepted Answer

A)  2 Cu(s) + Mn2+(aq) → Mn(s) + 2 Cu2+(aq) 
B)  Cu(s) + Cu2+(aq) → Mn(s) + Mn2+(aq) 
C)  Cu(s) + Mn2+(aq) → Mn(s) + Cu2+(aq) 
D)  2 Mn(s) + Cu2+(aq) → Cu(s) + 2Mn2+(aq) 
E)  Mn(s) + Cu2+(aq) → Cu(s) + Mn2+(aq)

Question 3

Which of the following are the expected products when an aqueous solution of lithium sulfate is electrolyzed?$$\begin{array} { l l } 
\text { Reduction Half-Reaction } & \mathrm { E } ^ { \circ } ( \mathrm { V } ) \
\mathrm { Li } ^ { + } ( \mathrm { aq } ) + \mathrm { e } ^ { - } \rightarrow \mathrm { Li } ( \mathrm { s } ) & - 3.04 \
2 \mathrm { H } _ { 2 } \mathrm { O } ( \ell ) + 2 \mathrm { e } ^ { - } \rightarrow \mathrm { H } _ { 2 } ( \mathrm {~g} ) + 2 \mathrm { OH } ^ { - } ( \mathrm { aq } ) & - 0.83 \
2 \mathrm { H } ^ { + } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - } \rightarrow \mathrm { H } _ { 2 } ( \mathrm {~g} ) & 0.00 \
\mathrm { O } _ { 2 } ( \mathrm {~g} ) + 4 \mathrm { H } ^ { + } ( \mathrm { aq } ) + 4 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { H } _ { 2 } \mathrm { O } ( \ell ) & 1.23 \
\mathrm {~S} _ { 2 } \mathrm { O } _ { 8 } { } ^ { 2 - } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { SO } _ { 4 } { } ^ { 2 - } ( \mathrm { aq } ) & 2.01
\end{array}$$

Accepted Answer

A)  Li(s) and H2(g) 
B)  H2(g), OH-(aq), O2(g), and H+(aq) 
C)  O2(g), H+(aq), and Li(s) 
D)  H2(g), OH-(aq), and Li(s) 
E)  H2(g), OH-(aq), and S2O82-(aq)

Question 4

Explain the function of a salt bridge in a voltaic cell.

Accepted Answer

The answer of Explain the function of a salt bridge...

Question 5

The value of E°cell is $0.59 \mathrm {~V}$ for the following reaction: 
Cl2(g) + 2 Fe2+(aq) ? 2 Fe3+(aq) + 2 Cl-(aq)
Calculate the value of E°cell for the reaction below.
Cl-(g) + Fe3+(aq) ? Fe2+(aq) + ½ Cl2(g)

Accepted Answer

A)  -1.18 V 
B)  -0.30 V 
C)  0.59 V 
D)  0.30 V 
E)  -0.59 V

Question 6

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl4-(aq) + 3 e- → Au(s) + 4 Cl-(aq)
The thermodynamic information is as follows:
Au3+(aq) + 3 e- → Au(s)
E° = +1.50 V
Au3+(aq) + 4 Cl-(aq) → AuCl4-(aq)
Kf = 2.3 × 1025

Accepted Answer

A)  -1.28 V 
B)  -0.50 V 
C)  +1.00 V 
D)  +1.28 V 
E)  +3.85 V

Question 7

Which of the following species are likely to behave as oxidizing agents? 
Li(s), H2(g), MnO4-(aq), and Cl-(aq)

Accepted Answer

A)  Li(s) 
B)  MnO4-(aq) 
C)  H2(g) and Cl-(aq) 
D)  Li(s) and MnO4-(aq) 
E)  Cl-(aq)

Question 8

How many electrons are transferred in the given reaction? 
Ni + 2 HCl → Ni Cl2 + H2

Accepted Answer

A)  0 
B)  1 
C)  2 
D)  3 
E)  4

Question 9

Which of the following is the cell notation for a voltaic cell based on the following reaction? 
Cu2+(aq) + Fe(s) → Cu(s) + Fe2+(aq)

Accepted Answer

A)  Cu(s) | Cu2+(aq) || Fe2+(aq) | Fe(s) 
B)  Fe(s) || Fe2+(aq), Cu2+(aq) | Cu(s) 
C)  Cu(s) || Cu2+(aq), Fe2+(aq) || Fe(s) 
D)  Cu(s) | Fe2+(aq) || Cu2+(aq) | Fe(s) 
E)  Fe(s) | Fe2+(aq) || Cu2+(aq) | Cu(s)

Question 10

Which of the following is the cell notation for a voltaic cell based on the following reaction? 
Cu2+(aq) + Pb(s) + SO42-(aq) → Cu(s) + PbSO4(s)

Accepted Answer

A)  Pb(s) | PbSO4(s) || Cu2+(aq) || Cu(s) 
B)  Cu(s) | Cu2+(aq) || SO42-(aq) | PbSO4(s) | Pb(s) 
C)  Cu(s) | Cu2+(aq), SO42-(aq) | PbSO4(s) | Pb(s) 
D)  Cu(s) | Cu2+(aq), SO42-(aq) || PbSO4(s) || Pb(s) 
E)  Pb(s) | PbSO4(s) | SO42-(aq) || Cu2+(aq) || Cu(s)

Question 11

How many moles of electrons are produced from a current of 17.0 A in 3.40 hours?

Accepted Answer

A)  5.99 × 10-4 mol 
B)  2.16 mol 
C)  57.8 mol 
D)  3.35 mol 
E)  9.33 × 103 mol

Question 12

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl-(aq, 1.0 M) || Cu2+(aq, 1.0 M) | Cu(s). The standard reduction potentials are as follows:
Cu2+(aq) + 2 e- ? Cu(s)
E° = +0.337 V
AgCl(s) + e- ? Ag(s) + Cl-(aq)
E° = +0.222 V

Accepted Answer

A)  -0.115 V 
B)  -0.107 V 
C)  +0.115 V 
D)  +0.452 V 
E)  +0.559 V

Question 13

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 
2 H+(aq) + 2 e- → H2(g); 0.00 V
K+(aq) + e- → K(s); -2.93 V
F2(g) + 2 e- → 2 F-(aq); 2.87 V
Al3+(aq) + 3 e- → Al(s); -1.66 V
Pb2+(aq) + 2 e- → Pb(s); -0.13 V

Accepted Answer

A)  Al3+ 
B)  H+ 
C)  Pb2+ 
D)  F- 
E)  K

Question 14

Which of the following reactions will require the use of an inert electrode when used in a voltaic cell?

Accepted Answer

A)  Co(s) + 2 Ag+(aq) → 2 Ag(s) + Co2+(aq) 
B)  3 Ni(s) + 2 Au3+(aq) → 3 Ni2+ + 2 Au(s) 
C)  Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s) 
D)  Zn(s) + 2 MnO2(s) + 2 NH4+(aq) → Zn2+(aq) + Mn2O3(s) + 2 NH3(aq) + H2O(l) 
E)  3 Zn2+(aq) + 2 Al(s) → 3 Zn(s) + 2 Al3+(aq)

Question 15

Consider the following half-reactions. 
Cl2(g) + 2 e- → 2 Cl-(aq)
E° = +1.36 V
Ag+(aq) + e- → Ag(s)
E° = +0.80 V
Cu2+(aq) + 2 e- → Cu(s)
E° = +0.34 V
Sn2+(aq) + 2 e- → Sn(s)
E° = -0.14 V
Al3+(aq) + 3 e- → Al(s)
E° = -1.66 V
Which of the following species will reduce Cu2+(aq) ion?

Accepted Answer

A)  Ag(s) and Sn2+(aq) 
B)  Cl-(aq) and Ag(s) 
C)  Cl2(g) and Ag+(aq) 
D)  Sn(s) and Al(s) 
E)  Sn2+(aq) and Al3+(aq)

Question 16

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? 
Pt2+(aq) + 2 e- ? Pt(s); E° = 1.180 V
Pb2+(aq) + 2 e- ? Pb(s); E° = -0.130 V

Accepted Answer

A)  Pt2+(aq) + Pb(s)? Pt(s) + Pb2+(aq); $E _ { \text {cell } } ^ { \circ }$ = 1.310 V 
B)  Pt(s) + Pb2+(aq) ? Pt2+(aq) + Pb(s); $E _ { \text {cell } } ^ { \circ }$ = ?1.310 V 
C)  Pt2+(aq) + Pb2+(aq) ? Pt(s) + Pb(s); $E _ { \text {cell } } ^ { \circ }$ = 1.050 V 
D)  Pt2+(aq) + Pb(s) ? Pt(s) + Pb2+(aq); $E _ { \text {cell } } ^ { \circ }$ =0.655 V 
E)  Pt(s) + Pb2+(aq) ? Pt2+(aq) + Pb(s); $E _ { \text {cell } } ^ { \circ }$ = ?0.655 V

Question 17

Calculate the value of the equilibrium constant (K) at 25 °C for the following cell reaction: 
Sn(s) + Pb2+(aq) → Sn2+(aq) + Pb(s); E°cell = 0.014 V

Accepted Answer

A)  0.014 
B)  1.7 
C)  0.4 
D)  1.0 
E)  3

Question 18

In the context of the diagram given below, which of the following statements is true concerning half-cell II?

Accepted Answer

A)  [Cu2+] decreases with time, and [K+] increases with time. 
B)  [Cu2+] increases with time, and [K+] increases with time. 
C)  [Cu2+] decreases with time, and [K+] decreases with time. 
D)  [Cu2+] decreases with time, and [SO42-] decreases with time. 
E)  [Cu2+] increases with time, and [SO42-] increases with time.

Question 19

The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H2(g, 1.00 atm) | H+(aq, 1.00 M) || Cl-(aq) | AgCl(s) | Ag
The standard reduction potential, E°, of AgCl(s) is +0.222 V. Calculate the Cl-(aq) ion concentration.

Accepted Answer

A)  1.9 × 10-19 M 
B)  5.5 × 10-10 M 
C)  0.018 M 
D)  1.03 M 
E)  1.8 × 109 M

Question 20

In an electrolytic cell, reduction occurs at the _____ and oxidation occurs at the _____.

Accepted Answer

The answer of In an electrolytic cell, reduction occurs at...

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu²⁺(aq) || Mn²⁺(aq) | Mn(s)

Explain the function of a salt bridge in a voltaic cell.

The value of E°_cell is $0.59 \mathrm {~V}$ for the following reaction: Cl₂(g) + 2 Fe²⁺(aq) ? 2 Fe³⁺(aq) + 2 Cl^-(aq) Calculate the value of E°_cell for the reaction below. Cl^-(g) + Fe³⁺(aq) ? Fe²⁺(aq) + ½ Cl₂(g)

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl₄^-(aq) + 3 e^- → Au(s) + 4 Cl^-(aq) The thermodynamic information is as follows: Au³⁺(aq) + 3 e^- → Au(s) E° = +1.50 V Au³⁺(aq) + 4 Cl^-(aq) → AuCl₄^-(aq) K_f = 2.3 × 10²⁵

Which of the following species are likely to behave as oxidizing agents? Li(s) , H₂(g) , MnO₄^-(aq) , and Cl^-(aq)

How many electrons are transferred in the given reaction? Ni + 2 HCl → Ni Cl₂ + H₂

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Fe(s) → Cu(s) + Fe²⁺(aq)

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Pb(s) + SO₄^2-(aq) → Cu(s) + PbSO₄(s)

How many moles of electrons are produced from a current of 17.0 A in 3.40 hours?

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl^-(aq, 1.0 M) || Cu²⁺(aq, 1.0 M) | Cu(s) . The standard reduction potentials are as follows: Cu²⁺(aq) + 2 e^- ? Cu(s) E° = +0.337 V AgCl(s) + e^- ? Ag(s) + Cl^-(aq) E° = +0.222 V

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H⁺(aq) + 2 e^- → H₂(g) ; 0.00 V K⁺(aq) + e^- → K(s) ; -2.93 V F₂(g) + 2 e^- → 2 F^-(aq) ; 2.87 V Al³⁺(aq) + 3 e^- → Al(s) ; -1.66 V Pb²⁺(aq) + 2 e^- → Pb(s) ; -0.13 V

Which of the following reactions will require the use of an inert electrode when used in a voltaic cell?

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt²⁺(aq) + 2 e- ? Pt(s) ; E° = 1.180 V Pb²⁺(aq) + 2 e- ? Pb(s) ; E° = -0.130 V

Calculate the value of the equilibrium constant (K) at 25 °C for the following cell reaction: Sn(s) + Pb²⁺(aq) → Sn²⁺(aq) + Pb(s) ; E°_cell= 0.014 V

In the context of the diagram given below, which of the following statements is true concerning half-cell II?

The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H₂(g, 1.00 atm) | H⁺(aq, 1.00 M) || Cl^-(aq) | AgCl(s) | Ag The standard reduction potential, E°, of AgCl(s) is +0.222 V. Calculate the Cl^-(aq) ion concentration.

In an electrolytic cell, reduction occurs at the _ and oxidation occurs at the _.

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu2+(aq) || Mn2+(aq) | Mn(s)

Explain the function of a salt bridge in a voltaic cell.

The value of E°cell is 0.59 V0.59 \mathrm {~V}0.59 V for the following reaction: Cl2(g) + 2 Fe2+(aq) ? 2 Fe3+(aq) + 2 Cl-(aq) Calculate the value of E°cell for the reaction below. Cl-(g) + Fe3+(aq) ? Fe2+(aq) + ½ Cl2(g)

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl4-(aq) + 3 e- → Au(s) + 4 Cl-(aq) The thermodynamic information is as follows: Au3+(aq) + 3 e- → Au(s) E° = +1.50 V Au3+(aq) + 4 Cl-(aq) → AuCl4-(aq) Kf = 2.3 × 1025

Which of the following species are likely to behave as oxidizing agents? Li(s) , H2(g) , MnO4-(aq) , and Cl-(aq)

How many electrons are transferred in the given reaction? Ni + 2 HCl → Ni Cl2 + H2

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu2+(aq) + Fe(s) → Cu(s) + Fe2+(aq)

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu2+(aq) + Pb(s) + SO42-(aq) → Cu(s) + PbSO4(s)

How many moles of electrons are produced from a current of 17.0 A in 3.40 hours?

Calculate Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​ for the electrochemical cell Ag(s) | AgCl(s) | Cl-(aq, 1.0 M) || Cu2+(aq, 1.0 M) | Cu(s) . The standard reduction potentials are as follows: Cu2+(aq) + 2 e- ? Cu(s) E° = +0.337 V AgCl(s) + e- ? Ag(s) + Cl-(aq) E° = +0.222 V

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H+(aq) + 2 e- → H2(g) ; 0.00 V K+(aq) + e- → K(s) ; -2.93 V F2(g) + 2 e- → 2 F-(aq) ; 2.87 V Al3+(aq) + 3 e- → Al(s) ; -1.66 V Pb2+(aq) + 2 e- → Pb(s) ; -0.13 V

Which of the following reactions will require the use of an inert electrode when used in a voltaic cell?

Consider the following half-reactions. Cl2(g) + 2 e- → 2 Cl-(aq) E° = +1.36 V Ag+(aq) + e- → Ag(s) E° = +0.80 V Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V Sn2+(aq) + 2 e- → Sn(s) E° = -0.14 V Al3+(aq) + 3 e- → Al(s) E° = -1.66 V Which of the following species will reduce Cu2+(aq) ion?

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt2+(aq) + 2 e- ? Pt(s) ; E° = 1.180 V Pb2+(aq) + 2 e- ? Pb(s) ; E° = -0.130 V

Calculate the value of the equilibrium constant (K) at 25 °C for the following cell reaction: Sn(s) + Pb2+(aq) → Sn2+(aq) + Pb(s) ; E°cell = 0.014 V

In the context of the diagram given below, which of the following statements is true concerning half-cell II?

The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H2(g, 1.00 atm) | H+(aq, 1.00 M) || Cl-(aq) | AgCl(s) | Ag The standard reduction potential, E°, of AgCl(s) is +0.222 V. Calculate the Cl-(aq) ion concentration.

In an electrolytic cell, reduction occurs at the _____ and oxidation occurs at the _____.

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu²⁺(aq) || Mn²⁺(aq) | Mn(s)

The value of E°_cell is $0.59 \mathrm {~V}$ for the following reaction: Cl₂(g) + 2 Fe²⁺(aq) ? 2 Fe³⁺(aq) + 2 Cl^-(aq) Calculate the value of E°_cell for the reaction below. Cl^-(g) + Fe³⁺(aq) ? Fe²⁺(aq) + ½ Cl₂(g)

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl₄^-(aq) + 3 e^- → Au(s) + 4 Cl^-(aq) The thermodynamic information is as follows: Au³⁺(aq) + 3 e^- → Au(s) E° = +1.50 V Au³⁺(aq) + 4 Cl^-(aq) → AuCl₄^-(aq) K_f = 2.3 × 10²⁵

Which of the following species are likely to behave as oxidizing agents? Li(s) , H₂(g) , MnO₄^-(aq) , and Cl^-(aq)

How many electrons are transferred in the given reaction? Ni + 2 HCl → Ni Cl₂ + H₂

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Fe(s) → Cu(s) + Fe²⁺(aq)

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Pb(s) + SO₄^2-(aq) → Cu(s) + PbSO₄(s)

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl^-(aq, 1.0 M) || Cu²⁺(aq, 1.0 M) | Cu(s) . The standard reduction potentials are as follows: Cu²⁺(aq) + 2 e^- ? Cu(s) E° = +0.337 V AgCl(s) + e^- ? Ag(s) + Cl^-(aq) E° = +0.222 V

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt²⁺(aq) + 2 e- ? Pt(s) ; E° = 1.180 V Pb²⁺(aq) + 2 e- ? Pb(s) ; E° = -0.130 V

Calculate the value of the equilibrium constant (K) at 25 °C for the following cell reaction: Sn(s) + Pb²⁺(aq) → Sn²⁺(aq) + Pb(s) ; E°_cell= 0.014 V

The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H₂(g, 1.00 atm) | H⁺(aq, 1.00 M) || Cl^-(aq) | AgCl(s) | Ag The standard reduction potential, E°, of AgCl(s) is +0.222 V. Calculate the Cl^-(aq) ion concentration.

In an electrolytic cell, reduction occurs at the _ and oxidation occurs at the _.