Question 1

What element is being reduced in the following (unbalanced)redox reaction? Cr(OH)4⁻(aq)+ ClO⁻(aq)→ CrO42-(aq)+ Cl⁻(aq)

Accepted Answer

A) Cr 
B) O 
C) H 
D) Cl 
A) Cr 
B) O 
C) H 
D) Cl D

Question 2

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.) Mg(s)+ Cu2+(aq)→ Cu(s)+ Mg2+(aq)
Mg2+(aq)+ 2 e⁻ → Mg(s) E° = -2.38 V
Cu2+(aq)+ 2 e⁻ → Cu(s) E° = +0.34 V

Accepted Answer

A) +2.04 V 
B) -2.04 V 
C) +2.72 V 
D) -1.36 V 
E) +1.36 V 
A) +2.04 V 
B) -2.04 V 
C) +2.72 V 
D) -1.36 V 
E) +1.36 V C

Question 3

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s)+ Ni2+ (aq)→ Zn2+ (aq)+ Ni(s)
The emf generated by the cell when [Ni2+] = 2.50 mol L-1 and [Zn2+] = 0.100 mol L-1 is

Accepted Answer

A) 0.40 
B) 0.50 
C) 0.52 
D) 0.56 
E) 0.44 
A) 0.40 
B) 0.50 
C) 0.52 
D) 0.56 
E) 0.44 C

Question 4

Why is sugar water not a good conductor of current?

Accepted Answer

Sugar wate

Question 5

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)∣ Ni2+(aq)∣∣ Cl2(g)∣ Cl-(aq)∣ C(s)

Accepted Answer

A) Ni(s)+ 2Cl-(aq)→ Ni2+(aq)+ Cl2(g) 
B) Ni(s)+ Cl2(g)→ Ni2+(aq)+ 2Cl-(aq) 
C) Ni2+(aq)+ 2Cl-(aq)→ Ni(s)+ Cl2(g) 
D) Ni2+(aq)+ 2Cl-(aq)→ NiCl2(s) 
A) Ni(s)+ 2Cl-(aq)→ Ni2+(aq)+ Cl2(g) 
B) Ni(s)+ Cl2(g)→ Ni2+(aq)+ 2Cl-(aq) 
C) Ni2+(aq)+ 2Cl-(aq)→ Ni(s)+ Cl2(g) 
D) Ni2+(aq)+ 2Cl-(aq)→ NiCl2(s)

Question 6

Which of the following is the weakest oxidizing agent?

Accepted Answer

A) Sn2+(aq) 
B) Cr3+(aq) 
C) Sn4+(aq) 
D) Cr(s) 
E) Sn(s) 
A) Sn2+(aq) 
B) Cr3+(aq) 
C) Sn4+(aq) 
D) Cr(s) 
E) Sn(s)

Question 7

Which of the following statements is true for the cell diagram below? Zn(s)∣ Zn2+(aq)   Cu2+(aq)∣ Cu(s)

Accepted Answer

A) Zn is oxidized, Cu is reduced; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge. 
B) Zn2+is oxidized, Cu is reduced; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge. 
C) Zn is oxidized, Cu2+ is reduced; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge. 
D) Zn is oxidized, Cu2+ is reduced; the single vertical lines represent salt bridges while the two vertical lines represent a phase boundary. 
E) Zn is reduced, Cu2+ is oxidized; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge. 
A) Zn is oxidized, Cu is reduced; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge. 
B) Zn2+is oxidized, Cu is reduced; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge. 
C) Zn is oxidized, Cu2+ is reduced; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge. 
D) Zn is oxidized, Cu2+ is reduced; the single vertical lines represent salt bridges while the two vertical lines represent a phase boundary. 
E) Zn is reduced, Cu2+ is oxidized; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge.

Question 8

Nickel can be plated from aqueous solution according to the following half-reaction. How long would it take (in min)to plate 29.6 g of nickel at 4.7 A? Ni2+(aq)+ 2 e⁻ → Ni(s)

Accepted Answer

A) 1.7 × 102 min 
B) 5.9 × 102 min 
C) 3.5 × 102 min 
D) 4.8 × 102 min 
E) 6.2 × 102 min 
A) 1.7 × 102 min 
B) 5.9 × 102 min 
C) 3.5 × 102 min 
D) 4.8 × 102 min 
E) 6.2 × 102 min

Question 9

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Al and F2 in the balanced reaction? Al(s)+ F2(g)→ Al3+(aq)+ F-(aq)

Accepted Answer

A) Al = 2, F2 = 3 
B) Al = 2, F2 = 6 
C) Al = 1, F2 = 1 
D) Al = 2, F2 = 1 
E) Al = 3, F2 = 2 
A) Al = 2, F2 = 3 
B) Al = 2, F2 = 6 
C) Al = 1, F2 = 1 
D) Al = 2, F2 = 1 
E) Al = 3, F2 = 2

Question 10

Which of the following is the weakest oxidizing agent?

Accepted Answer

A) H2O2(aq) 
B) Fe3+(aq) 
C) ClO2(g) 
D) I2(s) 
E) Fe(s) 
A) H2O2(aq) 
B) Fe3+(aq) 
C) ClO2(g) 
D) I2(s) 
E) Fe(s)

Question 11

Which of the following is the strongest reducing agent?

Accepted Answer

A) Na(s) 
B) Li+(aq) 
C) Ca(s) 
D) Ca2+(aq) 
E) Li(s) 
A) Na(s) 
B) Li+(aq) 
C) Ca(s) 
D) Ca2+(aq) 
E) Li(s)

Question 12

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C. (The equation is balanced.) Pb(s)+ Br2(l)→ Pb2+(aq)+ 2 Br⁻(aq)
Pb2+(aq)+ 2 e⁻ → Pb(s) E° = -0.13 V
Br2(l)+ 2 e⁻ → 2 Br⁻(aq)E° = +1.07 V

Accepted Answer

A) +1.20 V 
B) +0.94 V 
C) -0.94 V 
D) -1.20 V 
E) -0.60 V 
A) +1.20 V 
B) +0.94 V 
C) -0.94 V 
D) -1.20 V 
E) -0.60 V

Question 13

A galvanic cell consists of one half-cell that contains Ag(s)and Ag+(aq), and one half-cell that contains Cu(s)and Cu2+(aq). What species are produced at the electrodes under standard conditions? Ag+(aq)+ e- → Ag(s)E° = +0.80 V
Cu2+(aq)+ 2 e- → Cu(s)E° = +0.34 V

Accepted Answer

A) Ag(aq)is formed at the cathode, and Cu(s)is formed at the anode. 
B) Ag(s)is formed at the cathode, and Cu2+(aq)is formed at the anode. 
C) Cu(s)is formed at the cathode, and Ag+(aq)is formed at the anode. 
D) Cu2+(aq)is formed at the cathode, and Cu(s)is formed at the anode. 
A) Ag(aq)is formed at the cathode, and Cu(s)is formed at the anode. 
B) Ag(s)is formed at the cathode, and Cu2+(aq)is formed at the anode. 
C) Cu(s)is formed at the cathode, and Ag+(aq)is formed at the anode. 
D) Cu2+(aq)is formed at the cathode, and Cu(s)is formed at the anode.

Question 14

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H⁺ and Fe3+ in the balanced reaction? Fe2+(aq)+ MnO4⁻(aq)→ Fe3+(aq)+ Mn2+(aq)

Accepted Answer

A) H⁺ = 2, Fe3+ = 3 
B) H⁺ = 8, Fe3+ = 5 
C) H⁺ = 3, Fe3+ = 2 
D) H⁺ = 5, Fe3+ = 1 
E) H⁺ = 8, Fe3+ = 1 
A) H⁺ = 2, Fe3+ = 3 
B) H⁺ = 8, Fe3+ = 5 
C) H⁺ = 3, Fe3+ = 2 
D) H⁺ = 5, Fe3+ = 1 
E) H⁺ = 8, Fe3+ = 1

Question 15

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? MnO4⁻ (aq)+ H2C2O4(aq)→ Mn2+(aq)+ CO2(g)

Accepted Answer

A) H2C2O4 = 5, H2O = 8 
B) H2C2O4 = 1, H2O = 1 
C) H2C2O4 = 5, H2O = 1 
D) H2C2O4 = 1, H2O = 4 
E) H2C2O4 = 3, H2O = 2 
A) H2C2O4 = 5, H2O = 8 
B) H2C2O4 = 1, H2O = 1 
C) H2C2O4 = 5, H2O = 1 
D) H2C2O4 = 1, H2O = 4 
E) H2C2O4 = 3, H2O = 2

Question 16

Which of the following metals will dissolve in nitric acid but not hydrochloric acid?

Accepted Answer

A) Cd; Eo(Cd2+/Cd)= -0.40V 
B) Cr; Eo(Cr3+/Cr)= -0.73V 
C) Mn; Eo(Mn2+/Mn)= -1.18V 
D) Ag; Eo(Ag+/Ag)= +0.80V 
E) Al; Eo(Al3+/Al)= -1.66V 
A) Cd; Eo(Cd2+/Cd)= -0.40V 
B) Cr; Eo(Cr3+/Cr)= -0.73V 
C) Mn; Eo(Mn2+/Mn)= -1.18V 
D) Ag; Eo(Ag+/Ag)= +0.80V 
E) Al; Eo(Al3+/Al)= -1.66V

Question 17

What is undergoing oxidation in the redox reaction represented by the following cell notation? Pb(s)∣ Pb2+(aq)   H+(aq)∣ H2(g)∣ Pt(s)

Accepted Answer

A) H2(g) 
B) H+(aq) 
C) Pb2+(aq) 
D) Pb(s) 
E) Pt(s) 
A) H2(g) 
B) H+(aq) 
C) Pb2+(aq) 
D) Pb(s) 
E) Pt(s)

Question 18

What is the oxidizing agent in the redox reaction represented by the following cell notation? Ni(s)∣ Ni2+(aq)   Ag+(aq)∣ Ag(s)

Accepted Answer

A) Ni(s) 
B) Ni2+(aq) 
C) Ag+(aq) 
D) Ag(s) 
E) Pt(s) 
A) Ni(s) 
B) Ni2+(aq) 
C) Ag+(aq) 
D) Ag(s) 
E) Pt(s)

Question 19

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.) 3Cl2(g)+ 2Fe(s)→ 6Cl⁻(aq)+ 2Fe3+(aq)
Cl2(g)+ 2 e⁻ → 2Cl⁻(aq)E° = +1.36 V
Fe3+(aq)+ 3 e⁻ → Fe(s)E° = -0.04 V

Accepted Answer

A) +4.16 V 
B) -1.40 V 
C) -1.32 V 
D) +1.32 V 
E) +1.40 V 
A) +4.16 V 
B) -1.40 V 
C) -1.32 V 
D) +1.32 V 
E) +1.40 V

Question 20

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Cd and Ag+ in the balanced reaction? Cd(s)+ Ag+(aq)→ Ag(s)+ Cd2+(aq)

Accepted Answer

A) Cd = 1, Ag⁺ = 2 
B) Cd = 1, Ag⁺ = 1 
C) Cd = 2, Ag⁺ = 1 
D) Cd = 2, Ag⁺ = 2 
E) Cd = 3, Ag⁺ = 1 
A) Cd = 1, Ag⁺ = 2 
B) Cd = 1, Ag⁺ = 1 
C) Cd = 2, Ag⁺ = 1 
D) Cd = 2, Ag⁺ = 2 
E) Cd = 3, Ag⁺ = 1

Exam 18: Electrochemistry

What element is being reduced in the following (unbalanced)redox reaction? Cr(OH)4⁻(aq)+ ClO⁻(aq)→ CrO42-(aq)+ Cl⁻(aq)

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s)+ Ni2+ (aq)→ Zn2+ (aq)+ Ni(s) The emf generated by the cell when [Ni2+] = 2.50 mol L-1 and [Zn2+] = 0.100 mol L-1 is

Why is sugar water not a good conductor of current?

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)∣ Ni2+(aq)∣∣ Cl2(g)∣ Cl-(aq)∣ C(s)

Which of the following is the weakest oxidizing agent?

Which of the following statements is true for the cell diagram below? Zn(s)∣ Zn2+(aq) Cu2+(aq)∣ Cu(s)

Nickel can be plated from aqueous solution according to the following half-reaction. How long would it take (in min)to plate 29.6 g of nickel at 4.7 A? Ni2+(aq)+ 2 e⁻ → Ni(s)

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Al and F2 in the balanced reaction? Al(s)+ F2(g)→ Al3+(aq)+ F-(aq)

Which of the following is the weakest oxidizing agent?

Which of the following is the strongest reducing agent?

A galvanic cell consists of one half-cell that contains Ag(s)and Ag+(aq), and one half-cell that contains Cu(s)and Cu2+(aq). What species are produced at the electrodes under standard conditions? Ag+(aq)+ e- → Ag(s)E° = +0.80 V Cu2+(aq)+ 2 e- → Cu(s)E° = +0.34 V

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H⁺ and Fe3+ in the balanced reaction? Fe2+(aq)+ MnO4⁻(aq)→ Fe3+(aq)+ Mn2+(aq)

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? MnO4⁻ (aq)+ H2C2O4(aq)→ Mn2+(aq)+ CO2(g)

Which of the following metals will dissolve in nitric acid but not hydrochloric acid?

What is undergoing oxidation in the redox reaction represented by the following cell notation? Pb(s)∣ Pb2+(aq) H+(aq)∣ H2(g)∣ Pt(s)

What is the oxidizing agent in the redox reaction represented by the following cell notation? Ni(s)∣ Ni2+(aq) Ag+(aq)∣ Ag(s)

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Cd and Ag+ in the balanced reaction? Cd(s)+ Ag+(aq)→ Ag(s)+ Cd2+(aq)

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What element is being reduced in the following (unbalanced)redox reaction? Cr(OH)₄⁻(aq)+ ClO⁻(aq)→ CrO₄^2-(aq)+ Cl⁻(aq)

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s)+ Ni²⁺ (aq)→ Zn²⁺ (aq)+ Ni(s) The emf generated by the cell when [Ni²⁺] = 2.50 mol L^-1 and [Zn²⁺] = 0.100 mol L^-1 is

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)∣ Ni²⁺(aq)∣∣ Cl₂(g)∣ Cl^-(aq)∣ C(s)

Which of the following statements is true for the cell diagram below? Zn(s)∣ Zn²⁺(aq) Cu²⁺(aq)∣ Cu(s)

Nickel can be plated from aqueous solution according to the following half-reaction. How long would it take (in min)to plate 29.6 g of nickel at 4.7 A? Ni²⁺(aq)+ 2 e⁻ → Ni(s)

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Aland F₂ in the balanced reaction? Al(s)+ F₂(g)→ Al³⁺(aq)+ F^-(aq)

A galvanic cell consists of one half-cell that contains Ag(s)and Ag⁺(aq), and one half-cell that contains Cu(s)and Cu²⁺(aq). What species are produced at the electrodes under standard conditions? Ag⁺(aq)+ e^- → Ag(s)E° = +0.80 V Cu²⁺(aq)+ 2 e^- → Cu(s)E° = +0.34 V

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H⁺and Fe³⁺ in the balanced reaction? Fe²⁺(aq)+ MnO₄⁻(aq)→ Fe³⁺(aq)+ Mn²⁺(aq)

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H₂C₂O₄and H₂O in the balanced reaction? MnO₄⁻ (aq)+ H₂C₂O₄(aq)→ Mn²⁺(aq)+ CO₂(g)

What is undergoing oxidation in the redox reaction represented by the following cell notation? Pb(s)∣ Pb²⁺(aq) H⁺(aq)∣ H₂(g)∣ Pt(s)

What is the oxidizing agent in the redox reaction represented by the following cell notation? Ni(s)∣ Ni²⁺(aq) Ag⁺(aq)∣ Ag(s)

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Cdand Ag⁺ in the balanced reaction? Cd(s)+ Ag⁺(aq)→ Ag(s)+ Cd²⁺(aq)