Question 1

The standard emf for the cell using the overall cell reaction below is +0.48 V: 
 \quad\quad Zn(s) +  Ni2+\mathrm { Ni } ^ { 2 + }Ni2+  (aq) ?  Zn2+\mathrm { Zn } ^ { 2 + }Zn2+  (aq) + Ni(s) 
The emf generated by the cell when [  Ni2+\mathrm { Ni } ^ { 2 + }Ni2+  ] = 6.50 mol L-1 and [  Zn2+\mathrm { Zn } ^ { 2 + }Zn2+  ] = 0.500 mol L-1 is --------  V. 	ext { V. } V.

Accepted Answer

A)  0.55
B)  0.45
C)  0.61
D)  0.50
E)  0.51

Question 2

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? 
 \quad\quad Zn(s) | Zn2+(aq) || Ni2+(aq) | Ni(s)

Accepted Answer

A)  Zn(s) → Zn2+(aq) + 2 e-
B)  Zn2+(aq) + 2 e- → Zn(s) 
C)  Ni(s) → Ni2+(aq) + 2 e-
D)  Ni2+(aq) + 2 e- → Ni(s)

Question 3

What is undergoing reduction in the redox reaction represented by the following cell notation? 
 \quad\quad\quad Fe(s) | Fe3+(aq)   ∥\|∥  Cl2(g) | Cl- (aq) | Pt(s)

Accepted Answer

A)  Fe(s) 
B)  Fe3+(aq) 
C)  Cl2(g) 
D)  Cl- (aq) 
E)  Pt(s)

Question 4

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: 
 \quad\quad\quad Sn(s) | Sn2+(aq,0.022 mol L-1)   ∥\|∥  Ag+(aq,2.7 mol L-1) | Ag(s) 
E°(Sn2+/Sn) = -0.14 V and E°(Ag+/Ag) = +0.80 V

Accepted Answer

A)  +1.01 V
B)  -0.83 V
C)  +1.31 V
D)  +0.01 V
E)  -0.66 V

Question 5

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

Accepted Answer

A)  Pb2+(aq) + Cu(s) ; if E°(Pb2+/Pb) = -0.13V and E°(Cu2+/Cu) = +0.16V
B)  Ag+(aq) + Br- (aq) ; if E°(Ag+/Ag) = 0.80V and E°(Br2/Br-) = +1.09V
C)  Li+(aq) + Al(s) ; if E°(Li+/Li) = -3.04V and E°(Al3+/Al) = -1.66V
D)  Fe3+(aq) + Ni(s) ; if E°(Fe3+/Fe) = -0.04V and E°(Ni2+/Ni) = -0.23V
E)  Cd2+(aq) + I-(aq) ; if E°(Cd2+/Cd) = -0.40V and E°(I2/I-) = + 0.54V

Question 6

Consider the following standard reduction potentials: 
 \quad\quad Ni2+(aq) + 2 e- → Ni(s) E° = -0.26 V
 \quad\quad I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V
Under standard conditions,

Accepted Answer

A)  Ni2+(aq) is a stronger oxidizing agent than I2(s) ,and I-(aq) is a stronger reducing agent than Ni(s) .
B)  I2(s) is a stronger oxidizing agent than Ni2+(aq) ,and Ni(s) is a stronger reducing agent than I-(aq) .
C)  Ni(s) is a stronger oxidizing agent than I-(aq) ,and Ni2+(aq) is a stronger reducing agent than I2(s) .
D)  I-(aq) is a stronger oxidizing agent than Ni(s) ,and I2(s) is a stronger reducing agent than Ni2+(aq) .

Question 7

Which of the following is the strongest oxidizing agent?

Accepted Answer

A)  Br2(l) 
B)  Au3+(aq) 
C)  Ag(s) 
D)  Br- (aq) 
E)  Au(s)

Exam 18: Electrochemistry

Correct Answer
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Which of the following is the strongest oxidizing agent?

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: $\quad$ $\quad$ $\quad$ Sn(s) | Sn²⁺(aq,0.022 mol L^-1) $\|$ Ag⁺(aq,2.7 mol L^-1) | Ag(s) E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

Correct Answer
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What is undergoing reduction in the redox reaction represented by the following cell notation? $\quad$ $\quad$ $\quad$ Fe(s) | Fe³⁺(aq) $\|$ Cl₂(g) | Cl^- (aq) | Pt(s)

Correct Answer
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Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

Correct Answer
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Consider the following standard reduction potentials: $\quad$ $\quad$ Ni²⁺(aq) + 2 e^- → Ni(s) E° = -0.26 V $\quad$ $\quad$ I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V Under standard conditions,

Correct Answer
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For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? $\quad$ $\quad$ Zn(s) | Zn²⁺(aq) || Ni²⁺(aq) | Ni(s)

Correct Answer
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Exam 18: Electrochemistry

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Which of the following is the strongest oxidizing agent?

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: \quad\quad\quad Sn(s) | Sn2+(aq,0.022 mol L-1) ∥\|∥ Ag+(aq,2.7 mol L-1) | Ag(s) E°(Sn2+/Sn) = -0.14 V and E°(Ag+/Ag) = +0.80 V

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What is undergoing reduction in the redox reaction represented by the following cell notation? \quad\quad\quad Fe(s) | Fe3+(aq) ∥\|∥ Cl2(g) | Cl- (aq) | Pt(s)

Correct AnswerverifiedShow Answer

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

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Consider the following standard reduction potentials: \quad\quad Ni2+(aq) + 2 e- → Ni(s) E° = -0.26 V \quad\quad I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V Under standard conditions,

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For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? \quad\quad Zn(s) | Zn2+(aq) || Ni2+(aq) | Ni(s)

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Correct Answer
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Correct Answer
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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: $\quad$ $\quad$ $\quad$ Sn(s) | Sn²⁺(aq,0.022 mol L^-1) $\|$ Ag⁺(aq,2.7 mol L^-1) | Ag(s) E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

Correct Answer
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What is undergoing reduction in the redox reaction represented by the following cell notation? $\quad$ $\quad$ $\quad$ Fe(s) | Fe³⁺(aq) $\|$ Cl₂(g) | Cl^- (aq) | Pt(s)

Correct Answer
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Correct Answer
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Consider the following standard reduction potentials: $\quad$ $\quad$ Ni²⁺(aq) + 2 e^- → Ni(s) E° = -0.26 V $\quad$ $\quad$ I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V Under standard conditions,

Correct Answer
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For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? $\quad$ $\quad$ Zn(s) | Zn²⁺(aq) || Ni²⁺(aq) | Ni(s)

Correct Answer
verified