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Deck 19: Electrochemistry
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A strip of iron is placed in a 1 M solution of iron(II)sulfate,and a strip of copper is placed in a 1 M solution of copper(II)chloride.The two solutions are connected with a salt bridge,and the two metals are connected by a wire.
Reduction Half-Reaction
E° (V)
Fe2+(aq)+ 2e-
Fe(s)
-0)41Cu2+(aq)+ 2e-
Cu(s)
0)34
Which of the following takes place?
A)Sulfur deposits at the iron electrode.
B)The Fe(II)concentration of the iron half-cell decreases.
C)Copper atoms deposit at the cathode.
D)Chlorine is produced at the copper electrode.
E)Chlorine is produced at the iron electrode.
Reduction Half-Reaction
E° (V)
Fe2+(aq)+ 2e-
Fe(s)-0)41Cu2+(aq)+ 2e-
Cu(s)0)34
Which of the following takes place?
A)Sulfur deposits at the iron electrode.
B)The Fe(II)concentration of the iron half-cell decreases.
C)Copper atoms deposit at the cathode.
D)Chlorine is produced at the copper electrode.
E)Chlorine is produced at the iron electrode.
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Which of the following statements is true concerning half-cell I as the voltaic cell shown below discharges? ![<strong>Which of the following statements is true concerning half-cell I as the voltaic cell shown below discharges? </strong> A)[Zn<sup>2+</sup>] increases with time,and [Cl-] increases with time. B)[Zn<sup>2+</sup>] decreases with time,and [Cl-] increases with time. C)[Zn<sup>2+</sup>] decreases with time,and [Cl-] decreases with time. D)[Zn<sup>2+</sup>] decreases with time,and [NO<sub>3</sub>-] increases with time. E)[Zn<sup>2+</sup>] increases with time,and [NO<sub>3</sub>-] increases with time. <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB2288/11ea7a3a_9f3a_6f52_a82d_f3caed6e7299_TB2288_00.jpg)
A)[Zn2+] increases with time,and [Cl-] increases with time.
B)[Zn2+] decreases with time,and [Cl-] increases with time.
C)[Zn2+] decreases with time,and [Cl-] decreases with time.
D)[Zn2+] decreases with time,and [NO3-] increases with time.
E)[Zn2+] increases with time,and [NO3-] increases with time.
A)[Zn2+] increases with time,and [Cl-] increases with time.
B)[Zn2+] decreases with time,and [Cl-] increases with time.
C)[Zn2+] decreases with time,and [Cl-] decreases with time.
D)[Zn2+] decreases with time,and [NO3-] increases with time.
E)[Zn2+] increases with time,and [NO3-] increases with time.
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Which of the following statements is true concerning the voltaic cell shown below? 
A)The Zn anode mass decreases as the cell discharges.
B)The Zn cathode mass increases as the cell discharges.
C)The Zn cathode mass decreases as the cell discharges.
D)The Zn anode mass increases as the cell discharges.
E)The mass of the Zn electrode neither increases nor decreases as the cell discharges.
A)The Zn anode mass decreases as the cell discharges.
B)The Zn cathode mass increases as the cell discharges.
C)The Zn cathode mass decreases as the cell discharges.
D)The Zn anode mass increases as the cell discharges.
E)The mass of the Zn electrode neither increases nor decreases as the cell discharges.
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Balance the following half-reaction occurring in acidic solution.
NO3-(aq)→
A)NO3-(aq)+ 10H+(aq)+ 8e− →
+ 3H2O(l)
B)NO3-(aq)+ 3H2O(l)+ 10e− →
+ 10H+(aq)
C)NO3-(aq)+ 10H+(aq)→
+ 3H2O(l)+ 10e−
D)NO3-(aq)+ 8e− →
+ 8H+(aq)+ 3H2O(l)
E)NO3-(aq)+ 10H+(aq)→
+ 3H2O(l)
NO3-(aq)→
A)NO3-(aq)+ 10H+(aq)+ 8e− →
+ 3H2O(l)B)NO3-(aq)+ 3H2O(l)+ 10e− →
+ 10H+(aq)C)NO3-(aq)+ 10H+(aq)→
+ 3H2O(l)+ 10e−D)NO3-(aq)+ 8e− →
+ 8H+(aq)+ 3H2O(l)E)NO3-(aq)+ 10H+(aq)→
+ 3H2O(l) Question
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Given:
Mn2+(aq)+ 2e-
Mn(s); E° = -1.18 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
Cr2O72-(aq)+ 14H+(aq)+ 6e-
2Cr3+(aq)+ 7H2O(l); E° = 1.33 V
Which of the following species is the strongest reducing agent?
A)Mn
B)Cu
C)Cr3+
D)Mn2+
E)Cr2O72-
Mn2+(aq)+ 2e-
Mn(s); E° = -1.18 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
Cr2O72-(aq)+ 14H+(aq)+ 6e-
2Cr3+(aq)+ 7H2O(l); E° = 1.33 V
Which of the following species is the strongest reducing agent?
A)Mn
B)Cu
C)Cr3+
D)Mn2+
E)Cr2O72-
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The cell potential of an electrochemical cell with the cell reaction
Al(s)+ Cr3+(aq)→ Cr(s)+ Al3+(aq)
Is 1.63 V.What is the maximum electrical work obtainable from this cell when 0.50 g of Al is consumed?
A)
J
B)
J
C)
J
D)
J
E)
J
Al(s)+ Cr3+(aq)→ Cr(s)+ Al3+(aq)
Is 1.63 V.What is the maximum electrical work obtainable from this cell when 0.50 g of Al is consumed?
A)
JB)
JC)
JD)
JE)
J Question
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The cell potential of an electrochemical cell with the cell reaction
2Al(s)+ 3Zn2+(aq)→ 3Zn(s)+ 2Al3+(aq)
Is 1.607 V.What is the maximum electrical work obtainable from this cell when 2.0 mol of Al is consumed?
A)
J
B)
J
C)
J
D)
J
E)
J
2Al(s)+ 3Zn2+(aq)→ 3Zn(s)+ 2Al3+(aq)
Is 1.607 V.What is the maximum electrical work obtainable from this cell when 2.0 mol of Al is consumed?
A)
JB)
JC)
JD)
JE)
J Question
What is the balanced spontaneous reaction and standard cell potential of an electrochemical cell constructed from half cells with the following half reactions?
Cu2+(aq)+ 2e¯ → Cu(s)E° = 0.337 V
E° = -0.130 V
A)Cu2+(aq)+ Pb(s)→ Cu(s)+ Pb2+(aq); 0.467 V
B)Cu(s)+ Pb2+(aq)→ Cu2+(aq)+ Pb(s); −0.467 V
C)Cu2+(aq)+ Pb2+(aq)→ Cu(s)+ Pb(s); 0.207 V
D)Cu2+(aq)+ Pb(s)→ Cu(s)+ Pb2+(aq); 0.234 V
E)Cu(s)+ Pb2+(aq)→ Cu2+(aq)+ Pb(s); −0.234 V
Cu2+(aq)+ 2e¯ → Cu(s)E° = 0.337 V
E° = -0.130 V
A)Cu2+(aq)+ Pb(s)→ Cu(s)+ Pb2+(aq); 0.467 V
B)Cu(s)+ Pb2+(aq)→ Cu2+(aq)+ Pb(s); −0.467 V
C)Cu2+(aq)+ Pb2+(aq)→ Cu(s)+ Pb(s); 0.207 V
D)Cu2+(aq)+ Pb(s)→ Cu(s)+ Pb2+(aq); 0.234 V
E)Cu(s)+ Pb2+(aq)→ Cu2+(aq)+ Pb(s); −0.234 V
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Given:
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
Cr2O72-(aq)+ 14H+(aq)+ 6e-
2Cr3+(aq)+ 7H2O(l); E° = 1.33 V
Which of the following species is the strongest oxidizing agent?
A)Zn
B)Cr3+
C)Cr2O72-
D)Zn2+
E)Cu
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VCr2O72-(aq)+ 14H+(aq)+ 6e-
2Cr3+(aq)+ 7H2O(l); E° = 1.33 VWhich of the following species is the strongest oxidizing agent?
A)Zn
B)Cr3+
C)Cr2O72-
D)Zn2+
E)Cu
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What is the cell notation for the voltaic cell shown below? 
A)Zn2+(aq)| Zn(s)|| Cu2+(aq)| Cu(s)
B)Zn(s)| Zn2+(aq)|| Cu(s)| Cu2+(aq)
C)Zn(s)| Cu(s)|| Zn2+(aq)| Cu2+(aq)
D)Zn(s)| Zn2+(aq)|| Cu2+(aq)| Cu(s)
E)Zn2+(aq)| Zn(s)|| Cu(s)| Cu2+(aq)
A)Zn2+(aq)| Zn(s)|| Cu2+(aq)| Cu(s)
B)Zn(s)| Zn2+(aq)|| Cu(s)| Cu2+(aq)
C)Zn(s)| Cu(s)|| Zn2+(aq)| Cu2+(aq)
D)Zn(s)| Zn2+(aq)|| Cu2+(aq)| Cu(s)
E)Zn2+(aq)| Zn(s)|| Cu(s)| Cu2+(aq)
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Consider the following standard electrode potentials:
Ag+(aq)+ e-
Ag(s); E° = 0.80 V
Mn2+(aq)+ 2e-
Mn(s); E° = -1.18 V
Which of the following statements is false concerning the electrochemical cell given below?
Mn(s)| Mn2+(aq)|| Ag+(aq)| Ag(s)
A)The anode half-cell reaction is Mn(s)→ Mn2+(aq)+ 2e-.
B)The reducing agent is Ag(s).
C)Under standard-state conditions,the cell potential is 1.98 V.
D)The cell potential decreases with time.
E)The oxidizing agent is Ag+(aq).
Ag+(aq)+ e-
Ag(s); E° = 0.80 VMn2+(aq)+ 2e-
Mn(s); E° = -1.18 VWhich of the following statements is false concerning the electrochemical cell given below?
Mn(s)| Mn2+(aq)|| Ag+(aq)| Ag(s)
A)The anode half-cell reaction is Mn(s)→ Mn2+(aq)+ 2e-.
B)The reducing agent is Ag(s).
C)Under standard-state conditions,the cell potential is 1.98 V.
D)The cell potential decreases with time.
E)The oxidizing agent is Ag+(aq).
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What is the cell reaction for the following voltaic cell?
Cr(s)| Cr3+(aq)|| Br-(aq)| Br2(g)| Pt(s)
A)2Cr(s)+ 3Br2(g)
2Cr3+(aq)+ 6Br-(aq)
B)Cr(s)+ Cr3+(aq)
Br-(aq)+ Br2(g)
C)2Cr3+(aq)+ 6Br-(aq)
2Cr(s)+ 3Br2(g)
D)Cr(s)+ 3Br2(g)
Cr3+(s)+ 2Br-(aq)
E)Cr(s)+ 2Br-(aq)
Br2(g)+ Cr3+(aq)
Cr(s)| Cr3+(aq)|| Br-(aq)| Br2(g)| Pt(s)
A)2Cr(s)+ 3Br2(g)
2Cr3+(aq)+ 6Br-(aq)B)Cr(s)+ Cr3+(aq)
Br-(aq)+ Br2(g)C)2Cr3+(aq)+ 6Br-(aq)
2Cr(s)+ 3Br2(g)D)Cr(s)+ 3Br2(g)
Cr3+(s)+ 2Br-(aq)E)Cr(s)+ 2Br-(aq)
Br2(g)+ Cr3+(aq) Question
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Given:
Ni2+(aq)+ 2e-
Ni(s); E° = -0.23 V
2H+(aq)+ 2e-
H2(g); E° = 0.00 VAg+(aq)+ e- 
Ag(s); E° = 0.80 V
NO3-(aq)+ 4H+(aq)+ 3e-
NO(g)+ 2H2O(l); E° = 0.96 V
Which of the following statements is true?
A)Ni2+ reacts spontaneously with 1 M H+(aq)to form H2.
B)Ni2+ reacts spontaneously with H2(g).
C)Ag(s)reacts spontaneously with Ni2+.
D)Ag(s)reacts spontaneously with 1 M NO3- in 1 M H+(aq).
E)Ag(s)reacts spontaneously with 1 M H+(aq).
Ni2+(aq)+ 2e-
Ni(s); E° = -0.23 V2H+(aq)+ 2e-
H2(g); E° = 0.00 VAg+(aq)+ e- Ag(s); E° = 0.80 VNO3-(aq)+ 4H+(aq)+ 3e-
NO(g)+ 2H2O(l); E° = 0.96 VWhich of the following statements is true?
A)Ni2+ reacts spontaneously with 1 M H+(aq)to form H2.
B)Ni2+ reacts spontaneously with H2(g).
C)Ag(s)reacts spontaneously with Ni2+.
D)Ag(s)reacts spontaneously with 1 M NO3- in 1 M H+(aq).
E)Ag(s)reacts spontaneously with 1 M H+(aq).
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Consider the following standard reduction potentials:
2H+(aq)+ 2e-
H2(g); E° = 0.00 V
Sn2+(aq)+ 2e-
Sn(s); E° = -0.15 V
Cd2+(aq)+ 2e-
Cd(s); E° = -0.40 V
Which pair of substances will react spontaneously under standard-state conditions?
A)Cd with H+
B)Cd with Sn
C)Sn2+ with Cd2+
D)Sn with Cd2+
E)Sn2+ with H+
2H+(aq)+ 2e-
H2(g); E° = 0.00 VSn2+(aq)+ 2e-
Sn(s); E° = -0.15 VCd2+(aq)+ 2e-
Cd(s); E° = -0.40 VWhich pair of substances will react spontaneously under standard-state conditions?
A)Cd with H+
B)Cd with Sn
C)Sn2+ with Cd2+
D)Sn with Cd2+
E)Sn2+ with H+
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Given:
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 V
Mg2+(aq)+ 2e-
Mg(s); E° = -2.38 V
Ag+(aq)+ e-
Ag(s); E° = 0.80 V
2H+(aq)+ 2e-
H2(g); E° = 0.00 V
Under standard-state conditions,which of the following species is the best reducing agent?
A)H2
B)Mg2+
C)Ag+
D)Pb
E)Ag
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 VMg2+(aq)+ 2e-
Mg(s); E° = -2.38 VAg+(aq)+ e-
Ag(s); E° = 0.80 V2H+(aq)+ 2e-
H2(g); E° = 0.00 VUnder standard-state conditions,which of the following species is the best reducing agent?
A)H2
B)Mg2+
C)Ag+
D)Pb
E)Ag
Question
Given:
Hg2+(aq)+ 2e-
Hg(s); E° = 0.85 V
Li+(aq)+ e-
Li(s); E° = -3.04 V
Br2(l)+ 2e-
2Br-(aq); E° = 1.07 V
Au+(aq)+ e-
Au(s); E° = 1.69 V
Cl2(g)+ 2e-
2Cl-(aq); E° = 1.36 V
Which of the following species is the best reducing agent?
A)Hg
B)Li+
C)Au
D)Cl-
E)Br-
Hg2+(aq)+ 2e-
Hg(s); E° = 0.85 VLi+(aq)+ e-
Li(s); E° = -3.04 VBr2(l)+ 2e-
2Br-(aq); E° = 1.07 VAu+(aq)+ e-
Au(s); E° = 1.69 VCl2(g)+ 2e-
2Cl-(aq); E° = 1.36 VWhich of the following species is the best reducing agent?
A)Hg
B)Li+
C)Au
D)Cl-
E)Br-
Question
Consider the following standard reduction potentials:
Mg2+(aq)+ 2e-
Mg(s); E° = -2.38 V
V2+(aq)+ 2e-
V(s); E° = -1.18 V
Cu2+(aq)+ e-
Cu+(aq); E° = 0.15 V
Which of the following reactions will proceed spontaneously from left to right under standard-state conditions?
A)Mg(s)+ 2Cu2+(aq)→ Mg2+(aq)+ 2Cu+(aq)
B)V2+(aq)+ 2Cu+(aq)→ V(s)+ 2Cu2+(aq)
C)Mg2+(aq)+ 2Cu+(aq)→ 2Cu2+(aq)+ Mg(s)
D)Mg2+(aq)+ V(s)→ V2+(aq)+ Mg(s)
E)2Cu2+(aq)+ 2Cu+(aq)→ Mg2+(aq)+ Mg(s)
Mg2+(aq)+ 2e-
Mg(s); E° = -2.38 V
V2+(aq)+ 2e-
V(s); E° = -1.18 V
Cu2+(aq)+ e-
Cu+(aq); E° = 0.15 V
Which of the following reactions will proceed spontaneously from left to right under standard-state conditions?
A)Mg(s)+ 2Cu2+(aq)→ Mg2+(aq)+ 2Cu+(aq)
B)V2+(aq)+ 2Cu+(aq)→ V(s)+ 2Cu2+(aq)
C)Mg2+(aq)+ 2Cu+(aq)→ 2Cu2+(aq)+ Mg(s)
D)Mg2+(aq)+ V(s)→ V2+(aq)+ Mg(s)
E)2Cu2+(aq)+ 2Cu+(aq)→ Mg2+(aq)+ Mg(s)
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What is E°cell for the cell reaction 2Cr(s)+ 3Sn4+ (aq)→ 3Sn2+(aq)+ 2Cr3+ (aq)?
Cr3+ (aq)+ 3e-
Cr(s); E° = -0.74V 
A)0.89V
B)-0.59V
C)
D)
E)0.59V
Cr3+ (aq)+ 3e-
Cr(s); E° = -0.74V
A)0.89V
B)-0.59V
C)
D)
E)0.59V
Question
Given:
W3+(aq)+ 3e-
W(s); E° = 2.72 V
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 V
Ni2+(aq)+ 2e-
Ni(s); E° = -0.23 V
Cd2+(aq)+ 2e-
Cd(s); E° = -0.40 V
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 V
Al3+(aq)+ 3e-
Al(s); E° = -1.66 V
Mg2+(aq)+ 2e-
Mg(s); E° = -2.38 V
Under standard-state conditions,which of the following metals will reduce W3+ to W but will not reduce Ni2+ to Ni?
A)Cd
B)Pb
C)Al
D)Zn
E)Mg
W3+(aq)+ 3e-
W(s); E° = 2.72 VPb2+(aq)+ 2e-
Pb(s); E° = -0.13 VNi2+(aq)+ 2e-
Ni(s); E° = -0.23 VCd2+(aq)+ 2e-
Cd(s); E° = -0.40 VZn2+(aq)+ 2e-
Zn(s); E° = -0.76 VAl3+(aq)+ 3e-
Al(s); E° = -1.66 VMg2+(aq)+ 2e-
Mg(s); E° = -2.38 VUnder standard-state conditions,which of the following metals will reduce W3+ to W but will not reduce Ni2+ to Ni?
A)Cd
B)Pb
C)Al
D)Zn
E)Mg
Question
Given:
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 V
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 V
Al3+(aq)+ 3e-
Al(s); E° = -1.66 V
Mg2+(aq)+ 2e-
Mg(s); E° = -2.38 V
V2+(aq)+ 2e-
V(s); E° = -1.18 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
Which of the following cations is capable of oxidizing Pb to Pb2+ under standard-state conditions?
A)Al3+
B)V2+
C)Cu2+
D)Mg2+
E)Zn2+
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 VZn2+(aq)+ 2e-
Zn(s); E° = -0.76 VAl3+(aq)+ 3e-
Al(s); E° = -1.66 VMg2+(aq)+ 2e-
Mg(s); E° = -2.38 VV2+(aq)+ 2e-
V(s); E° = -1.18 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VWhich of the following cations is capable of oxidizing Pb to Pb2+ under standard-state conditions?
A)Al3+
B)V2+
C)Cu2+
D)Mg2+
E)Zn2+
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Given:
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 V
2H+(aq)+ 2e-
H2(g); E° = 0.00 V
I2(s)+ 2e-
2I-(aq); E° = 0.54 V
Br2(l)+ 2e-
2Br-(aq); E° = 1.07 V
Ni2+(aq)+ 2e-
Ni(s); E° = -0.23 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
Which of the following species will oxidize Ni but not Cu?
A)Zn2+
B)Br-
C)H+
D)I2
E)Zn
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 V2H+(aq)+ 2e-
H2(g); E° = 0.00 VI2(s)+ 2e-
2I-(aq); E° = 0.54 VBr2(l)+ 2e-
2Br-(aq); E° = 1.07 VNi2+(aq)+ 2e-
Ni(s); E° = -0.23 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VWhich of the following species will oxidize Ni but not Cu?
A)Zn2+
B)Br-
C)H+
D)I2
E)Zn
Question
Given:
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 V
Co2+(aq)+ 2e-
Co(s); E° = -0.28 V
Sn2+(aq)+ 2e-
Sn(s); E° = -0.15 V
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 V
Fe3+(aq)+ e-
Fe2+(aq); E° = 0.77 V
Under standard-state conditions,which of the following pairs of elements or ions is capable of reducing Sn2+(aq)to Sn(s)?
A)Zn(s)or Co(s)
B)Pb(s)or Fe2+(aq)
C)Co(s)or Pb(s)
D)Fe2+(aq)or Zn(s)
E)Zn2+(aq)or Co2+(aq)
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 VCo2+(aq)+ 2e-
Co(s); E° = -0.28 VSn2+(aq)+ 2e-
Sn(s); E° = -0.15 VPb2+(aq)+ 2e-
Pb(s); E° = -0.13 VFe3+(aq)+ e-
Fe2+(aq); E° = 0.77 VUnder standard-state conditions,which of the following pairs of elements or ions is capable of reducing Sn2+(aq)to Sn(s)?
A)Zn(s)or Co(s)
B)Pb(s)or Fe2+(aq)
C)Co(s)or Pb(s)
D)Fe2+(aq)or Zn(s)
E)Zn2+(aq)or Co2+(aq)
Question
Consider the following cell reaction:
2Cr(s)+ 6H+(aq)→ 2Cr3+(aq)+ 3H2(g); E°cell = 0.74V
Under standard-state conditions,what is E° for the following half-reaction?
Cr3+(aq)+ 3e− → Cr(s)
A)-0.74 V
B)
C)-0.37 V
D)0.37 V
E)0.74 V
2Cr(s)+ 6H+(aq)→ 2Cr3+(aq)+ 3H2(g); E°cell = 0.74V
Under standard-state conditions,what is E° for the following half-reaction?
Cr3+(aq)+ 3e− → Cr(s)
A)-0.74 V
B)
C)-0.37 V
D)0.37 V
E)0.74 V
Question
Given:
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 V
2H+(aq)+ 2e-
H2(g); E° = 0.00 V
NO3-(aq)+4H+(aq)+ 3e-
NO(g)+ 2H2O(l); E° = 0.96 V
O2(g)+ 4H+(aq)+ 4e-
2H2O(l); E° = 1.23 V
PbO2(s)+ SO42-(aq)+ 4H+(aq)+ 2e-
PbSO4(s)+ 2H2O(l); E° = 1.69 V
Under standard-state conditions,which of the following is the best oxidizing agent?
A)H+
B)Pb2+
C)PbO2
D)O2
E)NO3-
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 V2H+(aq)+ 2e-
H2(g); E° = 0.00 VNO3-(aq)+4H+(aq)+ 3e-
NO(g)+ 2H2O(l); E° = 0.96 VO2(g)+ 4H+(aq)+ 4e-
2H2O(l); E° = 1.23 VPbO2(s)+ SO42-(aq)+ 4H+(aq)+ 2e-
PbSO4(s)+ 2H2O(l); E° = 1.69 VUnder standard-state conditions,which of the following is the best oxidizing agent?
A)H+
B)Pb2+
C)PbO2
D)O2
E)NO3-
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Question
Consider the following reduction potentials:
Cd2+(aq)+ 2e-
Cd(s); E° = -0.40 V
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
Br2(l)+ 2e-
2Br-(aq); E° = 1.07 V
Under standard-state conditions,which of the following reactions is spontaneous?
A)Cd2+(aq)+ Pb(s)→ Cd(s)+ Pb2+(aq)
B)Pb2+(aq)+ Cu(s)→ Pb(s)+ Cu2+(aq)
C)2Br-(aq)+ Pb2+(aq)→ Br2(l)+ Pb(s)
D)2Br-(aq)+ Cu2+(aq)→ Br2(l)+ Cu(s)
E)Cu2+(aq)+ Cd(s)→ Cu(s)+ Cd2+(aq)
Cd2+(aq)+ 2e-
Cd(s); E° = -0.40 VPb2+(aq)+ 2e-
Pb(s); E° = -0.13 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VBr2(l)+ 2e-
2Br-(aq); E° = 1.07 VUnder standard-state conditions,which of the following reactions is spontaneous?
A)Cd2+(aq)+ Pb(s)→ Cd(s)+ Pb2+(aq)
B)Pb2+(aq)+ Cu(s)→ Pb(s)+ Cu2+(aq)
C)2Br-(aq)+ Pb2+(aq)→ Br2(l)+ Pb(s)
D)2Br-(aq)+ Cu2+(aq)→ Br2(l)+ Cu(s)
E)Cu2+(aq)+ Cd(s)→ Cu(s)+ Cd2+(aq)
Question
Question
Given:
Li+(aq)+ e-
Li(s); E° = -3.04 V
Mg2+(aq)+ 2e-
Mg(s); E° = -2.38 V
Fe2+(aq)+ 2e-
Fe(s); E° = -0.41 V
Ag+(aq)+ e-
Ag(s); E° = 0.80 V
Br2(l)+ 2e-
2Br-(aq); E° = 1.07 V
Which of the following species is the best oxidizing agent?
A)Mg2+
B)Br-
C)Fe2+
D)Li
E)Ag+
Li+(aq)+ e-
Li(s); E° = -3.04 VMg2+(aq)+ 2e-
Mg(s); E° = -2.38 VFe2+(aq)+ 2e-
Fe(s); E° = -0.41 VAg+(aq)+ e-
Ag(s); E° = 0.80 VBr2(l)+ 2e-
2Br-(aq); E° = 1.07 VWhich of the following species is the best oxidizing agent?
A)Mg2+
B)Br-
C)Fe2+
D)Li
E)Ag+
Question
Given:
2H+(aq)+ 2e-
H2(g); E° = 0.00 V
K+(aq)+ e-
K(s); E° = 2.7182818285 V
F2(g)+ 2e-
2FS1U1
1-(aq); E° = 2.87 V
Al3+(aq)+ 3e-
Al(s); E° = -1.66 V
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 V
Under standard-state conditions,which is the strongest reducing agent?
A)Pb2+
B)Al3+
C)F-
D)K
E)H+
2H+(aq)+ 2e-
H2(g); E° = 0.00 VK+(aq)+ e-
K(s); E° = 2.7182818285 VF2(g)+ 2e-
2FS1U11-(aq); E° = 2.87 V
Al3+(aq)+ 3e-
Al(s); E° = -1.66 VPb2+(aq)+ 2e-
Pb(s); E° = -0.13 VUnder standard-state conditions,which is the strongest reducing agent?
A)Pb2+
B)Al3+
C)F-
D)K
E)H+
Question
Given:
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 V
Cr3+(aq)+ 3e-
Cr(s); E° = -0.74 V
Fe2+(aq)+ 2e-
Fe(s); E° = -0.41 V
Cd2+(aq)+ 2e-
Cd(s); E° = -0.40 V
Sn2+(aq)+ 2e-
Sn(s); E° = -0.15 V
Hg2+(aq)+ 2e-
Hg(s); E° = 0.85 V
Au+(aq)+ e-
Au(s); E° = 1.69 V
Under standard-state conditions,which of the following metals will reduce Hg2+ to Hg but will not reduce Cd2+ to Cd?
A)Cr
B)Zn
C)Fe
D)Sn
E)Au
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 VCr3+(aq)+ 3e-
Cr(s); E° = -0.74 VFe2+(aq)+ 2e-
Fe(s); E° = -0.41 VCd2+(aq)+ 2e-
Cd(s); E° = -0.40 VSn2+(aq)+ 2e-
Sn(s); E° = -0.15 VHg2+(aq)+ 2e-
Hg(s); E° = 0.85 VAu+(aq)+ e-
Au(s); E° = 1.69 VUnder standard-state conditions,which of the following metals will reduce Hg2+ to Hg but will not reduce Cd2+ to Cd?
A)Cr
B)Zn
C)Fe
D)Sn
E)Au
Question
Given: 
Cl2 (g)+ 2e¯
2Cl¯ (aq); Eº = 1.36V
What is
For the following cell reaction?
2AlCl3(aq)
2Al(s)+ 3Cl2(g)
A)-5.8 × 105 J
B)5.8 × 105 J
C)
D)-1.7 × 106 J
E)1.7 × 106 J
Cl2 (g)+ 2e¯
2Cl¯ (aq); Eº = 1.36VWhat is
For the following cell reaction?
2AlCl3(aq)
2Al(s)+ 3Cl2(g)A)-5.8 × 105 J
B)5.8 × 105 J
C)
D)-1.7 × 106 J
E)1.7 × 106 J
Question
The cell potential of the following cell is determined using an unspecified concentration of acid.What is [H+] given that the measured cell potential is -0.464 V and the anode reduction potential (E°)is 0.222 V at 25°C?
Ag(s)| AgCl(s)| Cl−(1.0 M)|| H+(aq,? M)| H2(g,1.0 atm)| Pt(s)
A)![<strong>The cell potential of the following cell is determined using an unspecified concentration of acid.What is [H<sup>+</sup>] given that the measured cell potential is -0.464 V and the anode reduction potential (E°)is 0.222 V at 25°C? Ag(s)| AgCl(s)| Cl−(1.0 M)|| H<sup>+</sup>(aq,? M)| H<sub>2</sub>(g,1.0 atm)| Pt(s)</strong> A) M B) M C) M D) M E) M <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB2288/11ea7a3a_9f43_6f8e_a82d_49fc1b032c3c_TB2288_11.jpg)
M
B)![<strong>The cell potential of the following cell is determined using an unspecified concentration of acid.What is [H<sup>+</sup>] given that the measured cell potential is -0.464 V and the anode reduction potential (E°)is 0.222 V at 25°C? Ag(s)| AgCl(s)| Cl−(1.0 M)|| H<sup>+</sup>(aq,? M)| H<sub>2</sub>(g,1.0 atm)| Pt(s)</strong> A) M B) M C) M D) M E) M <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB2288/11ea7a3a_9f43_6f8f_a82d_2961b83b13e1_TB2288_11.jpg)
M
C)![<strong>The cell potential of the following cell is determined using an unspecified concentration of acid.What is [H<sup>+</sup>] given that the measured cell potential is -0.464 V and the anode reduction potential (E°)is 0.222 V at 25°C? Ag(s)| AgCl(s)| Cl−(1.0 M)|| H<sup>+</sup>(aq,? M)| H<sub>2</sub>(g,1.0 atm)| Pt(s)</strong> A) M B) M C) M D) M E) M <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB2288/11ea7a3a_9f43_96a0_a82d_4f0aa18fb8a5_TB2288_11.jpg)
M
D)![<strong>The cell potential of the following cell is determined using an unspecified concentration of acid.What is [H<sup>+</sup>] given that the measured cell potential is -0.464 V and the anode reduction potential (E°)is 0.222 V at 25°C? Ag(s)| AgCl(s)| Cl−(1.0 M)|| H<sup>+</sup>(aq,? M)| H<sub>2</sub>(g,1.0 atm)| Pt(s)</strong> A) M B) M C) M D) M E) M <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB2288/11ea7a3a_9f43_96a1_a82d_67c4968829e6_TB2288_11.jpg)
M
E)![<strong>The cell potential of the following cell is determined using an unspecified concentration of acid.What is [H<sup>+</sup>] given that the measured cell potential is -0.464 V and the anode reduction potential (E°)is 0.222 V at 25°C? Ag(s)| AgCl(s)| Cl−(1.0 M)|| H<sup>+</sup>(aq,? M)| H<sub>2</sub>(g,1.0 atm)| Pt(s)</strong> A) M B) M C) M D) M E) M <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB2288/11ea7a3a_9f43_96a2_a82d_6b70702b703a_TB2288_11.jpg)
M
Ag(s)| AgCl(s)| Cl−(1.0 M)|| H+(aq,? M)| H2(g,1.0 atm)| Pt(s)
A)
MB)
MC)
MD)
ME)
M Question
If the cell is initially at standard-state conditions,which of the following statements is true? 
Zn2+(aq)+ 2e- 
Zn(s); E° = -0.76 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
A)Initially
,and it will become more positive with time.
B)Initially
,and it will not change with time.
C)Initially
,and it will become more negative with time.
D)Initially
,and it will become more positive with time.
E)Initially
,and it will become more negative with time.
Zn2+(aq)+ 2e- Zn(s); E° = -0.76 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VA)Initially
,and it will become more positive with time.B)Initially
,and it will not change with time.C)Initially
,and it will become more negative with time.D)Initially
,and it will become more positive with time.E)Initially
,and it will become more negative with time. Question
What is the logarithm of the equilibrium constant,log K,at 25°C of the voltaic cell constructed from the following two half-reactions?
Fe2+ (aq)+ 2e¯
Fe(s); E° = - 0.41V
Ag+(aq)+ e-
Ag(s); E° = 0.80 V
A)6.7
B)40.9
C)20.3
D)13.2
E)67.6
Fe2+ (aq)+ 2e¯
Fe(s); E° = - 0.41VAg+(aq)+ e-
Ag(s); E° = 0.80 VA)6.7
B)40.9
C)20.3
D)13.2
E)67.6
Question
Question
Question
Given: 
Pb2+ (aq)+ 2e-
Pb(s); Eº = -0.13 V
What is the standard cell potential for the following reaction?
2Cr(s)+ 3Pb2+ (aq)→ 3Pb(s)+ 2Cr3+ (aq)
A)-0.87V
B)
C)-0.61V
D)0.61V
E)0.87V
Pb2+ (aq)+ 2e-
Pb(s); Eº = -0.13 VWhat is the standard cell potential for the following reaction?
2Cr(s)+ 3Pb2+ (aq)→ 3Pb(s)+ 2Cr3+ (aq)
A)-0.87V
B)
C)-0.61V
D)0.61V
E)0.87V
Question
Question
Given: 
Pb2+ (aq)+ 2e¯
Pb(s); Eº = -0.13V
What is the standard Gibbs free-energy change for the following reaction?
2Cr(s)+ 3Pb2+ (aq)→ 3Pb(s)+ 2Cr3+ (aq)
A)353kJ
B)118kJ
C)
D)-353kJ
E)
Pb2+ (aq)+ 2e¯
Pb(s); Eº = -0.13VWhat is the standard Gibbs free-energy change for the following reaction?
2Cr(s)+ 3Pb2+ (aq)→ 3Pb(s)+ 2Cr3+ (aq)
A)353kJ
B)118kJ
C)
D)-353kJ
E)
Question
Which of the following statements is true concerning the electrochemical cell depicted below?
Zn | Zn2+(aq)|| Cu2+(aq)| Cu
Zn2+(aq)+ 2e−
Zn(s); E° = -2.87 V
Cu2+(aq)+ 2e−
Cu(s); E° = -2.38 V
A)The cell is at equilibrium.
B)The cell reaction is spontaneous with a standard cell potential of 0.49 V.
C)The cell reaction is spontaneous with a standard cell potential of 5.25 V.
D)The cell reaction is nonspontaneous with a standard cell potential of -5.25 V.
E)The cell reaction is nonspontaneous with a standard cell potential of -0.49 V.
Zn | Zn2+(aq)|| Cu2+(aq)| Cu
Zn2+(aq)+ 2e−
Zn(s); E° = -2.87 VCu2+(aq)+ 2e−
Cu(s); E° = -2.38 VA)The cell is at equilibrium.
B)The cell reaction is spontaneous with a standard cell potential of 0.49 V.
C)The cell reaction is spontaneous with a standard cell potential of 5.25 V.
D)The cell reaction is nonspontaneous with a standard cell potential of -5.25 V.
E)The cell reaction is nonspontaneous with a standard cell potential of -0.49 V.
Question
Question
Question
A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+ concentration is 2.0 × 10-5 M and by placing a Pt electrode in the other compartment,in which the H+ concentration is 3.4 M and 
= 1.00 atm.The Fe2+/Fe half-cell reduction potential is -0.41 V,and the H+/H2 half-cell reduction potential is 0.00 V.What is the value of E° for this cell,and which electrode is the anode?
A)0.41 V,Fe
B)0.90 V,Pt
C)-0.41 V,Pt
D)-0.41 V,Fe
E)0.41 V,Pt
= 1.00 atm.The Fe2+/Fe half-cell reduction potential is -0.41 V,and the H+/H2 half-cell reduction potential is 0.00 V.What is the value of E° for this cell,and which electrode is the anode?A)0.41 V,Fe
B)0.90 V,Pt
C)-0.41 V,Pt
D)-0.41 V,Fe
E)0.41 V,Pt
Question
Question
Which of the following statements is true concerning the hypthetical electrochemical cell depicted below? (M1 and M2 are differing metals)
M1 | M12+(aq)|| M2+(aq)| M2
M12+(aq)+ 2e−
M1(s); E° = -2.91 V
M22+(aq)+ e−
M2(s); E° = -2.98 V
A)The cell reaction is nonspontaneous with a standard cell potential of -0.07 V.
B)The cell reaction is spontaneous with a standard cell potential of 5.89 V.
C)The cell is at equilibrium.
D)The cell reaction is spontaneous with a standard cell potential of 0.07 V.
E)The cell reaction is nonspontaneous with a standard cell potential of -5.89 V.
M1 | M12+(aq)|| M2+(aq)| M2
M12+(aq)+ 2e−
M1(s); E° = -2.91 VM22+(aq)+ e−
M2(s); E° = -2.98 VA)The cell reaction is nonspontaneous with a standard cell potential of -0.07 V.
B)The cell reaction is spontaneous with a standard cell potential of 5.89 V.
C)The cell is at equilibrium.
D)The cell reaction is spontaneous with a standard cell potential of 0.07 V.
E)The cell reaction is nonspontaneous with a standard cell potential of -5.89 V.
Question
Question
If E°cell for a certain reaction is 1 V (n = 4),and ΔS° is 11.2 J/(K⋅mol),what is ΔH° in units of J/mol at 25°C?
A)
× 105 J/mol
B)
× 105 J/mol
C)
× 105 J/mol
D)
× 104 J/mol
E)
J/mol
A)
× 105 J/molB)
× 105 J/molC)
× 105 J/molD)
× 104 J/molE)
J/mol Question
Question
Question
If the cell is initially at standard-state conditions,which of the following statements is true? 
Zn2+(aq)+ 2e- 
Zn(s); E° = -0.76 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
A)Initially Kc = 2 × 10-37,and it decreases with time.
B)Initially Kc = 2 × 1037,and it does not change with time.
C)Initially Kc = 2 × 1037,and it decreases with time.
D)Initially Kc = 2 × 1037,and it increases with time.
E)Initially Kc = 2 × 10-37,and it increases with time.
Zn2+(aq)+ 2e- Zn(s); E° = -0.76 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VA)Initially Kc = 2 × 10-37,and it decreases with time.
B)Initially Kc = 2 × 1037,and it does not change with time.
C)Initially Kc = 2 × 1037,and it decreases with time.
D)Initially Kc = 2 × 1037,and it increases with time.
E)Initially Kc = 2 × 10-37,and it increases with time.
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Deck 19: Electrochemistry
1
Which of the following cell reactions would require the use of an inert electrode?
A)Cu(s)+ 2Ag+(aq)→ 2Ag(s)+ Cu2+(aq)
B)3Fe(s)+ 2Au3+(aq)→ 3Fe2+ + 2Au(s)
C)Zn(s)+ 2Ag+(aq)→ Zn2+(aq)+ 2Ag(s)
D)Ni(s)+ 2MnO2(s)+ 2NH4+(aq)→ Ni2+(aq)+ Mn2O3(s)+ 2NH3(aq)+ H2O(l)
E)3Zn2+(aq)+ 2Al(s)→ 3Zn(s)+ 2Al3+(aq)
A)Cu(s)+ 2Ag+(aq)→ 2Ag(s)+ Cu2+(aq)
B)3Fe(s)+ 2Au3+(aq)→ 3Fe2+ + 2Au(s)
C)Zn(s)+ 2Ag+(aq)→ Zn2+(aq)+ 2Ag(s)
D)Ni(s)+ 2MnO2(s)+ 2NH4+(aq)→ Ni2+(aq)+ Mn2O3(s)+ 2NH3(aq)+ H2O(l)
E)3Zn2+(aq)+ 2Al(s)→ 3Zn(s)+ 2Al3+(aq)
Ni(s)+ 2MnO2(s)+ 2NH4+(aq)→ Ni2+(aq)+ Mn2O3(s)+ 2NH3(aq)+ H2O(l)
2
When the following oxidation-reduction reaction in basic solution is balanced,what is the lowest whole-number coefficient for OH-,and on which side of the balanced equation should it appear?
Cr2O3(s)→ Cr(OH)2(aq)+ CrO42-(aq)
A)2,reactant side
B)10,product side
C)4,product side
D)4,reactant side
E)2,product side
Cr2O3(s)→ Cr(OH)2(aq)+ CrO42-(aq)
A)2,reactant side
B)10,product side
C)4,product side
D)4,reactant side
E)2,product side
2,reactant side
3
Which statement concerning the anode in an electrochemical cell is correct?
A)Metal ions may be deposited as metal atoms on the anode during cell discharge.
B)When connected to an external circuit,the anode develops a positive charge.
C)Reduction occurs at the anode during cell discharge.
D)Positive ions flow towards the anode during cell discharge.
E)None of the above.
A)Metal ions may be deposited as metal atoms on the anode during cell discharge.
B)When connected to an external circuit,the anode develops a positive charge.
C)Reduction occurs at the anode during cell discharge.
D)Positive ions flow towards the anode during cell discharge.
E)None of the above.
None of the above.
4
When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for Rb+(aq)?
Rb(s)+ Sr2+(aq)→ Rb+(aq)+ Sr(s)
A)5
B)4
C)1
D)3
E)2
Rb(s)+ Sr2+(aq)→ Rb+(aq)+ Sr(s)
A)5
B)4
C)1
D)3
E)2
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5
A strip of iron is placed in a 1 M solution of iron(II)sulfate,and a strip of copper is placed in a 1 M solution of copper(II)chloride.The two solutions are connected with a salt bridge,and the two metals are connected by a wire.
Reduction Half-Reaction
E° (V)
Fe2+(aq)+ 2e-Fe(s)
-0)41Cu2+(aq)+ 2e-Cu(s)
0)34
Which of the following takes place?
A)Sulfur deposits at the iron electrode.
B)The Fe(II)concentration of the iron half-cell decreases.
C)Copper atoms deposit at the cathode.
D)Chlorine is produced at the copper electrode.
E)Chlorine is produced at the iron electrode.
Reduction Half-Reaction
E° (V)
Fe2+(aq)+ 2e-
Fe(s)-0)41Cu2+(aq)+ 2e-
Cu(s)0)34
Which of the following takes place?
A)Sulfur deposits at the iron electrode.
B)The Fe(II)concentration of the iron half-cell decreases.
C)Copper atoms deposit at the cathode.
D)Chlorine is produced at the copper electrode.
E)Chlorine is produced at the iron electrode.
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6
Which reaction would be most likely to occur at the anode of a voltaic cell?
A)PbSO4(s)+ 2e- → Pb(s)+ SO42-(aq)
B)2H2O(l)+ 2e- → H2(g)+ 2OH-(aq)
C)2H2O(l)→ O2(g)+ 4H+(aq)+ 4e-
D)PbSO4(s)→ Pb2+(aq)+ SO42-(aq)
E)2H2O(l)→ 2H2(g)+ O2(g)
A)PbSO4(s)+ 2e- → Pb(s)+ SO42-(aq)
B)2H2O(l)+ 2e- → H2(g)+ 2OH-(aq)
C)2H2O(l)→ O2(g)+ 4H+(aq)+ 4e-
D)PbSO4(s)→ Pb2+(aq)+ SO42-(aq)
E)2H2O(l)→ 2H2(g)+ O2(g)
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7
Balance the following oxidation-reduction occurring in acidic solution.
MnO4-(aq)+ Co2+(aq)→ Mn2+(aq)+ Co3+(aq)
A)MnO4-(aq)+ 8H+(aq)+ 5Co2+(aq)→ Mn2+(aq)+ 4H2O(aq)+ 5Co3+(aq)
B)MnO4-(aq)+ 8H+(aq)+ Co2+(aq)→ Mn2+(aq)+ 4H2O(aq)+ Co3+(aq)
C)MnO4-(aq)+ 4H2(g)+ 5Co2+(aq)→ Mn2+(aq)+ 4H2O(aq)+ 5Co3+(aq)
D)MnO4-(aq)+ 8H+(aq)+ 2Co2+(aq)→ Mn2+(aq)+ 4H2O(aq)+ 2Co3+(aq)
E)MnO4-(aq)+ Co2+(aq)→ Mn2+(aq)+ 2O2(g)+ Co3+(aq)
MnO4-(aq)+ Co2+(aq)→ Mn2+(aq)+ Co3+(aq)
A)MnO4-(aq)+ 8H+(aq)+ 5Co2+(aq)→ Mn2+(aq)+ 4H2O(aq)+ 5Co3+(aq)
B)MnO4-(aq)+ 8H+(aq)+ Co2+(aq)→ Mn2+(aq)+ 4H2O(aq)+ Co3+(aq)
C)MnO4-(aq)+ 4H2(g)+ 5Co2+(aq)→ Mn2+(aq)+ 4H2O(aq)+ 5Co3+(aq)
D)MnO4-(aq)+ 8H+(aq)+ 2Co2+(aq)→ Mn2+(aq)+ 4H2O(aq)+ 2Co3+(aq)
E)MnO4-(aq)+ Co2+(aq)→ Mn2+(aq)+ 2O2(g)+ Co3+(aq)
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8
Balance the following half-reaction occurring in basic solution.
MnO2(s)→ Mn(OH)2(s)
A)MnO2(s)+ 2H2O(l)+ 2e−→ Mn(OH)2(s)+ 2OH−(aq)
B)MnO2(s)+ 2H2O(l)+ 4e−→ Mn(OH)2(s)+ (OH)2−(aq)
C)MnO2(s)+ H22+(aq)+ 2e−→ Mn(OH)2(s)
D)MnO2(s)+ H2(g)→ Mn(OH)2(s)+ 2e−
E)MnO2(s)+ 2H2O(l)→ Mn(OH)2(s)+ 2OH−(aq)
MnO2(s)→ Mn(OH)2(s)
A)MnO2(s)+ 2H2O(l)+ 2e−→ Mn(OH)2(s)+ 2OH−(aq)
B)MnO2(s)+ 2H2O(l)+ 4e−→ Mn(OH)2(s)+ (OH)2−(aq)
C)MnO2(s)+ H22+(aq)+ 2e−→ Mn(OH)2(s)
D)MnO2(s)+ H2(g)→ Mn(OH)2(s)+ 2e−
E)MnO2(s)+ 2H2O(l)→ Mn(OH)2(s)+ 2OH−(aq)
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9
The following reactions take place in a lead storage battery.
Discharging: Pb(s)+ PbO2(s)+ 4H+(aq)+ 2SO42-(aq)→ 2PbSO4(s)+ 2H2O(l)
Charging: 2PbSO4(s)+ 2H2O(l)→ Pb(s)+ PbO2(s)+ 4H+(aq)+ 2SO42-(aq)
Which of the following statements is true?
A)The concentration of H2SO4 increases as the battery discharges.
B)Pb is formed at the anode during discharge.
C)Pb is formed at the cathode during charging.
D)The mass of Pb decreases during charging.
E)The mass of PbSO4 remains constant during charging and discharging.
Discharging: Pb(s)+ PbO2(s)+ 4H+(aq)+ 2SO42-(aq)→ 2PbSO4(s)+ 2H2O(l)
Charging: 2PbSO4(s)+ 2H2O(l)→ Pb(s)+ PbO2(s)+ 4H+(aq)+ 2SO42-(aq)
Which of the following statements is true?
A)The concentration of H2SO4 increases as the battery discharges.
B)Pb is formed at the anode during discharge.
C)Pb is formed at the cathode during charging.
D)The mass of Pb decreases during charging.
E)The mass of PbSO4 remains constant during charging and discharging.
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10
Which of the following statements is true concerning half-cell I as the voltaic cell shown below discharges?
A)[Zn2+] increases with time,and [Cl-] increases with time.
B)[Zn2+] decreases with time,and [Cl-] increases with time.
C)[Zn2+] decreases with time,and [Cl-] decreases with time.
D)[Zn2+] decreases with time,and [NO3-] increases with time.
E)[Zn2+] increases with time,and [NO3-] increases with time.
A)[Zn2+] increases with time,and [Cl-] increases with time.
B)[Zn2+] decreases with time,and [Cl-] increases with time.
C)[Zn2+] decreases with time,and [Cl-] decreases with time.
D)[Zn2+] decreases with time,and [NO3-] increases with time.
E)[Zn2+] increases with time,and [NO3-] increases with time.
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11
When balancing oxidation-reduction reactions in acidic solution by the half-reaction method,the addition of the reactant H+ is required to balance the product
A)O2.
B)OH-.
C)O.
D)H2O.
E)none of these
A)O2.
B)OH-.
C)O.
D)H2O.
E)none of these
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12
When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for H+,and on which side of the balanced equation should it appear?
S2O82-(aq)+ NO(g)→ SO42-(aq)+ NO3-(aq)
A)4,product side
B)8,reactant side
C)12,reactant side
D)8,product side
E)4,reactant side
S2O82-(aq)+ NO(g)→ SO42-(aq)+ NO3-(aq)
A)4,product side
B)8,reactant side
C)12,reactant side
D)8,product side
E)4,reactant side
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13
The anode in a voltaic cell and in an electrolytic cell is
A)the site of oxidation and of reduction,respectively.
B)the site of reduction and of oxidation,respectively.
C)positive in both cells.
D)the site of reduction in both cells.
E)the site of oxidation in both cells.
A)the site of oxidation and of reduction,respectively.
B)the site of reduction and of oxidation,respectively.
C)positive in both cells.
D)the site of reduction in both cells.
E)the site of oxidation in both cells.
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14
Which of the following statements is true concerning the voltaic cell shown below?
A)The Zn anode mass decreases as the cell discharges.
B)The Zn cathode mass increases as the cell discharges.
C)The Zn cathode mass decreases as the cell discharges.
D)The Zn anode mass increases as the cell discharges.
E)The mass of the Zn electrode neither increases nor decreases as the cell discharges.
A)The Zn anode mass decreases as the cell discharges.
B)The Zn cathode mass increases as the cell discharges.
C)The Zn cathode mass decreases as the cell discharges.
D)The Zn anode mass increases as the cell discharges.
E)The mass of the Zn electrode neither increases nor decreases as the cell discharges.
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15
The electrochemical reaction which powers a lead-acid storage battery is as follows:
Pb(s)+ PbO2(s)+ 4H+(aq)+ 2SO42-(aq)→ 2PbSO4(s)+ 2H2O(l)
A single cell of this battery consists of a Pb electrode and a PbO2 electrode,each submerged in sulfuric acid.What reaction occurs at the cathode during discharge?
A)Pb(s)is reduced to PbSO4(s).
B)PbO2(s)is reduced to PbSO4(s).
C)PbO2(s)is oxidized to PbSO4(s).
D)Pb(s)is oxidized to PbSO4(s).
E)H+ is oxidized to H2O(l).
Pb(s)+ PbO2(s)+ 4H+(aq)+ 2SO42-(aq)→ 2PbSO4(s)+ 2H2O(l)
A single cell of this battery consists of a Pb electrode and a PbO2 electrode,each submerged in sulfuric acid.What reaction occurs at the cathode during discharge?
A)Pb(s)is reduced to PbSO4(s).
B)PbO2(s)is reduced to PbSO4(s).
C)PbO2(s)is oxidized to PbSO4(s).
D)Pb(s)is oxidized to PbSO4(s).
E)H+ is oxidized to H2O(l).
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16
According to the following cell notation,which species is undergoing oxidation?
Zn | Zn2+(aq)|| Mn2+(aq)| MnO2(s)| Pt(s)
A)Mn2+(aq)
B)Zn2+(aq)
C)MnO2(s)
D)Zn(s)
E)Pt(s)
Zn | Zn2+(aq)|| Mn2+(aq)| MnO2(s)| Pt(s)
A)Mn2+(aq)
B)Zn2+(aq)
C)MnO2(s)
D)Zn(s)
E)Pt(s)
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17
Balance the following half-reaction occurring in acidic solution.
NO3-(aq)→
A)NO3-(aq)+ 10H+(aq)+ 8e− → + 3H2O(l)
B)NO3-(aq)+ 3H2O(l)+ 10e− → + 10H+(aq)
C)NO3-(aq)+ 10H+(aq)→ + 3H2O(l)+ 10e−
D)NO3-(aq)+ 8e− → + 8H+(aq)+ 3H2O(l)
E)NO3-(aq)+ 10H+(aq)→ + 3H2O(l)
NO3-(aq)→
A)NO3-(aq)+ 10H+(aq)+ 8e− →
+ 3H2O(l)B)NO3-(aq)+ 3H2O(l)+ 10e− →
+ 10H+(aq)C)NO3-(aq)+ 10H+(aq)→
+ 3H2O(l)+ 10e−D)NO3-(aq)+ 8e− →
+ 8H+(aq)+ 3H2O(l)E)NO3-(aq)+ 10H+(aq)→
+ 3H2O(l) Unlock Deck
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18
A lead storage battery involves the following two half-reactions:
PbSO4(s)+ 2e- → Pb(s)+ SO42-(aq); E° = -0.36 V
PbO2(s)+ 4H+(aq)+ SO42-(aq)+ 2e- → PbSO4(s)+ 2H2O(l); E° = 1.69 V
During the discharge reaction of the lead storage battery at 1.0 M concentrations,the cell potential and the reducing agent are,respectively,
A)2.05 V and PbO2.
B)-2.05 V and PbO2.
C)1.33 V and Pb.
D)-2.05 V and Pb.
E)2.05 V and Pb.
PbSO4(s)+ 2e- → Pb(s)+ SO42-(aq); E° = -0.36 V
PbO2(s)+ 4H+(aq)+ SO42-(aq)+ 2e- → PbSO4(s)+ 2H2O(l); E° = 1.69 V
During the discharge reaction of the lead storage battery at 1.0 M concentrations,the cell potential and the reducing agent are,respectively,
A)2.05 V and PbO2.
B)-2.05 V and PbO2.
C)1.33 V and Pb.
D)-2.05 V and Pb.
E)2.05 V and Pb.
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19
Which of the following statements is true for a voltaic (galvanic)cell?
A)The electron flow is from the anode to the cathode.
B)The electron flow is from the positive electrode to the negative electrode.
C)The electron flow is from the negative cathode to the positive anode.
D)The electron flow is through the salt bridge.
E)The electron flow is from the oxidizing agent to the reducing agent through an external circuit.
A)The electron flow is from the anode to the cathode.
B)The electron flow is from the positive electrode to the negative electrode.
C)The electron flow is from the negative cathode to the positive anode.
D)The electron flow is through the salt bridge.
E)The electron flow is from the oxidizing agent to the reducing agent through an external circuit.
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20
When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for H+,and on which side of the balanced equation should it appear?
MnO4-(aq)+ I-(aq)→ Mn2+(aq)+ I2(s)
A)1,reactant side
B)2,product side
C)8,reactant side
D)16,reactant side
E)4,product side
MnO4-(aq)+ I-(aq)→ Mn2+(aq)+ I2(s)
A)1,reactant side
B)2,product side
C)8,reactant side
D)16,reactant side
E)4,product side
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21
What is the cell reaction for the following electrochemical cell?
Cu | Cu2+(aq)|| Mn2+(aq)| Mn
A)2Cu(s)+ Mn2+(aq)→ Mn(s)+ 2Cu2+(aq)
B)Cu(s)+ Cu2+(aq)→ Mn(s)+ Mn2+(aq)
C)Cu(s)+ Mn2+(aq)→ Mn(s)+ Cu2+(aq)
D)2Mn(s)+ Cu2+(aq)→ Cu(s)+ 2Mn2+(aq)
E)Mn(s)+ Cu2+(aq)→ Cu(s)+ Mn2+(aq)
Cu | Cu2+(aq)|| Mn2+(aq)| Mn
A)2Cu(s)+ Mn2+(aq)→ Mn(s)+ 2Cu2+(aq)
B)Cu(s)+ Cu2+(aq)→ Mn(s)+ Mn2+(aq)
C)Cu(s)+ Mn2+(aq)→ Mn(s)+ Cu2+(aq)
D)2Mn(s)+ Cu2+(aq)→ Cu(s)+ 2Mn2+(aq)
E)Mn(s)+ Cu2+(aq)→ Cu(s)+ Mn2+(aq)
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22
For a galvanic cell using Fe | Fe2+(1.0 M)and Pb | Pb2+(1.0 M)half-cells,which of the following statements is correct?
Fe2+(aq)+ 2e- → Fe(s); E° = -0.41 V
Pb2+(aq)+ 2e- → Pb(s); E° = -0.13 V
A)The iron electrode is the cathode.
B)When the cell has completely discharged,the concentration of Pb2+ is zero.
C)The mass of the iron electrode increases during discharge.
D)The concentration of Pb2+ decreases during discharge.
E)Electrons leave the lead electrode to pass through the external circuit during discharge.
Fe2+(aq)+ 2e- → Fe(s); E° = -0.41 V
Pb2+(aq)+ 2e- → Pb(s); E° = -0.13 V
A)The iron electrode is the cathode.
B)When the cell has completely discharged,the concentration of Pb2+ is zero.
C)The mass of the iron electrode increases during discharge.
D)The concentration of Pb2+ decreases during discharge.
E)Electrons leave the lead electrode to pass through the external circuit during discharge.
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23
In the following electrochemical cell,what is the role of the platinum?
Cu(s)| Cu2+(aq)|| Fe3+(aq),Fe2+(aq)| Pt(s)
A)The platinum serves as the anode.
B)The oxidation of Fe2+ takes place at the surface of the platinum as the cell discharges.
C)The reduction of Fe3+ takes place at the surface of the platinum as the cell discharges.
D)A and C.
E)A and B.
Cu(s)| Cu2+(aq)|| Fe3+(aq),Fe2+(aq)| Pt(s)
A)The platinum serves as the anode.
B)The oxidation of Fe2+ takes place at the surface of the platinum as the cell discharges.
C)The reduction of Fe3+ takes place at the surface of the platinum as the cell discharges.
D)A and C.
E)A and B.
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24
What is the correct cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Ce4+(aq)+ e− → Ce3+(aq).
A)Pt(s)| H2(g)| H+(aq)|| Ce4+(aq),Ce3+(aq)| Pt(s)
B)Pt(s)| H2(g)| H+(aq)|| Ce4+(aq),Ce3+(aq)
C)Ce3+(aq),Ce4+(aq)|| H+(aq)| H2(g)| Pt(s)
D)Pt(s)| Ce3+(aq),Ce4+(aq)|| H+(aq)| H2(g)| Pt(s)
E)H2(g)| H+(aq)|| Ce3+(aq),Ce4+(aq)
A)Pt(s)| H2(g)| H+(aq)|| Ce4+(aq),Ce3+(aq)| Pt(s)
B)Pt(s)| H2(g)| H+(aq)|| Ce4+(aq),Ce3+(aq)
C)Ce3+(aq),Ce4+(aq)|| H+(aq)| H2(g)| Pt(s)
D)Pt(s)| Ce3+(aq),Ce4+(aq)|| H+(aq)| H2(g)| Pt(s)
E)H2(g)| H+(aq)|| Ce3+(aq),Ce4+(aq)
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25
What is the SI unit of potential difference?
A)coulomb
B)farad
C)volt
D)joule
E)ampere
A)coulomb
B)farad
C)volt
D)joule
E)ampere
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26
Given:
Mn2+(aq)+ 2e-
Mn(s); E° = -1.18 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
Cr2O72-(aq)+ 14H+(aq)+ 6e-
2Cr3+(aq)+ 7H2O(l); E° = 1.33 V
Which of the following species is the strongest reducing agent?
A)Mn
B)Cu
C)Cr3+
D)Mn2+
E)Cr2O72-
Mn2+(aq)+ 2e-
Mn(s); E° = -1.18 V
Cu2+(aq)+ 2e-
Cu(s); E° = 0.34 V
Cr2O72-(aq)+ 14H+(aq)+ 6e-
2Cr3+(aq)+ 7H2O(l); E° = 1.33 V
Which of the following species is the strongest reducing agent?
A)Mn
B)Cu
C)Cr3+
D)Mn2+
E)Cr2O72-
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27
The cell potential of an electrochemical cell with the cell reaction
Al(s)+ Cr3+(aq)→ Cr(s)+ Al3+(aq)
Is 1.63 V.What is the maximum electrical work obtainable from this cell when 0.50 g of Al is consumed?
A) J
B) J
C) J
D) J
E) J
Al(s)+ Cr3+(aq)→ Cr(s)+ Al3+(aq)
Is 1.63 V.What is the maximum electrical work obtainable from this cell when 0.50 g of Al is consumed?
A)
JB)
JC)
JD)
JE)
J Unlock Deck
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28
In the following electrochemical cell,what is the reduction half reaction?
Mn(s)| Mn2+(aq)|| Fe3+(aq),Fe2+(aq)| Pt(s)
A)Fe3+(aq)+ e− → Fe2+(aq)
B)Fe2+(aq)+ e− → Fe3+(aq)
C)Fe2+(aq)+ Pt(s)→ Fe3+(aq)+ e−
D)Mn2+(aq)→ Mn(s)+ 2e−
E)Mn(s)→ Mn2+(aq)+ 2e−
Mn(s)| Mn2+(aq)|| Fe3+(aq),Fe2+(aq)| Pt(s)
A)Fe3+(aq)+ e− → Fe2+(aq)
B)Fe2+(aq)+ e− → Fe3+(aq)
C)Fe2+(aq)+ Pt(s)→ Fe3+(aq)+ e−
D)Mn2+(aq)→ Mn(s)+ 2e−
E)Mn(s)→ Mn2+(aq)+ 2e−
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29
A fuel cell designed to react grain alcohol with oxygen has the following net reaction:
C2H5OH(l)+ 3O2(g)→ 2CO2(g)+ 3H2O(l)
The maximum work that 1 mol of alcohol can yield by this process is 1320 kJ.What is the theoretical maximum voltage that this cell can achieve?
A)1.14 V
B)2.28 V
C)2.01 V
D)0.760 V
E)13.7 V
C2H5OH(l)+ 3O2(g)→ 2CO2(g)+ 3H2O(l)
The maximum work that 1 mol of alcohol can yield by this process is 1320 kJ.What is the theoretical maximum voltage that this cell can achieve?
A)1.14 V
B)2.28 V
C)2.01 V
D)0.760 V
E)13.7 V
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30
What is the cell reaction for the following electrochemical cell?
Zn | Zn2+(aq)|| Sc3+(aq)| Sc
A)3Zn(s)+ 2Sc3+(aq)→ 2Sc(s)+ 3Zn2+(aq)
B)2Sc(s)+ 3Zn2+(aq)→ 3Zn(s)+ 2Sc3+(aq)
C)Zn(s)+ Zn2+(aq)→ Sc(s)+ Sc3+(aq)
D)Zn(s)+ Sc3+(aq)→ Sc(s)+ Zn2+(aq)
E)Sc(s)+ Zn2+(aq)→ Zn(s)+ Sc3+(aq)
Zn | Zn2+(aq)|| Sc3+(aq)| Sc
A)3Zn(s)+ 2Sc3+(aq)→ 2Sc(s)+ 3Zn2+(aq)
B)2Sc(s)+ 3Zn2+(aq)→ 3Zn(s)+ 2Sc3+(aq)
C)Zn(s)+ Zn2+(aq)→ Sc(s)+ Sc3+(aq)
D)Zn(s)+ Sc3+(aq)→ Sc(s)+ Zn2+(aq)
E)Sc(s)+ Zn2+(aq)→ Zn(s)+ Sc3+(aq)
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31
The cell potential of an electrochemical cell with the cell reaction
2Al(s)+ 3Zn2+(aq)→ 3Zn(s)+ 2Al3+(aq)
Is 1.607 V.What is the maximum electrical work obtainable from this cell when 2.0 mol of Al is consumed?
A) J
B) J
C) J
D) J
E) J
2Al(s)+ 3Zn2+(aq)→ 3Zn(s)+ 2Al3+(aq)
Is 1.607 V.What is the maximum electrical work obtainable from this cell when 2.0 mol of Al is consumed?
A)
JB)
JC)
JD)
JE)
J Unlock Deck
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32
What is the balanced spontaneous reaction and standard cell potential of an electrochemical cell constructed from half cells with the following half reactions?
Cu2+(aq)+ 2e¯ → Cu(s)E° = 0.337 V
E° = -0.130 V
A)Cu2+(aq)+ Pb(s)→ Cu(s)+ Pb2+(aq); 0.467 V
B)Cu(s)+ Pb2+(aq)→ Cu2+(aq)+ Pb(s); −0.467 V
C)Cu2+(aq)+ Pb2+(aq)→ Cu(s)+ Pb(s); 0.207 V
D)Cu2+(aq)+ Pb(s)→ Cu(s)+ Pb2+(aq); 0.234 V
E)Cu(s)+ Pb2+(aq)→ Cu2+(aq)+ Pb(s); −0.234 V
Cu2+(aq)+ 2e¯ → Cu(s)E° = 0.337 V
E° = -0.130 V
A)Cu2+(aq)+ Pb(s)→ Cu(s)+ Pb2+(aq); 0.467 V
B)Cu(s)+ Pb2+(aq)→ Cu2+(aq)+ Pb(s); −0.467 V
C)Cu2+(aq)+ Pb2+(aq)→ Cu(s)+ Pb(s); 0.207 V
D)Cu2+(aq)+ Pb(s)→ Cu(s)+ Pb2+(aq); 0.234 V
E)Cu(s)+ Pb2+(aq)→ Cu2+(aq)+ Pb(s); −0.234 V
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33
Given:
Zn2+(aq)+ 2e-Zn(s); E° = -0.76 V
Cu2+(aq)+ 2e-Cu(s); E° = 0.34 V
Cr2O72-(aq)+ 14H+(aq)+ 6e-2Cr3+(aq)+ 7H2O(l); E° = 1.33 V
Which of the following species is the strongest oxidizing agent?
A)Zn
B)Cr3+
C)Cr2O72-
D)Zn2+
E)Cu
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VCr2O72-(aq)+ 14H+(aq)+ 6e-
2Cr3+(aq)+ 7H2O(l); E° = 1.33 VWhich of the following species is the strongest oxidizing agent?
A)Zn
B)Cr3+
C)Cr2O72-
D)Zn2+
E)Cu
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34
What is the cell notation for the voltaic cell shown below?
A)Zn2+(aq)| Zn(s)|| Cu2+(aq)| Cu(s)
B)Zn(s)| Zn2+(aq)|| Cu(s)| Cu2+(aq)
C)Zn(s)| Cu(s)|| Zn2+(aq)| Cu2+(aq)
D)Zn(s)| Zn2+(aq)|| Cu2+(aq)| Cu(s)
E)Zn2+(aq)| Zn(s)|| Cu(s)| Cu2+(aq)
A)Zn2+(aq)| Zn(s)|| Cu2+(aq)| Cu(s)
B)Zn(s)| Zn2+(aq)|| Cu(s)| Cu2+(aq)
C)Zn(s)| Cu(s)|| Zn2+(aq)| Cu2+(aq)
D)Zn(s)| Zn2+(aq)|| Cu2+(aq)| Cu(s)
E)Zn2+(aq)| Zn(s)|| Cu(s)| Cu2+(aq)
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35
Consider the following standard electrode potentials:
Ag+(aq)+ e-Ag(s); E° = 0.80 V
Mn2+(aq)+ 2e-Mn(s); E° = -1.18 V
Which of the following statements is false concerning the electrochemical cell given below?
Mn(s)| Mn2+(aq)|| Ag+(aq)| Ag(s)
A)The anode half-cell reaction is Mn(s)→ Mn2+(aq)+ 2e-.
B)The reducing agent is Ag(s).
C)Under standard-state conditions,the cell potential is 1.98 V.
D)The cell potential decreases with time.
E)The oxidizing agent is Ag+(aq).
Ag+(aq)+ e-
Ag(s); E° = 0.80 VMn2+(aq)+ 2e-
Mn(s); E° = -1.18 VWhich of the following statements is false concerning the electrochemical cell given below?
Mn(s)| Mn2+(aq)|| Ag+(aq)| Ag(s)
A)The anode half-cell reaction is Mn(s)→ Mn2+(aq)+ 2e-.
B)The reducing agent is Ag(s).
C)Under standard-state conditions,the cell potential is 1.98 V.
D)The cell potential decreases with time.
E)The oxidizing agent is Ag+(aq).
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36
What is the cell reaction for the following electrochemical cell?
Pt | Fe2+(aq),Fe3+(aq)|| Cr3+(aq)| Cr
A)3Fe2+(aq)+ Cr3+(s)→ Cr(s)+ 3Fe3+(aq)
B)3Fe2+(aq)+ 3Fe3+(aq)→ Cr(s)+ Cr3+(aq)
C)Cr(s)+ 3Fe3+(aq)→ Cr3+(aq)+ 3Fe2+(aq)
D)Pt(s)+ Fe2+(aq)+ Cr3+(aq)→ Cr(s)+ Pt2+(aq)+ Fe3+(aq)
E)Cr(s)+ Cr3+(aq)→ 3Fe2+(aq)+ 3Fe3+(aq)
Pt | Fe2+(aq),Fe3+(aq)|| Cr3+(aq)| Cr
A)3Fe2+(aq)+ Cr3+(s)→ Cr(s)+ 3Fe3+(aq)
B)3Fe2+(aq)+ 3Fe3+(aq)→ Cr(s)+ Cr3+(aq)
C)Cr(s)+ 3Fe3+(aq)→ Cr3+(aq)+ 3Fe2+(aq)
D)Pt(s)+ Fe2+(aq)+ Cr3+(aq)→ Cr(s)+ Pt2+(aq)+ Fe3+(aq)
E)Cr(s)+ Cr3+(aq)→ 3Fe2+(aq)+ 3Fe3+(aq)
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37
What is the cell reaction for the following voltaic cell?
Cr(s)| Cr3+(aq)|| Br-(aq)| Br2(g)| Pt(s)
A)2Cr(s)+ 3Br2(g) 2Cr3+(aq)+ 6Br-(aq)
B)Cr(s)+ Cr3+(aq) Br-(aq)+ Br2(g)
C)2Cr3+(aq)+ 6Br-(aq) 2Cr(s)+ 3Br2(g)
D)Cr(s)+ 3Br2(g) Cr3+(s)+ 2Br-(aq)
E)Cr(s)+ 2Br-(aq) Br2(g)+ Cr3+(aq)
Cr(s)| Cr3+(aq)|| Br-(aq)| Br2(g)| Pt(s)
A)2Cr(s)+ 3Br2(g)
2Cr3+(aq)+ 6Br-(aq)B)Cr(s)+ Cr3+(aq)
Br-(aq)+ Br2(g)C)2Cr3+(aq)+ 6Br-(aq)
2Cr(s)+ 3Br2(g)D)Cr(s)+ 3Br2(g)
Cr3+(s)+ 2Br-(aq)E)Cr(s)+ 2Br-(aq)
Br2(g)+ Cr3+(aq) Unlock Deck
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38
A zinc-copper voltaic cell is represented as follows:
Zn(s)| Zn2+(1.0 M)|| Cu2+(1.0 M)| Cu(s)
Which of the following statements is false?
A)The copper electrode is the anode.
B)Reduction occurs at the copper electrode during discharge.
C)The mass of the zinc electrode decreases during discharge.
D)Electrons flow through the external circuit from the zinc electrode to the copper electrode.
E)The concentration of Cu2+ decreases during discharge.
Zn(s)| Zn2+(1.0 M)|| Cu2+(1.0 M)| Cu(s)
Which of the following statements is false?
A)The copper electrode is the anode.
B)Reduction occurs at the copper electrode during discharge.
C)The mass of the zinc electrode decreases during discharge.
D)Electrons flow through the external circuit from the zinc electrode to the copper electrode.
E)The concentration of Cu2+ decreases during discharge.
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39
In a table of standard reduction potentials,the strongest reducing agents are the _______ species in the half-reactions with the _______ E° values.
A)reduced,most negative
B)oxidized,most positive
C)reduced,most positive
D)oxidized,most negative
E)none of these
A)reduced,most negative
B)oxidized,most positive
C)reduced,most positive
D)oxidized,most negative
E)none of these
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40
The Faraday constant is defined as
A)The charge per mole of electrons.
B)The charge on a single electron.
C)The maximum work obtainable from an electrochemical cell.
D)The electromotive force of the cell.
E)The amount of charge moved between electrodes.
A)The charge per mole of electrons.
B)The charge on a single electron.
C)The maximum work obtainable from an electrochemical cell.
D)The electromotive force of the cell.
E)The amount of charge moved between electrodes.
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41
Given:
Ni2+(aq)+ 2e-Ni(s); E° = -0.23 V
2H+(aq)+ 2e-H2(g); E° = 0.00 VAg+(aq)+ e- Ag(s); E° = 0.80 V
NO3-(aq)+ 4H+(aq)+ 3e-NO(g)+ 2H2O(l); E° = 0.96 V
Which of the following statements is true?
A)Ni2+ reacts spontaneously with 1 M H+(aq)to form H2.
B)Ni2+ reacts spontaneously with H2(g).
C)Ag(s)reacts spontaneously with Ni2+.
D)Ag(s)reacts spontaneously with 1 M NO3- in 1 M H+(aq).
E)Ag(s)reacts spontaneously with 1 M H+(aq).
Ni2+(aq)+ 2e-
Ni(s); E° = -0.23 V2H+(aq)+ 2e-
H2(g); E° = 0.00 VAg+(aq)+ e- Ag(s); E° = 0.80 VNO3-(aq)+ 4H+(aq)+ 3e-
NO(g)+ 2H2O(l); E° = 0.96 VWhich of the following statements is true?
A)Ni2+ reacts spontaneously with 1 M H+(aq)to form H2.
B)Ni2+ reacts spontaneously with H2(g).
C)Ag(s)reacts spontaneously with Ni2+.
D)Ag(s)reacts spontaneously with 1 M NO3- in 1 M H+(aq).
E)Ag(s)reacts spontaneously with 1 M H+(aq).
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42
Consider the following standard reduction potentials:
2H+(aq)+ 2e-H2(g); E° = 0.00 V
Sn2+(aq)+ 2e-Sn(s); E° = -0.15 V
Cd2+(aq)+ 2e-Cd(s); E° = -0.40 V
Which pair of substances will react spontaneously under standard-state conditions?
A)Cd with H+
B)Cd with Sn
C)Sn2+ with Cd2+
D)Sn with Cd2+
E)Sn2+ with H+
2H+(aq)+ 2e-
H2(g); E° = 0.00 VSn2+(aq)+ 2e-
Sn(s); E° = -0.15 VCd2+(aq)+ 2e-
Cd(s); E° = -0.40 VWhich pair of substances will react spontaneously under standard-state conditions?
A)Cd with H+
B)Cd with Sn
C)Sn2+ with Cd2+
D)Sn with Cd2+
E)Sn2+ with H+
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43
For a certain oxidation-reduction reaction,E°cell is negative.This means that
A)ΔG° is positive and K is less than 1.
B)ΔG° is negative and K is greater than 1.
C)ΔG° is positive and K is greater than 1.
D)ΔG° is negative and K is less than 1.
E)ΔG° is zero and K is greater than 1.
A)ΔG° is positive and K is less than 1.
B)ΔG° is negative and K is greater than 1.
C)ΔG° is positive and K is greater than 1.
D)ΔG° is negative and K is less than 1.
E)ΔG° is zero and K is greater than 1.
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44
Given:
Pb2+(aq)+ 2e-Pb(s); E° = -0.13 V
Mg2+(aq)+ 2e-Mg(s); E° = -2.38 V
Ag+(aq)+ e-Ag(s); E° = 0.80 V
2H+(aq)+ 2e-H2(g); E° = 0.00 V
Under standard-state conditions,which of the following species is the best reducing agent?
A)H2
B)Mg2+
C)Ag+
D)Pb
E)Ag
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 VMg2+(aq)+ 2e-
Mg(s); E° = -2.38 VAg+(aq)+ e-
Ag(s); E° = 0.80 V2H+(aq)+ 2e-
H2(g); E° = 0.00 VUnder standard-state conditions,which of the following species is the best reducing agent?
A)H2
B)Mg2+
C)Ag+
D)Pb
E)Ag
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45
Given:
Hg2+(aq)+ 2e-Hg(s); E° = 0.85 V
Li+(aq)+ e-Li(s); E° = -3.04 V
Br2(l)+ 2e-2Br-(aq); E° = 1.07 V
Au+(aq)+ e-Au(s); E° = 1.69 V
Cl2(g)+ 2e-2Cl-(aq); E° = 1.36 V
Which of the following species is the best reducing agent?
A)Hg
B)Li+
C)Au
D)Cl-
E)Br-
Hg2+(aq)+ 2e-
Hg(s); E° = 0.85 VLi+(aq)+ e-
Li(s); E° = -3.04 VBr2(l)+ 2e-
2Br-(aq); E° = 1.07 VAu+(aq)+ e-
Au(s); E° = 1.69 VCl2(g)+ 2e-
2Cl-(aq); E° = 1.36 VWhich of the following species is the best reducing agent?
A)Hg
B)Li+
C)Au
D)Cl-
E)Br-
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46
Consider the following standard reduction potentials:
Mg2+(aq)+ 2e-
Mg(s); E° = -2.38 V
V2+(aq)+ 2e-
V(s); E° = -1.18 V
Cu2+(aq)+ e-
Cu+(aq); E° = 0.15 V
Which of the following reactions will proceed spontaneously from left to right under standard-state conditions?
A)Mg(s)+ 2Cu2+(aq)→ Mg2+(aq)+ 2Cu+(aq)
B)V2+(aq)+ 2Cu+(aq)→ V(s)+ 2Cu2+(aq)
C)Mg2+(aq)+ 2Cu+(aq)→ 2Cu2+(aq)+ Mg(s)
D)Mg2+(aq)+ V(s)→ V2+(aq)+ Mg(s)
E)2Cu2+(aq)+ 2Cu+(aq)→ Mg2+(aq)+ Mg(s)
Mg2+(aq)+ 2e-
Mg(s); E° = -2.38 V
V2+(aq)+ 2e-
V(s); E° = -1.18 V
Cu2+(aq)+ e-
Cu+(aq); E° = 0.15 V
Which of the following reactions will proceed spontaneously from left to right under standard-state conditions?
A)Mg(s)+ 2Cu2+(aq)→ Mg2+(aq)+ 2Cu+(aq)
B)V2+(aq)+ 2Cu+(aq)→ V(s)+ 2Cu2+(aq)
C)Mg2+(aq)+ 2Cu+(aq)→ 2Cu2+(aq)+ Mg(s)
D)Mg2+(aq)+ V(s)→ V2+(aq)+ Mg(s)
E)2Cu2+(aq)+ 2Cu+(aq)→ Mg2+(aq)+ Mg(s)
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47
What is E°cell for the cell reaction 2Cr(s)+ 3Sn4+ (aq)→ 3Sn2+(aq)+ 2Cr3+ (aq)?
Cr3+ (aq)+ 3e-Cr(s); E° = -0.74V
A)0.89V
B)-0.59V
C)
D)
E)0.59V
Cr3+ (aq)+ 3e-
Cr(s); E° = -0.74V
A)0.89V
B)-0.59V
C)
D)
E)0.59V
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48
Given:
W3+(aq)+ 3e-W(s); E° = 2.72 V
Pb2+(aq)+ 2e-Pb(s); E° = -0.13 V
Ni2+(aq)+ 2e-Ni(s); E° = -0.23 V
Cd2+(aq)+ 2e-Cd(s); E° = -0.40 V
Zn2+(aq)+ 2e-Zn(s); E° = -0.76 V
Al3+(aq)+ 3e-Al(s); E° = -1.66 V
Mg2+(aq)+ 2e-Mg(s); E° = -2.38 V
Under standard-state conditions,which of the following metals will reduce W3+ to W but will not reduce Ni2+ to Ni?
A)Cd
B)Pb
C)Al
D)Zn
E)Mg
W3+(aq)+ 3e-
W(s); E° = 2.72 VPb2+(aq)+ 2e-
Pb(s); E° = -0.13 VNi2+(aq)+ 2e-
Ni(s); E° = -0.23 VCd2+(aq)+ 2e-
Cd(s); E° = -0.40 VZn2+(aq)+ 2e-
Zn(s); E° = -0.76 VAl3+(aq)+ 3e-
Al(s); E° = -1.66 VMg2+(aq)+ 2e-
Mg(s); E° = -2.38 VUnder standard-state conditions,which of the following metals will reduce W3+ to W but will not reduce Ni2+ to Ni?
A)Cd
B)Pb
C)Al
D)Zn
E)Mg
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49
Given:
Pb2+(aq)+ 2e-Pb(s); E° = -0.13 V
Zn2+(aq)+ 2e-Zn(s); E° = -0.76 V
Al3+(aq)+ 3e-Al(s); E° = -1.66 V
Mg2+(aq)+ 2e-Mg(s); E° = -2.38 V
V2+(aq)+ 2e-V(s); E° = -1.18 V
Cu2+(aq)+ 2e-Cu(s); E° = 0.34 V
Which of the following cations is capable of oxidizing Pb to Pb2+ under standard-state conditions?
A)Al3+
B)V2+
C)Cu2+
D)Mg2+
E)Zn2+
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 VZn2+(aq)+ 2e-
Zn(s); E° = -0.76 VAl3+(aq)+ 3e-
Al(s); E° = -1.66 VMg2+(aq)+ 2e-
Mg(s); E° = -2.38 VV2+(aq)+ 2e-
V(s); E° = -1.18 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VWhich of the following cations is capable of oxidizing Pb to Pb2+ under standard-state conditions?
A)Al3+
B)V2+
C)Cu2+
D)Mg2+
E)Zn2+
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50
Which of the following statements is true about a voltaic cell for which E°cell = 1.00 V?
A)The cathode is at a higher energy than the anode.
B)It has ΔG° > 0.
C)The reaction is spontaneous.
D)The system is at equilibrium.
E)It has K = 1.
A)The cathode is at a higher energy than the anode.
B)It has ΔG° > 0.
C)The reaction is spontaneous.
D)The system is at equilibrium.
E)It has K = 1.
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51
Given:
Zn2+(aq)+ 2e-Zn(s); E° = -0.76 V
2H+(aq)+ 2e-H2(g); E° = 0.00 V
I2(s)+ 2e-2I-(aq); E° = 0.54 V
Br2(l)+ 2e-2Br-(aq); E° = 1.07 V
Ni2+(aq)+ 2e-Ni(s); E° = -0.23 V
Cu2+(aq)+ 2e-Cu(s); E° = 0.34 V
Which of the following species will oxidize Ni but not Cu?
A)Zn2+
B)Br-
C)H+
D)I2
E)Zn
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 V2H+(aq)+ 2e-
H2(g); E° = 0.00 VI2(s)+ 2e-
2I-(aq); E° = 0.54 VBr2(l)+ 2e-
2Br-(aq); E° = 1.07 VNi2+(aq)+ 2e-
Ni(s); E° = -0.23 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VWhich of the following species will oxidize Ni but not Cu?
A)Zn2+
B)Br-
C)H+
D)I2
E)Zn
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52
Given:
Zn2+(aq)+ 2e-Zn(s); E° = -0.76 V
Co2+(aq)+ 2e-Co(s); E° = -0.28 V
Sn2+(aq)+ 2e-Sn(s); E° = -0.15 V
Pb2+(aq)+ 2e-Pb(s); E° = -0.13 V
Fe3+(aq)+ e-Fe2+(aq); E° = 0.77 V
Under standard-state conditions,which of the following pairs of elements or ions is capable of reducing Sn2+(aq)to Sn(s)?
A)Zn(s)or Co(s)
B)Pb(s)or Fe2+(aq)
C)Co(s)or Pb(s)
D)Fe2+(aq)or Zn(s)
E)Zn2+(aq)or Co2+(aq)
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 VCo2+(aq)+ 2e-
Co(s); E° = -0.28 VSn2+(aq)+ 2e-
Sn(s); E° = -0.15 VPb2+(aq)+ 2e-
Pb(s); E° = -0.13 VFe3+(aq)+ e-
Fe2+(aq); E° = 0.77 VUnder standard-state conditions,which of the following pairs of elements or ions is capable of reducing Sn2+(aq)to Sn(s)?
A)Zn(s)or Co(s)
B)Pb(s)or Fe2+(aq)
C)Co(s)or Pb(s)
D)Fe2+(aq)or Zn(s)
E)Zn2+(aq)or Co2+(aq)
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53
Consider the following cell reaction:
2Cr(s)+ 6H+(aq)→ 2Cr3+(aq)+ 3H2(g); E°cell = 0.74V
Under standard-state conditions,what is E° for the following half-reaction?
Cr3+(aq)+ 3e− → Cr(s)
A)-0.74 V
B)
C)-0.37 V
D)0.37 V
E)0.74 V
2Cr(s)+ 6H+(aq)→ 2Cr3+(aq)+ 3H2(g); E°cell = 0.74V
Under standard-state conditions,what is E° for the following half-reaction?
Cr3+(aq)+ 3e− → Cr(s)
A)-0.74 V
B)
C)-0.37 V
D)0.37 V
E)0.74 V
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54
Given:
Pb2+(aq)+ 2e-Pb(s); E° = -0.13 V
2H+(aq)+ 2e-H2(g); E° = 0.00 V
NO3-(aq)+4H+(aq)+ 3e-NO(g)+ 2H2O(l); E° = 0.96 V
O2(g)+ 4H+(aq)+ 4e-2H2O(l); E° = 1.23 V
PbO2(s)+ SO42-(aq)+ 4H+(aq)+ 2e-PbSO4(s)+ 2H2O(l); E° = 1.69 V
Under standard-state conditions,which of the following is the best oxidizing agent?
A)H+
B)Pb2+
C)PbO2
D)O2
E)NO3-
Pb2+(aq)+ 2e-
Pb(s); E° = -0.13 V2H+(aq)+ 2e-
H2(g); E° = 0.00 VNO3-(aq)+4H+(aq)+ 3e-
NO(g)+ 2H2O(l); E° = 0.96 VO2(g)+ 4H+(aq)+ 4e-
2H2O(l); E° = 1.23 VPbO2(s)+ SO42-(aq)+ 4H+(aq)+ 2e-
PbSO4(s)+ 2H2O(l); E° = 1.69 VUnder standard-state conditions,which of the following is the best oxidizing agent?
A)H+
B)Pb2+
C)PbO2
D)O2
E)NO3-
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55
Consider the following cell reaction:
2Hg2+(aq)+ H2(g)→ 2H+(aq)+ Hg22+(aq); E°cell = 0.92 V
Under standard-state conditions,what is E° for the following half-reaction?
Hg2+(aq)+ 2e- → Hg22+(aq)
A)0.92 V
B)-0.46 V
C)0.46 V
D)-0.92 V
E)1.10 V
2Hg2+(aq)+ H2(g)→ 2H+(aq)+ Hg22+(aq); E°cell = 0.92 V
Under standard-state conditions,what is E° for the following half-reaction?
Hg2+(aq)+ 2e- → Hg22+(aq)
A)0.92 V
B)-0.46 V
C)0.46 V
D)-0.92 V
E)1.10 V
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56
Consider the following reduction potentials:
Cd2+(aq)+ 2e-Cd(s); E° = -0.40 V
Pb2+(aq)+ 2e-Pb(s); E° = -0.13 V
Cu2+(aq)+ 2e-Cu(s); E° = 0.34 V
Br2(l)+ 2e-2Br-(aq); E° = 1.07 V
Under standard-state conditions,which of the following reactions is spontaneous?
A)Cd2+(aq)+ Pb(s)→ Cd(s)+ Pb2+(aq)
B)Pb2+(aq)+ Cu(s)→ Pb(s)+ Cu2+(aq)
C)2Br-(aq)+ Pb2+(aq)→ Br2(l)+ Pb(s)
D)2Br-(aq)+ Cu2+(aq)→ Br2(l)+ Cu(s)
E)Cu2+(aq)+ Cd(s)→ Cu(s)+ Cd2+(aq)
Cd2+(aq)+ 2e-
Cd(s); E° = -0.40 VPb2+(aq)+ 2e-
Pb(s); E° = -0.13 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VBr2(l)+ 2e-
2Br-(aq); E° = 1.07 VUnder standard-state conditions,which of the following reactions is spontaneous?
A)Cd2+(aq)+ Pb(s)→ Cd(s)+ Pb2+(aq)
B)Pb2+(aq)+ Cu(s)→ Pb(s)+ Cu2+(aq)
C)2Br-(aq)+ Pb2+(aq)→ Br2(l)+ Pb(s)
D)2Br-(aq)+ Cu2+(aq)→ Br2(l)+ Cu(s)
E)Cu2+(aq)+ Cd(s)→ Cu(s)+ Cd2+(aq)
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57
Which of the following is true for a reaction that is nonspontaneous as written?
A)ΔG° > 0; E°cell < 0
B)ΔG° < 0; E°cell < 0
C)ΔG° < 0; E°cell < 0
D)ΔG° > 0; E°cell > 0
E)ΔG° > 0; E°cell = 0
A)ΔG° > 0; E°cell < 0
B)ΔG° < 0; E°cell < 0
C)ΔG° < 0; E°cell < 0
D)ΔG° > 0; E°cell > 0
E)ΔG° > 0; E°cell = 0
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58
Given:
Li+(aq)+ e-Li(s); E° = -3.04 V
Mg2+(aq)+ 2e-Mg(s); E° = -2.38 V
Fe2+(aq)+ 2e-Fe(s); E° = -0.41 V
Ag+(aq)+ e-Ag(s); E° = 0.80 V
Br2(l)+ 2e-2Br-(aq); E° = 1.07 V
Which of the following species is the best oxidizing agent?
A)Mg2+
B)Br-
C)Fe2+
D)Li
E)Ag+
Li+(aq)+ e-
Li(s); E° = -3.04 VMg2+(aq)+ 2e-
Mg(s); E° = -2.38 VFe2+(aq)+ 2e-
Fe(s); E° = -0.41 VAg+(aq)+ e-
Ag(s); E° = 0.80 VBr2(l)+ 2e-
2Br-(aq); E° = 1.07 VWhich of the following species is the best oxidizing agent?
A)Mg2+
B)Br-
C)Fe2+
D)Li
E)Ag+
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59
Given:
2H+(aq)+ 2e-H2(g); E° = 0.00 V
K+(aq)+ e-K(s); E° = 2.7182818285 V
F2(g)+ 2e-2FS1U1
1-(aq); E° = 2.87 V
Al3+(aq)+ 3e-Al(s); E° = -1.66 V
Pb2+(aq)+ 2e-Pb(s); E° = -0.13 V
Under standard-state conditions,which is the strongest reducing agent?
A)Pb2+
B)Al3+
C)F-
D)K
E)H+
2H+(aq)+ 2e-
H2(g); E° = 0.00 VK+(aq)+ e-
K(s); E° = 2.7182818285 VF2(g)+ 2e-
2FS1U11-(aq); E° = 2.87 V
Al3+(aq)+ 3e-
Al(s); E° = -1.66 VPb2+(aq)+ 2e-
Pb(s); E° = -0.13 VUnder standard-state conditions,which is the strongest reducing agent?
A)Pb2+
B)Al3+
C)F-
D)K
E)H+
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60
Given:
Zn2+(aq)+ 2e-Zn(s); E° = -0.76 V
Cr3+(aq)+ 3e-Cr(s); E° = -0.74 V
Fe2+(aq)+ 2e-Fe(s); E° = -0.41 V
Cd2+(aq)+ 2e-Cd(s); E° = -0.40 V
Sn2+(aq)+ 2e-Sn(s); E° = -0.15 V
Hg2+(aq)+ 2e-Hg(s); E° = 0.85 V
Au+(aq)+ e-Au(s); E° = 1.69 V
Under standard-state conditions,which of the following metals will reduce Hg2+ to Hg but will not reduce Cd2+ to Cd?
A)Cr
B)Zn
C)Fe
D)Sn
E)Au
Zn2+(aq)+ 2e-
Zn(s); E° = -0.76 VCr3+(aq)+ 3e-
Cr(s); E° = -0.74 VFe2+(aq)+ 2e-
Fe(s); E° = -0.41 VCd2+(aq)+ 2e-
Cd(s); E° = -0.40 VSn2+(aq)+ 2e-
Sn(s); E° = -0.15 VHg2+(aq)+ 2e-
Hg(s); E° = 0.85 VAu+(aq)+ e-
Au(s); E° = 1.69 VUnder standard-state conditions,which of the following metals will reduce Hg2+ to Hg but will not reduce Cd2+ to Cd?
A)Cr
B)Zn
C)Fe
D)Sn
E)Au
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61
Given:
Cl2 (g)+ 2e¯2Cl¯ (aq); Eº = 1.36V
What is
For the following cell reaction?
2AlCl3(aq)2Al(s)+ 3Cl2(g)
A)-5.8 × 105 J
B)5.8 × 105 J
C)
D)-1.7 × 106 J
E)1.7 × 106 J
Cl2 (g)+ 2e¯
2Cl¯ (aq); Eº = 1.36VWhat is
For the following cell reaction?
2AlCl3(aq)
2Al(s)+ 3Cl2(g)A)-5.8 × 105 J
B)5.8 × 105 J
C)
D)-1.7 × 106 J
E)1.7 × 106 J
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62
The cell potential of the following cell is determined using an unspecified concentration of acid.What is [H+] given that the measured cell potential is -0.464 V and the anode reduction potential (E°)is 0.222 V at 25°C?
Ag(s)| AgCl(s)| Cl−(1.0 M)|| H+(aq,? M)| H2(g,1.0 atm)| Pt(s)
A) M
B) M
C) M
D) M
E) M
Ag(s)| AgCl(s)| Cl−(1.0 M)|| H+(aq,? M)| H2(g,1.0 atm)| Pt(s)
A)
MB)
MC)
MD)
ME)
M Unlock Deck
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63
If the cell is initially at standard-state conditions,which of the following statements is true? Zn2+(aq)+ 2e- Zn(s); E° = -0.76 V
Cu2+(aq)+ 2e-Cu(s); E° = 0.34 V
A)Initially ,and it will become more positive with time.
B)Initially ,and it will not change with time.
C)Initially ,and it will become more negative with time.
D)Initially ,and it will become more positive with time.
E)Initially ,and it will become more negative with time.
Zn2+(aq)+ 2e- Zn(s); E° = -0.76 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VA)Initially
,and it will become more positive with time.B)Initially
,and it will not change with time.C)Initially
,and it will become more negative with time.D)Initially
,and it will become more positive with time.E)Initially
,and it will become more negative with time. Unlock Deck
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64
What is the logarithm of the equilibrium constant,log K,at 25°C of the voltaic cell constructed from the following two half-reactions?
Fe2+ (aq)+ 2e¯Fe(s); E° = - 0.41V
Ag+(aq)+ e-
Ag(s); E° = 0.80 V
A)6.7
B)40.9
C)20.3
D)13.2
E)67.6
Fe2+ (aq)+ 2e¯
Fe(s); E° = - 0.41VAg+(aq)+ e-
Ag(s); E° = 0.80 VA)6.7
B)40.9
C)20.3
D)13.2
E)67.6
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65
The cell potential of the following cell is determined using an unspecified concentration of acid.What is the pH of the acid solution given that the measured cell potential is -0.508 V and the anode reduction potential (E°)is 0.222 V at 25°C?
Ag(s)| AgCl(s)| Cl−(1.0 M)|| H+(aq,? M)| H2(g,1.0 atm)| Pt(s)
A)4.83
B)12.30
C)5.33
D)9.66
E)2.16
Ag(s)| AgCl(s)| Cl−(1.0 M)|| H+(aq,? M)| H2(g,1.0 atm)| Pt(s)
A)4.83
B)12.30
C)5.33
D)9.66
E)2.16
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66
Calculate the maximum electrical work obtainable at 25oC from the following voltaic cell.
Cd(s)|Cd2+(0.840M)||Cl2(g,0.0354atm)|Cl-(0.0473M)|Pt;Eºcell = 1.76V
A)-3.39 × 105 J
B)-3.55 × 105 J
C)-3.32 × 105 J
D)-3.47 × 105 J
E)-3.40 × 105 J
Cd(s)|Cd2+(0.840M)||Cl2(g,0.0354atm)|Cl-(0.0473M)|Pt;Eºcell = 1.76V
A)-3.39 × 105 J
B)-3.55 × 105 J
C)-3.32 × 105 J
D)-3.47 × 105 J
E)-3.40 × 105 J
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67
Given:
Pb2+ (aq)+ 2e-
Pb(s); Eº = -0.13 V
What is the standard cell potential for the following reaction?
2Cr(s)+ 3Pb2+ (aq)→ 3Pb(s)+ 2Cr3+ (aq)
A)-0.87V
B)
C)-0.61V
D)0.61V
E)0.87V
Pb2+ (aq)+ 2e-
Pb(s); Eº = -0.13 VWhat is the standard cell potential for the following reaction?
2Cr(s)+ 3Pb2+ (aq)→ 3Pb(s)+ 2Cr3+ (aq)
A)-0.87V
B)
C)-0.61V
D)0.61V
E)0.87V
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68
Calculate the solubility product of silver iodide at 25°C given the following data:
E°(V)
AgI(s)+ e- → Ag(s)+ I-
-0)15
I2(s)+ 2e- → 2I-
+0)54
Ag+ + e- → Ag(s)
+0)80
A)2 × 10-12
B)3 × 10-3
C)2 × 10-24
D)9 × 10-17
E)2 × 10-4
E°(V)
AgI(s)+ e- → Ag(s)+ I-
-0)15
I2(s)+ 2e- → 2I-
+0)54
Ag+ + e- → Ag(s)
+0)80
A)2 × 10-12
B)3 × 10-3
C)2 × 10-24
D)9 × 10-17
E)2 × 10-4
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69
Given:
Pb2+ (aq)+ 2e¯Pb(s); Eº = -0.13V
What is the standard Gibbs free-energy change for the following reaction?
2Cr(s)+ 3Pb2+ (aq)→ 3Pb(s)+ 2Cr3+ (aq)
A)353kJ
B)118kJ
C)
D)-353kJ
E)
Pb2+ (aq)+ 2e¯
Pb(s); Eº = -0.13VWhat is the standard Gibbs free-energy change for the following reaction?
2Cr(s)+ 3Pb2+ (aq)→ 3Pb(s)+ 2Cr3+ (aq)
A)353kJ
B)118kJ
C)
D)-353kJ
E)
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70
Which of the following statements is true concerning the electrochemical cell depicted below?
Zn | Zn2+(aq)|| Cu2+(aq)| Cu
Zn2+(aq)+ 2e−Zn(s); E° = -2.87 V
Cu2+(aq)+ 2e−Cu(s); E° = -2.38 V
A)The cell is at equilibrium.
B)The cell reaction is spontaneous with a standard cell potential of 0.49 V.
C)The cell reaction is spontaneous with a standard cell potential of 5.25 V.
D)The cell reaction is nonspontaneous with a standard cell potential of -5.25 V.
E)The cell reaction is nonspontaneous with a standard cell potential of -0.49 V.
Zn | Zn2+(aq)|| Cu2+(aq)| Cu
Zn2+(aq)+ 2e−
Zn(s); E° = -2.87 VCu2+(aq)+ 2e−
Cu(s); E° = -2.38 VA)The cell is at equilibrium.
B)The cell reaction is spontaneous with a standard cell potential of 0.49 V.
C)The cell reaction is spontaneous with a standard cell potential of 5.25 V.
D)The cell reaction is nonspontaneous with a standard cell potential of -5.25 V.
E)The cell reaction is nonspontaneous with a standard cell potential of -0.49 V.
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71
What is 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
A)0.014
B)1.7
C)0.4
D)1.0
E)3
Sn(s)+ Pb2+ (aq)→ Sn2+ (aq)+ Pb(s); E°cell = 0.014 V
A)0.014
B)1.7
C)0.4
D)1.0
E)3
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72
For a certain reaction,ΔHº = -75.4kJ and ΔSº = -225J/K.If n = 3,calculate E°cell for the reaction at 25°C.
A)0.0288 V
B)0.0961 V
C)0.241 V
D)0.492 V
E)0.0654 V
A)0.0288 V
B)0.0961 V
C)0.241 V
D)0.492 V
E)0.0654 V
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73
A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+ concentration is 2.0 × 10-5 M and by placing a Pt electrode in the other compartment,in which the H+ concentration is 3.4 M and = 1.00 atm.The Fe2+/Fe half-cell reduction potential is -0.41 V,and the H+/H2 half-cell reduction potential is 0.00 V.What is the value of E° for this cell,and which electrode is the anode?
A)0.41 V,Fe
B)0.90 V,Pt
C)-0.41 V,Pt
D)-0.41 V,Fe
E)0.41 V,Pt
= 1.00 atm.The Fe2+/Fe half-cell reduction potential is -0.41 V,and the H+/H2 half-cell reduction potential is 0.00 V.What is the value of E° for this cell,and which electrode is the anode?A)0.41 V,Fe
B)0.90 V,Pt
C)-0.41 V,Pt
D)-0.41 V,Fe
E)0.41 V,Pt
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74
A voltaic cell is made by placing a zinc electrode in a compartment in which the Zn2+ concentration is 2.0 × 10-5 M and by placing a Pt electrode in the other compartment,in which the H+ concentration is 3.4 M and PH2 = 1.00 atm.The Zn2+/Zn half-cell reduction potential is -0.76 V,and the H+/H2 half-cell reduction potential is 0.00 V.What is the equilibrium constant at 25°C for the spontaneous cell reaction?
A)4 × 104
B)5 × 1020
C)5 × 1022
D)7 × 10 12
E)5 × 10 25
A)4 × 104
B)5 × 1020
C)5 × 1022
D)7 × 10 12
E)5 × 10 25
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75
Which of the following statements is true concerning the hypthetical electrochemical cell depicted below? (M1 and M2 are differing metals)
M1 | M12+(aq)|| M2+(aq)| M2
M12+(aq)+ 2e−M1(s); E° = -2.91 V
M22+(aq)+ e−M2(s); E° = -2.98 V
A)The cell reaction is nonspontaneous with a standard cell potential of -0.07 V.
B)The cell reaction is spontaneous with a standard cell potential of 5.89 V.
C)The cell is at equilibrium.
D)The cell reaction is spontaneous with a standard cell potential of 0.07 V.
E)The cell reaction is nonspontaneous with a standard cell potential of -5.89 V.
M1 | M12+(aq)|| M2+(aq)| M2
M12+(aq)+ 2e−
M1(s); E° = -2.91 VM22+(aq)+ e−
M2(s); E° = -2.98 VA)The cell reaction is nonspontaneous with a standard cell potential of -0.07 V.
B)The cell reaction is spontaneous with a standard cell potential of 5.89 V.
C)The cell is at equilibrium.
D)The cell reaction is spontaneous with a standard cell potential of 0.07 V.
E)The cell reaction is nonspontaneous with a standard cell potential of -5.89 V.
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76
For a reaction in a voltaic cell,both ΔH° and ΔS° are positive.Which of the following statements is true?
A)E°cell will increase with an increase in temperature.
B)E°cell will not change when the temperature increases.
C)E°cell will decrease with an increase in temperature.
D)ΔG° > 0 for all temperatures.
E)None of the above statements is true.
A)E°cell will increase with an increase in temperature.
B)E°cell will not change when the temperature increases.
C)E°cell will decrease with an increase in temperature.
D)ΔG° > 0 for all temperatures.
E)None of the above statements is true.
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77
If E°cell for a certain reaction is 1 V (n = 4),and ΔS° is 11.2 J/(K⋅mol),what is ΔH° in units of J/mol at 25°C?
A) × 105 J/mol
B) × 105 J/mol
C) × 105 J/mol
D) × 104 J/mol
E) J/mol
A)
× 105 J/molB)
× 105 J/molC)
× 105 J/molD)
× 104 J/molE)
J/mol Unlock Deck
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78
If the value of E°cell is 2.10 V for the reaction
F2 (g)+ 2Fe2+ (aq)→ 2Fe3+ (aq)+ 2F- (aq),
What is the value of E°cell for
F- (aq)+ Fe3+ (aq)→ Fe2+ (aq)+ 1/2 F2(g)?
A)-4.20 V
B)-1.05 V
C)2.10V
D)1.05 V
E)-2.10V
F2 (g)+ 2Fe2+ (aq)→ 2Fe3+ (aq)+ 2F- (aq),
What is the value of E°cell for
F- (aq)+ Fe3+ (aq)→ Fe2+ (aq)+ 1/2 F2(g)?
A)-4.20 V
B)-1.05 V
C)2.10V
D)1.05 V
E)-2.10V
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79
What is E of the following cell reaction at 25°C? E°cell = 0.460 V.Cu(s)| Cu2+(0.020M)|| Ag+(0.16M)| Ag(s)
A)0.463 V
B)0.282 V
C)0.460 V
D)0.487 V
E)0.467 V
A)0.463 V
B)0.282 V
C)0.460 V
D)0.487 V
E)0.467 V
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80
If the cell is initially at standard-state conditions,which of the following statements is true? Zn2+(aq)+ 2e- Zn(s); E° = -0.76 V
Cu2+(aq)+ 2e-Cu(s); E° = 0.34 V
A)Initially Kc = 2 × 10-37,and it decreases with time.
B)Initially Kc = 2 × 1037,and it does not change with time.
C)Initially Kc = 2 × 1037,and it decreases with time.
D)Initially Kc = 2 × 1037,and it increases with time.
E)Initially Kc = 2 × 10-37,and it increases with time.
Zn2+(aq)+ 2e- Zn(s); E° = -0.76 VCu2+(aq)+ 2e-
Cu(s); E° = 0.34 VA)Initially Kc = 2 × 10-37,and it decreases with time.
B)Initially Kc = 2 × 1037,and it does not change with time.
C)Initially Kc = 2 × 1037,and it decreases with time.
D)Initially Kc = 2 × 1037,and it increases with time.
E)Initially Kc = 2 × 10-37,and it increases with time.
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