Question 1

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E °\degree° Fe = -0.44 V; all E °\degree°  values refer to the M2+/M half-cell reactions.

Accepted Answer

A)   manganese, Mn, E °\degree° = -1.18 V
B)   cadmium, Cd, E °\degree°  = -0.40 V
C)   magnesium, Mg, E °\degree°  = -2.37 V
D)   zinc, Zn, E °\degree°  = -0.76 V
E)   All of these metals are capable of acting as sacrificial anodes with iron. F) C) and D)
G) B) and D)

Question 2

In the shorthand notation for cells, a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Accepted Answer

A) True 
 B)False  False

Question 3

In the electrolysis of water, how many grams of oxygen gas will be produced for every gram of hydrogen gas formed? Reaction: 2H2O(l)   →\rightarrow→ 2H2(g)  + O2(g)

Accepted Answer

A)   31.7 g
B)   15.9 g
C)   7.94 g
D)   3.97 g
E)   1.98 g F) A) and D)
G) B) and E)

Question 4

Calculate  Δ\DeltaΔ G °\degree° for the reaction of iron(II)  ions with one mole of permanganate ions.

Accepted Answer

A)   -71.4 kJ
B)   -286 kJ
C)   -357 kJ
D)   -428 kJ
E)   None of these choices is correct. F) A) and D)
G) B) and E)

Question 5

Which component of the following cell notation is the anode? P | Q || R | S

Accepted Answer

A)   P
B)   Q
C)   R
D)   S
E)   One of the | symbols is the anode.F) A) and C)
G) B) and D)

Question 6

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. 4¯(aq)  B)  Mn2+(aq)  C)  K+(aq)  D)  F2O(aq)  E)  H+(aq) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   AuBr4¯(aq) 
B)   Mn2+(aq) 
C)   K+(aq) 
D)   F2O(aq) 
E)   H+(aq) F) All of the above
G) A) and B)

Question 7

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Accepted Answer

A) True 
 B)False

Question 8

In the electrolyte of an electrochemical cell, current is carried by electrons moving from the anode to the cathode.

Accepted Answer

A) True 
 B)False

Question 9

Consider the reaction in the lead-acid cell cell = 2.04 V at 298 K.  \Delta G  \degree for this reaction is A)  -3.94 * 105 kJ. B)  -3.94 * 102 kJ. C)  -1.97*105 kJ. D)  -7.87* 102 kJ. E)  None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" > for which E  °\degree° cell = 2.04 V at 298 K.  Δ\DeltaΔ G  °\degree° for this reaction is

Accepted Answer

A)   -3.94 * 105 kJ.
B)   -3.94 * 102 kJ.
C)   -1.97*105 kJ.
D)   -7.87* 102 kJ.
E)   None of these choices is correct. F) B) and C)
G) A) and D)

Question 10

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states) ?

Accepted Answer

A)   HCl and Cl¯
B)   H+ and OH¯
C)   H2O and H+
D)   Fe3+ and Fe2O3
E)   MnO2 and Mn2+F) All of the above
G) B) and E)

Question 11

Which one of the following is not a redox reaction?

Accepted Answer

A)   Al(OH) 4¯(aq)  + 4H+(aq)  →\rightarrow→  Al3+(aq)  + 4H2O(l) 
B)   C6H12O6(s)  + 6O2(g)   →\rightarrow→ 6CO2(g)  + 6H2O(l) 
C)   Na6FeCl8(s)  + 2Na(l)   →\rightarrow→  8NaCl(s)  + Fe(s) 
D)   2H2O2(aq)   →\rightarrow→  2H2O(l)  + O2(g) 
E)   CO2(g)  + H2(g)   →\rightarrow→  CO(g)  + H2O(g)  F) A) and C)
G) None of the above

Question 12

Which one of the following statements relating to the glass electrode is correct?

Accepted Answer

A)   The glass electrode detects hydrogen gas.
B)   The glass of a glass electrode serves to conduct electrons.
C)   When pH is measured, only a single electrode, the glass electrode, need be used.
D)   The potential of the glass electrode varies linearly with the pH of the solution.
E)   None of these choices is correct.F) B) and C)
G) A) and B)

Question 13

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

Accepted Answer

A)   sodium from Na3PO4(aq) 
B)   sulfur from K2SO4(aq) 
C)   oxygen from H2SO4(aq) 
D)   potassium from KCl(aq) 
E)   nitrogen from AgNO3(aq) F) A) and B)
G) A) and C)

Question 14

Examine the following half-reactions and select the strongest reducing agent among the species listed. 4¯(aq)  E)  Zn(OH) 2(s) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Hg(l) 
B)   Zn(s) 
C)   Ag(s) 
D)   BH4¯(aq) 
E)   Zn(OH) 2(s) F) None of the above
G) D) and E)

Question 15

The following half-reactions occur in the mercury battery used in calculators. If E °\degree° 1U1B1cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25 °\degree° C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.)  HgO(s)  + H2O(l)  + 2e¯  = 1.357 V, calculate the equilibrium constant for the cell reaction at 25 \degree C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.)  HgO(s)  + H2O(l)  + 2e¯   Hg(l)  + 2OH¯(aq)  ZnO(s)  + H2O(l)  + 2e¯   Zn(s)  + 2OH¯(aq)  A)  9.4 * 1022 B)  7.5 *1045 C)  6.4 * 1063 D)  7.8 * 1091 E)  > 9.9* 1099 " class="answers-bank-image d-inline" rel="preload" > Hg(l)  + 2OH¯(aq) 
ZnO(s)  + H2O(l)  + 2e¯  = 1.357 V, calculate the equilibrium constant for the cell reaction at 25 \degree C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.)  HgO(s)  + H2O(l)  + 2e¯   Hg(l)  + 2OH¯(aq)  ZnO(s)  + H2O(l)  + 2e¯   Zn(s)  + 2OH¯(aq)  A)  9.4 * 1022 B)  7.5 *1045 C)  6.4 * 1063 D)  7.8 * 1091 E)  > 9.9* 1099 " class="answers-bank-image d-inline" rel="preload" > Zn(s)  + 2OH¯(aq)

Accepted Answer

A)   9.4 * 1022
B)   7.5 *1045
C)   6.4 * 1063
D)   7.8 * 1091
E)   > 9.9* 1099 F) A) and C)
G) A) and D)

Question 16

The voltaic cell made up of cobalt, copper and their M2+ ions, has E  °\degree° cell = 0.62 V. If E  °\degree°  of the cathode half-cell is 0.34 V, what is E  °\degree°  of the anode half-cell? Cu2+(aq)  + Co(s)   →\rightarrow→  Cu(s)  + Co2+(aq)

Accepted Answer

A)   -0.28 V
B)   -0.96V
C)   0.28 V
D)   0.96 V
E)   None of these choices is correct. F) A) and C)
G) C) and D) A

Question 17

What is the value of the equilibrium constant for the cell reaction below at 25 °\degree° C? 
E °\degree° cell = 0.30 V Sn2+(aq)  + Fe(s)  cell = 0.30 V Sn2+(aq)  + Fe(s)    Sn(s)  + Fe2+(aq)  A)  1.2* 105 B)  1.4 * 1010 C)  8.6 * 10¯6 D)  7.1 * 10¯11 E)  2.3 * 1023 " class="answers-bank-image d-inline" rel="preload" > Sn(s)  + Fe2+(aq)

Accepted Answer

A)   1.2* 105
B)   1.4 * 1010
C)   8.6 * 10¯6
D)   7.1 * 10¯11
E)   2.3 * 1023 F) B) and D)
G) B) and E)

Question 18

The line notation, Al(s)  | Al3+(aq)  || Co2+(aq)  | Co(s) , indicates that

Accepted Answer

A)   Co is the reducing agent.
B)   Co2+ ions are oxidized.
C)   Al is the reducing agent.
D)   Al3+ is the reducing agent.
E)   aluminum metal is the cathode.F) A) and B)
G) C) and E) C

Question 19

Predict the products of the cell reaction when a molten salt mixture of sodium bromide and calcium fluoride is electrolyzed (spectator ions are not considered to be products) .

Accepted Answer

A)   calcium and bromine
B)   sodium and fluorine
C)   calcium bromide
D)   calcium and fluorine
E)   sodium and bromineF) All of the above
G) D) and E)

Question 20

A voltaic cell consists of an Au/Au3+ electrode (E °\degree° = 1.50 V)  and a Cu/Cu2+ electrode (E °\degree°  = 0.34 V) . Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25 °\degree° C.

Accepted Answer

A)   0.001 M
B)   0.002 M
C)   0.01 M
D)   0.02 M
E)   0.04 M F) A) and E)
G) A) and D)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E $\degree$ _Fe = -0.44 V; all E $\degree$ values refer to the M²⁺/M half-cell reactions.

Correct Answer
verified

In the shorthand notation for cells, a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Correct Answer
verified
False

In the electrolysis of water, how many grams of oxygen gas will be produced for every gram of hydrogen gas formed? Reaction: 2H₂O(l) $\rightarrow$ 2H₂(g) + O₂(g)

Correct Answer
verified

Calculate $\Delta$ G $\degree$ for the reaction of iron(II) ions with one mole of permanganate ions. $Calculate \Delta G \degree for the reaction of iron(II) ions with one mole of permanganate ions. A) -71.4 kJ B) -286 kJ C) -357 kJ D) -428 kJ E) None of these choices is correct.$

Correct Answer
verified

Which component of the following cell notation is the anode? P | Q || R | S

Correct Answer
verified

Examine the following half-reactions and select the weakest oxidizing agent among the species listed.

Correct Answer
verified

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Correct Answer
verified

In the electrolyte of an electrochemical cell, current is carried by electrons moving from the anode to the cathode.

Correct Answer
verified

Correct Answer
verified

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states) ?

Correct Answer
verified

Which one of the following is not a redox reaction?

Correct Answer
verified

Which one of the following statements relating to the glass electrode is correct?

Correct Answer
verified

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

Correct Answer
verified

Examine the following half-reactions and select the strongest reducing agent among the species listed.

Correct Answer
verified

Correct Answer
verified

The voltaic cell made up of cobalt, copper and their M²⁺ ions, has E $\degree$ _cell = 0.62 V. If E $\degree$ of the cathode half-cell is 0.34 V, what is E $\degree$ of the anode half-cell? Cu²⁺(aq) + Co(s) $\rightarrow$ Cu(s) + Co²⁺(aq)

Correct Answer
verified
A

Correct Answer
verified

The line notation, Al(s) | Al³⁺(aq) || Co²⁺(aq) | Co(s) , indicates that

Correct Answer
verified
C

Predict the products of the cell reaction when a molten salt mixture of sodium bromide and calcium fluoride is electrolyzed (spectator ions are not considered to be products) .

Correct Answer
verified

A voltaic cell consists of an Au/Au³⁺ electrode (E $\degree$ = 1.50 V) and a Cu/Cu²⁺ electrode (E $\degree$ = 0.34 V) . Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25 $\degree$ C.

Correct Answer
verified

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E °\degree° Fe = -0.44 V; all E °\degree° values refer to the M2+/M half-cell reactions.

Correct AnswerverifiedShow Answer

In the shorthand notation for cells, a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Correct AnswerverifiedFalse

In the electrolysis of water, how many grams of oxygen gas will be produced for every gram of hydrogen gas formed? Reaction: 2H2O(l) →\rightarrow→ 2H2(g) + O2(g)

Correct AnswerverifiedShow Answer

Calculate Δ\DeltaΔ G °\degree° for the reaction of iron(II) ions with one mole of permanganate ions.

Correct AnswerverifiedShow Answer

Which component of the following cell notation is the anode? P | Q || R | S

Correct AnswerverifiedShow Answer

Examine the following half-reactions and select the weakest oxidizing agent among the species listed.

Correct AnswerverifiedShow Answer

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Correct AnswerverifiedShow Answer

In the electrolyte of an electrochemical cell, current is carried by electrons moving from the anode to the cathode.

Correct AnswerverifiedShow Answer

Consider the reaction in the lead-acid cell for which E °\degree° cell = 2.04 V at 298 K. Δ\DeltaΔ G °\degree° for this reaction is

Correct AnswerverifiedShow Answer

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states) ?

Correct AnswerverifiedShow Answer

Which one of the following is not a redox reaction?

Correct AnswerverifiedShow Answer

Which one of the following statements relating to the glass electrode is correct?

Correct AnswerverifiedShow Answer

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

Correct AnswerverifiedShow Answer

Examine the following half-reactions and select the strongest reducing agent among the species listed.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The voltaic cell made up of cobalt, copper and their M2+ ions, has E °\degree° cell = 0.62 V. If E °\degree° of the cathode half-cell is 0.34 V, what is E °\degree° of the anode half-cell? Cu2+(aq) + Co(s) →\rightarrow→ Cu(s) + Co2+(aq)

Correct AnswerverifiedA

What is the value of the equilibrium constant for the cell reaction below at 25 °\degree° C? E °\degree° cell = 0.30 V Sn2+(aq) + Fe(s) Sn(s) + Fe2+(aq)

Correct AnswerverifiedShow Answer

The line notation, Al(s) | Al3+(aq) || Co2+(aq) | Co(s) , indicates that

Correct AnswerverifiedC

Predict the products of the cell reaction when a molten salt mixture of sodium bromide and calcium fluoride is electrolyzed (spectator ions are not considered to be products) .

Correct AnswerverifiedShow Answer

A voltaic cell consists of an Au/Au3+ electrode (E °\degree° = 1.50 V) and a Cu/Cu2+ electrode (E °\degree° = 0.34 V) . Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25 °\degree° C.

Correct AnswerverifiedShow Answer

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E $\degree$ _Fe = -0.44 V; all E $\degree$ values refer to the M²⁺/M half-cell reactions.

Correct Answer
verified

Correct Answer
verified
False

In the electrolysis of water, how many grams of oxygen gas will be produced for every gram of hydrogen gas formed? Reaction: 2H₂O(l) $\rightarrow$ 2H₂(g) + O₂(g)

Correct Answer
verified

Calculate $\Delta$ G $\degree$ for the reaction of iron(II) ions with one mole of permanganate ions. $Calculate \Delta G \degree for the reaction of iron(II) ions with one mole of permanganate ions. A) -71.4 kJ B) -286 kJ C) -357 kJ D) -428 kJ E) None of these choices is correct.$

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The voltaic cell made up of cobalt, copper and their M²⁺ ions, has E $\degree$ _cell = 0.62 V. If E $\degree$ of the cathode half-cell is 0.34 V, what is E $\degree$ of the anode half-cell? Cu²⁺(aq) + Co(s) $\rightarrow$ Cu(s) + Co²⁺(aq)

Correct Answer
verified
A

Correct Answer
verified

The line notation, Al(s) | Al³⁺(aq) || Co²⁺(aq) | Co(s) , indicates that

Correct Answer
verified
C

Correct Answer
verified

A voltaic cell consists of an Au/Au³⁺ electrode (E $\degree$ = 1.50 V) and a Cu/Cu²⁺ electrode (E $\degree$ = 0.34 V) . Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25 $\degree$ C.

Correct Answer
verified