Question 1

Find the emf of the cell described by the cell diagram Fe | Fe2+ (1.500M) || Au3+ (0.00400M) | Au.

Accepted Answer

A)  1.99 V 
B)  1.89 V 
C)  1.94 V 
D)  1.66 V 
E)  1.91 V 
A)  1.99 V 
B)  1.89 V 
C)  1.94 V 
D)  1.66 V 
E)  1.91 V B

Question 2

Suppose the reaction Pb(s) + 2H+(aq) $\rarr$ Pb2+(aq) + H2(g) is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II) ions that causes this reaction to be at equilibrium is

Accepted Answer

A)  2.5 M. 
B)  1.6 * 10-2 M. 
C)  2.5 * 10-4 M. 
D)  1.6 * 10-6 M. 
E)  0.40 M. 
A)  2.5 M. 
B)  1.6 * 10-2 M. 
C)  2.5 * 10-4 M. 
D)  1.6 * 10-6 M. 
E)  0.40 M. C

Question 3

A galvanic cell has the overall reaction:
 Zn(s) + 2Eu(NO3)3(aq) $\rarr$ Zn(NO3)2(aq) + 2Eu(NO3)2(aq)
Which is the half reaction occurring at the anode

Accepted Answer

A) NO3-(aq) + 4H+(aq) + 3e- $\rarr$ NO(g) + 2H2O(l) 
B) NO2(g) + H2O(l) $\rarr$ NO3-(aq) + 2H+(aq) + e- 
C) Zn(s) $\rarr$Zn2+(aq) + 2e- 
D) Eu3+(aq) + e- $\rarr$ Eu2+ 
E) Zn(s) + 2e- $\rarr$ Zn2+(aq)- 
A) NO3-(aq) + 4H+(aq) + 3e- $\rarr$ NO(g) + 2H2O(l) 
B) NO2(g) + H2O(l) $\rarr$ NO3-(aq) + 2H+(aq) + e- 
C) Zn(s) $\rarr$Zn2+(aq) + 2e- 
D) Eu3+(aq) + e- $\rarr$ Eu2+ 
E) Zn(s) + 2e- $\rarr$ Zn2+(aq)- C

Question 4

Complete and balance the following redox equation. When properly balanced using the smallest whole-number coefficients, the coefficient of S is H2S + HNO3 $\rarr$ S + NO (acidic solution)

Accepted Answer

A)  1. 
B)  2. 
C)  3. 
D)  5. 
E)  6. 
A)  1. 
B)  2. 
C)  3. 
D)  5. 
E)  6.

Question 5

Consider a voltaic cell based on the following cell reaction: Ni(s) + At2(s) $\rarr$ Ni2+(aq) + 2At- (aq)
Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine
[E$\circ$(Ni2+/Ni) = -0.25 V]

Accepted Answer

A)  0.80 V 
B)  0.30 V 
C)  -0.30 V 
D)  -0.80 V 
E)  0.43 V 
A)  0.80 V 
B)  0.30 V 
C)  -0.30 V 
D)  -0.80 V 
E)  0.43 V

Question 6

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25$\circ$C

Accepted Answer

A)  Ag 
B)  Au 
C)  Hg 
D)  Cu 
E)  Zn 
A)  Ag 
B)  Au 
C)  Hg 
D)  Cu 
E)  Zn

Question 7

H2(g) will form when Sn is placed in 1.0 M HCl.

Accepted Answer

A) True 
 B)False

Question 8

Using a table of standard electrode potentials, decide which of the following statements is completely true.

Accepted Answer

A)  Cu2+ can oxidize H2, and Fe can reduce Mn2+. 
B)  Ni2+ can oxidize Cu2+, and Fe2+ can reduce H+. 
C)  Fe2+ can oxidize H2, and Fe2+ can reduce Au3+. 
D)  Br2 can oxidize Ni, and H2 can reduce Mn2+. 
E)  H+ can oxidize Fe, and Ni can reduce Br2. 
A)  Cu2+ can oxidize H2, and Fe can reduce Mn2+. 
B)  Ni2+ can oxidize Cu2+, and Fe2+ can reduce H+. 
C)  Fe2+ can oxidize H2, and Fe2+ can reduce Au3+. 
D)  Br2 can oxidize Ni, and H2 can reduce Mn2+. 
E)  H+ can oxidize Fe, and Ni can reduce Br2.

Question 9

How many coulombs would be required to electroplate 35.0 grams of chromium by passing an electrical current through a solution containing CrCl3

Accepted Answer

A)  6.50 * 104 C 
B)  2.16 * 104 C 
C)  6.40 * 104 C 
D)  1.95 * 105 C 
E)  1.01 * 107 C 
A)  6.50 * 104 C 
B)  2.16 * 104 C 
C)  6.40 * 104 C 
D)  1.95 * 105 C 
E)  1.01 * 107 C

Question 10

Which one of the following reagents is capable of oxidizing Br- (aq) to Br2(l) under standard-state conditions

Accepted Answer

A)  I- (aq) 
B)  NO3- (aq) 
C)  Ag+ (aq) 
D)  Al3+ (aq) 
E)  Au3+ (aq) 
A)  I- (aq) 
B)  NO3- (aq) 
C)  Ag+ (aq) 
D)  Al3+ (aq) 
E)  Au3+ (aq)

Question 11

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl3 for 45.0 min

Accepted Answer

A)  9.3 * 10-4 g 
B)  0.042 g 
C)  2.5 g 
D)  24 g 
E)  2.3 * 1010 g 
A)  9.3 * 10-4 g 
B)  0.042 g 
C)  2.5 g 
D)  24 g 
E)  2.3 * 1010 g

Question 12

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl2 for 4.50 hours. How many moles of calcium metal should be deposited

Accepted Answer

A)  5.83 * 10-5 mol 
B)  0.210 mol 
C)  0.420 mol 
D)  0.840 mol 
E)  1.95 * 109 mol 
A)  5.83 * 10-5 mol 
B)  0.210 mol 
C)  0.420 mol 
D)  0.840 mol 
E)  1.95 * 109 mol

Question 13

If the measured voltage of the cell Zn(s) | Zn2+(aq) || Ag+(aq) | Ag(s) is 1.37 V when the concentration of Zn2+ ion is 0.010 M, what is the Ag+ ion concentration

Accepted Answer

A)  2.5 M 
B)  4.0* 10-9 M 
C)  6.2 * 10-3 M 
D)  2.6 * 10-51 M 
E)  6.2 * 10-5 M 
A)  2.5 M 
B)  4.0* 10-9 M 
C)  6.2 * 10-3 M 
D)  2.6 * 10-51 M 
E)  6.2 * 10-5 M

Question 14

How many moles of H2 are produced by 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 102 s

Accepted Answer

A)  0.0104 mol 
B)  0.0124 mol 
C)  0.0144 mol 
D)  0.0164 mol 
E)  None of the above 
A)  0.0104 mol 
B)  0.0124 mol 
C)  0.0144 mol 
D)  0.0164 mol 
E)  None of the above

Question 15

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge.
- a Fe electrode in 1.0 M FeCl2 solution 
- a Sn electrode in 1.0 M Sn(NO3)2 solution
When the cell is running spontaneously, which choice includes only true statements and no false ones

Accepted Answer

A)  The tin electrode loses mass and the tin electrode is the cathode. 
B)  The tin electrode gains mass and the tin electrode is the cathode. 
C)  The iron electrode gains mass and the iron electrode is the anode. 
D)  The iron electrode loses mass and the iron electrode is the cathode. 
E)  The iron electrode gains mass and the iron electrode is the cathode. 
A)  The tin electrode loses mass and the tin electrode is the cathode. 
B)  The tin electrode gains mass and the tin electrode is the cathode. 
C)  The iron electrode gains mass and the iron electrode is the anode. 
D)  The iron electrode loses mass and the iron electrode is the cathode. 
E)  The iron electrode gains mass and the iron electrode is the cathode.

Question 16

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Br2 $\rarr$ BrO3- + Br- (basic solution)

Accepted Answer

A)  9. 
B)  12. 
C)  18. 
D)  21. 
E)  None of the above. 
A)  9. 
B)  12. 
C)  18. 
D)  21. 
E)  None of the above.

Question 17

Determine the cell diagram for the reaction below. Assume a platinum electrode is used when no other solid is present.
2Fe2+(aq) + Pb2+(aq) $\rarr$ 2Fe3+(aq) + Pb(s)

Accepted Answer

A)  Pt(s) | Fe2+(aq), Fe3+(aq) || Pb2+(aq) | Pb(s) 
B)  Pb(s) | Pb2+(aq) || Fe2+(aq), Fe3+(aq) | Pt(s) 
C)  Pt(s) | Fe3+(aq), Fe2+(aq) || Pb(s) | Pb2+(aq) | Pt(s) 
D)  Pt(s) | Pb2+(aq) | Pb(s) || Fe2+(aq), Fe3+(aq) | Pt(s) 
E)  Pt(s) | Fe2+(aq), Pb2+(aq) || Fe3+(aq) | Pb(s) 
A)  Pt(s) | Fe2+(aq), Fe3+(aq) || Pb2+(aq) | Pb(s) 
B)  Pb(s) | Pb2+(aq) || Fe2+(aq), Fe3+(aq) | Pt(s) 
C)  Pt(s) | Fe3+(aq), Fe2+(aq) || Pb(s) | Pb2+(aq) | Pt(s) 
D)  Pt(s) | Pb2+(aq) | Pb(s) || Fe2+(aq), Fe3+(aq) | Pt(s) 
E)  Pt(s) | Fe2+(aq), Pb2+(aq) || Fe3+(aq) | Pb(s)

Question 18

Determine the cell diagram for the reaction below. Assume platinum electrodes are used when no other solid is present.
Cl2(g) + Sn2+(aq) $\rarr$ Sn4+(aq) + 2Cl-(aq)

Accepted Answer

A)  Pt(s) | Cl2(g) | Cl-(aq) || Sn2+(aq), Sn4+(aq) | Pt(s) 
B)  Pt(s) | Sn2+(aq), Sn4+(aq) || Cl2(g) | Cl-(aq) | Pt(s) 
C)  Pt(s) | Sn4+(aq), Sn2+(aq) || Cl-(aq) | Cl2(g) | Pt(s) 
D)  Pt(s) | Cl-(g) | Cl2(aq) || Sn4+(aq), Sn2+(aq) | Pt(s) 
E)  Pt(s) | Cl2(g) | Sn2+(aq) || Sn4+(aq), Cl-(aq) | Pt(s) 
A)  Pt(s) | Cl2(g) | Cl-(aq) || Sn2+(aq), Sn4+(aq) | Pt(s) 
B)  Pt(s) | Sn2+(aq), Sn4+(aq) || Cl2(g) | Cl-(aq) | Pt(s) 
C)  Pt(s) | Sn4+(aq), Sn2+(aq) || Cl-(aq) | Cl2(g) | Pt(s) 
D)  Pt(s) | Cl-(g) | Cl2(aq) || Sn4+(aq), Sn2+(aq) | Pt(s) 
E)  Pt(s) | Cl2(g) | Sn2+(aq) || Sn4+(aq), Cl-(aq) | Pt(s)

Question 19

Write the formula of the strongest oxidizing agent given the following standard reduction potentials in acid solution: $\begin{array}{ll}
\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightarrow 2 \mathrm{H}_{2} \mathrm{O} & \mathrm{E}^{\circ}=+1.23 \mathrm{~V} \
\mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}^{2+} & \mathrm{E}^{\circ}=+0.13 \mathrm{~V} \
\mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(\mathrm{~s}) & \mathrm{E}^{\circ}=-0.76 \mathrm{~V}
\end{array}$

Accepted Answer

A)  Sn4+ 
B)  O2 
C)  Zn2+ 
D)  2H2O 
E)  None of the above 
A)  Sn4+ 
B)  O2 
C)  Zn2+ 
D)  2H2O 
E)  None of the above

Question 20

Consider an electrochemical cell based on the following cell diagram: 
Pt | Pu3+(aq), Pu4+(aq) || Cl2(g), Cl- (aq) | Pt
Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E$\circ$(Pu4+/Pu3+)

Accepted Answer

A)  2.37 V 
B)  1.01 V 
C)  -1.71 V 
D)  -1.01 V 
E)  1.71 V 
A)  2.37 V 
B)  1.01 V 
C)  -1.71 V 
D)  -1.01 V 
E)  1.71 V

Exam 18: Electrochemistry

Find the emf of the cell described by the cell diagram Fe | Fe2+ (1.500M) || Au3+ (0.00400M) | Au.

Suppose the reaction Pb(s) + 2H+(aq) →\rarr→ Pb2+(aq) + H2(g) is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II) ions that causes this reaction to be at equilibrium is

A galvanic cell has the overall reaction: Zn(s) + 2Eu(NO3)3(aq) →\rarr→ Zn(NO3)2(aq) + 2Eu(NO3)2(aq) Which is the half reaction occurring at the anode

Complete and balance the following redox equation. When properly balanced using the smallest whole-number coefficients, the coefficient of S is H2S + HNO3 →\rarr→ S + NO (acidic solution)

Consider a voltaic cell based on the following cell reaction: Ni(s) + At2(s) →\rarr→ Ni2+(aq) + 2At- (aq) Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine [E ∘\circ∘ (Ni2+/Ni) = -0.25 V]

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25 ∘\circ∘ C

H2(g) will form when Sn is placed in 1.0 M HCl.

Using a table of standard electrode potentials, decide which of the following statements is completely true.

How many coulombs would be required to electroplate 35.0 grams of chromium by passing an electrical current through a solution containing CrCl3

Which one of the following reagents is capable of oxidizing Br- (aq) to Br2(l) under standard-state conditions

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl3 for 45.0 min

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl2 for 4.50 hours. How many moles of calcium metal should be deposited

If the measured voltage of the cell Zn(s) | Zn2+(aq) || Ag+(aq) | Ag(s) is 1.37 V when the concentration of Zn2+ ion is 0.010 M, what is the Ag+ ion concentration

How many moles of H2 are produced by 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 102 s

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl2 solution - a Sn electrode in 1.0 M Sn(NO3)2 solution When the cell is running spontaneously, which choice includes only true statements and no false ones

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Br2 →\rarr→ BrO3- + Br- (basic solution)

Determine the cell diagram for the reaction below. Assume a platinum electrode is used when no other solid is present. 2Fe2+(aq) + Pb2+(aq) →\rarr→ 2Fe3+(aq) + Pb(s)

Determine the cell diagram for the reaction below. Assume platinum electrodes are used when no other solid is present. Cl2(g) + Sn2+(aq) →\rarr→ Sn4+(aq) + 2Cl-(aq)

Write the formula of the strongest oxidizing agent given the following standard reduction potentials in acid solution: +4+4\rightarrow2 =+1.23 +2\rightarrow =+0.13 +2\rightarrow() =-0.76

Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq) || Cl2(g), Cl- (aq) | Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E ∘\circ∘ (Pu4+/Pu3+)

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Find the emf of the cell described by the cell diagram Fe | Fe²⁺ (1.500M) || Au³⁺ (0.00400M) | Au.

Suppose the reaction Pb(s) + 2H⁺(aq) $\rarr$ Pb²⁺(aq) + H₂(g) is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II) ions that causes this reaction to be at equilibrium is

A galvanic cell has the overall reaction: Zn(s) + 2Eu(NO₃)₃(aq) $\rarr$ Zn(NO₃)₂(aq) + 2Eu(NO₃)₂(aq) Which is the half reaction occurring at the anode

Complete and balance the following redox equation. When properly balanced using the smallest whole-number coefficients, the coefficient of S is H₂S + HNO₃ $\rarr$ S + NO (acidic solution)

Consider a voltaic cell based on the following cell reaction: Ni(s) + At₂(s) $\rarr$ Ni²⁺(aq) + 2At^- (aq) Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine [E^$\circ$(Ni²⁺/Ni) = -0.25 V]

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25^$\circ$C

H₂(g) will form when Sn is placed in 1.0 M HCl.

How many coulombs would be required to electroplate 35.0 grams of chromium by passing an electrical current through a solution containing CrCl₃

Which one of the following reagents is capable of oxidizing Br^- (aq) to Br₂(l) under standard-state conditions

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl₃ for 45.0 min

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl₂ for 4.50 hours. How many moles of calcium metal should be deposited

If the measured voltage of the cell Zn(s) | Zn²⁺(aq) || Ag⁺(aq) | Ag(s) is 1.37 V when the concentration of Zn²⁺ ion is 0.010 M, what is the Ag⁺ ion concentration

How many moles of H₂ are produced by 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 10² s

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl₂ solution - a Sn electrode in 1.0 M Sn(NO₃)₂ solution When the cell is running spontaneously, which choice includes only true statements and no false ones

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Br₂ $\rarr$ BrO₃^- + Br^- (basic solution)

Determine the cell diagram for the reaction below. Assume a platinum electrode is used when no other solid is present. 2Fe²⁺(aq) + Pb²⁺(aq) $\rarr$ 2Fe³⁺(aq) + Pb(s)

Determine the cell diagram for the reaction below. Assume platinum electrodes are used when no other solid is present. Cl₂(g) + Sn²⁺(aq) $\rarr$ Sn⁴⁺(aq) + 2Cl^-(aq)