Question 1

Predict the products of the electrolysis of aqueous potassium chloride KCl(aq).

Accepted Answer

A)  Cl-(aq) and K(s) 
B)  Cl2(g) and K(s) 
C)  Cl2(g) and H2(g) and OH-(aq) 
D)  Cl2(g) and K+(aq) 
E)  Cl-(aq) and K+(aq) 
A)  Cl-(aq) and K(s) 
B)  Cl2(g) and K(s) 
C)  Cl2(g) and H2(g) and OH-(aq) 
D)  Cl2(g) and K+(aq) 
E)  Cl-(aq) and K+(aq)

Question 2

Which of the following is true concerning a galvanic cell

Accepted Answer

A)  Reduction occurs at the anode and is where anions move towards 
B)  Reduction occurs at the cathode and is where anions move towards 
C)  Reduction occurs at the cathode and is where cations move towards 
D)  Oxidation occurs at the anode and is where cations move towards 
E)  Oxidation occurs at the cathode and is where cations move towards 
A)  Reduction occurs at the anode and is where anions move towards 
B)  Reduction occurs at the cathode and is where anions move towards 
C)  Reduction occurs at the cathode and is where cations move towards 
D)  Oxidation occurs at the anode and is where cations move towards 
E)  Oxidation occurs at the cathode and is where cations move towards

Question 3

Consider the reaction Hg2+(aq) + Hg(l) $\leftrightharpoons$ Hg22+(aq). Find the equilibrium constant for this reaction at 25$\circ$C.

Accepted Answer

A)  2 *101 
B)  6 * 1059 
C)  4 * 10-3 
D)  7 * 10-2 
E)  2 * 102 
A)  2 *101 
B)  6 * 1059 
C)  4 * 10-3 
D)  7 * 10-2 
E)  2 * 102

Question 4

Given the following standard reduction potentials, $\begin{array}{ll}
\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(\mathrm{s}) & \mathrm{E}^{\circ}=0.80 \mathrm{~V} \
\mathrm{AgCN}(\mathrm{s})+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(\mathrm{s})+\mathrm{CN}^{-}(\mathrm{aq}) & \mathrm{E}^{\circ}=-0.01 \mathrm{~V}
\end{array}$ calculate the solubility product of AgCN at 25$\circ$C.

Accepted Answer

A)  4.3 * 10-14 
B)  2.3 * 1013 
C)  2.1 * 10-14 
D)  5.1 * 1013 
E)  None of these 
A)  4.3 * 10-14 
B)  2.3 * 1013 
C)  2.1 * 10-14 
D)  5.1 * 1013 
E)  None of these

Question 5

A balanced redox equation must have which of the following: 
I. The same number of each type of atom on both sides of the equation
II. The total number electrons lost in the oxidation equal to total number of electrons gained in the reduction
III. The same total charge of all ionic species on both sides of the reaction
IV. H2O present as a product or a reactant

Accepted Answer

A)  I, II, and III 
B)  I and II 
C)  I, III, and IV 
D)  I, II, III, and IV 
E)  III and IV 
A)  I, II, and III 
B)  I and II 
C)  I, III, and IV 
D)  I, II, III, and IV 
E)  III and IV

Question 6

Predict the products of the electrolysis of aqueous aluminum bromide AlBr3(aq). (Balancing is not required.)

Accepted Answer

A)  Al + Br2 
B)  Al + O2 + H+ 
C)  H2 + OH- + Br2 
D)  H2 + O2 
A)  Al + Br2 
B)  Al + O2 + H+ 
C)  H2 + OH- + Br2 
D)  H2 + O2

Question 7

Consider the following standard reduction potentials in acid solution: $\begin{array}{ll}
&\underline{\mathrm{E}^\circ(V)}\
\mathrm{Al}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Al}(\mathrm{~s}) & -1.66 \
\mathrm{AgBr}(\mathrm{~s})+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(\mathrm{~s})+\mathrm{Br}^- & +0.07 \
\mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}^{2+} & +0.14 \
\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+} & +0.77
\end{array}$ The strongest reducing agent among those shown above is

Accepted Answer

A)  Fe3+. 
B)  Fe2+. 
C)  Br-. 
D)  Al3+. 
E)  Al. 
A)  Fe3+. 
B)  Fe2+. 
C)  Br-. 
D)  Al3+. 
E)  Al.

Question 8

Under basic conditions, the correctly balanced redox reaction for
PO33-(aq) + MnO4-(aq) $\rarr$PO43-(aq) + MnO2(s) is:
3PO33-(aq) + 2MnO4-(aq) + H2O(l) $\rarr$ 3PO43-(aq) + 2MnO2(s) + 2OH-(aq)

Accepted Answer

A) True 
 B)False

Question 9

Consider the following standard reduction potentials in acid solution: $\begin{array}{ll}
&\underline{\mathrm{E}^\circ(V)}\
\mathrm{Al}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Al}(\mathrm{~s}) & -1.66 \
\mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}^{2+} & +0.14 \
\mathrm{I}_{2}(\mathrm{s})+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{I}^{-}(\mathrm{aq}) & +0.53
\end{array}$ Which is the weakest oxidizing agent in this list

Accepted Answer

A)  Al3+(aq) 
B)  Al(s) 
C)  I-(aq) 
D)  I2(s) 
E)  Sn4+(aq) 
A)  Al3+(aq) 
B)  Al(s) 
C)  I-(aq) 
D)  I2(s) 
E)  Sn4+(aq)

Question 10

In an electrolytic cell, electrical energy is used to cause a chemical reaction to occur that would otherwise be nonspontaneous.

Accepted Answer

A) True 
 B)False

Question 11

Which one of the following is consistent with a galvanic cell

Accepted Answer

A) ($\Delta$G) cell > 0, Q cell cell  K 
D) ($\Delta$G) > 0, Ecell  0, Ecell  K 
A) ($\Delta$G) cell > 0, Q cell cell  K 
D) ($\Delta$G) > 0, Ecell  0, Ecell  K

Question 12

Complete and balance the following redox equation using the set of smallest whole-number coefficients. Now sum the coefficients of all species in the balanced equation. (Remember the coefficients that are equal to one.) The sum of the coefficients is BrO3-(aq) + Sb3+(aq) $\rarr$ Br-(aq) + Sb5+(aq) (acidic solution)

Accepted Answer

A)  4. 
B)  12. 
C)  13. 
D)  17. 
E)  None of these. 
A)  4. 
B)  12. 
C)  13. 
D)  17. 
E)  None of these.

Question 13

Calculate the cell emf for the following reaction at 25$\circ$C: 2Ag+(0.010 M) + H2(1 atm) $\rarr$ 2Ag(s) + 2H+(pH = 10.0)

Accepted Answer

A)  1.04 V 
B)  1.27 V 
C)  0.92 V 
D)  0.56 V 
E)  0.80 V 
A)  1.04 V 
B)  1.27 V 
C)  0.92 V 
D)  0.56 V 
E)  0.80 V

Question 14

Consider the following standard reduction potentials in acid solution: $\begin{array}{ll}
&\underline{\mathrm{E}^\circ(V)}\
\mathrm{Al}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Al}(\mathrm{~s}) & -1.66 \
\mathrm{AgBr}(\mathrm{~s})+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(\mathrm{~s})+\mathrm{Br}^- & +0.07 \
\mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}^{2+} & +0.14 \
\mathrm{Fe}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Fe}^{2+} & +0.77
\end{array}$ The strongest oxidizing agent among those shown above is

Accepted Answer

A)  Fe3+. 
B)  Fe2+. 
C)  Br-. 
D)  Al3+. 
E)  Al. 
A)  Fe3+. 
B)  Fe2+. 
C)  Br-. 
D)  Al3+. 
E)  Al.

Question 15

Which one of the following reactions will occur spontaneously at standard-state conditions and 25$\circ$C

Accepted Answer

A) Br2(l) + Sn(s) $\rarr$ 2Br-(aq) + Sn2+(aq) 
B) Fe2+(aq) + Ni(s) $\rarr$ Fe(s) + Ni2+(aq) 
C) 2Ag+(aq) 2H2O(l) $\rarr$ 2Ag(s) + 2H+(aq) + H2O2(aq) 
D) Mn2+(aq) + Cd(s) $\rarr$ Mn(s) + Cd2+(aq) 
E) Cr3+(aq) + 3Cu+(aq) $\rarr$ Cr(s) + 3Cu2+(aq) 
A) Br2(l) + Sn(s) $\rarr$ 2Br-(aq) + Sn2+(aq) 
B) Fe2+(aq) + Ni(s) $\rarr$ Fe(s) + Ni2+(aq) 
C) 2Ag+(aq) 2H2O(l) $\rarr$ 2Ag(s) + 2H+(aq) + H2O2(aq) 
D) Mn2+(aq) + Cd(s) $\rarr$ Mn(s) + Cd2+(aq) 
E) Cr3+(aq) + 3Cu+(aq) $\rarr$ Cr(s) + 3Cu2+(aq)

Question 16

The balanced overall redox equation for the following cell diagram:
Cr(s) | Cr3+(aq) || Sn4+(aq),Sn2+(aq) | Pt(s) is:
2Cr(s) + 3Sn4+(aq) $\rarr$ 2Cr3+(aq) + 3Sn2+(aq)

Accepted Answer

A) True 
 B)False

Question 17

Consider the following electrochemical cell: U | U3+(aq) || Cl-(aq),Cl2(g) | Pt
If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium

Accepted Answer

A)  -3.16 V 
B)  +3.16 V 
C)  -1.80 V 
D)  +1.80 V 
E)  +1.36 V 
A)  -3.16 V 
B)  +3.16 V 
C)  -1.80 V 
D)  +1.80 V 
E)  +1.36 V

Question 18

Which one of the following is consistent with a dead battery (an electrochemical cell at equilibrium)

Accepted Answer

A) ($\Delta$G) = 0, Ecell = 0, Q = K 
B) ($\Delta$G) cell > 0, Q cell  0, Ecell  0, Ecell = 0, Q > K 
A) ($\Delta$G) = 0, Ecell = 0, Q = K 
B) ($\Delta$G) cell > 0, Q cell  0, Ecell  0, Ecell = 0, Q > K

Question 19

Consider the following standard reduction potentials in acid solution: $\begin{array}{ll}
\mathrm{Cr}^{3+}+3 \mathrm{e}^{-} \rightarrow \mathrm{Cr} & \mathrm{E}^{\circ}=-0.74 \mathrm{~V} \
\mathrm{Co}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Co} & \mathrm{E}^{\circ}=-0.28 \mathrm{~V} \
\mathrm{MnO}_{4^{-}}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O} & \mathrm{E}^{\circ}=+1.51 \mathrm{~V}
\end{array}$ The weakest reducing agent listed above is

Accepted Answer

A)  Cr3+. 
B)  Cr. 
C)  Mn2+. 
D)  Co. 
E)  MnO4-. 
A)  Cr3+. 
B)  Cr. 
C)  Mn2+. 
D)  Co. 
E)  MnO4-.

Question 20

Which of these metals will not reduce water to hydrogen in basic solution under standard conditions

Accepted Answer

A)  Cd 
B)  Sr 
C)  Mg 
D)  Ba 
E)  K 
A)  Cd 
B)  Sr 
C)  Mg 
D)  Ba 
E)  K

Exam 18: Electrochemistry

Predict the products of the electrolysis of aqueous potassium chloride KCl(aq).

Which of the following is true concerning a galvanic cell

Consider the reaction Hg2+(aq) + Hg(l) ⇋\leftrightharpoons⇋ Hg22+(aq). Find the equilibrium constant for this reaction at 25 ∘\circ∘ C.

Given the following standard reduction potentials, ()+\rightarrow() =0.80 ()+\rightarrow()+() =-0.01 calculate the solubility product of AgCN at 25 ∘\circ∘ C.

Predict the products of the electrolysis of aqueous aluminum bromide AlBr3(aq). (Balancing is not required.)

Consider the following standard reduction potentials in acid solution: +3\rightarrow() -1.66 ()+\rightarrow()+ +0.07 +2\rightarrow +0.14 +\rightarrow +0.77 The strongest reducing agent among those shown above is

Under basic conditions, the correctly balanced redox reaction for PO33-(aq) + MnO4-(aq) →\rarr→ PO43-(aq) + MnO2(s) is: 3PO33-(aq) + 2MnO4-(aq) + H2O(l) →\rarr→ 3PO43-(aq) + 2MnO2(s) + 2OH-(aq)

Consider the following standard reduction potentials in acid solution: +3\rightarrow() -1.66 +2\rightarrow +0.14 ()+2\rightarrow2() +0.53 Which is the weakest oxidizing agent in this list

In an electrolytic cell, electrical energy is used to cause a chemical reaction to occur that would otherwise be nonspontaneous.

Which one of the following is consistent with a galvanic cell

Calculate the cell emf for the following reaction at 25 ∘\circ∘ C: 2Ag+(0.010 M) + H2(1 atm) →\rarr→ 2Ag(s) + 2H+(pH = 10.0)

Consider the following standard reduction potentials in acid solution: +3\rightarrow() -1.66 ()+\rightarrow()+ +0.07 +2\rightarrow +0.14 +\rightarrow +0.77 The strongest oxidizing agent among those shown above is

Which one of the following reactions will occur spontaneously at standard-state conditions and 25 ∘\circ∘ C

The balanced overall redox equation for the following cell diagram: Cr(s) | Cr3+(aq) || Sn4+(aq),Sn2+(aq) | Pt(s) is: 2Cr(s) + 3Sn4+(aq) →\rarr→ 2Cr3+(aq) + 3Sn2+(aq)

Consider the following electrochemical cell: U | U3+(aq) || Cl-(aq),Cl2(g) | Pt If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium

Which one of the following is consistent with a dead battery (an electrochemical cell at equilibrium)

Consider the following standard reduction potentials in acid solution: +3\rightarrow =-0.74 +2\rightarrow =-0.28 +8+5\rightarrow+4 =+1.51 The weakest reducing agent listed above is

Which of these metals will not reduce water to hydrogen in basic solution under standard conditions

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Consider the reaction Hg²⁺(aq) + Hg(l) $\leftrightharpoons$ Hg₂²⁺(aq). Find the equilibrium constant for this reaction at 25^$\circ$C.

Given the following standard reduction potentials, ()+\rightarrow() =0.80 ()+\rightarrow()+() =-0.01 calculate the solubility product of AgCN at 25^$\circ$C.

Predict the products of the electrolysis of aqueous aluminum bromide AlBr₃(aq). (Balancing is not required.)

Under basic conditions, the correctly balanced redox reaction for PO₃^3-(aq) + MnO₄^-(aq) $\rarr$ PO₄^3-(aq) + MnO₂(s) is: 3PO₃^3-(aq) + 2MnO₄^-(aq) + H₂O(l) $\rarr$ 3PO₄^3-(aq) + 2MnO₂(s) + 2OH^-(aq)

Calculate the cell emf for the following reaction at 25^$\circ$C: 2Ag⁺(0.010 M) + H₂(1 atm) $\rarr$ 2Ag(s) + 2H⁺(pH = 10.0)

Which one of the following reactions will occur spontaneously at standard-state conditions and 25^$\circ$C

The balanced overall redox equation for the following cell diagram: Cr(s) | Cr³⁺(aq) || Sn⁴⁺(aq),Sn²⁺(aq) | Pt(s) is: 2Cr(s) + 3Sn⁴⁺(aq) $\rarr$ 2Cr³⁺(aq) + 3Sn²⁺(aq)

Consider the following electrochemical cell: U | U³⁺(aq) || Cl^-(aq),Cl₂(g) | Pt If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium