Question 1

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.F) None of the above
G) A) and C)

Question 2

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 VF) A) and E)
G) A) and C) B

Question 3

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)  F) None of the above
G) C) and D)

Question 4

Write the formula of the strongest oxidizing agent given the following standard reduction potentials in acid solution:  O2+4H++4e−→2H2OE∘=+1.23 VSn4++2e−→Sn2+E∘=+0.13 VZn2++2e−→Zn( s) E∘=−0.76 V\begin{array}{ll}\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{-} ightarrow 2 \mathrm{H}_{2} \mathrm{O} & \mathrm{E}^{\circ}=+1.23 \mathrm{~V} \\mathrm{Sn}^{4+}+2 \mathrm{e}^{-} ightarrow \mathrm{Sn}^{2+} & \mathrm{E}^{\circ}=+0.13 \mathrm{~V} \\mathrm{Zn}^{2+}+2 \mathrm{e}^{-} ightarrow \mathrm{Zn}(\mathrm{~s})  & \mathrm{E}^{\circ}=-0.76 \mathrm{~V}\end{array}O2​+4H++4e−→2H2​OSn4++2e−→Sn2+Zn2++2e−→Zn( s) ​E∘=+1.23 VE∘=+0.13 VE∘=−0.76 V​

Accepted Answer

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

Question 5

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 F) A) and D)
G) B) and D)

Question 6

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) F) B) and E)
G) A) and C)

Question 7

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 molF) A) and C)
G) C) and E)

Question 8

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 MF) C) and D)
G) A) and C)

Question 9

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) - F) A) and E)
G) B) and C) C

Question 10

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. F) A) and B)
G) C) and D)

Question 11

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 CF) A) and B)
G) C) and E)

Question 12

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 F) B) and E)
G) A) and E)

Question 13

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

Accepted Answer

A) True 
 B)False

Question 14

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. F) A) and B)
G) D) and E) C

Question 15

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.F) B) and C)
G) None of the above

Question 16

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 gF) D) and E)
G) B) and E)

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)  F) B) and D)
G) A) and C)

Question 18

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 aboveF) A) and E)
G) A) and C)

Question 19

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. F) A) and B)
G) C) and E)

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 F) B) and D)
G) C) and D)

Exam 18: Electrochemistry

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

Correct Answer
verified

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

Correct Answer
verified
B

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)

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified
C

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)

Correct Answer
verified

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

Correct Answer
verified

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]

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified
C

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

Correct Answer
verified

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

Correct Answer
verified

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)

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Exam 18: Electrochemistry

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedB

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)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedC

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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]

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedC

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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+)

Correct AnswerverifiedShow Answer

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

Correct Answer
verified

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

Correct Answer
verified
B

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)

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified
C

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)

Correct Answer
verified

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

Correct Answer
verified

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]

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified
C

Correct Answer
verified

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

Correct Answer
verified

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)

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified