Question 1

An electroplating solution is made up of nickel(II)sulfate.How much time would it take to deposit 0.500 g of metallic nickel on a custom car part using a current of 3.00 A?

Accepted Answer

The answer of An electroplating solution is made up of...

Question 2

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 $\times$ 104 C 
B) 2.16 $\times$ 104 C 
C) 6.40 $\times$ 104 C 
D) 1.95 $\times$ 105 C 
E) 1.01 $\times$ 107 C 
A) 6.50 $\times$ 104 C 
B) 2.16 $\times$ 104 C 
C) 6.40 $\times$ 104 C 
D) 1.95 $\times$ 105 C 
E) 1.01 $\times$ 107 C

Question 3

The half-reaction that should occur at the anode during electrolysis of an aqueous potassium bromide solution is

Accepted Answer

A) Br2 + 2e- $\to$ 2Br-. 
B) Na $\to$ Na+ + e-. 
C) Na+ + e- $\to$ Na. 
D) 2Br- $\to$ Br2 + 2e-. 
E) 2H2O $\to$O2 + 4H+ + 4e-. 
A) Br2 + 2e- $\to$ 2Br-. 
B) Na $\to$ Na+ + e-. 
C) Na+ + e- $\to$ Na. 
D) 2Br- $\to$ Br2 + 2e-. 
E) 2H2O $\to$O2 + 4H+ + 4e-.

Question 4

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 5

Consider the following standard reduction potentials in acid solution:   The strongest oxidizing agent listed above is

Accepted Answer

A) Cr3+. 
B) Cr. 
C) Mn2+. 
D) Co2+. 
E) MnO4-. 
A) Cr3+. 
B) Cr. 
C) Mn2+. 
D) Co2+. 
E) MnO4-.

Question 6

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO4 for a period of 19.0 min?

Accepted Answer

Question 7

Which one of the following reagents is capable of transforming Cu2+(1 M)to Cu(s)?

Accepted Answer

A) I- (1 M) 
B) Ni(s) 
C) Al3+ (1 M) 
D) F- (1 M) 
E) Ag(s) 
A) I- (1 M) 
B) Ni(s) 
C) Al3+ (1 M) 
D) F- (1 M) 
E) Ag(s)

Question 8

The measured voltage of the cell Pt(s)| H2 (1.0 atm)| H+(aq)|| Ag+(1.0 M)| Ag(s)is 1.02 V at 25°C. Calculate the pH of the solution.

Accepted Answer

A) 1.86 
B) 1.69 
C) 3.72 
D) 3.89 
E) 7.43 
A) 1.86 
B) 1.69 
C) 3.72 
D) 3.89 
E) 7.43

Question 9

How many coulombs (C)of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca2+ ion to calcium metal?

Accepted Answer

A) 190,000 C 
B) 85,000 C 
C) 21,000 C 
D) 42,500 C 
E) 0.88 C 
A) 190,000 C 
B) 85,000 C 
C) 21,000 C 
D) 42,500 C 
E) 0.88 C

Question 10

Consider the reaction Fe + Sn2+(1 $\times$ 10-3 M)$\to$ Fe2+(1.0 M)+ Sn. In what direction do the Cl-  ions in the KCl salt bridge flow?

Accepted Answer

away from the cathod

Question 11

Given the following standard reduction potentials in acid solution   write a balanced equation for a spontaneous reaction which involves the tin and zinc redox couples.

Accepted Answer

Zn + Sn⁴⁺

Question 12

The half-cell reaction for the oxidation of H2O(l)to O2(g)is given below. 2H2O(l)$\to$O2(g)+ 4H+(aq)+ 4e-
 Which choice lists all of the following species that can oxidize H2O to O2(g)under standard-state conditions?
MnO4-(aq), Cl2(g), Pb2+(aq), Cl- (aq), Ag+(aq)

Accepted Answer

A) Cl-(aq)only 
B) Cl2(g)only 
C) Pb2+(aq)and Ag+(aq) 
D) Cl-(aq)and MnO4-(aq) 
E) MnO4-(aq)and Cl2(g) 
A) Cl-(aq)only 
B) Cl2(g)only 
C) Pb2+(aq)and Ag+(aq) 
D) Cl-(aq)and MnO4-(aq) 
E) MnO4-(aq)and Cl2(g)

Question 13

Determine the equilibrium constant for the following reaction at 25°C.
2I- (aq)+ Br2(l)   I2(s)+ 2Br-(aq).

Accepted Answer

1.8 @#LAT-DLM& 10<su

Question 14

Calculate the cell emf for the following reaction at 25°C: Ni(s)+ 2Cu2+(0.010 M)$\to$ Ni2+(0.0010 M)+ 2Cu+(1.0 M)

Accepted Answer

A) 0.40 V 
B) -0.43 V 
C) 0.43 V 
D) 0.34 V 
E) 0.37 V 
A) 0.40 V 
B) -0.43 V 
C) 0.43 V 
D) 0.34 V 
E) 0.37 V

Question 15

Calculate the standard cell emf for the following cell: Mg | Mg2+ || NO3- (acid soln)| NO(g)| Pt

Accepted Answer

A) 3.33 V 
B) 1.41 V 
C) -1.41 V 
D) 8.46 V 
E) -8.46 V 
A) 3.33 V 
B) 1.41 V 
C) -1.41 V 
D) 8.46 V 
E) -8.46 V

Question 16

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is MnO4- + H+ + Br- $\to$ Mn2+ + Br2 + H2O (acidic solution)

Accepted Answer

A) 6 
B) 17 
C) 21 
D) 29 
E) 43 
A) 6 
B) 17 
C) 21 
D) 29 
E) 43

Question 17

The half-reaction that occurs at the cathode during electrolysis of an aqueous sodium iodide solution is

Accepted Answer

A) Na+ + e- $\to$Na. 
B) Na $\to$Na+ + e-. 
C) 2H2O + 2e- $\to$ H2 + 2OH-. 
D) I2 + 2e- $\to$ 2I-. 
E) 2I- $\to$ I2 + 2e-. 
A) Na+ + e- $\to$Na. 
B) Na $\to$Na+ + e-. 
C) 2H2O + 2e- $\to$ H2 + 2OH-. 
D) I2 + 2e- $\to$ 2I-. 
E) 2I- $\to$ I2 + 2e-.

Question 18

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn2+ is 2.0 M, what is the concentration of Cu2+?

Accepted Answer

1.5 @#LAT-DLM& 10<su

Question 19

Consider the following standard reduction potentials in acid solution:   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 20

Find the emf of the cell described by the cell diagram Ni | Ni2+ (0.750 M)|| Cu2+ (0.0500 M)| Cu

Accepted Answer

A) 0.62 V 
B) 0.52 V 
C) 0.59 V 
D) 0.66 V 
E) 0.56 V 
A) 0.62 V 
B) 0.52 V 
C) 0.59 V 
D) 0.66 V 
E) 0.56 V

Exam 19: Electrochemistry

An electroplating solution is made up of nickel(II)sulfate.How much time would it take to deposit 0.500 g of metallic nickel on a custom car part using a current of 3.00 A?

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

The half-reaction that should occur at the anode during electrolysis of an aqueous potassium bromide solution is

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?

Consider the following standard reduction potentials in acid solution: The strongest oxidizing agent listed above is

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO4 for a period of 19.0 min?

Which one of the following reagents is capable of transforming Cu2+(1 M)to Cu(s)?

The measured voltage of the cell Pt(s)| H2 (1.0 atm)| H+(aq)|| Ag+(1.0 M)| Ag(s)is 1.02 V at 25°C. Calculate the pH of the solution.

How many coulombs (C)of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca2+ ion to calcium metal?

Consider the reaction Fe + Sn2+(1 ×\times× 10-3 M) →\to→ Fe2+(1.0 M)+ Sn. In what direction do the Cl- ions in the KCl salt bridge flow?

Given the following standard reduction potentials in acid solution write a balanced equation for a spontaneous reaction which involves the tin and zinc redox couples.

The half-cell reaction for the oxidation of H2O(l)to O2(g)is given below. 2H2O(l) →\to→ O2(g)+ 4H+(aq)+ 4e- Which choice lists all of the following species that can oxidize H2O to O2(g)under standard-state conditions? MnO4-(aq), Cl2(g), Pb2+(aq), Cl- (aq), Ag+(aq)

Determine the equilibrium constant for the following reaction at 25°C. 2I- (aq)+ Br2(l) I2(s)+ 2Br-(aq).

Calculate the cell emf for the following reaction at 25°C: Ni(s)+ 2Cu2+(0.010 M) →\to→ Ni2+(0.0010 M)+ 2Cu+(1.0 M)

Calculate the standard cell emf for the following cell: Mg | Mg2+ || NO3- (acid soln)| NO(g)| Pt

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is MnO4- + H+ + Br- →\to→ Mn2+ + Br2 + H2O (acidic solution)

The half-reaction that occurs at the cathode during electrolysis of an aqueous sodium iodide solution is

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn2+ is 2.0 M, what is the concentration of Cu2+?

Consider the following standard reduction potentials in acid solution: Which is the weakest oxidizing agent in this list?

Find the emf of the cell described by the cell diagram Ni | Ni2+ (0.750 M)|| Cu2+ (0.0500 M)| Cu

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

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO₄ for a period of 19.0 min?

Which one of the following reagents is capable of transforming Cu²⁺(1 M)to Cu(s)?

The measured voltage of the cell Pt(s)| H₂ (1.0 atm)| H⁺(aq)|| Ag⁺(1.0 M)| Ag(s)is 1.02 V at 25°C. Calculate the pH of the solution.

How many coulombs (C)of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca²⁺ ion to calcium metal?

Consider the reaction Fe + Sn²⁺(1 $\times$ 10^-3 M) $\to$ Fe²⁺(1.0 M)+ Sn. In what direction do the Cl^- ions in the KCl salt bridge flow?

The half-cell reaction for the oxidation of H₂O(l)to O₂(g)is given below. 2H₂O(l) $\to$ O₂(g)+ 4H⁺(aq)+ 4e^- Which choice lists all of the following species that can oxidize H₂O to O₂(g)under standard-state conditions? MnO₄^-(aq), Cl₂(g), Pb²⁺(aq), Cl^-(aq), Ag⁺(aq)

Determine the equilibrium constant for the following reaction at 25°C. 2I^-(aq)+ Br₂(l) I₂(s)+ 2Br^-(aq).

Calculate the cell emf for the following reaction at 25°C: Ni(s)+ 2Cu²⁺(0.010 M) $\to$ Ni²⁺(0.0010 M)+ 2Cu⁺(1.0 M)

Calculate the standard cell emf for the following cell: Mg | Mg²⁺ || NO₃^-(acid soln)| NO(g)| Pt

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is MnO₄^- + H⁺ + Br^- $\to$ Mn²⁺ + Br₂ + H₂O (acidic solution)

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn²⁺ is 2.0 M, what is the concentration of Cu²⁺?

Find the emf of the cell described by the cell diagram Ni | Ni²⁺ (0.750 M)|| Cu²⁺ (0.0500 M)| Cu