Question 1

Complete and balance the following redox reaction under acidic conditions:
MnO4-(aq)+ C2O42-(aq)$\to$  Mn2+(aq)+ CO2(aq)

Accepted Answer

2MnO₄^-(aq)+ 5C₂O₄^2-(aq)+ 16H⁺(aq)$\to$ 2Mn²⁺(aq)+ 10CO₂(aq)+ 8H₂O(l)

Question 2

Calculate the value of E°cell for the following reaction: 2Au(s)+ 3Ca2+(aq)$\to$ 2Au3+(aq)+ 3Ca(s)

Accepted Answer

A) -4.37 V 
B) -1.37 V 
C) -11.6 V 
D) 1.37 V 
E) 4.37 V 
A) -4.37 V 
B) -1.37 V 
C) -11.6 V 
D) 1.37 V 
E) 4.37 V A

Question 3

The half-reaction occurring at the cathode during electrolysis of an aqueous copper(II)iodide solution is

Accepted Answer

A) I2 + 2e- $\to$ 2I-. 
B) Cu $\to$ Cu2+ + 2e-. 
C) Cu2+ + 2e- $\to$ Cu. 
D) 2I-  $\to$ I2 + 2e-. 
E) 2e- + 2H2O $\to$ H2 + 2OH-. 
A) I2 + 2e- $\to$ 2I-. 
B) Cu $\to$ Cu2+ + 2e-. 
C) Cu2+ + 2e- $\to$ Cu. 
D) 2I-  $\to$ I2 + 2e-. 
E) 2e- + 2H2O $\to$ H2 + 2OH-. C

Question 4

Given the following standard reduction potentials in acid solution   write the formula of the weakest reducing agent.

Accepted Answer

The answer of Given the following standard reduction potentials in...

Question 5

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO4(aq)and Pb(NO3)2 (aq)solutions, respectively. If sulfuric acid is then added to the Pb(NO3)2 solution, thereby forming a precipitate of PbSO4, what will happen to the cell potential?

Accepted Answer

The cell p

Question 6

Under standard-state conditions, which of the following half-reactions occurs at the cathode during the electrolysis of aqueous nickel sulfate at 25°C?

Accepted Answer

A) 2H2O $\to$ O2 + 4H+ + 4e- 
B) Ni2+ + 2e- $\to$ Ni 
C) 2H2O + 2e- $\to$ H2 + 2OH- 
D) Ni $\to$ Ni2+ + 2e- 
A) 2H2O $\to$ O2 + 4H+ + 4e- 
B) Ni2+ + 2e- $\to$ Ni 
C) 2H2O + 2e- $\to$ H2 + 2OH- 
D) Ni $\to$ Ni2+ + 2e-

Question 7

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn2+ || NO3- (acid soln), NO(g)| Pt

Accepted Answer

A) Sn 
B) Sn2+ 
C) NO3- 
D) NO 
E) Pt 
A) Sn 
B) Sn2+ 
C) NO3- 
D) NO 
E) Pt

Question 8

You wish to electroplate a metal utensil with a surface area of 736 cm2 with gold to give an average thickness of 0.025 mm over the entire surface.Starting with a solution of excess Au3+ and applying a constant current of 14 A, how long will it take to electroplate the utensil? The density of gold is 19.3 g/cm3.

Accepted Answer

Question 9

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)$\to$ 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 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

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Br2 $\to$ 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 12

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl2. If Ecell is found to be 0.24 V, what is the pH of the acetic acid solution?

Accepted Answer

Question 13

Complete and balance the following redox reaction under acidic conditions:
Cr2O72-(aq)+ I-(aq)$\to$ Cr3+(aq)+ IO3-(aq)

Accepted Answer

Cr<sub>2</sub>O<sub>7</sub><su

Question 14

Given the following standard reduction potentials in acid solution   write the formula of the strongest oxidizing agent.

Accepted Answer

The answer of Given the following standard reduction potentials in...

Question 15

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min?

Accepted Answer

A) 0.20 g 
B) 0.40 g 
C) 12 g 
D) 24 g 
E) 47 g 
A) 0.20 g 
B) 0.40 g 
C) 12 g 
D) 24 g 
E) 47 g

Question 16

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO3(aq)using a current of 6.0 A?

Accepted Answer

Question 17

Complete and balance the following redox reaction under acidic conditions:
Cu(s)+ NO3-(aq)$\to$ Cu2+(aq)+ NO2(g)

Accepted Answer

Cu(s)+ 2NO₃^-</

Question 18

Complete and balance the following redox equation using the smallest whole-number coefficients. What is the coefficient of Sn in the balanced equation? Sn + HNO3 $\to$ SnO2 + NO2 + H2O (acidic solution)

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 5 
A) 1 
B) 2 
C) 3 
D) 4 
E) 5

Question 19

What concentration of Ni2+ ion remains in solution after electrolysis of 100.mL of 0.250 M NiSO4 solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

Accepted Answer

Question 20

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO2(s)+ Cl- $\to$ Pb2+ + Cl2(g)(acidic solution)

Accepted Answer

A) 2 
B) 4 
C) 5 
D) 9 
E) 11 
A) 2 
B) 4 
C) 5 
D) 9 
E) 11

Exam 19: Electrochemistry

Complete and balance the following redox reaction under acidic conditions: MnO4-(aq)+ C2O42-(aq) →\to→ Mn2+(aq)+ CO2(aq)

Calculate the value of E°cell for the following reaction: 2Au(s)+ 3Ca2+(aq) →\to→ 2Au3+(aq)+ 3Ca(s)

The half-reaction occurring at the cathode during electrolysis of an aqueous copper(II)iodide solution is

Given the following standard reduction potentials in acid solution write the formula of the weakest reducing agent.

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO4(aq)and Pb(NO3)2 (aq)solutions, respectively. If sulfuric acid is then added to the Pb(NO3)2 solution, thereby forming a precipitate of PbSO4, what will happen to the cell potential?

Under standard-state conditions, which of the following half-reactions occurs at the cathode during the electrolysis of aqueous nickel sulfate at 25°C?

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn2+ || NO3- (acid soln), NO(g)| Pt

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

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

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl2. If Ecell is found to be 0.24 V, what is the pH of the acetic acid solution?

Complete and balance the following redox reaction under acidic conditions: Cr2O72-(aq)+ I-(aq) →\to→ Cr3+(aq)+ IO3-(aq)

Given the following standard reduction potentials in acid solution write the formula of the strongest oxidizing agent.

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min?

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO3(aq)using a current of 6.0 A?

Complete and balance the following redox reaction under acidic conditions: Cu(s)+ NO3-(aq) →\to→ Cu2+(aq)+ NO2(g)

Complete and balance the following redox equation using the smallest whole-number coefficients. What is the coefficient of Sn in the balanced equation? Sn + HNO3 →\to→ SnO2 + NO2 + H2O (acidic solution)

What concentration of Ni2+ ion remains in solution after electrolysis of 100.mL of 0.250 M NiSO4 solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO2(s)+ Cl- →\to→ Pb2+ + Cl2(g)(acidic solution)

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Complete and balance the following redox reaction under acidic conditions: MnO₄^-(aq)+ C₂O₄^2-(aq) $\to$ Mn²⁺(aq)+ CO₂(aq)

Calculate the value of E°_cell for the following reaction: 2Au(s)+ 3Ca²⁺(aq) $\to$ 2Au³⁺(aq)+ 3Ca(s)

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO₄(aq)and Pb(NO₃)₂ (aq)solutions, respectively. If sulfuric acid is then added to the Pb(NO₃)₂ solution, thereby forming a precipitate of PbSO₄, what will happen to the cell potential?

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn²⁺ || NO₃^-(acid soln), NO(g)| Pt

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

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl₂. If E_cell is found to be 0.24 V, what is the pH of the acetic acid solution?

Complete and balance the following redox reaction under acidic conditions: Cr₂O₇^2-(aq)+ I^-(aq) $\to$ Cr³⁺(aq)+ IO₃^-(aq)

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO₄ for 90.0 min?

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO₃(aq)using a current of 6.0 A?

Complete and balance the following redox reaction under acidic conditions: Cu(s)+ NO₃^-(aq) $\to$ Cu²⁺(aq)+ NO₂(g)

Complete and balance the following redox equation using the smallest whole-number coefficients. What is the coefficient of Sn in the balanced equation? Sn + HNO₃ $\to$ SnO₂ + NO₂ + H₂O (acidic solution)

What concentration of Ni²⁺ ion remains in solution after electrolysis of 100.mL of 0.250 M NiSO₄ solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO₂(s)+ Cl^- $\to$ Pb²⁺ + Cl₂(g)(acidic solution)