Question 1

How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of
30)0 amp for 10.0 hours ?

Accepted Answer

A)  448 
B)  0.0622 
C)  112 
D)  224 
E)  22.4 
A)  448 
B)  0.0622 
C)  112 
D)  224 
E)  22.4

Question 2

The lead- containing reactant(s) consumed during recharging of a lead- acid battery is/are
)

Accepted Answer

A)  PbO2 (s) only 
B)  PbSO4 (s) only 
C)  Pb (s) only 
D)  both PbO2 (s) and PbSO4 (s) 
E)  both Pb (s) and PbO2 (s) 
A)  PbO2 (s) only 
B)  PbSO4 (s) only 
C)  Pb (s) only 
D)  both PbO2 (s) and PbSO4 (s) 
E)  both Pb (s) and PbO2 (s)

Question 3

The standard cell potential (E°cell) for the voltaic cell based on the reaction below is V.

Accepted Answer

A)  +0.89 
B)  - 0.59 
C)  - 1.02 
D)  +1.94 
E)  +2.53 
A)  +0.89 
B)  - 0.59 
C)  - 1.02 
D)  +1.94 
E)  +2.53

Question 4

The electrolysis of molten AlCl3 for 3.25 hr with an electrical current of 15.0 A produces
G of aluminum metal.

Accepted Answer

A)  16.4 
B)  4.55 × 10- 3 
C)  147 
D)  0.606 
E)  49.1 
A)  16.4 
B)  4.55 × 10- 3 
C)  147 
D)  0.606 
E)  49.1

Question 5

The standard cell potential (E°cell) of the reaction below is +0.126 V. The value of OG° for the reaction is kJ/mol.
Pb (s) + 2H+ (aq) -Pb2+ (aq) + H2 (g)

Accepted Answer

A)  - 24 
B)  +24 
C)  - 12 
D)  +12 
E)  - 50 
A)  - 24 
B)  +24 
C)  - 12 
D)  +12 
E)  - 50

Question 6

is the oxidizing agent in the reaction below.

Accepted Answer

A)  S4O62-  
B)  Cr2O72-  
C)  H+  
D)  Cr3+  
E)  S2O32- 
A)  S4O62-  
B)  Cr2O72-  
C)  H+  
D)  Cr3+  
E)  S2O32-

Question 7

Which substance is serving as the reducing agent in the following reaction?

Accepted Answer

A)  Ni2+  
B)  Cr2O72-  
C)  Ni 
D)  H+  
E)  H2O 
A)  Ni2+  
B)  Cr2O72-  
C)  Ni 
D)  H+  
E)  H2O

Question 8

The anode of the alkaline battery is powdered zinc in a gel that contacts .

Accepted Answer

KOH; potas

Question 9

Consider an electrochemical cell based on the reaction:
 
Which of the following actions would change the measured cell potential?

Accepted Answer

A)  lowering the pH in the cathode compartment 
B)  increasing the pressure of hydrogen gas in the cathode compartment 
C)  increasing the pH in the cathode compartment 
D)  increasing the [Sn2+] in the anode compartment 
E)  Any of the above will change the measure cell potential. 
A)  lowering the pH in the cathode compartment 
B)  increasing the pressure of hydrogen gas in the cathode compartment 
C)  increasing the pH in the cathode compartment 
D)  increasing the [Sn2+] in the anode compartment 
E)  Any of the above will change the measure cell potential.

Question 10

The electrode at which oxidation occurs is called the .

Accepted Answer

A)  oxidizing agent 
B)  voltaic cell 
C)  anode 
D)  reducing agent 
E)  cathode 
A)  oxidizing agent 
B)  voltaic cell 
C)  anode 
D)  reducing agent 
E)  cathode

Question 11

How many minutes will it take to plate out 2.19 g of chromium metal from a solution of Cr3+ using a current of 35.2 amps in an electrolyte cell ?

Accepted Answer

A)  17.3 
B)  1.92 
C)  5.77 
D)  346 
E)  115 
A)  17.3 
B)  1.92 
C)  5.77 
D)  346 
E)  115

Question 12

Which transformation could take place at the anode of an electrochemical cell?

Accepted Answer

A)  CO2 -C2O42- 
B)  O2  -H2O2 
C)  VO2+ - VO2+ 
D)  NO - NO3- 
E)  H2AsO4  -H3AsO3 
A)  CO2 -C2O42- 
B)  O2  -H2O2 
C)  VO2+ - VO2+ 
D)  NO - NO3- 
E)  H2AsO4  -H3AsO3

Question 13

The half- reaction occurring at the anode in the balanced reaction shown below is .

Accepted Answer

A)  2MnO4- (aq) + 12H+ (aq) + 6e- - 2Mn2+ (aq) + 3H2O (l) 
B)  Fe (s) -Fe2+ (aq) + 2e- 
C)  Fe (s) -Fe3+ (aq) + 3e- 
D)  Fe2+ (aq) - Fe3+ (aq) + e- 
E)  MnO4-  (aq) + 8H+ (aq) + 5e-  -Mn2+ (aq) + 4H2O (l) 
A)  2MnO4- (aq) + 12H+ (aq) + 6e- - 2Mn2+ (aq) + 3H2O (l) 
B)  Fe (s) -Fe2+ (aq) + 2e- 
C)  Fe (s) -Fe3+ (aq) + 3e- 
D)  Fe2+ (aq) - Fe3+ (aq) + e- 
E)  MnO4-  (aq) + 8H+ (aq) + 5e-  -Mn2+ (aq) + 4H2O (l)

Question 14

Which one of the following is the best oxidizing agent ?

Accepted Answer

A)  O2  
B)  Na 
C)  H2  
D)  Ca 
E)  Li 
A)  O2  
B)  Na 
C)  H2  
D)  Ca 
E)  Li

Question 15

Disadvantages of the methanol fuel cell compared to the hydrogen fuel cell are consumption of catalyst and environmentally safe product.

Accepted Answer

A) True 
 B)False

Question 16

The most useful ore of aluminum is bauxite, in which Al is present as hydrated oxides,
Al2O3 ÷ H2O. The number of kilowatt- hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is when the applied emf is
5)00 V.

Accepted Answer

A)  59.6 
B)  0.0168 
C)  39.7 
D)  19.9 
E)  0.0596 
A)  59.6 
B)  0.0168 
C)  39.7 
D)  19.9 
E)  0.0596

Question 17

Using Table 20.1, which substance can be oxidized by O2 (g) in acidic aqueous solution?

Accepted Answer

A)  Ni2+ (aq) 
B)  Br- (aq) 
C)  Cu2+ (aq) 
D)  Ag (s) 
E)  Br2 (l) 
A)  Ni2+ (aq) 
B)  Br- (aq) 
C)  Cu2+ (aq) 
D)  Ag (s) 
E)  Br2 (l)

Question 18

When the cell potential is negative in a voltaic cell the cell reaction will not proceed spontaneously.

Accepted Answer

A) True 
 B)False

Question 19

What current (in a) is required to plate out 1.22 g of nickel from a solution of Ni2+ in 1.0 hour __________ ?

Accepted Answer

A)  12.9 
B)  1.11 
C)  4.01 × 103  
D)  2.34 
E)  65.4 
A)  12.9 
B)  1.11 
C)  4.01 × 103  
D)  2.34 
E)  65.4

Question 20

The standard reduction potential of X is 1.23 V and that of Y is - 0.44 V therefore X is oxidized by Y.

Accepted Answer

A) True 
 B)False

Exam 20: Electrochemistry

How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of 30)0 amp for 10.0 hours ?

The lead- containing reactant(s) consumed during recharging of a lead- acid battery is/are )

The standard cell potential (E°cell) for the voltaic cell based on the reaction below is V.

The electrolysis of molten AlCl3 for 3.25 hr with an electrical current of 15.0 A produces G of aluminum metal.

The standard cell potential (E°cell) of the reaction below is +0.126 V. The value of OG° for the reaction is kJ/mol. Pb (s) + 2H+ (aq) -Pb2+ (aq) + H2 (g)

is the oxidizing agent in the reaction below.

Which substance is serving as the reducing agent in the following reaction?

The anode of the alkaline battery is powdered zinc in a gel that contacts .

Consider an electrochemical cell based on the reaction: Which of the following actions would change the measured cell potential?

The electrode at which oxidation occurs is called the .

How many minutes will it take to plate out 2.19 g of chromium metal from a solution of Cr3+ using a current of 35.2 amps in an electrolyte cell ?

Which transformation could take place at the anode of an electrochemical cell?

The half- reaction occurring at the anode in the balanced reaction shown below is .

Which one of the following is the best oxidizing agent ?

Disadvantages of the methanol fuel cell compared to the hydrogen fuel cell are consumption of catalyst and environmentally safe product.

The most useful ore of aluminum is bauxite, in which Al is present as hydrated oxides, Al2O3 ÷ H2O. The number of kilowatt- hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is when the applied emf is 5)00 V.

Using Table 20.1, which substance can be oxidized by O2 (g) in acidic aqueous solution?

When the cell potential is negative in a voltaic cell the cell reaction will not proceed spontaneously.

What current (in a) is required to plate out 1.22 g of nickel from a solution of Ni2+ in 1.0 hour __________ ?

The standard reduction potential of X is 1.23 V and that of Y is - 0.44 V therefore X is oxidized by Y.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

Filters

How many grams of Ca metal are produced by the electrolysis of molten CaBr₂using a current of 30)0 amp for 10.0 hours ?

The standard cell potential (E°_cell) for the voltaic cell based on the reaction below is V.

The electrolysis of molten AlCl₃for 3.25 hr with an electrical current of 15.0 A produces G of aluminum metal.

The standard cell potential (E°_cell) of the reaction below is +0.126 V. The value of OG° for the reaction is kJ/mol. Pb (s) + 2H⁺(aq) -Pb²⁺(aq) + H₂(g)

How many minutes will it take to plate out 2.19 g of chromium metal from a solution of Cr³⁺using a current of 35.2 amps in an electrolyte cell ?

The most useful ore of aluminum is bauxite, in which Al is present as hydrated oxides, Al₂O₃÷ H₂O. The number of kilowatt- hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is when the applied emf is 5)00 V.

Using Table 20.1, which substance can be oxidized by O₂(g) in acidic aqueous solution?

What current (in a) is required to plate out 1.22 g of nickel from a solution of Ni²⁺in 1.0 hour __________ ?