Question 1

A constant current of 10.0 A is passed through an electrolytic cell for 90.0 min.How many Coulombs of charge are passed through the cell?

Accepted Answer

A) 0.00933 
B) 0.560 
C) 0.00560 
D) 900 
E) 15 
A) 0.00933 
B) 0.560 
C) 0.00560 
D) 900 
E) 15

Question 2

An electrolysis is carried out by passing an electric current through a solution of copper sulfate using inert electrodes.This causes:

Accepted Answer

A) Cu(s)to plate out on the negative electrode 
B) Cu(s)to plate out on the anode 
C) oxygen to form on the negative electrode 
D) H2(g)to form at the negative electrode 
E) sulfur to form on the positive electrode 
A) Cu(s)to plate out on the negative electrode 
B) Cu(s)to plate out on the anode 
C) oxygen to form on the negative electrode 
D) H2(g)to form at the negative electrode 
E) sulfur to form on the positive electrode

Question 3

What is Keq at 25 °C of the spontaneous cell made from the Zn2+(aq)/Zn(s)(-0.76 V)and Br2(l)/2Br-(aq)(1.07 V)half cells?

Accepted Answer

A) 3 × 1010  
B) 3 × 10-11  
C) 8 × 1061  
D) 2 × 1036  
E) 5 × 1025  
A) 3 × 1010  
B) 3 × 10-11  
C) 8 × 1061  
D) 2 × 1036  
E) 5 × 1025

Question 4

If the voltage of an electrochemical cell is negative then the cell reaction is:

Accepted Answer

A) nonspontaneous 
B) slow 
C) exothermic 
D) spontaneous 
E) fast 
A) nonspontaneous 
B) slow 
C) exothermic 
D) spontaneous 
E) fast

Question 5

Choose the INCORRECT statement.

Accepted Answer

A) SHE stands for Standard Helium Electrodes. 
B) E° is the standard electrode potential. 
C) The standard electrode potential is the reduction potential of a half cell. 
D) The standard cell potential is the potential difference between two half cells. 
E) E°cell is the standard cell potential. 
A) SHE stands for Standard Helium Electrodes. 
B) E° is the standard electrode potential. 
C) The standard electrode potential is the reduction potential of a half cell. 
D) The standard cell potential is the potential difference between two half cells. 
E) E°cell is the standard cell potential.

Question 6

A copper electrode weighs 35.42 g before the electrolysis of a copper (II)sulfate solution and 36.69 g after the electrolysis has run for 20.0 s.What was the amperage of the current used?

Accepted Answer

A) 2.12 A 
B) 0.0335 A 
C) 48.2 A 
D) 96.4 A 
E) 193 A 
A) 2.12 A 
B) 0.0335 A 
C) 48.2 A 
D) 96.4 A 
E) 193 A

Question 7

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 60.0 minutes?

Accepted Answer

A) 10.9 g 
B) 16.4 g 
C) 32.8 g 
D) 36.3 g 
A) 10.9 g 
B) 16.4 g 
C) 32.8 g 
D) 36.3 g

Question 8

Choose the INCORRECT statement.

Accepted Answer

A) An electrode is often a strip of metal. 
B) An electrode in a solution of its ions is a half cell. 
C) An electrochemical cell is a half cell. 
D) The electromotive force (emf)is the cell potential. 
E) The cell potential is the potential difference between the half cells. 
A) An electrode is often a strip of metal. 
B) An electrode in a solution of its ions is a half cell. 
C) An electrochemical cell is a half cell. 
D) The electromotive force (emf)is the cell potential. 
E) The cell potential is the potential difference between the half cells.

Question 9

The hydrogen standard electrode is the most convenient standard electrode to use.

Accepted Answer

A) True 
 B)False

Question 10

Choose the INCORRECT statement.

Accepted Answer

A) One mole of hydrogen ions will have a positive charge of one Faraday. 
B) One Faraday of charge will release 35.5 g of Cl2(g)in the electrolysis of a chloride solution. 
C) One Faraday of charge will plate out two moles of Cu(s)from a solution of CuSO4(aq). 
D) One mole of electrons has a charge of l Faraday. 
E) One mole of hydrogen gas requires 2 Faradays. 
A) One mole of hydrogen ions will have a positive charge of one Faraday. 
B) One Faraday of charge will release 35.5 g of Cl2(g)in the electrolysis of a chloride solution. 
C) One Faraday of charge will plate out two moles of Cu(s)from a solution of CuSO4(aq). 
D) One mole of electrons has a charge of l Faraday. 
E) One mole of hydrogen gas requires 2 Faradays.

Question 11

Choose the INCORRECT statement.

Accepted Answer

A) When a half reaction is reversed,the sign of the potential is changed. 
B) Reversing a half reaction makes it a reduction potential. 
C) Each electrochemical cell consists of a reduction half cell and an oxidation half cell. 
D) A voltaic cell is also called a battery. 
E) The potential difference of a cell is the voltage of the cell. 
A) When a half reaction is reversed,the sign of the potential is changed. 
B) Reversing a half reaction makes it a reduction potential. 
C) Each electrochemical cell consists of a reduction half cell and an oxidation half cell. 
D) A voltaic cell is also called a battery. 
E) The potential difference of a cell is the voltage of the cell.

Question 12

Determine E°cell for the reaction: Pb(s)+ Cu2+(aq)→ Pb2+(aq)+ Cu(s).The half reactions are:
Pb2+(aq)+ 2 e- → Pb(s)E° = -0.125 V
Cu2+(aq)+ 2 e- → Cu(s)E° = 0.340 V

Accepted Answer

A) 0.215 V 
B) 0.465 V 
C) 0.930 V 
D) -0.215 V 
E) -0.465 V 
A) 0.215 V 
B) 0.465 V 
C) 0.930 V 
D) -0.215 V 
E) -0.465 V

Question 13

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr3+ ions for 320.minutes?

Accepted Answer

A) 27.6 g 
B) 49.2 g 
C) 82.4 g 
D) 248 g 
A) 27.6 g 
B) 49.2 g 
C) 82.4 g 
D) 248 g

Question 14

For the reaction: Mg(s)+ AgNO3(aq)→ Ag(s)+ Mg(NO3)2(aq)
Ag+(aq)+ e- → Ag(s) E° = 0.800 V
Mg2+(aq)+ 2 e- → Mg(s)E° = -2.356 V
For the reaction,determine E° for the cell.

Accepted Answer

A) 1.556 V 
B) -3.156 V 
C) 3.156 V 
D) 0.800 V 
E) 2.356 V 
A) 1.556 V 
B) -3.156 V 
C) 3.156 V 
D) 0.800 V 
E) 2.356 V

Question 15

Given the following half-reactions occurring in the silver-zinc hearing aid battery,calculate the voltage at 25 °C of this battery.
ZnO(s)+ H2O(l)+ 2 e- → Zn(s)+ 2 OH-(aq)E° = -1.260 V
Ag2O(s)+ H2O(l)+ 2 e- → 2 Ag(s)+ 2 OH-(aq)E° = +0.342 V

Accepted Answer

A) +1.602 V 
B) +1.402 V 
C) +0.858 V 
D) -0.858 V 
E) -1.602 V 
A) +1.602 V 
B) +1.402 V 
C) +0.858 V 
D) -0.858 V 
E) -1.602 V

Question 16

Given the table below predict the numerical value of the standard cell potential for the reaction:
2 Cr(s)+ 3 Cu2+(aq)→ 2 Cr3+(aq)+ 3 Cu(s)
Half Reaction E° (volts)
(1)Cr3+(aq)+ 3 e- → Cr(s)-0.74
(2)Cr3+(aq)+ e- → Cr2+(aq)-0.41
(3)Cr2O72-(aq)+ 14 H+(aq)+ 6 e- → 2 Cr3+(aq)+ 7 H2O(l)1.33
(4)Cu+(aq)+ e- → Cu(s)0.52
(5)Cu2+(aq)+ 2 e- → Cu(s)0.34
(6)Cu2+(aq)+ e- → Cu+(aq)0.16

Accepted Answer

A) 2.50 volts 
B) 0.417 volts 
C) -1.08 volts 
D) 1.08 volts 
E) -0.40 volts 
A) 2.50 volts 
B) 0.417 volts 
C) -1.08 volts 
D) 1.08 volts 
E) -0.40 volts

Question 17

One mole of electrons has a charge of:

Accepted Answer

A) 96,485 A 
B) 1.60 × 10-19  
C) 6.02 × 1023 A 
D) 96,485 C 
E) 96,485 F 
A) 96,485 A 
B) 1.60 × 10-19  
C) 6.02 × 1023 A 
D) 96,485 C 
E) 96,485 F

Question 18

A constant current of 15.0 A is passed through an electrolytic cell for 60.0 min.How many Coulombs of charge are passed through the cell?

Accepted Answer

A) 0.00933 
B) 0.560 
C) 0.00560 
D) 900 
E) 15 
A) 0.00933 
B) 0.560 
C) 0.00560 
D) 900 
E) 15

Question 19

The standard emf for the cell using the overall cell reaction below is +0.48 V:
Zn(s)+   (aq)→   (aq)+ Ni(s)
The emf generated by the cell when [   ] = 2.50 mol L-1 and [   ] = 0.100 mol L-1 is

Accepted Answer

A) 0.40 
B) 0.50 
C) 0.52 
D) 0.56 
E) 0.44 
A) 0.40 
B) 0.50 
C) 0.52 
D) 0.56 
E) 0.44

Question 20

A galvanic cell consists of one half-cell that contains Ag(s)and Ag+(aq),and one half-cell that contains Cu(s)and Cu2+(aq).What species are produced at the electrodes under standard conditions?
Ag+(aq)+ e- → Ag(s)E° = +0.80 V
Cu2+(aq)+ 2 e- → Cu(s)E° = +0.34 V

Accepted Answer

A) Ag(aq)is formed at the cathode,and Cu(s)is formed at the anode. 
B) Ag(s)is formed at the cathode,and Cu2+(aq)is formed at the anode. 
C) Cu(s)is formed at the cathode,and Ag+(aq)is formed at the anode. 
D) Cu2+(aq)is formed at the cathode,and Cu(s)is formed at the anode. 
A) Ag(aq)is formed at the cathode,and Cu(s)is formed at the anode. 
B) Ag(s)is formed at the cathode,and Cu2+(aq)is formed at the anode. 
C) Cu(s)is formed at the cathode,and Ag+(aq)is formed at the anode. 
D) Cu2+(aq)is formed at the cathode,and Cu(s)is formed at the anode.

Exam 19: Electrochemistry

A constant current of 10.0 A is passed through an electrolytic cell for 90.0 min.How many Coulombs of charge are passed through the cell?

An electrolysis is carried out by passing an electric current through a solution of copper sulfate using inert electrodes.This causes:

What is Keq at 25 °C of the spontaneous cell made from the Zn2+(aq)/Zn(s)(-0.76 V)and Br2(l)/2Br-(aq)(1.07 V)half cells?

If the voltage of an electrochemical cell is negative then the cell reaction is:

Choose the INCORRECT statement.

A copper electrode weighs 35.42 g before the electrolysis of a copper (II)sulfate solution and 36.69 g after the electrolysis has run for 20.0 s.What was the amperage of the current used?

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 60.0 minutes?

Choose the INCORRECT statement.

The hydrogen standard electrode is the most convenient standard electrode to use.

Choose the INCORRECT statement.

Choose the INCORRECT statement.

Determine E°cell for the reaction: Pb(s)+ Cu2+(aq)→ Pb2+(aq)+ Cu(s).The half reactions are: Pb2+(aq)+ 2 e- → Pb(s)E° = -0.125 V Cu2+(aq)+ 2 e- → Cu(s)E° = 0.340 V

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr3+ ions for 320.minutes?

For the reaction: Mg(s)+ AgNO3(aq)→ Ag(s)+ Mg(NO3)2(aq) Ag+(aq)+ e- → Ag(s) E° = 0.800 V Mg2+(aq)+ 2 e- → Mg(s)E° = -2.356 V For the reaction,determine E° for the cell.

Given the following half-reactions occurring in the silver-zinc hearing aid battery,calculate the voltage at 25 °C of this battery. ZnO(s)+ H2O(l)+ 2 e- → Zn(s)+ 2 OH-(aq)E° = -1.260 V Ag2O(s)+ H2O(l)+ 2 e- → 2 Ag(s)+ 2 OH-(aq)E° = +0.342 V

One mole of electrons has a charge of:

A constant current of 15.0 A is passed through an electrolytic cell for 60.0 min.How many Coulombs of charge are passed through the cell?

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s)+ (aq)→ (aq)+ Ni(s) The emf generated by the cell when [ ] = 2.50 mol L-1 and [ ] = 0.100 mol L-1 is

A galvanic cell consists of one half-cell that contains Ag(s)and Ag+(aq),and one half-cell that contains Cu(s)and Cu2+(aq).What species are produced at the electrodes under standard conditions? Ag+(aq)+ e- → Ag(s)E° = +0.80 V Cu2+(aq)+ 2 e- → Cu(s)E° = +0.34 V

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

What is Keq at 25 °C of the spontaneous cell made from the Zn²⁺(aq)/Zn(s)(-0.76 V)and Br₂(l)/2Br^-(aq)(1.07 V)half cells?

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 60.0 minutes?

Determine E°_ce_ll for the reaction: Pb(s)+ Cu²⁺(aq)→ Pb²⁺(aq)+ Cu(s).The half reactions are: Pb²⁺(aq)+ 2 e^- → Pb(s)E° = -0.125 V Cu²⁺(aq)+ 2 e^- → Cu(s)E° = 0.340 V

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr³⁺ ions for 320.minutes?

For the reaction: Mg(s)+ AgNO₃(aq)→ Ag(s)+ Mg(NO₃)₂(aq) Ag⁺(aq)+ e^- → Ag(s) E° = 0.800 V Mg²⁺(aq)+ 2 e^- → Mg(s)E° = -2.356 V For the reaction,determine E° for the cell.

Given the following half-reactions occurring in the silver-zinc hearing aid battery,calculate the voltage at 25 °C of this battery. ZnO(s)+ H₂O(l)+ 2 e^- → Zn(s)+ 2 OH^-(aq)E° = -1.260 V Ag₂O(s)+ H₂O(l)+ 2 e^- → 2 Ag(s)+ 2 OH^-(aq)E° = +0.342 V

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s)+ (aq)→ (aq)+ Ni(s) The emf generated by the cell when [ ] = 2.50 mol L^-1 and [ ] = 0.100 mol L^-1 is

A galvanic cell consists of one half-cell that contains Ag(s)and Ag⁺(aq),and one half-cell that contains Cu(s)and Cu²⁺(aq).What species are produced at the electrodes under standard conditions? Ag⁺(aq)+ e^- → Ag(s)E° = +0.80 V Cu²⁺(aq)+ 2 e^- → Cu(s)E° = +0.34 V