Question 1

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

Question 2

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

Accepted Answer

A) True 
 B)False

Question 3

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

Question 4

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.

Question 5

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

Question 6

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

Question 7

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

Question 8

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

Question 9

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

Question 10

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.

Question 11

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

Question 12

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

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

Question 14

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

Question 15

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

Question 16

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.

Question 17

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

Question 18

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.

Question 19

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.

Question 20

The standard emf for the cell using the overall cell reaction below is +0.48 V:
Zn(s) + -1 and [   ] = 0.100 mol L-1 is   A) 0.40 B) 0.50 C) 0.52 D) 0.56 E) 0.44" class="answers-bank-image d-inline" rel="preload" > (aq) → -1 and [   ] = 0.100 mol L-1 is   A) 0.40 B) 0.50 C) 0.52 D) 0.56 E) 0.44" class="answers-bank-image d-inline" rel="preload" > (aq) + Ni(s) 
The emf generated by the cell when [ -1 and [   ] = 0.100 mol L-1 is   A) 0.40 B) 0.50 C) 0.52 D) 0.56 E) 0.44" class="answers-bank-image d-inline" rel="preload" > ] = 2.50 mol L-1 and [ -1 and [   ] = 0.100 mol L-1 is   A) 0.40 B) 0.50 C) 0.52 D) 0.56 E) 0.44" class="answers-bank-image d-inline" rel="preload" > ] = 0.100 mol L-1 is -1 and [   ] = 0.100 mol L-1 is   A) 0.40 B) 0.50 C) 0.52 D) 0.56 E) 0.44" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

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

Exam 19: Electrochemistry

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?

Correct Answer
verified

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

Correct Answer
verified

Choose the INCORRECT statement.

Correct Answer
verified

One mole of electrons has a charge of:

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified

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.

Correct Answer
verified

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?

Correct Answer
verified

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?

Correct Answer
verified

Choose the INCORRECT statement.

Correct Answer
verified

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?

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Choose the INCORRECT statement.

Correct Answer
verified

Choose the INCORRECT statement.

Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified

Exam 19: Electrochemistry

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Choose the INCORRECT statement.

Correct AnswerverifiedShow Answer

One mole of electrons has a charge of:

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Choose the INCORRECT statement.

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Choose the INCORRECT statement.

Correct AnswerverifiedShow Answer

Choose the INCORRECT statement.

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

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?

Correct Answer
verified

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.

Correct Answer
verified

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?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified