Laser_3

What is the reduction half reaction for the following chemical reaction in a basic solution?ClO-(aq)

What is the reduction half reaction for the following chemical reaction in a basic solution?ClO-(aq)

What is the reduction half reaction for the following chemical reaction in a basic solution?

ClO-(aq) + Cr(OH)4-(aq) → CrO42-(aq) + Cl-(aq)

A) ClO-(aq) + 2 H+(aq) + 2e- → Cl-(aq) + H2O(l)
B) ClO-(aq) + H2O(l) + 2e- → Cl-(aq

Whelan   263   1 Reply

hbutler2

What is the oxidation half reaction in the following chemical reaction?Cr2O72-(aq) + 6 Cl-(aq) + 14

What is the oxidation half reaction in the following chemical reaction?Cr2O72-(aq) + 6 Cl-(aq) + 14

What is the oxidation half reaction in the following chemical reaction?

Cr2O72-(aq) + 6 Cl-(aq) + 14 H+(aq) → 2 Cr3+(aq) + 3 Cl2(aq) + 7 H2O(l)

A) Cr2O72-(aq) + 14 H+(aq) + 6e- → 2 Cr3+(aq) + 7 H2O(l)
B) Cr2O72-(aq) + 14 H+

Whelan   288   1 Reply

hbutler2

Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq) is needed to

Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq) is needed to

Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq) is needed to completely react with 12.44 mL of 0.125 M KI3(aq)?

2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq)

A) 3.11 mL
B) 6.22 mL

Whelan   774   1 Reply

hbutler2

Which of the following terms can be used to describe an electrochemical cell in which a spontaneous

Which of the following terms can be used to describe an electrochemical cell in which a spontaneous

Which of the following terms can be used to describe an electrochemical cell in which a spontaneous chemical reaction generates an electric current?

   I.   an electrolytic cell
   II.   a galvanic cell
   III.   a voltaic cell

A)

Whelan   174   1 Reply

hbutler2

Which cell involves a nonspontaneous redox reaction?

Which cell involves a nonspontaneous redox reaction?

Which cell involves a nonspontaneous redox reaction?
A) concentration cell
B) electrolytic cell
C) fuel cell
D) galvanic cell

Whelan   283   1 Reply

hbutler2

For a galvanic cell, the cathode has a ________ sign and is the site of ________.

For a galvanic cell, the cathode has a ________ sign and is the site of ________.

For a galvanic cell, the cathode has a ________ sign and is the site of ________.
A) negative, oxidation
B) negative, reduction
C) positive, oxidation
D) positive, reduction

Whelan   232   1 Reply

hbutler2

In a galvanic cell, the half-reaction MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l) isA) an oxid

In a galvanic cell, the half-reaction MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l) isA) an oxid

In a galvanic cell, the half-reaction MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l) is
A) an oxidation half-reaction and occurs at the anode.
B) an oxidation half-reaction and occurs at the cathode.
C) a reduction half-reaction and

Whelan   218   1 Reply

hbutler2

In a galvanic cell, the half-reaction H2(g) + 2 OH-(aq) → 2 H2O(l) + 2 e- isA) an oxidation half-rea

In a galvanic cell, the half-reaction H2(g) + 2 OH-(aq) → 2 H2O(l) + 2 e- isA) an oxidation half-rea

In a galvanic cell, the half-reaction H2(g) + 2 OH-(aq) → 2 H2O(l) + 2 e- is
A) an oxidation half-reaction and occurs at the anode.
B) an oxidation half-reaction and occurs at the cathode.
C) a reduction half-reaction and occurs at the

Whelan   311   1 Reply

hbutler2

What species is oxidized in the reaction: CuSO4(aq) + Mg(s) → MgSO4(aq) + Cu(s)?

What species is oxidized in the reaction: CuSO4(aq) + Mg(s) → MgSO4(aq) + Cu(s)?

What species is oxidized in the reaction: CuSO4(aq) + Mg(s) → MgSO4(aq) + Cu(s)?
A) CuSO4 (aq)
B) Mg (s)
C) MgSO4 (aq)
D) Cu (s)

Whelan   483   1 Reply

hbutler2

What is the reduction half-reaction for the following overall cell reaction?Ni2+(aq) + 2 Ag(s) → Ni(

What is the reduction half-reaction for the following overall cell reaction?Ni2+(aq) + 2 Ag(s) → Ni(

What is the reduction half-reaction for the following overall cell reaction?

Ni2+(aq) + 2 Ag(s) → Ni(s) + 2 Ag+(aq)

A) Ag(s) + e- → Ag+(aq)
B) Ag+(aq) + e- → Ag(s)
C) Ni2+(aq) + 2 e- → Ni(s)
D) Ni2+(aq) + e- → Ni(

Whelan   210   1 Reply

hbutler2

The iron content of foods can be determined by dissolving them in acid (forming Fe3+), reducing the

The iron content of foods can be determined by dissolving them in acid (forming Fe3+), reducing the

The iron content of foods can be determined by dissolving them in acid (forming Fe3+), reducing the iron(III) to iron(II), and titrating with cerium(IV):

 Fe2+(aq) + Ce4+(aq) → Fe3+(aq) + Ce3+(aq).

Identify the two half-reaction

Whelan   237   1 Reply

hbutler2

For a galvanic cell that uses the following two half-reactions,Cr2O72-(aq) + 14 H+(aq) + 6 e- → 2 Cr

For a galvanic cell that uses the following two half-reactions,Cr2O72-(aq) + 14 H+(aq) + 6 e- → 2 Cr

For a galvanic cell that uses the following two half-reactions,

Cr2O72-(aq) + 14 H+(aq) + 6 e- → 2 Cr3+(aq) + 7 H2O(l)
Pb(s) → Pb2+(aq) + 2 e-

how many moles of Pb(s) are oxidized by one mole of Cr2O72-?
A) 1
B) 2

Whelan   222   1 Reply

hbutler2

What is the shorthand notation that represents the following galvanic cell reaction?2 Fe2+(aq) + Cl2

What is the shorthand notation that represents the following galvanic cell reaction?2 Fe2+(aq) + Cl2

What is the shorthand notation that represents the following galvanic cell reaction?

2 Fe2+(aq) + Cl2(g) → 2 Fe3+(aq) + 2 Cl-(aq)

A) Fe2+(aq) ∣ Fe3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq)
B) Fe(s) ∣ Fe2+(aq) ∣∣ Fe3+(aq) Cl2(g) ∣ Cl-(aq) ∣

Whelan   293   1 Reply

hbutler2

What is the shorthand notation for a galvanic cell that represents the following galvanic cell react

What is the shorthand notation for a galvanic cell that represents the following galvanic cell react

What is the shorthand notation for a galvanic cell that represents the following galvanic cell reaction?

Br2(l) + 2 I-(aq) → 2 Br-(aq) + I2(s)

A) I-(aq)|I2(s) ∣∣Br2(l)|Br-(aq)
B) I-(aq)|I2(s) ∣∣Br2(l)|Br-(aq)|Pt(s)
C)

Whelan   301   1 Reply

hbutler2

The shorthand notation for the galvanic cell reaction Fe3+(aq) + 2 I-(aq) → Fe2+(aq) + I2(s) require

The shorthand notation for the galvanic cell reaction Fe3+(aq) + 2 I-(aq) → Fe2+(aq) + I2(s) require

The shorthand notation for the galvanic cell reaction Fe3+(aq) + 2 I-(aq) → Fe2+(aq) + I2(s) requires an inert electrode on
A) both sides of the salt bridge.
B) neither side of the salt bridge.
C) only on the left side of the salt brid

Whelan   272   1 Reply

hbutler2

If the cell reaction involves ions in solution, as the cell reaction in a galvanic cell continues,A)

If the cell reaction involves ions in solution, as the cell reaction in a galvanic cell continues,A)

If the cell reaction involves ions in solution, as the cell reaction in a galvanic cell continues,
A) E for the cell increases.
B) E for the cell decreases.
C) E° for the cell increases.
D) E° for the cell decreases.

Whelan   347   1 Reply

hbutler2

Consider the half-reaction: MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l). The formation of MnO4

Consider the half-reaction: MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l). The formation of MnO4

Consider the half-reaction: MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l). The formation of MnO4- from Mn2+ occurs most readily when the solution is
A) acidic.
B) neutral.
C) basic.
D) The reaction is not dependent upon pH.

Whelan   227   1 Reply

hbutler2

Which is most often used in the laboratory to measure pH?

Which is most often used in the laboratory to measure pH?

Which is most often used in the laboratory to measure pH?
A) a standard hydrogen electrode
B) a glass electrode
C) a Daniell cell
D) a conductivity cell

Whelan   218   1 Reply

hbutler2

The following cell has a potential of 0.45 V at 25°C. Pt(s) ∣ H2(1 atm)|H+(? M) ∣∣ Cl-(1 M) ∣ Hg2Cl2

The following cell has a potential of 0.45 V at 25°C. Pt(s) ∣ H2(1 atm)|H+(? M) ∣∣ Cl-(1 M) ∣ Hg2Cl2

The following cell has a potential of 0.45 V at 25°C.

Pt(s) ∣ H2(1 atm)|H+(? M) ∣∣ Cl-(1 M) ∣ Hg2Cl2(s)|Hg(l)

The standard half-cell potential for the half-reaction Hg2Cl2(s) + 2 e- → 2 Hg(l) + 2 Cl-(aq) is 0.28 V. What is the

Whelan   233   1 Reply

hbutler2

A cell based on the reaction below has a standard potential of +0.42 V at 25°C. If all of the specie

A cell based on the reaction below has a standard potential of +0.42 V at 25°C. If all of the specie

A cell based on the reaction below has a standard potential of +0.42 V at 25°C. If all of the species are at standard conditions except [H+], at what pH will the cell have a potential of zero?

H2O2(aq) + 2 H+(aq) + 2 Cl-(aq) → Cl2(aq) + 2

Whelan   675   1 Reply

hbutler2

When a cell reaction reaches equilibrium,

When a cell reaction reaches equilibrium,

When a cell reaction reaches equilibrium,
A) E° = 0.
B) E = 0.
C) both E° and E = 0.
D) neither E° nor E = 0.

Whelan   325   1 Reply

hbutler2

For a particular battery based on one of the following reactions, E is expected to remain constant w

For a particular battery based on one of the following reactions, E is expected to remain constant w

For a particular battery based on one of the following reactions, E is expected to remain constant with time until the cell reactants are almost completely consumed. Which is the appropriate reaction?
A) Zn(s) + 2 MnO2(s) + 2 NH4+(aq) → 2 NH3(a

Whelan   213   1 Reply

hbutler2

Which of the following reactions is most suitable for a fuel cell?

Which of the following reactions is most suitable for a fuel cell?

Which of the following reactions is most suitable for a fuel cell?
A) MnO2(s) + Li(s) → LiMnO2(s)
B) Pb(s) + PbO2(s) + 2 H+(aq) + HSO4-(aq) → PbSO4(s) + 2 H2O(l)
C) HgO(l) + Zn(s) → ZnO(s) + Hg(l)
D) 2 CO(g) + O2(g) → 2 CO2(g)

Whelan   394   1 Reply

hbutler2

Which of the following statements concerning the rusting of iron is false?

Which of the following statements concerning the rusting of iron is false?

Which of the following statements concerning the rusting of iron is false?
A) The oxidation site can occur at a different place on the metal surface than the reduction site.
B) The metal is reduced.
C) The rusting of iron requires bot

Whelan   452   1 Reply

hbutler2

What is least easily oxidized?

What is least easily oxidized?

What is least easily oxidized?
A) Al
B) Fe
C) Mg
D) Zn

Whelan   180   1 Reply

hbutler2

A steel pipe can be protected from corrosion by attaching the pipe to a piece of magnesium becauseA)

A steel pipe can be protected from corrosion by attaching the pipe to a piece of magnesium becauseA)

A steel pipe can be protected from corrosion by attaching the pipe to a piece of magnesium because
A) magnesium forms a tight oxide coating.
B) magnesium is more easily oxidized than iron.
C) magnesium is inert.
D) magnesium and s

Whelan   398   1 Reply

hbutler2

An electrolytic cell is (Multiple Choice Question)

An electrolytic cell is (Multiple Choice Question)

An electrolytic cell is
A) a battery.
B) a cell in which the cell reaction is spontaneous.
C) a cell in which an electric current drives a nonspontaneous reaction.
D) a cell in which reactants are continuously supplied to the cell

Whelan   338   1 Reply

hbutler2

Which statement is true? (Multiple Choice)

Which statement is true? (Multiple Choice)

Which statement is true?
A) The cathode is positive for a galvanic cell and negative for an electrolytic cell.
B) Electrons flow through the external circuit to the cathode in a galvanic cell and to the anode in an electrolytic cell.
C

Whelan   187   1 Reply

hbutler2

The chlor-alkali industry is based on the electrolysis of aqueous NaCl. What are the products of thi

The chlor-alkali industry is based on the electrolysis of aqueous NaCl. What are the products of thi

The chlor-alkali industry is based on the electrolysis of aqueous NaCl. What are the products of this electrolysis?
A) Na and Cl2
B) NaOH, H2, and O2
C) NaOH, H2, and Cl2
D) NaOH, O2, and Cl2

Whelan   179   1 Reply

hbutler2

The cell reaction 2 Fe3+(aq) + Zn(s) → Zn2+(aq) + 2 Fe2+(aq) occurs in the galvanic cell shown above

The cell reaction 2 Fe3+(aq) + Zn(s) → Zn2+(aq) + 2 Fe2+(aq) occurs in the galvanic cell shown above

The cell reaction 2 Fe3+(aq) + Zn(s) → Zn2+(aq) + 2 Fe2+(aq) occurs in the galvanic cell shown above. Which would be the most appropriate choices for the solid electrode in half-cell (A) and in half-cell (B)?
A) Fe(s) for half-cell (A) and Zn(s)

Whelan   304   1 Reply

hbutler2

Identify and give the sign of each electrode.

Identify and give the sign of each electrode.

Identify and give the sign of each electrode.
A) a is Ag and (+), c is Cu and (-).
B) a is Ag and (-), c is Cu and (+).
C) a is Cu and (+), c is Ag and (-).
D) a is Cu and (-), c is Ag and (+).

Whelan   249   1 Reply

hbutler2

NaNO3(aq) is employed in the salt bridge. Give the direction of electron flow and the direction of i

NaNO3(aq) is employed in the salt bridge. Give the direction of electron flow and the direction of i

NaNO3(aq) is employed in the salt bridge. Give the direction of electron flow and the direction of ion flow from the salt bridge.
A) Electrons flow from a to c; Na+ flows into b and NO3- flows into d.
B) Electrons flow from a to c; NO3- flo

Whelan   575   1 Reply

hbutler2

Identify the anode and cathode half-reactions and categorize each as either oxidation or reduction.A

Identify the anode and cathode half-reactions and categorize each as either oxidation or reduction.A

Identify the anode and cathode half-reactions and categorize each as either oxidation or reduction.
A) Anode reaction: Ag+(aq) + e- → Ag(s) (oxidation)
Cathode reaction: Cu(s) → Cu2+(aq) + 2e- (reduction)
B) Anode reaction: Ag+(aq) + e

Whelan   298   1 Reply

hbutler2

What is the shorthand notation for this cell?

What is the shorthand notation for this cell?

What is the shorthand notation for this cell?
A) Cu2+(aq) ∣ Cu(s) ∣∣ Ag+(aq) ∣ Ag(s)
B) Cu(s) ∣ Cu2+(aq) ∣∣ Ag(s) ∣ Ag+(aq)
C) Cu2+(aq) ∣ Cu(s) ∣∣ Ag(s) ∣ Ag+(aq)
D) Cu(s) ∣ Cu2+(aq) ∣∣ Ag+(aq) ∣ Ag(s)

Whelan   132   1 Reply

hbutler2

Given the half-cell potentials below, calculate the cell potential.Ag+(aq) + e- → Ag(s)0.80 VCu2+(aq

Given the half-cell potentials below, calculate the cell potential.Ag+(aq) + e- → Ag(s)0.80 VCu2+(aq

Given the half-cell potentials below, calculate the cell potential.

   Ag+(aq) + e- → Ag(s)   0.80 V
   Cu2+(aq) + 2 e- → Cu(s)   0.34 V

A) 0.46 V
B) 1.14 V
C) 1.26 V
D) 1.94 V

Whelan   208   1 Reply

hbutler2

If the concentrations of Ag+(aq) and Cu2+(aq) are varied in this galvanic cell, which of the followi

If the concentrations of Ag+(aq) and Cu2+(aq) are varied in this galvanic cell, which of the followi

If the concentrations of Ag+(aq) and Cu2+(aq) are varied in this galvanic cell, which of the following four cells has the largest cell potential?
A) [Ag+] = 0.10 M and [Cu2+] = 0.10 M
B) [Ag+] = 1.0 M and [Cu2+] = 0.10 M
C) [Ag+] = 0.1

Whelan   251   1 Reply

hbutler2

The initial concentrations of Ag+(aq) and Cu2+(aq) are both 1.0 M. What will happen to the cell volt

The initial concentrations of Ag+(aq) and Cu2+(aq) are both 1.0 M. What will happen to the cell volt

The initial concentrations of Ag+(aq) and Cu2+(aq) are both 1.0 M. What will happen to the cell voltage if 5.0 M AgNO3 is added to the compartment containing the 1.0 M Ag+(aq)? The cell voltage will
A) decrease.
B) increase.
C) remain

Whelan   245   1 Reply

hbutler2

What is the quantitative change in the cell voltage on increasing the ion concentration in the catho

What is the quantitative change in the cell voltage on increasing the ion concentration in the catho

What is the quantitative change in the cell voltage on increasing the ion concentration in the cathode compartment by a factor of 10?
A) +0.06 V
B) +0.03 V
C) -0.03 V
D) -0.06 V

Whelan   313   1 Reply

hbutler2

Determine whether this is a galvanic or an electrolytic cell and give the reaction occurring at the

Determine whether this is a galvanic or an electrolytic cell and give the reaction occurring at the

Determine whether this is a galvanic or an electrolytic cell and give the reaction occurring at the anode and the reaction occurring at the cathode.
A) Electrolytic cell
Anode reaction: K(s) → K+(l) + e-
Cathode reaction: Cl2(g) + 2e-

Whelan   148   1 Reply

hbutler2

Determine the direction of electron flow and the direction of ion flow.

Determine the direction of electron flow and the direction of ion flow.

Determine the direction of electron flow and the direction of ion flow.
A) Electrons flow from a to c; K+ ions flow toward a and Cl- ions flow toward c.
B) Electrons flow from a to c; Cl- ions flow toward a and K+ ions flow toward c.
C

Whelan   224   1 Reply

hbutler2