Question 1

In the following electrochemical cell,what is the reduction half reaction?
Cu(s)| Cu2+(aq)|| Fe3+(aq),Fe2+(aq)| Pt(s)

Accepted Answer

A)  Fe3-(aq)+ e-$\to$Fe2(aq) 
B)  Fe2-(aq)+ e-$\to$ Fe3+(aq) 
C)  Fe2+(aq)+ Pt(s)$\to$Fe3+0(aq)+ e- 
D)  Cu2+(aq)$\to$Cu(s)+ 2e- 
E)  Cu(s)$\to$Cu2+(aq)+ 2e- 
A)  Fe3-(aq)+ e-$\to$Fe2(aq) 
B)  Fe2-(aq)+ e-$\to$ Fe3+(aq) 
C)  Fe2+(aq)+ Pt(s)$\to$Fe3+0(aq)+ e- 
D)  Cu2+(aq)$\to$Cu(s)+ 2e- 
E)  Cu(s)$\to$Cu2+(aq)+ 2e- A

Question 2

The use of electrical energy to produce chemical change is known as ________.An example of this process is the reduction of NaCl(    )to produce Na(s).

Accepted Answer

electrolysis

Question 3

What is the correct cell notation for a voltaic cell based on the reaction below?
Cu2+(aq)+ Fe(s)$\to$ Cu(s)+ Fe2+(aq)

Accepted Answer

A)  Cu(s)| Cu2+(aq)|| Fe2+(aq)| Fe(s) 
B)  Fe(s)|| Fe2+(aq),Cu2+(aq)| Cu(s) 
C)  Cu(s)|| Cu2+(aq),Fe2+(aq)|| Fe(s) 
D)  Cu(s)| Fe2+(aq)|| Cu2+(aq)| Fe(s) 
E)  Fe(s)| Fe2+(aq)|| Cu2+(aq)| Cu(s) 
A)  Cu(s)| Cu2+(aq)|| Fe2+(aq)| Fe(s) 
B)  Fe(s)|| Fe2+(aq),Cu2+(aq)| Cu(s) 
C)  Cu(s)|| Cu2+(aq),Fe2+(aq)|| Fe(s) 
D)  Cu(s)| Fe2+(aq)|| Cu2+(aq)| Fe(s) 
E)  Fe(s)| Fe2+(aq)|| Cu2+(aq)| Cu(s) E

Question 4

The unit for electromotive force,emf,is the Volt.A Volt is equal to

Accepted Answer

A)  one joule per second. 
B)  one coulomb per joule. 
C)  one joule per coulomb. 
D)  one coulomb per second. 
E)  one second per joule. 
A)  one joule per second. 
B)  one coulomb per joule. 
C)  one joule per coulomb. 
D)  one coulomb per second. 
E)  one second per joule.

Question 5

What is the correct cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is 
Pb4+(aq)+ 2e- Pb2+(aq).

Accepted Answer

A)  Pt(s)| H2(g)| H+(aq)|| Pb4+(aq),Pb2+(aq)| Pt(s) 
B)  Pt(s)| H2(g)| H+(aq)|| Pb4+(aq),Pb2+(aq) 
C)  Pb2+(aq),Pb4+(aq)|| H+(aq)| H2(g)| Pt(s) 
D)  Pt(s)| Pb2+(aq),Pb4+(aq)|| H+(aq)| H2(g)| Pt(s) 
E)  H2(g)| H+(aq)|| Pb2+(aq),Pb4+(aq) 
A)  Pt(s)| H2(g)| H+(aq)|| Pb4+(aq),Pb2+(aq)| Pt(s) 
B)  Pt(s)| H2(g)| H+(aq)|| Pb4+(aq),Pb2+(aq) 
C)  Pb2+(aq),Pb4+(aq)|| H+(aq)| H2(g)| Pt(s) 
D)  Pt(s)| Pb2+(aq),Pb4+(aq)|| H+(aq)| H2(g)| Pt(s) 
E)  H2(g)| H+(aq)|| Pb2+(aq),Pb4+(aq)

Question 6

Write a balanced chemical equation for the overall reaction represented by the cell notation below.Mn(s)| Mn2+(aq)|| Zn2+(aq)| Zn(s)

Accepted Answer

A)  2Mn(s)+ Zn2+(aq)$\to$ Zn(s)+ 2Mn2+(aq) 
B)  Mn(s)+ Mn2+(aq)$\to$ Zn(s)+ Zn2+(aq) 
C)  Mn(s)+ Zn2+(aq)$\to$ Zn(s)+ Mn2+(aq) 
D)  2Zn(s)+ Mn2+(aq)$\to$Mn(s)+ 2Zn2+(aq) 
E)  Zn(s)+ Mn2+(aq)$\to$Mn(s)+ Zn2+(aq) 
A)  2Mn(s)+ Zn2+(aq)$\to$ Zn(s)+ 2Mn2+(aq) 
B)  Mn(s)+ Mn2+(aq)$\to$ Zn(s)+ Zn2+(aq) 
C)  Mn(s)+ Zn2+(aq)$\to$ Zn(s)+ Mn2+(aq) 
D)  2Zn(s)+ Mn2+(aq)$\to$Mn(s)+ 2Zn2+(aq) 
E)  Zn(s)+ Mn2+(aq)$\to$Mn(s)+ Zn2+(aq)

Question 7

The following reaction occurs spontaneously.
2 Fe(s)+ 3 Cl2(aq)$\to$2 Fe3+(aq)+ 6 Cl-(aq)
Write the balanced oxidation half-reaction.

Accepted Answer

A)  Fe(s)$\to$ Fe3+(aq)+ 3 e- 
B)  Fe(s)+ 3 e- $\to$Fe3+(aq) 
C)  Fe(s)+ 3/2 Cl2(aq)$\to$FeCl3(aq) 
D)  Cl2(aq)$\to$ 2 Cl-(aq)+ 2 e- 
E)  Cl2(aq)+ 2 e- $\to$ 2 Cl-(aq) 
A)  Fe(s)$\to$ Fe3+(aq)+ 3 e- 
B)  Fe(s)+ 3 e- $\to$Fe3+(aq) 
C)  Fe(s)+ 3/2 Cl2(aq)$\to$FeCl3(aq) 
D)  Cl2(aq)$\to$ 2 Cl-(aq)+ 2 e- 
E)  Cl2(aq)+ 2 e- $\to$ 2 Cl-(aq)

Question 8

Explain the function of a salt bridge in a voltaic cell.

Accepted Answer

The salt bridge physically connects the

Question 9

Which of the following statements is/are CORRECT?
1)A nickel-cadmium battery is an example of a secondary or rechargeable battery,often used in rechargeable cordless appliances.
2)Hydrogen-oxygen fuel cells use the heat of combustion of hydrogen to recharge lead storage batteries.
3)LeClanché cells are the most efficient rechargeable batteries,but they are rarely used due their high cost of production.

Accepted Answer

A)  1 only 
B)  2 only 
C)  3 only 
D)  1 and 3 
E)  1,2,and 3 
A)  1 only 
B)  2 only 
C)  3 only 
D)  1 and 3 
E)  1,2,and 3

Question 10

Calculate Ecell for the following electrochemical cell at 25°C given that the standard cell potential,
E°cell,is 0.460 V.
Cu(s)| Cu2+(aq,0.012 M)|| Ag+(aq,0.17 M)| Ag(s)

Accepted Answer

A)  0.471 V 
B)  0.282 V 
C)  0.460 V 
D)  0.494 V 
E)  0.486 V 
A)  0.471 V 
B)  0.282 V 
C)  0.460 V 
D)  0.494 V 
E)  0.486 V

Question 11

Al3+ is reduced to Al(s)at an electrode.If a current of 2.75 ampere is passed for 36 hours,what mass of aluminum is deposited at the electrode? Assume 100% current efficiency.

Accepted Answer

A)  9.2 $\times$ 10-3 g 
B)  3.3 $\times$ 101 g 
C)  9.9 $\times$ 101 g 
D)  1.0 $\times$ 102 g 
E)  3.0 $\times$ 102 g 
A)  9.2 $\times$ 10-3 g 
B)  3.3 $\times$ 101 g 
C)  9.9 $\times$ 101 g 
D)  1.0 $\times$ 102 g 
E)  3.0 $\times$ 102 g

Question 12

An SHE electrode has been assigned a standard reduction potential,ES1U1P1$\circ$S1S1P0,of 0.00 Volts.Which reaction occurs at this electrode?

Accepted Answer

A)  2 H2O(   )+ 2 e- $\to$ H2(g)+ 2 OH-(aq) 
B)  O2(g)+ 4 e- $\to$2 O2-(aq) 
C)  Hg2Cl2(s)+ 2 e- $\to$ 2 Hg(   )+ 2 Cl-(aq) 
D)  Li+(aq)+ e- $\to$ Li(s) 
E)  2 H+(aq)+ 2 e- $\to$ H2(g) 
A)  2 H2O(   )+ 2 e- $\to$ H2(g)+ 2 OH-(aq) 
B)  O2(g)+ 4 e- $\to$2 O2-(aq) 
C)  Hg2Cl2(s)+ 2 e- $\to$ 2 Hg(   )+ 2 Cl-(aq) 
D)  Li+(aq)+ e- $\to$ Li(s) 
E)  2 H+(aq)+ 2 e- $\to$ H2(g)

Question 13

Write balanced reduction and oxidation half-reactions for the processes that occur at the cathode and anode of a fuel cell used aboard NASA's space shuttles.

Accepted Answer

Cathode: O₂(g)+ 2 H

Question 14

Calculate   for the electrochemical cell below,
Ag(s)| AgCl(s)| Cl-(aq,1.0 M)|| Cu2+(aq,1.0 M)| Cu(s)
Given the following standard reduction potentials.

Cu2+(aq)+ 2 e- $\to$ Cu(s)$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0= +0.337 V
AgCl(s)+ e- $\to$Ag(s)+ Cl-(aq)$~~~~~~~~$ES1U1P1$\circ$S1S1P0 = +0.222 V

Accepted Answer

A)  -0.115 V 
B)  -0.107 V 
C)  +0.115 V 
D)  +0.452 V 
E)  +0.559 V 
A)  -0.115 V 
B)  -0.107 V 
C)  +0.115 V 
D)  +0.452 V 
E)  +0.559 V

Question 15

What is the standard cell potential (   )for the following below,
2Ag(s)+ Pb2+(aq)$\to$ 2Ag+(aq)+ Pb(s)
Given the following standard reduction potentials.
Ag+(aq)+ e-$\to$ Ag(s)$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0 =0.8 V
Pb2+(aq)+2e-$\to$ Pb(s)$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0 =-0.126 V

Accepted Answer

A)  -0.926 V 
B)  0.926 V 
C)  -1.726 V 
D)  1.726 V 
E)  1.474 V 
A)  -0.926 V 
B)  0.926 V 
C)  -1.726 V 
D)  1.726 V 
E)  1.474 V

Question 16

Consider the following half-reactions:
Cl2(g)+ 2 e- $\to$ 2 Cl-(aq)$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0 = +1.36 V
Ag+(aq)+ e- $\to$ Ag(s)$~~~ ~~~~$$~~~~ ~~~$$~~ ~~~~$ES1U1P1$\circ$S1S1P0 = +0.80 V
Cu2+(aq)+ 2 e- $\to$ Cu(s)$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0= +0.34 V
Sn2+(aq)+ 2 e- $\to$Sn(s)$~~~~~ ~$$~~~ ~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0= -0.14 V
Al3+(aq)+ 3 e- $\to$ Al(s)$~~~~~~~~$$~~~ ~~~~$$ ~~~$ES1U1P1$\circ$S1S1P0 = -1.66 V
Which of the above elements or ions will reduce Cu2+(aq)?

Accepted Answer

A)  Ag(s)and Sn2+(aq) 
B)  Cl-(aq)and Ag(s) 
C)  Cl2(g)and Ag+(aq) 
D)  Sn(s)and Al(s) 
E)  Sn2+(aq)and Al3+(aq) 
A)  Ag(s)and Sn2+(aq) 
B)  Cl-(aq)and Ag(s) 
C)  Cl2(g)and Ag+(aq) 
D)  Sn(s)and Al(s) 
E)  Sn2+(aq)and Al3+(aq)

Question 17

Which of the following are standard conditions for an electrochemical cell?
1)Solutes in aqueous solution has a concentration of 1 M.
2)Gaseous reactants or products have a pressure of 1 bar.
3)Solids are present in quantities of 1 mole.

Accepted Answer

A)  1 only 
B)  2 only 
C)  3 only 
D)  1 and 2 
E)  1,2,and 3 
A)  1 only 
B)  2 only 
C)  3 only 
D)  1 and 2 
E)  1,2,and 3

Question 18

For the cell reaction   l )
The standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

Accepted Answer

A)  8 
B)  10 
C)  5 
D)  2 
E)  6 
A)  8 
B)  10 
C)  5 
D)  2 
E)  6

Question 19

Calculate E°cell for the cell for the reaction below,
2Cr(s)+ 3Sn4+(aq)$\to$ 3Sn2+(aq)+2Cr3+(aq)
Given the following standard reduction potentials.
Cr3+(aq)+ 3e-$\to$ Cr(s)$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0 = -0.74 V
Sn4+(aq)+ 2e-$\to$ Sn2+(aq)$~~~~~~~~$$~ ~~$ES1U1P1$\circ$S1S1P0 = 0.15V

Accepted Answer

A)  0.89 V 
B)  0.59 V 
C)  0.42 V 
D)  -0.59 V 
E)  (-0.89) V 
A)  0.89 V 
B)  0.59 V 
C)  0.42 V 
D)  -0.59 V 
E)  (-0.89) V

Question 20

Given the following two half-reactions,write the overall reaction in the direction in which it is spontaneous and calculate the standard cell potential.
Pb2+(aq)+ 2 e- $\to$ Pb(s)$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0 = -0.126 V
Fe3+(aq)+ e- $\to$ Fe2+(s)$~~~~~~~~$$~~~~~~~~$ES1U1P1$\circ$S1S1P0 = +0.771 V

Accepted Answer

A)  Pb2+(aq)+ 2 Fe2+(s)$\to$Pb(s)+ 2 Fe3+(aq)   = +0.897 V 
B)  Pb2+(aq)+ Fe2+(s)$\to$ Pb(s)+ Fe3+(aq)   = +0.645 V 
C)  Pb(s)+ 2 Fe3+(aq)$\to$Pb2+(aq)+ 2 Fe2+(s)   = +1.416 V 
D)  Pb(s)+ 2 Fe3+(aq)$\to$ Pb2+(aq)+ 2 Fe2+(s)   = +0.897 V 
E)  Pb(s)+ Fe3+(aq)$\to$Pb2+(aq)+ Fe2+(s)   = +0.645 V 
A)  Pb2+(aq)+ 2 Fe2+(s)$\to$Pb(s)+ 2 Fe3+(aq)   = +0.897 V 
B)  Pb2+(aq)+ Fe2+(s)$\to$ Pb(s)+ Fe3+(aq)   = +0.645 V 
C)  Pb(s)+ 2 Fe3+(aq)$\to$Pb2+(aq)+ 2 Fe2+(s)   = +1.416 V 
D)  Pb(s)+ 2 Fe3+(aq)$\to$ Pb2+(aq)+ 2 Fe2+(s)   = +0.897 V 
E)  Pb(s)+ Fe3+(aq)$\to$Pb2+(aq)+ Fe2+(s)   = +0.645 V

Exam 20: Principles of Reactivity: Electron Transfer Reactions

In the following electrochemical cell,what is the reduction half reaction? Cu(s)| Cu2+(aq)|| Fe3+(aq),Fe2+(aq)| Pt(s)

The use of electrical energy to produce chemical change is known as ________.An example of this process is the reduction of NaCl( )to produce Na(s).

What is the correct cell notation for a voltaic cell based on the reaction below? Cu2+(aq)+ Fe(s) →\to→ Cu(s)+ Fe2+(aq)

The unit for electromotive force,emf,is the Volt.A Volt is equal to

What is the correct cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Pb4+(aq)+ 2e- Pb2+(aq).

Write a balanced chemical equation for the overall reaction represented by the cell notation below.Mn(s)| Mn2+(aq)|| Zn2+(aq)| Zn(s)

The following reaction occurs spontaneously. 2 Fe(s)+ 3 Cl2(aq) →\to→ 2 Fe3+(aq)+ 6 Cl-(aq) Write the balanced oxidation half-reaction.

Explain the function of a salt bridge in a voltaic cell.

Calculate Ecell for the following electrochemical cell at 25°C given that the standard cell potential, E°cell,is 0.460 V. Cu(s)| Cu2+(aq,0.012 M)|| Ag+(aq,0.17 M)| Ag(s)

Al3+ is reduced to Al(s)at an electrode.If a current of 2.75 ampere is passed for 36 hours,what mass of aluminum is deposited at the electrode? Assume 100% current efficiency.

An SHE electrode has been assigned a standard reduction potential,E ∘\circ∘ ,of 0.00 Volts.Which reaction occurs at this electrode?

Write balanced reduction and oxidation half-reactions for the processes that occur at the cathode and anode of a fuel cell used aboard NASA's space shuttles.

Calculate for the electrochemical cell below, Ag(s)| AgCl(s)| Cl-(aq,1.0 M)|| Cu2+(aq,1.0 M)| Cu(s) Given the following standard reduction potentials. Cu2+(aq)+ 2 e- →\to→ Cu(s) ~~~~~~~~ ~~~~~~~~ E ∘\circ∘ = +0.337 V AgCl(s)+ e- →\to→ Ag(s)+ Cl-(aq) ~~~~~~~~ E ∘\circ∘ = +0.222 V

What is the standard cell potential ( )for the following below, 2Ag(s)+ Pb2+(aq) →\to→ 2Ag+(aq)+ Pb(s) Given the following standard reduction potentials. Ag+(aq)+ e- →\to→ Ag(s) ~~~~~~~~ ~~~~~~~~ E ∘\circ∘ =0.8 V Pb2+(aq)+2e- →\to→ Pb(s) ~~~~~~~~ ~~~~~~~~ E ∘\circ∘ =-0.126 V

Which of the following are standard conditions for an electrochemical cell? 1)Solutes in aqueous solution has a concentration of 1 M. 2)Gaseous reactants or products have a pressure of 1 bar. 3)Solids are present in quantities of 1 mole.

For the cell reaction l ) The standard cell potential is 1.34 V.To determine the cell potential at nonstandard conditions,what is the value that should be used for n in the Nernst equation?

Calculate E°cell for the cell for the reaction below, 2Cr(s)+ 3Sn4+(aq) →\to→ 3Sn2+(aq)+2Cr3+(aq) Given the following standard reduction potentials. Cr3+(aq)+ 3e- →\to→ Cr(s) ~~~~~~~~ ~~~~~~~~ E ∘\circ∘ = -0.74 V Sn4+(aq)+ 2e- →\to→ Sn2+(aq) ~~~~~~~~ ~ ~~ E ∘\circ∘ = 0.15V

Basic Concepts of Chemistry

Mathlets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Chemistry of Solids

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Reactivity: Chemical Equilibria

The Chemistry of Acids and Bases

Principles of Reactivity: Other Aspects of Aqueous Equilibria

Entropy and Free Energy

Environmental Chemistry Earths Environment,energy,and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

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In the following electrochemical cell,what is the reduction half reaction? Cu(s)| Cu²⁺(aq)|| Fe³⁺(aq),Fe²⁺(aq)| Pt(s)

What is the correct cell notation for a voltaic cell based on the reaction below? Cu²⁺(aq)+ Fe(s) $\to$ Cu(s)+ Fe²⁺(aq)

What is the correct cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Pb⁴⁺(aq)+ 2e^- Pb²⁺(aq).

Write a balanced chemical equation for the overall reaction represented by the cell notation below.Mn(s)| Mn²⁺(aq)|| Zn²⁺(aq)| Zn(s)

The following reaction occurs spontaneously. 2 Fe(s)+ 3 Cl₂(aq) $\to$ 2 Fe³⁺(aq)+ 6 Cl^-(aq) Write the balanced oxidation half-reaction.

Calculate E_cell for the following electrochemical cell at 25°C given that the standard cell potential, E°_cell,is 0.460 V. Cu(s)| Cu²⁺(aq,0.012 M)|| Ag⁺(aq,0.17 M)| Ag(s)

Al³⁺ is reduced to Al(s)at an electrode.If a current of 2.75 ampere is passed for 36 hours,what mass of aluminum is deposited at the electrode? Assume 100% current efficiency.

An SHE electrode has been assigned a standard reduction potential,E^$\circ$,of 0.00 Volts.Which reaction occurs at this electrode?

Calculate E°_cell for the cell for the reaction below, 2Cr(s)+ 3Sn⁴⁺(aq) $\to$ 3Sn²⁺(aq)+2Cr³⁺(aq) Given the following standard reduction potentials. Cr³⁺(aq)+ 3e^- $\to$ Cr(s) $$ $$ E^$\circ$ = -0.74 V Sn⁴⁺(aq)+ 2e^- $\to$ Sn²⁺(aq) $$ $~ ~~$ E^$\circ$ = 0.15V