Question 1

You have an abundant supply of NaCl salt from which you would like to prepare pure metallic sodium.

Accepted Answer

A)  As the reduction potential of the aqueous Na+/Na couple is -1.662 V, this process is accomplished spontaneously in aqueous solution. 
B)  As the reduction potential of the aqueous Na+/Na couple is -1.662 V, this process is accomplished spontaneously from molten NaCl. 
C)  You prepare an aqueous solution of NaCl, apply a voltage of 1.662 V and collect metallic Na. 
D)  Na is produced by electrolysis of molten liquid NaCl at elevated temperature (NaCl mp. is 800o
C) . 
E)  Na is produced by electrolysis of solid NaCl. 
A)  As the reduction potential of the aqueous Na+/Na couple is -1.662 V, this process is accomplished spontaneously in aqueous solution. 
B)  As the reduction potential of the aqueous Na+/Na couple is -1.662 V, this process is accomplished spontaneously from molten NaCl. 
C)  You prepare an aqueous solution of NaCl, apply a voltage of 1.662 V and collect metallic Na. 
D)  Na is produced by electrolysis of molten liquid NaCl at elevated temperature (NaCl mp. is 800o
C) . 
E)  Na is produced by electrolysis of solid NaCl.

Question 2

Calculate the standard free energy change for the following redox reaction: ($\Delta$G$\degree$ = 77.11 (Ag+) and 65.49 kj/mol 
(Cu+2)2 Ag+ (aq) + Cu (s) $\rightarrow$ 2 Ag (s) + Cu2+ (aq)

Accepted Answer

The answer of Calculate the standard free energy change for...

Question 3

At an engine block rebuilding factory you are in charge of replating Mn on the interiors of engine blocks. Based on the surface area and thickness needed, you determine that you need 35g of Mn to plate out by performing electrolysis on the engine block. Your plating solution is 3 M Mn(NO3)2. How long do you need to perform electrolysis if your machine performs at 220 Amps?

Accepted Answer

837 sec or

Question 4

Which of the following combinations would provide the largest potential for a battery?(If needed, refer to Table 17-1in the text)

Accepted Answer

A)  Br2 and Fe 
B)  Br-1 and Fe+2 
C)  Al and Cu+2 
D)  Al+3 and Cu+2 
E)  Al and Br- 
A)  Br2 and Fe 
B)  Br-1 and Fe+2 
C)  Al and Cu+2 
D)  Al+3 and Cu+2 
E)  Al and Br-

Question 5

What is the correct description, in line notation, for an electrochemical cell comprised of only Ag wire, AgNO3 electrolyte solution, and a salt bridge having  $\Delta$ G = -2 kJ?If needed, use the following equation:$\Delta$G° = -nFE°, E°   , E = E? 
-   , moles e- =   (If needed, refer to Table 17-1 in the text )

Accepted Answer

A)  Ag(s)  $\mid$ Ag+( aq, 1.00 M)  $\parallel$  Ag+(aq, 2.25 M)  $\mid$ Ag(s) 
B)  Ag(s)  $\mid$ Ag+( aq, 1.00 M)  $\parallel$ Ag+(aq, 1.00 M)  $\mid$ Ag(s) 
C)  Ag(s)  $\mid$ Ag+( aq, 2.25 M)  $\parallel$ Ag+(aq, 1.00 M)  $\mid$ Ag(s) 
D)  Ag(s)  $\mid$ Ag+( aq, 0.445 M)  $\parallel$ Ag+(aq, 1.00 M)  $\mid$ Ag(s) 
E)  Ag(s)  $\mid$ Ag+( aq, 1.00 M), Ag+(aq, 2.25 M)  $\mid$ Ag(s) 
A)  Ag(s)  $\mid$ Ag+( aq, 1.00 M)  $\parallel$  Ag+(aq, 2.25 M)  $\mid$ Ag(s) 
B)  Ag(s)  $\mid$ Ag+( aq, 1.00 M)  $\parallel$ Ag+(aq, 1.00 M)  $\mid$ Ag(s) 
C)  Ag(s)  $\mid$ Ag+( aq, 2.25 M)  $\parallel$ Ag+(aq, 1.00 M)  $\mid$ Ag(s) 
D)  Ag(s)  $\mid$ Ag+( aq, 0.445 M)  $\parallel$ Ag+(aq, 1.00 M)  $\mid$ Ag(s) 
E)  Ag(s)  $\mid$ Ag+( aq, 1.00 M), Ag+(aq, 2.25 M)  $\mid$ Ag(s)

Question 6

You determine that for proper protection of an engine part you need to put a coating of 3.0g of Cr(s) on your part. How long do you need to perform electrolysis on your engine part if your current is 30.0 Amps, and your Cr is in the form of Cr(NO3)3(aq)?

Accepted Answer

Question 7

How is aluminium protected from oxidation?(If needed, refer to Table 17-1in the text)

Accepted Answer

A)  formation of an oxide layer 
B)  attaching it to a block of zinc 
C)  coating it with iron 
D)  Aluminium is not protected from oxidation, since Eo for Al is -1.662 V it will always corrode. 
E)  Provide a protective paint on the surface of the aluminium metal. 
A)  formation of an oxide layer 
B)  attaching it to a block of zinc 
C)  coating it with iron 
D)  Aluminium is not protected from oxidation, since Eo for Al is -1.662 V it will always corrode. 
E)  Provide a protective paint on the surface of the aluminium metal.

Question 8

Consider the redox reaction of permanganate and sulphur:
MnO4- + S $\rarr$Mn2+ + SO42- (acidic solution)If the coefficient of MnO4- is 6 in the balanced equation, what is the coefficient of H2O?

Accepted Answer

A)  2 
B)  3 
C)  4 
D)  5 
E)  6 
A)  2 
B)  3 
C)  4 
D)  5 
E)  6

Question 9

For the galvanic cell shown in the diagram, identify the anode and mark which direction the cations are moving in the salt bridge.

Accepted Answer

The Cu⁺²/Cuside is the

Question 10

Draw three molecular pictures illustrating direct electron transfer in the reaction of silver (I) ions with copper metal.

Accepted Answer

The answer of Draw three molecular pictures illustrating direct electron...

Question 11

For the working galvanic cell shown at standard conditions, how would you increase the cell potential?(If needed, refer to Table 17-1 in the text )

Accepted Answer

A)  Make the Pt electrode larger. 
B)  Make the Copper electrode larger. 
C)  Increase the concentration of KI. 
D)  Increase the concentration of I2. 
E)  Make the Cu electrode smaller. 
A)  Make the Pt electrode larger. 
B)  Make the Copper electrode larger. 
C)  Increase the concentration of KI. 
D)  Increase the concentration of I2. 
E)  Make the Cu electrode smaller.

Question 12

Use the half-reaction method to balance the following redox reaction:
I2 + S2O32-$\rightarrow$I - + S4O62- (basic solution)

Accepted Answer

2 S<sub>2</sub>O<sub>3</sub><s

Question 13

Aluminium is used in a battery in which the following reaction occurs:
4 Al (s) + 3 O2 (g) + 4 OH- (aq) + 6 H2O $\rightarrow$4 Al(OH) (-,4) (aq)If the battery must supply a current of 78 A for 4.0 hours, what mass of Al (ing) must be contained in the battery?(If needed, refer to Table 17-1 in the text)

Accepted Answer

1.0 x 10<s

Question 14

Calculate the equilibrium constant for the following redox reaction:
Fe3+ (aq) + Cu+ (aq) $\rightarrow$ Fe2+ (aq) + Cu2+ (aq)[E°(Fe3+, 2+) = 0.771 V] [E°(Cu2+,1+) = 0.153 V](If needed, refer to Table 17-1 in the text)

Accepted Answer

E°= 0.618

Question 15

For the following galvanic cell what will be its potential when the reaction reaches equilibrium?(If needed, refer to Table 17-1in the text )

Accepted Answer

A)  0.0 V 
B)  0.458 V 
C)  1.142 V 
D)  0.272 V 
E)  1.26 V 
A)  0.0 V 
B)  0.458 V 
C)  1.142 V 
D)  0.272 V 
E)  1.26 V

Question 16

Which of the following is NOT a redox reaction?

Accepted Answer

A)  4 NH3 + 5 O2  $\rarr$  4 NO + 6 H2O 
B)  2 CO + O2  $\rarr$  2 CO2 
C)  S + 2 F2$\rarr$SF4 
D)  AgNO3 + KI $\rarr$AgI(s) + KNO3 
E)  Cl2 + 2H2O (\rarr\) 2Cl- + 2OCl- + 4H+ 
A)  4 NH3 + 5 O2  $\rarr$  4 NO + 6 H2O 
B)  2 CO + O2  $\rarr$  2 CO2 
C)  S + 2 F2$\rarr$SF4 
D)  AgNO3 + KI $\rarr$AgI(s) + KNO3 
E)  Cl2 + 2H2O (\rarr\) 2Cl- + 2OCl- + 4H+

You have an abundant supply of NaCl salt from which you would like to prepare pure metallic sodium.

Calculate the standard free energy change for the following redox reaction: ( $\Delta$ G $\degree$ = 77.11 (Ag⁺) and 65.49 kj/mol (Cu⁺²)2 Ag⁺ (aq) + Cu (s) $\rightarrow$ 2 Ag (s) + Cu²⁺ (aq)

Which of the following combinations would provide the largest potential for a battery?(If needed, refer to Table 17-1in the text)

You determine that for proper protection of an engine part you need to put a coating of 3.0g of Cr_(s) on your part. How long do you need to perform electrolysis on your engine part if your current is 30.0 Amps, and your Cr is in the form of Cr(NO₃)_3(aq)?

How is aluminium protected from oxidation?(If needed, refer to Table 17-1in the text)

Consider the redox reaction of permanganate and sulphur: MnO₄^- + S $\rarr$ Mn²⁺ + SO₄^2- (acidic solution)If the coefficient of MnO₄^- is 6 in the balanced equation, what is the coefficient of H₂O?

For the galvanic cell shown in the diagram, identify the anode and mark which direction the cations are moving in the salt bridge.

Draw three molecular pictures illustrating direct electron transfer in the reaction of silver (I) ions with copper metal.

For the working galvanic cell shown at standard conditions, how would you increase the cell potential?(If needed, refer to Table 17-1 in the text )

Use the half-reaction method to balance the following redox reaction: I₂ + S₂O₃^2- $\rightarrow$ I ^- + S₄O₆^2- (basic solution)

Calculate the equilibrium constant for the following redox reaction: Fe³⁺ (aq) + Cu⁺ (aq) $\rightarrow$ Fe²⁺(aq) + Cu²⁺(aq)[E°(Fe^{3+, 2+}) = 0.771 V] [E°(Cu^2+,1+) = 0.153 V](If needed, refer to Table 17-1 in the text)

For the following galvanic cell what will be its potential when the reaction reaches equilibrium?(If needed, refer to Table 17-1in the text )

Which of the following is NOT a redox reaction?

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

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Exam 17: Electron Transfer Reactions

You have an abundant supply of NaCl salt from which you would like to prepare pure metallic sodium.

Calculate the standard free energy change for the following redox reaction: ( Δ\DeltaΔ G °\degree° = 77.11 (Ag+) and 65.49 kj/mol (Cu+2)2 Ag+ (aq) + Cu (s) →\rightarrow→ 2 Ag (s) + Cu2+ (aq)

Which of the following combinations would provide the largest potential for a battery?(If needed, refer to Table 17-1in the text)

You determine that for proper protection of an engine part you need to put a coating of 3.0g of Cr(s) on your part. How long do you need to perform electrolysis on your engine part if your current is 30.0 Amps, and your Cr is in the form of Cr(NO3)3(aq)?

How is aluminium protected from oxidation?(If needed, refer to Table 17-1in the text)

Consider the redox reaction of permanganate and sulphur: MnO4- + S →\rarr→ Mn2+ + SO42- (acidic solution)If the coefficient of MnO4- is 6 in the balanced equation, what is the coefficient of H2O?

For the galvanic cell shown in the diagram, identify the anode and mark which direction the cations are moving in the salt bridge.

Draw three molecular pictures illustrating direct electron transfer in the reaction of silver (I) ions with copper metal.

For the working galvanic cell shown at standard conditions, how would you increase the cell potential?(If needed, refer to Table 17-1 in the text )

Use the half-reaction method to balance the following redox reaction: I2 + S2O32- →\rightarrow→ I - + S4O62- (basic solution)

Calculate the equilibrium constant for the following redox reaction: Fe3+ (aq) + Cu+ (aq) →\rightarrow→ Fe2+ (aq) + Cu2+ (aq)[E°(Fe3+, 2+) = 0.771 V] [E°(Cu2+,1+) = 0.153 V](If needed, refer to Table 17-1 in the text)

For the following galvanic cell what will be its potential when the reaction reaches equilibrium?(If needed, refer to Table 17-1in the text )

Which of the following is NOT a redox reaction?

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Calculate the standard free energy change for the following redox reaction: ( $\Delta$ G $\degree$ = 77.11 (Ag⁺) and 65.49 kj/mol (Cu⁺²)2 Ag⁺ (aq) + Cu (s) $\rightarrow$ 2 Ag (s) + Cu²⁺ (aq)

You determine that for proper protection of an engine part you need to put a coating of 3.0g of Cr_(s) on your part. How long do you need to perform electrolysis on your engine part if your current is 30.0 Amps, and your Cr is in the form of Cr(NO₃)_3(aq)?

Consider the redox reaction of permanganate and sulphur: MnO₄^- + S $\rarr$ Mn²⁺ + SO₄^2- (acidic solution)If the coefficient of MnO₄^- is 6 in the balanced equation, what is the coefficient of H₂O?

Use the half-reaction method to balance the following redox reaction: I₂ + S₂O₃^2- $\rightarrow$ I ^- + S₄O₆^2- (basic solution)

Calculate the equilibrium constant for the following redox reaction: Fe³⁺ (aq) + Cu⁺ (aq) $\rightarrow$ Fe²⁺(aq) + Cu²⁺(aq)[E°(Fe^{3+, 2+}) = 0.771 V] [E°(Cu^2+,1+) = 0.153 V](If needed, refer to Table 17-1 in the text)