Question 1

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 2

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 3

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.F) B) and C)
G) A) and E)

Question 4

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 VF) A) and E)
G) A) and D)

Question 5

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-F) C) and E)
G) B) and D)

Question 6

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 7

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 )  2. E)  Make the Cu electrode smaller." class="answers-bank-image d-inline" rel="preload" >

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.F) A) and B)
G) A) and C)

Question 8

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 9

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 F) A) and D)
G) B) and D)

Question 10

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 11

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   Δ\DeltaΔ  G = -2 kJ?If needed, use the following equation: Δ\DeltaΔ G° = -nFE°, E° 3 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 )  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)  " class="answers-bank-image d-inline" rel="preload" > , E = E? 
- 3 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 )  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)  " class="answers-bank-image d-inline" rel="preload" > , moles e- = 3 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 )  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)  " class="answers-bank-image d-inline" rel="preload" > (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)  F) A) and E)
G) A) and B)

Question 12

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 13

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 14

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 15

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.F) B) and C)
G) C) and D)

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+ F) B) and E)
G) All of the above

Exam 17: Electron Transfer Reactions

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

Correct Answer
verified

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)?

Correct Answer
verified

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 )

Correct Answer
verified

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)

Correct Answer
verified
E°= 0.618 ...
View Answer

Correct Answer
verified

Correct Answer
verified
1.0 x 10
View Answer

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

Correct Answer
verified
2 S₂O₃
View Answer

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

Correct Answer
verified

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

Correct Answer
verified

Which of the following is NOT a redox reaction?

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

Correct Answer
verified
The Cu⁺²/Cuside is the...
View Answer

Correct Answer
verified
837 sec or...
View Answer

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

Correct Answer
verified

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)

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified

Exam 17: Electron Transfer Reactions

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

Correct AnswerverifiedShow Answer

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)?

Correct AnswerverifiedShow Answer

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 )

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedE°= 0.618 ...View AnswerShow Answer

Correct AnswerverifiedShow Answer

Correct Answerverified1.0 x 10View AnswerShow Answer

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

Correct Answerverified2 S2O3View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Which of the following is NOT a redox reaction?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedThe Cu+2/Cu side is the...View AnswerShow Answer

Correct Answerverified837 sec or...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Correct Answer
verified

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)?

Correct Answer
verified

Correct Answer
verified

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)

Correct Answer
verified
E°= 0.618 ...
View Answer

Correct Answer
verified

Correct Answer
verified
1.0 x 10
View Answer

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

Correct Answer
verified
2 S₂O₃
View Answer

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
The Cu⁺²/Cuside is the...
View Answer

Correct Answer
verified
837 sec or...
View Answer

Correct Answer
verified

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)

Correct Answer
verified

Correct Answer
verified

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?

Correct Answer
verified