Question 1

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25°C?

Accepted Answer

A)  Ag
B)  Au
C)  Hg
D)  Cu
E)  ZnF) C) and E)
G) D) and E)

Question 2

The measured voltage of a cell in which the following reaction occurs is 0.96 V: H2(g, 1.0 atm) + 2Ag+(aq, 1.0 M)  →\rarr→ 2H+(aq, pH = ?) + 2Ag(s) 
Calculate the pH of the H+(aq) solution.

Accepted Answer

A)  1.4
B)  2.7
C)  5.4
D)  7.1
E)  14.9 F) A) and E)
G) B) and E)

Question 3

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Bi(OH) 3 + SnO22-  →\rarr→  Bi + SnO32-  (basic solution)

Accepted Answer

A)  32.
B)  25.
C)  16.
D)  13.
E)  None of these. F) D) and E)
G) B) and C)

Question 4

Predict the products of the electrolysis of aqueous aluminum bromide AlBr3(aq) . (Balancing is not required.)

Accepted Answer

A)  Al + Br2
B)  Al + O2 + H+
C)  H2 + OH-  + Br2
D)  H2 + O2E) None of the above
F) All of the above

Question 5

Consider the following electrochemical cell: U | U3+(aq) || Cl-(aq) ,Cl2(g) | Pt
If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium?

Accepted Answer

A)  -3.16 V
B)  +3.16 V
C)  -1.80 V
D)  +1.80 V
E)  +1.36 VF) B) and E)
G) A) and E)

Question 6

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn2+ is 2.0 M, what is the concentration of Cu2+?

Accepted Answer

1.5 * 10<s...

Question 7

Given the following standard reduction potentials, Ag+(aq) + e-  →\rarr→  Ag(s) E° = 0.80 V
AgCN(s) + e-  →\rarr→ Ag(s) + CN-(aq) E° = -0.01 V
Calculate the solubility product of AgCN at 25°C.

Accepted Answer

A)  4.3 * 10-14
B)  2.3 * 1013
C)  2.1 * 10-14
D)  5.1 * 1013
E)  None of these F) All of the above
G) A) and E)

Question 8

Complete and balance the following redox reaction under acidic conditions:
ClO2-(aq)$\rarr$ ClO2(g)+ Cl-(aq)

Accepted Answer

5ClO₂^-(a...

Question 9

Consider a voltaic cell based on the following cell reaction: Ni(s) + At2(s)  →\rarr→ Ni2+(aq) + 2At- (aq) 
Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E°(Ni2+/Ni) = -0.25 V]

Accepted Answer

A)  0.80 V
B)  0.30 V
C)  -0.30 V
D)  -0.80 V
E)  0.43 V F) C) and D)
G) A) and B)

Question 10

Determine the equilibrium constant for the following reaction at 298 K.
2Fe3+(aq)+ H2O2(aq)$\rarr$ 2H+(aq)+ O2(g)+ 2Fe2+(aq).

Accepted Answer

The answer of Determine the equilibrium constant for the following...

Question 11

You wish to electroplate a metal utensil with a surface area of 736 cm2 with gold to give an average thickness of 0.025 mm over the entire surface. Starting with a solution of excess Au3+ and applying a constant current of 14 A, how long will it take to electroplate the utensil? The density of gold is 19.3 g/cm3.

Accepted Answer

Question 12

Complete and balance the following redox equation. What is the coefficient of OH- when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + I-  →\rarr→ MnO2 + IO3-  (basic solution)

Accepted Answer

A)  1
B)  2
C)  4
D)  10
E)  None of these. F) None of the above
G) A) and B)

Question 13

Aluminum metal is formed by the electrolysis of Al2O3 in molten cryolite. How many grams of Al are produced when 6.50 * 103 C pass through the cell?

Accepted Answer

The answer of Aluminum metal is formed by the electrolysis...

Question 14

Complete and balance the following redox equation using the set of smallest whole-number coefficients. Now sum the coefficients of all species in the balanced equation. (Remember the coefficients that are equal to one.) The sum of the coefficients is BrO3-(aq) + Sb3+(aq)  →\rarr→  Br-(aq) + Sb5+(aq) (acidic solution)

Accepted Answer

A)  4.
B)  12.
C)  13.
D)  17.
E)  None of these. F) B) and C)
G) B) and E)

Question 15

How long will it take to produce 78 g of Al metal by the reduction of Al3+ in an electrolytic cell with a current of 2.0 A?

Accepted Answer

A)  0.01 s
B)  420 s
C)  13 h
D)  116 h
E)  1.0 * 1012 sF) A) and B)
G) A) and C)

Question 16

Consider the following standard reduction potentials in acid solution: 3+. B) Cr. C) Mn2+. D) Co2+. E) MnO4-." class="answers-bank-image d-inline" rel="preload" > The strongest oxidizing agent listed above is

Accepted Answer

A)  Cr3+.
B)  Cr.
C)  Mn2+.
D)  Co2+.
E)  MnO4-.F) A) and E)
G) D) and E)

Question 17

Consider the reaction Pb(s) + 2H+(aq)   →\rarr→  Pb2+(aq) + H2(g) . If the hydrogen gas pressure is maintained at 1.00 atm and the lead(II) ion concentration is 0.025 M, find the pH at which this reaction is at equilibrium.

Accepted Answer

A)  2.8
B)  3.2
C)  6.0
D)  3.0
E)  5.7 F) B) and C)
G) A) and B)

Question 18

Calculate the cell voltage for the following reaction: Cu2+ (0.010 M) + H2(1 atm)  →\rarr→  Cu(s) + 2H+(pH = 7.0)

Accepted Answer

A)  0.19 V
B)  -0.01 V
C)  0.34 V
D)  0.69 V
E)  0.49 V F) A) and D)
G) None of the above

Question 19

What current is needed to deposit 0.500 g of chromium metal from a solution of Cr3+ in a period of 1.00 hr?

Accepted Answer

Question 20

Consider the reaction Fe + Sn2+(1 * 10-3  M)$\rarr$Fe2+(1.0 M)+ Sn. In what direction do the Cl-  ions in the KCl salt bridge flow?

Accepted Answer

away from the cathod...

Exam 19: Redox Reactions and Electrochemistry

Consider the following standard reduction potentials in acid solution: The strongest oxidizing agent listed above is

Correct Answer
verified

Calculate the cell voltage for the following reaction: Cu²⁺ (0.010 M) + H₂(1 atm) $\rarr$ Cu(s) + 2H⁺(pH = 7.0)

Correct Answer
verified

Consider the following electrochemical cell: U | U³⁺(aq) || Cl^-(aq) ,Cl₂(g) | Pt If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium?

Correct Answer
verified

Predict the products of the electrolysis of aqueous aluminum bromide AlBr₃(aq) . (Balancing is not required.)

Correct Answer
verified

Consider a voltaic cell based on the following cell reaction: Ni(s) + At₂(s) $\rarr$ Ni²⁺(aq) + 2At^-(aq) Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E°(Ni²⁺/Ni) = -0.25 V]

Correct Answer
verified

Complete and balance the following redox reaction under acidic conditions: ClO₂^-(aq) $\rarr$ ClO₂(g)+ Cl^-(aq)

Correct Answer
verified
5ClO₂^-(a...
View Answer

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25°C?

Correct Answer
verified

How long will it take to produce 78 g of Al metal by the reduction of Al³⁺ in an electrolytic cell with a current of 2.0 A?

Correct Answer
verified

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M) $\rarr$ Fe²⁺(1.0 M)+ Sn. In what direction do the Cl^- ions in the KCl salt bridge flow?

Correct Answer
verified
away from the cathod...
View Answer

Consider the reaction Pb(s) + 2H⁺(aq) $\rarr$ Pb²⁺(aq) + H₂(g) . If the hydrogen gas pressure is maintained at 1.00 atm and the lead(II) ion concentration is 0.025 M, find the pH at which this reaction is at equilibrium.

Correct Answer
verified

Correct Answer
verified

Determine the equilibrium constant for the following reaction at 298 K. 2Fe³⁺(aq)+ H₂O₂(aq) $\rarr$ 2H⁺(aq)+ O₂(g)+ 2Fe²⁺(aq).

Correct Answer
verified

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn²⁺ is 2.0 M, what is the concentration of Cu²⁺?

Correct Answer
verified
1.5 * 10
View Answer

The measured voltage of a cell in which the following reaction occurs is 0.96 V: H₂(g, 1.0 atm) + 2Ag⁺(aq, 1.0 M) $\rarr$ 2H⁺(aq, pH = ?) + 2Ag(s) Calculate the pH of the H⁺(aq) solution.

Correct Answer
verified

Given the following standard reduction potentials, Ag⁺(aq) + e^- $\rarr$ Ag(s) E° = 0.80 V AgCN(s) + e^- $\rarr$ Ag(s) + CN^-(aq) E° = -0.01 V Calculate the solubility product of AgCN at 25°C.

Correct Answer
verified

What current is needed to deposit 0.500 g of chromium metal from a solution of Cr³⁺ in a period of 1.00 hr?

Correct Answer
verified

Correct Answer
verified

Complete and balance the following redox equation. What is the coefficient of OH^-when the equation is balanced using the set of smallest whole-number coefficients? MnO₄^- + I^- $\rarr$ MnO₂ + IO₃^- (basic solution)

Correct Answer
verified

Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite. How many grams of Al are produced when 6.50 * 10³ C pass through the cell?

Correct Answer
verified

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Bi(OH) ₃ + SnO₂^2- $\rarr$ Bi + SnO₃^2- (basic solution)

Correct Answer
verified

Exam 19: Redox Reactions and Electrochemistry

Consider the following standard reduction potentials in acid solution: The strongest oxidizing agent listed above is

Correct AnswerverifiedShow Answer

Calculate the cell voltage for the following reaction: Cu2+ (0.010 M) + H2(1 atm) →\rarr→ Cu(s) + 2H+(pH = 7.0)

Correct AnswerverifiedShow Answer

Consider the following electrochemical cell: U | U3+(aq) || Cl-(aq) ,Cl2(g) | Pt If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium?

Correct AnswerverifiedShow Answer

Predict the products of the electrolysis of aqueous aluminum bromide AlBr3(aq) . (Balancing is not required.)

Correct AnswerverifiedShow Answer

Consider a voltaic cell based on the following cell reaction: Ni(s) + At2(s) →\rarr→ Ni2+(aq) + 2At- (aq) Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E°(Ni2+/Ni) = -0.25 V]

Correct AnswerverifiedShow Answer

Complete and balance the following redox reaction under acidic conditions: ClO2-(aq) →\rarr→ ClO2(g)+ Cl-(aq)

Correct Answerverified5ClO2-(a...View AnswerShow Answer

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25°C?

Correct AnswerverifiedShow Answer

How long will it take to produce 78 g of Al metal by the reduction of Al3+ in an electrolytic cell with a current of 2.0 A?

Correct AnswerverifiedShow Answer

Consider the reaction Fe + Sn2+(1 * 10-3 M) →\rarr→ Fe2+(1.0 M)+ Sn. In what direction do the Cl- ions in the KCl salt bridge flow?

Correct Answerverifiedaway from the cathod...View AnswerShow Answer

Consider the reaction Pb(s) + 2H+(aq) →\rarr→ Pb2+(aq) + H2(g) . If the hydrogen gas pressure is maintained at 1.00 atm and the lead(II) ion concentration is 0.025 M, find the pH at which this reaction is at equilibrium.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Determine the equilibrium constant for the following reaction at 298 K. 2Fe3+(aq)+ H2O2(aq) →\rarr→ 2H+(aq)+ O2(g)+ 2Fe2+(aq).

Correct AnswerverifiedShow Answer

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn2+ is 2.0 M, what is the concentration of Cu2+?

Correct Answerverified1.5 * 10View AnswerShow Answer

The measured voltage of a cell in which the following reaction occurs is 0.96 V: H2(g, 1.0 atm) + 2Ag+(aq, 1.0 M) →\rarr→ 2H+(aq, pH = ?) + 2Ag(s) Calculate the pH of the H+(aq) solution.

Correct AnswerverifiedShow Answer

Given the following standard reduction potentials, Ag+(aq) + e- →\rarr→ Ag(s) E° = 0.80 V AgCN(s) + e- →\rarr→ Ag(s) + CN-(aq) E° = -0.01 V Calculate the solubility product of AgCN at 25°C.

Correct AnswerverifiedShow Answer

What current is needed to deposit 0.500 g of chromium metal from a solution of Cr3+ in a period of 1.00 hr?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Complete and balance the following redox equation. What is the coefficient of OH- when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + I- →\rarr→ MnO2 + IO3- (basic solution)

Correct AnswerverifiedShow Answer

Aluminum metal is formed by the electrolysis of Al2O3 in molten cryolite. How many grams of Al are produced when 6.50 * 103 C pass through the cell?

Correct AnswerverifiedShow Answer

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Bi(OH) 3 + SnO22- →\rarr→ Bi + SnO32- (basic solution)

Correct AnswerverifiedShow Answer

Correct Answer
verified

Calculate the cell voltage for the following reaction: Cu²⁺ (0.010 M) + H₂(1 atm) $\rarr$ Cu(s) + 2H⁺(pH = 7.0)

Correct Answer
verified

Consider the following electrochemical cell: U | U³⁺(aq) || Cl^-(aq) ,Cl₂(g) | Pt If the standard cell emf is 3.16 V, what is the standard reduction potential for uranium?

Correct Answer
verified

Predict the products of the electrolysis of aqueous aluminum bromide AlBr₃(aq) . (Balancing is not required.)

Correct Answer
verified

Consider a voltaic cell based on the following cell reaction: Ni(s) + At₂(s) $\rarr$ Ni²⁺(aq) + 2At^-(aq) Given that the standard cell emf is 0.55 V, what is the standard reduction potential for astatine? [E°(Ni²⁺/Ni) = -0.25 V]

Correct Answer
verified

Complete and balance the following redox reaction under acidic conditions: ClO₂^-(aq) $\rarr$ ClO₂(g)+ Cl^-(aq)

Correct Answer
verified
5ClO₂^-(a...
View Answer

Correct Answer
verified

How long will it take to produce 78 g of Al metal by the reduction of Al³⁺ in an electrolytic cell with a current of 2.0 A?

Correct Answer
verified

Consider the reaction Fe + Sn²⁺(1 * 10^-3 M) $\rarr$ Fe²⁺(1.0 M)+ Sn. In what direction do the Cl^- ions in the KCl salt bridge flow?

Correct Answer
verified
away from the cathod...
View Answer

Consider the reaction Pb(s) + 2H⁺(aq) $\rarr$ Pb²⁺(aq) + H₂(g) . If the hydrogen gas pressure is maintained at 1.00 atm and the lead(II) ion concentration is 0.025 M, find the pH at which this reaction is at equilibrium.

Correct Answer
verified

Correct Answer
verified

Determine the equilibrium constant for the following reaction at 298 K. 2Fe³⁺(aq)+ H₂O₂(aq) $\rarr$ 2H⁺(aq)+ O₂(g)+ 2Fe²⁺(aq).

Correct Answer
verified

If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn²⁺ is 2.0 M, what is the concentration of Cu²⁺?

Correct Answer
verified
1.5 * 10
View Answer

The measured voltage of a cell in which the following reaction occurs is 0.96 V: H₂(g, 1.0 atm) + 2Ag⁺(aq, 1.0 M) $\rarr$ 2H⁺(aq, pH = ?) + 2Ag(s) Calculate the pH of the H⁺(aq) solution.

Correct Answer
verified

Given the following standard reduction potentials, Ag⁺(aq) + e^- $\rarr$ Ag(s) E° = 0.80 V AgCN(s) + e^- $\rarr$ Ag(s) + CN^-(aq) E° = -0.01 V Calculate the solubility product of AgCN at 25°C.

Correct Answer
verified

What current is needed to deposit 0.500 g of chromium metal from a solution of Cr³⁺ in a period of 1.00 hr?

Correct Answer
verified

Correct Answer
verified

Complete and balance the following redox equation. What is the coefficient of OH^-when the equation is balanced using the set of smallest whole-number coefficients? MnO₄^- + I^- $\rarr$ MnO₂ + IO₃^- (basic solution)

Correct Answer
verified

Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite. How many grams of Al are produced when 6.50 * 10³ C pass through the cell?

Correct Answer
verified

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Bi(OH) ₃ + SnO₂^2- $\rarr$ Bi + SnO₃^2- (basic solution)

Correct Answer
verified