Question 1

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

Accepted Answer

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

Question 2

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. 
A) 1 
B) 2 
C) 4 
D) 10 
E) None of these.

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

Question 4

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 5

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 
A) 2.8 
B) 3.2 
C) 6.0 
D) 3.0 
E) 5.7

Question 6

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 7

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

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

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

Question 10

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 11

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 
A) 0.80 V 
B) 0.30 V 
C) -0.30 V 
D) -0.80 V 
E) 0.43 V

Question 12

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 
A) 1.4 
B) 2.7 
C) 5.4 
D) 7.1 
E) 14.9

Question 13

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

Question 14

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

Question 15

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) Zn 
A) Ag 
B) Au 
C) Hg 
D) Cu 
E) Zn

Question 16

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 
A) 0.19 V 
B) -0.01 V 
C) 0.34 V 
D) 0.69 V 
E) 0.49 V

Question 17

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 18

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 19

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 + O2 
A) Al + Br2 
B) Al + O2 + H+ 
C) H2 + OH-  + Br2 
D) H2 + O2

Question 20

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 
A) 4.3 * 10-14 
B) 2.3 * 1013 
C) 2.1 * 10-14 
D) 5.1 * 1013 
E) None of these

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

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)

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)

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⁺?

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.

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?

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

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?

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

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]

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.

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?

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

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

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?

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

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

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.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Exam 19: Redox Reactions and Electrochemistry

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

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)

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)

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+?

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.

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?

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

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?

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

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]

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.

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?

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

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

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?

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

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

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.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

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)

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)

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⁺?

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.

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?

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

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?

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

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]

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.

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?

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

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?

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

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

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.