Question 1

Calculate the standard cell emf for the following cell: Mg | Mg2+ || NO3- (acid soln)| NO(g)| Pt

Accepted Answer

A) 3.33 V 
B) 1.41 V 
C) -1.41 V 
D) 8.46 V 
E) -8.46 V 
A) 3.33 V 
B) 1.41 V 
C) -1.41 V 
D) 8.46 V 
E) -8.46 V

Question 2

Complete and balance the following redox reaction under acidic conditions:
MnO4-(aq)+ C2O42-(aq)$\rarr$Mn2+(aq)+ CO2(aq)

Accepted Answer

2MnO₄-(aq)+ 5C

Question 3

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl3 for 45.0 min?

Accepted Answer

A) 9.3 * 10-4 g 
B) 0.042 g 
C) 2.5 g 
D) 24 g 
E) 2.3 * 1010 g 
A) 9.3 * 10-4 g 
B) 0.042 g 
C) 2.5 g 
D) 24 g 
E) 2.3 * 1010 g

Question 4

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl2 for 4.50 hours. How many moles of calcium metal should be deposited?

Accepted Answer

A) 5.83 * 10-5 mol 
B) 0.210 mol 
C) 0.420 mol 
D) 0.840 mol 
E) 1.95 * 109 mol 
A) 5.83 * 10-5 mol 
B) 0.210 mol 
C) 0.420 mol 
D) 0.840 mol 
E) 1.95 * 109 mol

Question 5

How many coulombs (C)of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca2+ ion to calcium metal?

Accepted Answer

A) 190,000 C 
B) 85,000 C 
C) 21,000 C 
D) 42,500 C 
E) 0.88 C 
A) 190,000 C 
B) 85,000 C 
C) 21,000 C 
D) 42,500 C 
E) 0.88 C

Question 6

The half-reaction that occurs at the cathode during electrolysis of an aqueous sodium iodide solution is

Accepted Answer

A) Na+ + e- $\rarr$ Na. 
B) Na $\rarr$ Na+ + e-. 
C) 2H2O + 2e- $\rarr$ H2 + 2OH-. 
D) I2 + 2e- $\rarr$ 2I-. 
E) 2I- $\rarr$I2 + 2e-. 
A) Na+ + e- $\rarr$ Na. 
B) Na $\rarr$ Na+ + e-. 
C) 2H2O + 2e- $\rarr$ H2 + 2OH-. 
D) I2 + 2e- $\rarr$ 2I-. 
E) 2I- $\rarr$I2 + 2e-.

Question 7

Will H2(g)form when Cu is placed in 1.0 M HCl?

Accepted Answer

Question 8

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO4 for a period of 19.0 min?

Accepted Answer

Question 9

Complete and balance the following redox equation. What is the coefficient of H2S when the equation is balanced using the set of smallest whole-number coefficients? H2S + MnO4- $\rarr$ Mn2+ + SO42-  (acidic solution)

Accepted Answer

A) 1 
B) 2 
C) 4 
D) 5 
E) None of these. 
A) 1 
B) 2 
C) 4 
D) 5 
E) None of these.

Question 10

For the reaction, 2Cr2+ + Cl2(g)$\rarr$ 2Cr3+ + 2Cl-, E°cell is 1.78 V. Calculate E°cell for the related reaction Cr3+ + Cl- $\rarr$ Cr2+ + 1/2Cl2(g).

Accepted Answer

A) 1.78 V 
B) 0.89 V 
C) -1.78 V 
D) -0.89 V 
E) None of these. 
A) 1.78 V 
B) 0.89 V 
C) -1.78 V 
D) -0.89 V 
E) None of these.

Question 11

Consider the following standard reduction potentials in acid solution:   The strongest reducing agent among those shown above is

Accepted Answer

A) Fe3+. 
B) Fe2+. 
C) Br-. 
D) Al3+. 
E) Al. 
A) Fe3+. 
B) Fe2+. 
C) Br-. 
D) Al3+. 
E) Al.

Question 12

Gold can be electrochemically "plated" onto a less expensive metal by submerging the object in a solution of gold(III)and applying an electric current to drive the following half-reaction:
Au3+ + 3e- $\rarr$ Au(s)
 How many grams of gold will be formed if a current of 2.37 A is applied for 71 minutes?

Accepted Answer

The answer of Gold can be electrochemically "plated" onto a...

Question 13

Complete and balance the following redox equation using the smallest whole-number coefficients. What is the coefficient of Sn in the balanced equation? Sn + HNO3 $\rarr$ SnO2 + NO2 + H2O (acidic solution)

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 5 
A) 1 
B) 2 
C) 3 
D) 4 
E) 5

Question 14

Consider an electrochemical cell involving the overall reaction 2AgBr(s)+ Pb(s)$\rarr$ Pb2+ + 2Ag(s)+ 2Br-
 Each half-reaction is carried out in a separate compartment. The anion included in the lead half-cell is NO3-. The cation in the silver half-cell is K+. The two half-cells are connected by a KNO3 salt bridge. If [Pb2+] = 1.0 M, what concentration of Br- ion will produce a cell emf of 0.25 V at 298 K?
Given: AgBr(s)+ e- $\rarr$ Ag + Br-, E° = +0.07 V.

Accepted Answer

A) 0.02 M 
B) 0.14 M 
C) 0.38 M 
D) 1.0 M 
E) 7.0 M 
A) 0.02 M 
B) 0.14 M 
C) 0.38 M 
D) 1.0 M 
E) 7.0 M

Question 15

Aluminum metal is formed by the electrolysis of Al2O3 in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Accepted Answer

Question 16

Which one of the following reagents is capable of transforming Fe3+ (1 M)to Fe2+ (1 M)?

Accepted Answer

A) H2(1 atm) 
B) NO3- (1 M) 
C) O2(1 atm) 
D) Br- (1 M) 
E) H+ (1 M) 
A) H2(1 atm) 
B) NO3- (1 M) 
C) O2(1 atm) 
D) Br- (1 M) 
E) H+ (1 M)

Question 17

Which statement is true for a spontaneous redox reaction carried out at standard-state conditions?

Accepted Answer

A) E°red is always negative. 
B) E°cell is always positive. 
C) E°ox is always positive. 
D) E°red is always positive. 
A) E°red is always negative. 
B) E°cell is always positive. 
C) E°ox is always positive. 
D) E°red is always positive.

Question 18

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours. Calculate the mass of cadmium metal deposited.

Accepted Answer

A) 3.2 * 10-7 g 
B) 1.2 * 10-3 g 
C) 4.2 g 
D) 8.4 g 
E) 16.8 g 
A) 3.2 * 10-7 g 
B) 1.2 * 10-3 g 
C) 4.2 g 
D) 8.4 g 
E) 16.8 g

Calculate the standard cell emf for the following cell: Mg | Mg²⁺ || NO₃^-(acid soln)| NO(g)| Pt

Complete and balance the following redox reaction under acidic conditions: MnO₄-(aq)+ C₂O₄^2-(aq) $\rarr$ Mn²⁺(aq)+ CO₂(aq)

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl₃ for 45.0 min?

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl₂ for 4.50 hours. How many moles of calcium metal should be deposited?

How many coulombs (C)of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca²⁺ ion to calcium metal?

The half-reaction that occurs at the cathode during electrolysis of an aqueous sodium iodide solution is

Will H₂(g)form when Cu is placed in 1.0 M HCl?

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO₄ for a period of 19.0 min?

Complete and balance the following redox equation. What is the coefficient of H₂S when the equation is balanced using the set of smallest whole-number coefficients? H₂S + MnO₄^- $\rarr$ Mn²⁺ + SO₄^2- (acidic solution)

For the reaction, 2Cr²⁺ + Cl₂(g) $\rarr$ 2Cr³⁺ + 2Cl^-, E°_cell is 1.78 V. Calculate E°_cell for the related reaction Cr³⁺ + Cl^- $\rarr$ Cr²⁺ + ¹/₂Cl₂(g).

Consider the following standard reduction potentials in acid solution: The strongest reducing agent among those shown above is

Complete and balance the following redox equation using the smallest whole-number coefficients. What is the coefficient of Sn in the balanced equation? Sn + HNO₃ $\rarr$ SnO₂ + NO₂ + H₂O (acidic solution)

Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Which one of the following reagents is capable of transforming Fe³⁺(1 M)to Fe²⁺(1 M)?

Which statement is true for a spontaneous redox reaction carried out at standard-state conditions?

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl₂ for 2.5 hours. Calculate the mass of cadmium metal deposited.

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

Calculate the standard cell emf for the following cell: Mg | Mg2+ || NO3- (acid soln)| NO(g)| Pt

Complete and balance the following redox reaction under acidic conditions: MnO4-(aq)+ C2O42-(aq) →\rarr→ Mn2+(aq)+ CO2(aq)

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl3 for 45.0 min?

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl2 for 4.50 hours. How many moles of calcium metal should be deposited?

How many coulombs (C)of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca2+ ion to calcium metal?

The half-reaction that occurs at the cathode during electrolysis of an aqueous sodium iodide solution is

Will H2(g)form when Cu is placed in 1.0 M HCl?

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO4 for a period of 19.0 min?

Complete and balance the following redox equation. What is the coefficient of H2S when the equation is balanced using the set of smallest whole-number coefficients? H2S + MnO4- →\rarr→ Mn2+ + SO42- (acidic solution)

For the reaction, 2Cr2+ + Cl2(g) →\rarr→ 2Cr3+ + 2Cl-, E°cell is 1.78 V. Calculate E°cell for the related reaction Cr3+ + Cl- →\rarr→ Cr2+ + 1/2Cl2(g).

Consider the following standard reduction potentials in acid solution: The strongest reducing agent among those shown above is

Complete and balance the following redox equation using the smallest whole-number coefficients. What is the coefficient of Sn in the balanced equation? Sn + HNO3 →\rarr→ SnO2 + NO2 + H2O (acidic solution)

Aluminum metal is formed by the electrolysis of Al2O3 in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Which one of the following reagents is capable of transforming Fe3+ (1 M)to Fe2+ (1 M)?

Which statement is true for a spontaneous redox reaction carried out at standard-state conditions?

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours. Calculate the mass of cadmium metal deposited.

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

Calculate the standard cell emf for the following cell: Mg | Mg²⁺ || NO₃^-(acid soln)| NO(g)| Pt

Complete and balance the following redox reaction under acidic conditions: MnO₄-(aq)+ C₂O₄^2-(aq) $\rarr$ Mn²⁺(aq)+ CO₂(aq)

How many grams of chromium would be electroplated by passing a constant current of 5.2 amperes through a solution containing CrCl₃ for 45.0 min?

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl₂ for 4.50 hours. How many moles of calcium metal should be deposited?

How many coulombs (C)of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca²⁺ ion to calcium metal?

Will H₂(g)form when Cu is placed in 1.0 M HCl?

How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current of 2.00 A is passed through a solution of CuSO₄ for a period of 19.0 min?

Complete and balance the following redox equation. What is the coefficient of H₂S when the equation is balanced using the set of smallest whole-number coefficients? H₂S + MnO₄^- $\rarr$ Mn²⁺ + SO₄^2- (acidic solution)

For the reaction, 2Cr²⁺ + Cl₂(g) $\rarr$ 2Cr³⁺ + 2Cl^-, E°_cell is 1.78 V. Calculate E°_cell for the related reaction Cr³⁺ + Cl^- $\rarr$ Cr²⁺ + ¹/₂Cl₂(g).

Complete and balance the following redox equation using the smallest whole-number coefficients. What is the coefficient of Sn in the balanced equation? Sn + HNO₃ $\rarr$ SnO₂ + NO₂ + H₂O (acidic solution)

Aluminum metal is formed by the electrolysis of Al₂O₃in molten cryolite. How many minutes are required to form 10.0 g of Al using a current of 30 A?

Which one of the following reagents is capable of transforming Fe³⁺(1 M)to Fe²⁺(1 M)?

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl₂ for 2.5 hours. Calculate the mass of cadmium metal deposited.