Question 1

Calculate E°cell for the following reaction: 2Fe2+(aq)+ Cd2+(aq)$\rarr$2Fe3+(aq)+ Cd(s)

Accepted Answer

A) -0.37 V 
B) 0.37 V 
C) -1.17 V 
D) 1.17 V 
E) None of these. 
A) -0.37 V 
B) 0.37 V 
C) -1.17 V 
D) 1.17 V 
E) None of these.

Question 2

What concentration of Ni2+ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO4 solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

Accepted Answer

Question 3

Which element is associated with the term "galvanized"?

Accepted Answer

A) Ga 
B) Zn 
C) Cd 
D) Hg 
E) Pb 
A) Ga 
B) Zn 
C) Cd 
D) Hg 
E) Pb

Question 4

The electrochemical cell that utilizes the reaction Zn + Cu2+ (1 M)$\rarr$Zn2+ (1 M)+ Cu will have a lower cell emf when the concentrations of Zn2+ and Cu2+ ions are decreased to 0.1 M.

Accepted Answer

A) True 
 B)False

Question 5

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn2+ || NO3- (acid soln), NO(g)| Pt

Accepted Answer

A) Sn 
B) Sn2+ 
C) NO3- 
D) NO 
E) Pt 
A) Sn 
B) Sn2+ 
C) NO3- 
D) NO 
E) Pt

Question 6

Predict the products obtained from electrolysis of a 1 M AlBr3 solution. Note that 2H2O(l)+ 2e- $\rarr$ H2(g)+ 2OH-(aq), E°red = -0.83 V, and
O2(g)+ 4H+(aq)+ 4e-  $\rarr$2H2O(l), E°red = +1.23 V

Accepted Answer

A) Al and Br2 
B) Al and O2 
C) H2 and O2 
D) H2 and Br2 
E) Al and H2 
A) Al and Br2 
B) Al and O2 
C) H2 and O2 
D) H2 and Br2 
E) Al and H2

Question 7

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO2(s)+ Cl- $\rarr$ Pb2+ + Cl2(g)(acidic solution)

Accepted Answer

A) 2 
B) 4 
C) 5 
D) 9 
E) 11 
A) 2 
B) 4 
C) 5 
D) 9 
E) 11

Question 8

Find the emf of the cell described by the cell diagram Ni | Ni2+ (0.750 M)|| Cu2+ (0.0500 M)| Cu

Accepted Answer

A) 0.62 V 
B) 0.52 V 
C) 0.59 V 
D) 0.66 V 
E) 0.56 V 
A) 0.62 V 
B) 0.52 V 
C) 0.59 V 
D) 0.66 V 
E) 0.56 V

Question 9

Many different ways have been proposed to make batteries. One cell is set up with copper and lead electrodes in contact with CuSO4(aq)and Pb(NO3)2 (aq), respectively. If the Pb2+ and Cu2+ concentrations are each 1.0 M, what is the overall cell potential?
Pb2+ + 2e- $\rarr$ Pb E° = -0.22 V
Cu2+ + 2e- $\rarr$ Cu E° = +0.34 V

Accepted Answer

The answer of Many different ways have been proposed to...

Question 10

Determine the equilibrium constant for the following reaction at 25°C.
2I- (aq)+ Br2(l)$\rarr$I2(s)+ 2Br-(aq).

Accepted Answer

1.8 * 10<s

Question 11

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl2. If Ecell is found to be 0.24 V, what is the pH of the acetic acid solution?

Accepted Answer

Question 12

Complete and balance the following redox reaction under basic conditions:
CrO42-(aq)+ SO32-(aq)$\rarr$ Cr(OH)3(s)+ SO42-(aq)

Accepted Answer

2CrO₄^2-(

Question 13

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min?

Accepted Answer

A) 0.20 g 
B) 0.40 g 
C) 12 g 
D) 24 g 
E) 47 g 
A) 0.20 g 
B) 0.40 g 
C) 12 g 
D) 24 g 
E) 47 g

Question 14

Suppose the reaction Pb(s)+ 2H+(aq) $\rarr$Pb2+(aq)+ H2(g)is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II)ions that causes this reaction to be at equilibrium is

Accepted Answer

A) 2.5 M. 
B) 1.6 * 10-2 M. 
C) 2.5 * 10-4 M. 
D) 1.6 * 10-6 M. 
E) 0.40 M. 
A) 2.5 M. 
B) 1.6 * 10-2 M. 
C) 2.5 * 10-4 M. 
D) 1.6 * 10-6 M. 
E) 0.40 M.

Question 15

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO3(aq)using a current of 6.0 A?

Accepted Answer

Question 16

Consider the following reaction: 2Fe2+(aq)+ Cu2+ $\rarr$2Fe3+(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

Accepted Answer

A) 0.43 V 
B) 1.11 V 
C) 0.78 V 
D) -0.43 V 
E) 0 V 
A) 0.43 V 
B) 1.11 V 
C) 0.78 V 
D) -0.43 V 
E) 0 V

Question 17

Which of the following species is the strongest oxidizing agent under standard-state conditions?

Accepted Answer

A) Ag+(aq) 
B) H2(g) 
C) H+(aq) 
D) Cl2(g) 
E) Al3+(aq) 
A) Ag+(aq) 
B) H2(g) 
C) H+(aq) 
D) Cl2(g) 
E) Al3+(aq)

Question 18

Consider the reaction 2Fe3+(aq)+ Fe(s)$\rarr$ 3Fe2+(aq). Find the equilibrium constant for this reaction at 25°C.

Accepted Answer

A) 1 * 1011 
B) 8 * 1040 
C) 3 * 1020 
D) 7 * 10-12 
E) 1 * 10-41 
A) 1 * 1011 
B) 8 * 1040 
C) 3 * 1020 
D) 7 * 10-12 
E) 1 * 10-41

Question 19

If the measured voltage of the cell Zn(s)| Zn2+(aq)|| Ag+(aq)| Ag(s)is 1.37 V when the concentration of Zn2+ ion is 0.010 M, what is the Ag+ ion concentration?

Accepted Answer

A) 2.5 M 
B) 4.0 * 10-9 M 
C) 6.2 * 10-3 M 
D) 2.6 * 10-51 M 
E) 6.2 * 10-5 M 
A) 2.5 M 
B) 4.0 * 10-9 M 
C) 6.2 * 10-3 M 
D) 2.6 * 10-51 M 
E) 6.2 * 10-5 M

Question 20

The measured voltage of the cell Pt(s)| H2 (1.0 atm)| H+(aq)|| Ag+(1.0 M)| Ag(s)is 1.02 V at 25°C. Calculate the pH of the solution.

Accepted Answer

A) 1.86 
B) 1.69 
C) 3.72 
D) 3.89 
E) 7.43 
A) 1.86 
B) 1.69 
C) 3.72 
D) 3.89 
E) 7.43

Exam 19: Redox Reactions and Electrochemistry

Calculate E°cell for the following reaction: 2Fe2+(aq)+ Cd2+(aq) →\rarr→ 2Fe3+(aq)+ Cd(s)

What concentration of Ni2+ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO4 solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

Which element is associated with the term "galvanized"?

The electrochemical cell that utilizes the reaction Zn + Cu2+ (1 M) →\rarr→ Zn2+ (1 M)+ Cu will have a lower cell emf when the concentrations of Zn2+ and Cu2+ ions are decreased to 0.1 M.

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn2+ || NO3- (acid soln), NO(g)| Pt

Predict the products obtained from electrolysis of a 1 M AlBr3 solution. Note that 2H2O(l)+ 2e- →\rarr→ H2(g)+ 2OH-(aq), E°red = -0.83 V, and O2(g)+ 4H+(aq)+ 4e- →\rarr→ 2H2O(l), E°red = +1.23 V

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO2(s)+ Cl- →\rarr→ Pb2+ + Cl2(g)(acidic solution)

Find the emf of the cell described by the cell diagram Ni | Ni2+ (0.750 M)|| Cu2+ (0.0500 M)| Cu

Determine the equilibrium constant for the following reaction at 25°C. 2I- (aq)+ Br2(l) →\rarr→ I2(s)+ 2Br-(aq).

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl2. If Ecell is found to be 0.24 V, what is the pH of the acetic acid solution?

Complete and balance the following redox reaction under basic conditions: CrO42-(aq)+ SO32-(aq) →\rarr→ Cr(OH)3(s)+ SO42-(aq)

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min?

Suppose the reaction Pb(s)+ 2H+(aq) →\rarr→ Pb2+(aq)+ H2(g)is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II)ions that causes this reaction to be at equilibrium is

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO3(aq)using a current of 6.0 A?

Consider the following reaction: 2Fe2+(aq)+ Cu2+ →\rarr→ 2Fe3+(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

Which of the following species is the strongest oxidizing agent under standard-state conditions?

Consider the reaction 2Fe3+(aq)+ Fe(s) →\rarr→ 3Fe2+(aq). Find the equilibrium constant for this reaction at 25°C.

If the measured voltage of the cell Zn(s)| Zn2+(aq)|| Ag+(aq)| Ag(s)is 1.37 V when the concentration of Zn2+ ion is 0.010 M, what is the Ag+ ion concentration?

The measured voltage of the cell Pt(s)| H2 (1.0 atm)| H+(aq)|| Ag+(1.0 M)| Ag(s)is 1.02 V at 25°C. Calculate the pH of the solution.

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 E°_cell for the following reaction: 2Fe²⁺(aq)+ Cd²⁺(aq) $\rarr$ 2Fe³⁺(aq)+ Cd(s)

What concentration of Ni²⁺ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO₄ solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

The electrochemical cell that utilizes the reaction Zn + Cu²⁺(1 M) $\rarr$ Zn²⁺(1 M)+ Cu will have a lower cell emf when the concentrations of Zn²⁺ and Cu²⁺ ions are decreased to 0.1 M.

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn²⁺ || NO₃^-(acid soln), NO(g)| Pt

Predict the products obtained from electrolysis of a 1 M AlBr₃solution. Note that 2H₂O(l)+ 2e^- $\rarr$ H₂(g)+ 2OH^-(aq), E°_red = -0.83 V, and O₂(g)+ 4H⁺(aq)+ 4e^- $\rarr$ 2H₂O(l), E°_red = +1.23 V

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO₂(s)+ Cl^- $\rarr$ Pb²⁺ + Cl₂(g)(acidic solution)

Find the emf of the cell described by the cell diagram Ni | Ni²⁺ (0.750 M)|| Cu²⁺ (0.0500 M)| Cu

Determine the equilibrium constant for the following reaction at 25°C. 2I^-(aq)+ Br₂(l) $\rarr$ I₂(s)+ 2Br^-(aq).

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl₂. If E_cell is found to be 0.24 V, what is the pH of the acetic acid solution?

Complete and balance the following redox reaction under basic conditions: CrO₄^2-(aq)+ SO₃^2-(aq) $\rarr$ Cr(OH)₃(s)+ SO₄^2-(aq)

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO₄ for 90.0 min?

Suppose the reaction Pb(s)+ 2H⁺(aq) $\rarr$ Pb²⁺(aq)+ H₂(g)is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II)ions that causes this reaction to be at equilibrium is

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO₃(aq)using a current of 6.0 A?

Consider the following reaction: 2Fe²⁺(aq)+ Cu²⁺ $\rarr$ 2Fe³⁺(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

Consider the reaction 2Fe³⁺(aq)+ Fe(s) $\rarr$ 3Fe²⁺(aq). Find the equilibrium constant for this reaction at 25°C.

If the measured voltage of the cell Zn(s)| Zn²⁺(aq)|| Ag⁺(aq)| Ag(s)is 1.37 V when the concentration of Zn²⁺ ion is 0.010 M, what is the Ag⁺ ion concentration?

The measured voltage of the cell Pt(s)| H₂ (1.0 atm)| H⁺(aq)|| Ag⁺(1.0 M)| Ag(s)is 1.02 V at 25°C. Calculate the pH of the solution.