Question 1

Calculate the value of E°cell for the following reaction: 2Au(s)+ 3Ca2+(aq)$\rarr$ 2Au3+(aq)+ 3Ca(s)

Accepted Answer

A) -4.37 V 
B) -1.37 V 
C) -11.6 V 
D) 1.37 V 
E) 4.37 V 
A) -4.37 V 
B) -1.37 V 
C) -11.6 V 
D) 1.37 V 
E) 4.37 V

Question 2

Consider the following standard reduction potentials in acid solution:   The weakest reducing agent listed above is

Accepted Answer

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

Question 3

Calculate the cell emf for the following reaction at 25°C: Ni(s)+ 2Cu2+(0.010 M)$\rarr$ Ni2+(0.0010 M)+ 2Cu+(1.0 M)

Accepted Answer

A) 0.40 V 
B) -0.43 V 
C) 0.43 V 
D) 0.34 V 
E) 0.37 V 
A) 0.40 V 
B) -0.43 V 
C) 0.43 V 
D) 0.34 V 
E) 0.37 V

Question 4

Complete and balance the following redox reaction under acidic conditions:
Cr2O72-(aq)+ -(aq) $\rarr$ Cr3+(aq)+ IO3-(aq)

Accepted Answer

Cr<sub>2</sub>O<sub>7</sub><su

Question 5

Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq)|| Cl2(g), Cl- (aq)| Pt
Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu4+/Pu3+)?

Accepted Answer

A) 2.37 V 
B) 1.01 V 
C) -1.71 V 
D) -1.01 V 
E) 1.71 V 
A) 2.37 V 
B) 1.01 V 
C) -1.71 V 
D) -1.01 V 
E) 1.71 V

Question 6

In the following half equation, which is the oxidizing agent? NO3-(aq)+ 4H+(aq)+ 3e- $\rarr$ NO(g)+ 2H2O

Accepted Answer

A) NO3- 
B) H+ 
C) e- 
D) NO 
E) H2O 
A) NO3- 
B) H+ 
C) e- 
D) NO 
E) H2O

Question 7

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl2(g)is evolved at the anode.

Accepted Answer

A) True 
 B)False

Question 8

The half-reaction occurring at the cathode during electrolysis of an aqueous copper(II)iodide solution is

Accepted Answer

A) I2 + 2e- $\rarr$ 2I-. 
B) Cu $\rarr$ Cu2+ + 2e-. 
C) Cu2+ + 2e- $\rarr$ Cu. 
D) 2I-  $\rarr$ I2 + 2e-. 
E) 2e- + 2H2O $\rarr$ H2 + 2OH-. 
A) I2 + 2e- $\rarr$ 2I-. 
B) Cu $\rarr$ Cu2+ + 2e-. 
C) Cu2+ + 2e- $\rarr$ Cu. 
D) 2I-  $\rarr$ I2 + 2e-. 
E) 2e- + 2H2O $\rarr$ H2 + 2OH-.

Question 9

When an aqueous solution of AgNO3 is electrolyzed, a gas is observed to form at the anode. The gas is

Accepted Answer

A) H2. 
B) O2. 
C) NO. 
D) NO2. 
A) H2. 
B) O2. 
C) NO. 
D) NO2.

Question 10

In an electrolytic cell, electrical energy is used to cause a chemical reaction to occur that would otherwise be nonspontaneous.

Accepted Answer

A) True 
 B)False

Question 11

How many coulombs would be required to electroplate 35.0 grams of chromium by passing an electrical current through a solution containing CrCl3?

Accepted Answer

A) 6.50 * 104 C 
B) 2.16 * 104 C 
C) 6.40 * 104 C 
D) 1.95 * 105 C 
E) 1.01 * 107 C 
A) 6.50 * 104 C 
B) 2.16 * 104 C 
C) 6.40 * 104 C 
D) 1.95 * 105 C 
E) 1.01 * 107 C

Question 12

An electrochemical cell based on the following reaction has a standard cell voltage (E°cell)of 0.48 V: Sn(s)+ Cu2+(aq)$\rarr$Sn2+(aq)+ Cu(s)
What is the standard reduction potential of tin(II)? (E°(Cu2+/Cu)= 0.34 V)

Accepted Answer

A) -0.14 V 
B) 0.14 V 
C) -0.82 V 
D) 0.82 V 
E) none of these 
A) -0.14 V 
B) 0.14 V 
C) -0.82 V 
D) 0.82 V 
E) none of these

Question 13

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

Accepted Answer

Question 14

Using a table of standard electrode potentials, decide which of the following statements is completely true.

Accepted Answer

A) Cu2+ can oxidize H2, and Fe can reduce Mn2+. 
B) Ni2+ can oxidize Cu2+, and Fe2+ can reduce H+. 
C) Fe2+ can oxidize H2, and Fe2+ can reduce Au3+. 
D) Br2 can oxidize Ni, and H2 can reduce Mn2+. 
E) H+ can oxidize Fe, and Ni can reduce Br2. 
A) Cu2+ can oxidize H2, and Fe can reduce Mn2+. 
B) Ni2+ can oxidize Cu2+, and Fe2+ can reduce H+. 
C) Fe2+ can oxidize H2, and Fe2+ can reduce Au3+. 
D) Br2 can oxidize Ni, and H2 can reduce Mn2+. 
E) H+ can oxidize Fe, and Ni can reduce Br2.

Question 15

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Br2 $\rarr$BrO3- + Br-  (basic solution)

Accepted Answer

A) 9. 
B) 12. 
C) 18. 
D) 21. 
E) None of the above. 
A) 9. 
B) 12. 
C) 18. 
D) 21. 
E) None of the above.

Question 16

The half-cell reaction for the oxidation of H2O(l)to O2(g)is given below. 2H2O(l) $\rarr$O2(g)+ 4H+(aq)+ 4e-
 Which choice lists all of the following species that can oxidize H2O to O2(g)under standard-state conditions?
MnO4-(aq), Cl2(g), Pb2+(aq), Cl- (aq), Ag+(aq)

Accepted Answer

A) Cl-(aq)only 
B) Cl2(g)only 
C) Pb2+(aq)and Ag+(aq) 
D) Cl-(aq)and MnO4-(aq) 
E) MnO4-(aq)and Cl2(g) 
A) Cl-(aq)only 
B) Cl2(g)only 
C) Pb2+(aq)and Ag+(aq) 
D) Cl-(aq)and MnO4-(aq) 
E) MnO4-(aq)and Cl2(g)

Question 17

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced with the set of smallest whole-number coefficients? H2O + 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 18

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl2 solution
- a Sn electrode in 1.0 M Sn(NO3 )2 solution
When the cell is running spontaneously, which choice includes only true statements and no false ones?

Accepted Answer

A) The tin electrode loses mass and the tin electrode is the cathode. 
B) The tin electrode gains mass and the tin electrode is the cathode. 
C) The iron electrode gains mass and the iron electrode is the anode. 
D) The iron electrode loses mass and the iron electrode is the cathode. 
E) The iron electrode gains mass and the iron electrode is the cathode. 
A) The tin electrode loses mass and the tin electrode is the cathode. 
B) The tin electrode gains mass and the tin electrode is the cathode. 
C) The iron electrode gains mass and the iron electrode is the anode. 
D) The iron electrode loses mass and the iron electrode is the cathode. 
E) The iron electrode gains mass and the iron electrode is the cathode.

Question 19

How many moles of H2 are produced by 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 102 s?

Accepted Answer

The answer of How many moles of H2 are produced...

Question 20

Given the following standard reduction potentials in acid solution
O2 + 4H+ + 4e- $\rarr$ 2H2O E° = +1.23 V
Sn4+ + 2e- $\rarr$ Sn2+ E° = +0.13 V
Zn2+ + 2e- $\rarr$ Zn(s)E° = -0.76 V
write a balanced equation for a spontaneous reaction which involves the tin and zinc redox couples.

Accepted Answer

Zn + Sn⁴⁺

Exam 19: Redox Reactions and Electrochemistry

Calculate the value of E°cell for the following reaction: 2Au(s)+ 3Ca2+(aq) →\rarr→ 2Au3+(aq)+ 3Ca(s)

Consider the following standard reduction potentials in acid solution: The weakest reducing agent listed above is

Calculate the cell emf for the following reaction at 25°C: Ni(s)+ 2Cu2+(0.010 M) →\rarr→ Ni2+(0.0010 M)+ 2Cu+(1.0 M)

Complete and balance the following redox reaction under acidic conditions: Cr2O72-(aq)+ -(aq) →\rarr→ Cr3+(aq)+ IO3-(aq)

Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq)|| Cl2(g), Cl- (aq)| Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu4+/Pu3+)?

In the following half equation, which is the oxidizing agent? NO3-(aq)+ 4H+(aq)+ 3e- →\rarr→ NO(g)+ 2H2O

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl2(g)is evolved at the anode.

The half-reaction occurring at the cathode during electrolysis of an aqueous copper(II)iodide solution is

When an aqueous solution of AgNO3 is electrolyzed, a gas is observed to form at the anode. The gas is

In an electrolytic cell, electrical energy is used to cause a chemical reaction to occur that would otherwise be nonspontaneous.

How many coulombs would be required to electroplate 35.0 grams of chromium by passing an electrical current through a solution containing CrCl3?

An electrochemical cell based on the following reaction has a standard cell voltage (E°cell)of 0.48 V: Sn(s)+ Cu2+(aq) →\rarr→ Sn2+(aq)+ Cu(s) What is the standard reduction potential of tin(II)? (E°(Cu2+/Cu)= 0.34 V)

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

Using a table of standard electrode potentials, decide which of the following statements is completely true.

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Br2 →\rarr→ BrO3- + Br- (basic solution)

The half-cell reaction for the oxidation of H2O(l)to O2(g)is given below. 2H2O(l) →\rarr→ O2(g)+ 4H+(aq)+ 4e- Which choice lists all of the following species that can oxidize H2O to O2(g)under standard-state conditions? MnO4-(aq), Cl2(g), Pb2+(aq), Cl- (aq), Ag+(aq)

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced with the set of smallest whole-number coefficients? H2O + MnO4- + I- →\rarr→ MnO2 + IO3- (basic solution)

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl2 solution - a Sn electrode in 1.0 M Sn(NO3 )2 solution When the cell is running spontaneously, which choice includes only true statements and no false ones?

How many moles of H2 are produced by 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 102 s?

Given the following standard reduction potentials in acid solution O2 + 4H+ + 4e- →\rarr→ 2H2O E° = +1.23 V Sn4+ + 2e- →\rarr→ Sn2+ E° = +0.13 V Zn2+ + 2e- →\rarr→ Zn(s)E° = -0.76 V write a balanced equation for a spontaneous reaction which involves the tin and zinc redox couples.

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

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Calculate the value of E°_cell for the following reaction: 2Au(s)+ 3Ca²⁺(aq) $\rarr$ 2Au³⁺(aq)+ 3Ca(s)

Calculate the cell emf for the following reaction at 25°C: Ni(s)+ 2Cu²⁺(0.010 M) $\rarr$ Ni²⁺(0.0010 M)+ 2Cu⁺(1.0 M)

Complete and balance the following redox reaction under acidic conditions: Cr2O7²^-(aq)+ ^-(aq) $\rarr$ Cr³+(aq)+ IO₃^-(aq)

Consider an electrochemical cell based on the following cell diagram: Pt | Pu³⁺(aq), Pu⁴⁺(aq)|| Cl₂(g), Cl^-(aq)| Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu⁴⁺/Pu³⁺)?

In the following half equation, which is the oxidizing agent? NO₃^-(aq)+ 4H⁺(aq)+ 3e^- $\rarr$ NO(g)+ 2H₂O

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl₂(g)is evolved at the anode.

When an aqueous solution of AgNO₃ is electrolyzed, a gas is observed to form at the anode. The gas is

How many coulombs would be required to electroplate 35.0 grams of chromium by passing an electrical current through a solution containing CrCl₃?

An electrochemical cell based on the following reaction has a standard cell voltage (E°_cell)of 0.48 V: Sn(s)+ Cu²⁺(aq) $\rarr$ Sn²⁺(aq)+ Cu(s) What is the standard reduction potential of tin(II)? (E°(Cu²⁺/Cu)= 0.34 V)

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

Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Br₂ $\rarr$ BrO₃^- + Br^- (basic solution)

The half-cell reaction for the oxidation of H₂O(l)to O₂(g)is given below. 2H₂O(l) $\rarr$ O₂(g)+ 4H⁺(aq)+ 4e^- Which choice lists all of the following species that can oxidize H₂O to O₂(g)under standard-state conditions? MnO₄^-(aq), Cl₂(g), Pb²⁺(aq), Cl^-(aq), Ag⁺(aq)

Complete and balance the following redox equation. What is the coefficient of H₂O when the equation is balanced with the set of smallest whole-number coefficients? H₂O + MnO₄^- + I^- $\rarr$ MnO₂ + IO₃^- (basic solution)

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl₂ solution - a Sn electrode in 1.0 M Sn(NO₃)₂ solution When the cell is running spontaneously, which choice includes only true statements and no false ones?

How many moles of H₂ are producedby 5.00 A of current passing through a cell containing aqueous NaCl for 4.00 * 10² s?