Question 1

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

Accepted Answer

A)  16.2 g 
B)  33.4 g 
C)  40.6 g 
D)  81.3 g 
E)  163 g 
A)  16.2 g 
B)  33.4 g 
C)  40.6 g 
D)  81.3 g 
E)  163 g

Question 2

Consider the non-aqueous cell reaction   for which E$\degree$cell = 2.35 V at 200$\degree$C. $\Delta$G$\degree$at this temperature is

Accepted Answer

A)  453 kJ. 
B)  -453 kJ. 
C)  907 kJ. 
D)  -907 kJ. 
E)  None of these choices is correct. 
A)  453 kJ. 
B)  -453 kJ. 
C)  907 kJ. 
D)  -907 kJ. 
E)  None of these choices is correct.

Question 3

Examine the following half-reactions and select the weakest reducing agent among the substances.

Accepted Answer

A)  Cr(s) 
B)  Sn(s) 
C)  Mn2+(aq) 
D)  Hg(l) 
E)  OH¯(aq) 
A)  Cr(s) 
B)  Sn(s) 
C)  Mn2+(aq) 
D)  Hg(l) 
E)  OH¯(aq)

Question 4

Examine the following half-reactions and select the strongest reducing agent among the species listed.

Accepted Answer

A)  Pb(s) 
B)  Ca(s) 
C)  Pt(s) 
D)  Br¯(aq) 
E)  Pt2+(aq) 
A)  Pb(s) 
B)  Ca(s) 
C)  Pt(s) 
D)  Br¯(aq) 
E)  Pt2+(aq)

Question 5

What is the value of the equilibrium constant for the cell reaction below at 25$\degree$C?
 E$\degree$cell = 0.61 V 2Cr(s) + 3Pb2+(aq)   3Pb(s) + 2Cr3+(aq)

Accepted Answer

A)  4.1 * 1020 
B)  8.2 * 1030 
C)  3.3* 1051 
D)  7.4 * 1061 
E)  > 9.9 *1099 
A)  4.1 * 1020 
B)  8.2 * 1030 
C)  3.3* 1051 
D)  7.4 * 1061 
E)  > 9.9 *1099

Question 6

Consider the following balanced redox reaction 
3CuO(s) + 2NH3(aq) $\rightarrow$ N2(g) + 3H2O(l) + 3Cu(s)
Which of the following statements is true?

Accepted Answer

A)  CuO(s) is the oxidizing agent and copper is reduced. 
B)  CuO(s) is the oxidizing agent and copper is oxidized. 
C)  CuO(s) is the reducing agent and copper is oxidized. 
D)  CuO(s) is the reducing agent and copper is reduced. 
E)  CuO(s) is the oxidizing agent and N2(g) is the reducing agent. 
A)  CuO(s) is the oxidizing agent and copper is reduced. 
B)  CuO(s) is the oxidizing agent and copper is oxidized. 
C)  CuO(s) is the reducing agent and copper is oxidized. 
D)  CuO(s) is the reducing agent and copper is reduced. 
E)  CuO(s) is the oxidizing agent and N2(g) is the reducing agent.

Question 7

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu2+(aq) + 2e¯ $\rightarrow$ Cu(s) and Ag+(aq) + e¯ $\rightarrow$ Ag(s)
For every 1.00 g of copper produced in the first process, how many grams of silver will be produced in the second one?

Accepted Answer

A)  0.294 g 
B)  0.588 g 
C)  0.850 g 
D)  1.70 g 
E)  3.40 g 
A)  0.294 g 
B)  0.588 g 
C)  0.850 g 
D)  1.70 g 
E)  3.40 g

Question 8

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____.

Accepted Answer

A)  2 
B)  3 
C)  6 
D)  8 
E)  None of these choices is correct. 
A)  2 
B)  3 
C)  6 
D)  8 
E)  None of these choices is correct.

Question 9

Consider the following balanced redox reaction 
Mn2+(aq) + S2O82¯(aq) + 2H2O(l) $\rightarrow$ MnO2(s) + 4H+(aq) + 2SO42¯(aq)
Which of the following statements is true?

Accepted Answer

A)  Mn2+(aq) is the oxidizing agent and is reduced. 
B)  Mn2+(aq) is the oxidizing agent and is oxidized. 
C)  Mn2+(aq) is the reducing agent and is oxidized. 
D)  Mn2+(aq) is the reducing agent and is reduced. 
E)  Manganese does not change its oxidation number in this reaction. 
A)  Mn2+(aq) is the oxidizing agent and is reduced. 
B)  Mn2+(aq) is the oxidizing agent and is oxidized. 
C)  Mn2+(aq) is the reducing agent and is oxidized. 
D)  Mn2+(aq) is the reducing agent and is reduced. 
E)  Manganese does not change its oxidation number in this reaction.

Question 10

A concentration cell consists of two Al/Al3+ electrodes. The electrolyte in compartment A is 0.050 M Al(NO3)3 and in compartment B is 1.25 M Al(NO3)3. What is the voltage of the cell at 25$\degree$C?

Accepted Answer

A)  0.083 V 
B)  0.062 V 
C)  0.041V 
D)  0.028 V 
E)  None of these choices is correct. 
A)  0.083 V 
B)  0.062 V 
C)  0.041V 
D)  0.028 V 
E)  None of these choices is correct.

Question 11

A solution is prepared by dissolving 32.0 g of NiSO4 in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Accepted Answer

A)  1.1 A 
B)  2.2 A 
C)  3.3 A 
D)  4.4 A 
E)  5.5 A 
A)  1.1 A 
B)  2.2 A 
C)  3.3 A 
D)  4.4 A 
E)  5.5 A

Question 12

What is the E$\degree$cell for the cell represented by the combination of the following half-reactions?

Accepted Answer

A)  -0.18 V 
B)  0.18 V 
C)  1.28 V 
D)  1.66 V 
E)  2.12 V 
A)  -0.18 V 
B)  0.18 V 
C)  1.28 V 
D)  1.66 V 
E)  2.12 V

Question 13

Calculate E$\degree$cell for the reaction of nickel(II) ions with cadmium metal at 25$\degree$C. K = 1.17 *105. Ni2+(aq) + Cd(s) $\rightarrow$ Cd2+(aq) + Ni(s)

Accepted Answer

A)  0.075 V 
B)  0.10 V 
C)  0.12 V 
D)  0.15 V 
E)  0.30 V 
A)  0.075 V 
B)  0.10 V 
C)  0.12 V 
D)  0.15 V 
E)  0.30 V

Question 14

A battery that cannot be recharged is a

Accepted Answer

A)  fuel cell. 
B)  primary battery. 
C)  secondary battery. 
D)  simple battery. 
E)  flow battery. 
A)  fuel cell. 
B)  primary battery. 
C)  secondary battery. 
D)  simple battery. 
E)  flow battery.

Question 15

Consider the reaction of iodine with manganese dioxide: 
3I2(s) + 2MnO2(s) + 8OH¯(aq)   6I¯(aq) + 2MnO4¯(aq) + 4H2O(l)
The equilibrium constant for the overall reaction is 8.30* 10¯7. Calculate $\Delta$G$\degree$ for the reaction at 25$\degree$C.

Accepted Answer

A)  -15.1 kJ 
B)  -34.7 kJ 
C)  15.1 kJ 
D)  34.7 kJ 
E)  None of these choices is correct. 
A)  -15.1 kJ 
B)  -34.7 kJ 
C)  15.1 kJ 
D)  34.7 kJ 
E)  None of these choices is correct.

Question 16

Examine the following half-reactions and select the strongest oxidizing agent among the substances.

Accepted Answer

A)  [PtCl4]2¯(aq) 
B)  RuO4(s) 
C)  HFeO4¯(aq) 
D)  H4XeO6(aq) 
E)  Cl¯(aq) 
A)  [PtCl4]2¯(aq) 
B)  RuO4(s) 
C)  HFeO4¯(aq) 
D)  H4XeO6(aq) 
E)  Cl¯(aq)

Question 17

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics. If E$\degree$cell = 1.587 V and E$\degree$of the cathode half-cell is 0.536 V, what is E$\degree$ of the anode half-cell?

Accepted Answer

A)  -1.051 V 
B)  -2.123 V 
C)  1.051 V 
D)  2.123 V 
E)  None of these choices is correct. 
A)  -1.051 V 
B)  -2.123 V 
C)  1.051 V 
D)  2.123 V 
E)  None of these choices is correct.

Question 18

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Accepted Answer

A)  0.419 g 
B)  6.29 g 
C)  12.6 g 
D)  25.2 g 
E)  33.4 g 
A)  0.419 g 
B)  6.29 g 
C)  12.6 g 
D)  25.2 g 
E)  33.4 g

Question 19

A voltaic cell consists of a Hg/Hg22+ electrode (E$\degree$ = 0.85 V) and a Sn/Sn2+ electrode (E$\degree$ = -0.14 V). Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25$\degree$C.

Accepted Answer

A)  0.0001 M 
B)  0.0007 M 
C)  0.005 M 
D)  0.03 M 
E)  0.05 M 
A)  0.0001 M 
B)  0.0007 M 
C)  0.005 M 
D)  0.03 M 
E)  0.05 M

Question 20

In a fuel cell, an external source of electrical power is used to drive a non-spontaneous reaction in which a fuel is produced.

Accepted Answer

A) True 
 B)False

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

Consider the non-aqueous cell reaction $Consider the non-aqueous cell reaction for which E \degree <sub>cell</sub> = 2.35 V at 200 \degree C. \Delta G \degree at this temperature is$ for which E $\degree$ _cell = 2.35 V at 200 $\degree$ C. $\Delta$ G $\degree$ at this temperature is

Examine the following half-reactions and select the weakest reducing agent among the substances.

Examine the following half-reactions and select the strongest reducing agent among the species listed.

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) $\rightarrow$ N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____.

Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈²¯(aq) + 2H₂O(l) $\rightarrow$ MnO₂(s) + 4H⁺(aq) + 2SO₄²¯(aq) Which of the following statements is true?

A concentration cell consists of two Al/Al³⁺ electrodes. The electrolyte in compartment A is 0.050 M Al(NO₃)₃ and in compartment B is 1.25 M Al(NO₃)₃. What is the voltage of the cell at 25 $\degree$ C?

A solution is prepared by dissolving 32.0 g of NiSO₄ in water. What current would be needed to deposit all of the nickel in 5.0 hours?

What is the E $\degree$ _cell for the cell represented by the combination of the following half-reactions? $What is the E \degree <sub>cell</sub> for the cell represented by the combination of the following half-reactions?$

Calculate E $\degree$ _cell for the reaction of nickel(II) ions with cadmium metal at 25 $\degree$ C. K = 1.17 *10⁵. Ni²⁺(aq) + Cd(s) $\rightarrow$ Cd²⁺(aq) + Ni(s)

A battery that cannot be recharged is a

Examine the following half-reactions and select the strongest oxidizing agent among the substances.

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E $\degree$ = 0.85 V) and a Sn/Sn²⁺ electrode (E $\degree$ = -0.14 V). Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25 $\degree$ C.

In a fuel cell, an external source of electrical power is used to drive a non-spontaneous reaction in which a fuel is produced.

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 21: Electrochemistry: Chemical Change and Electrical Work

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

Consider the non-aqueous cell reaction for which E °\degree° cell = 2.35 V at 200 °\degree° C. Δ\DeltaΔ G °\degree° at this temperature is

Examine the following half-reactions and select the weakest reducing agent among the substances.

Examine the following half-reactions and select the strongest reducing agent among the species listed.

What is the value of the equilibrium constant for the cell reaction below at 25 °\degree° C? E °\degree° cell = 0.61 V 2Cr(s) + 3Pb2+(aq) 3Pb(s) + 2Cr3+(aq)

Consider the following balanced redox reaction 3CuO(s) + 2NH3(aq) →\rightarrow→ N2(g) + 3H2O(l) + 3Cu(s) Which of the following statements is true?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____.

Consider the following balanced redox reaction Mn2+(aq) + S2O82¯(aq) + 2H2O(l) →\rightarrow→ MnO2(s) + 4H+(aq) + 2SO42¯(aq) Which of the following statements is true?

A concentration cell consists of two Al/Al3+ electrodes. The electrolyte in compartment A is 0.050 M Al(NO3)3 and in compartment B is 1.25 M Al(NO3)3. What is the voltage of the cell at 25 °\degree° C?

A solution is prepared by dissolving 32.0 g of NiSO4 in water. What current would be needed to deposit all of the nickel in 5.0 hours?

What is the E °\degree° cell for the cell represented by the combination of the following half-reactions?

Calculate E °\degree° cell for the reaction of nickel(II) ions with cadmium metal at 25 °\degree° C. K = 1.17 *105. Ni2+(aq) + Cd(s) →\rightarrow→ Cd2+(aq) + Ni(s)

A battery that cannot be recharged is a

Consider the reaction of iodine with manganese dioxide: 3I2(s) + 2MnO2(s) + 8OH¯(aq) 6I¯(aq) + 2MnO4¯(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30* 10¯7. Calculate Δ\DeltaΔ G °\degree° for the reaction at 25 °\degree° C.

Examine the following half-reactions and select the strongest oxidizing agent among the substances.

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics. If E °\degree° cell = 1.587 V and E °\degree° of the cathode half-cell is 0.536 V, what is E °\degree° of the anode half-cell?

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

A voltaic cell consists of a Hg/Hg22+ electrode (E °\degree° = 0.85 V) and a Sn/Sn2+ electrode (E °\degree° = -0.14 V). Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25 °\degree° C.

In a fuel cell, an external source of electrical power is used to drive a non-spontaneous reaction in which a fuel is produced.

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

Consider the non-aqueous cell reaction $Consider the non-aqueous cell reaction for which E \degree <sub>cell</sub> = 2.35 V at 200 \degree C. \Delta G \degree at this temperature is$ for which E $\degree$ _cell = 2.35 V at 200 $\degree$ C. $\Delta$ G $\degree$ at this temperature is

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) $\rightarrow$ N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈²¯(aq) + 2H₂O(l) $\rightarrow$ MnO₂(s) + 4H⁺(aq) + 2SO₄²¯(aq) Which of the following statements is true?

A concentration cell consists of two Al/Al³⁺ electrodes. The electrolyte in compartment A is 0.050 M Al(NO₃)₃ and in compartment B is 1.25 M Al(NO₃)₃. What is the voltage of the cell at 25 $\degree$ C?

A solution is prepared by dissolving 32.0 g of NiSO₄ in water. What current would be needed to deposit all of the nickel in 5.0 hours?

What is the E $\degree$ _cell for the cell represented by the combination of the following half-reactions? $What is the E \degree <sub>cell</sub> for the cell represented by the combination of the following half-reactions?$

Calculate E $\degree$ _cell for the reaction of nickel(II) ions with cadmium metal at 25 $\degree$ C. K = 1.17 *10⁵. Ni²⁺(aq) + Cd(s) $\rightarrow$ Cd²⁺(aq) + Ni(s)

A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E $\degree$ = 0.85 V) and a Sn/Sn²⁺ electrode (E $\degree$ = -0.14 V). Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25 $\degree$ C.