Question 1

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.

Accepted Answer

A) Sn4+(aq)+ Mg(s) 
B) Cr3+(aq)+ Ni(s) 
C) Zn(s)+ Na+(aq) 
D) Fe(s)+ Ba2+(aq) 
E) None of the above pairs will react. 
A) Sn4+(aq)+ Mg(s) 
B) Cr3+(aq)+ Ni(s) 
C) Zn(s)+ Na+(aq) 
D) Fe(s)+ Ba2+(aq) 
E) None of the above pairs will react.

Question 2

What element is being reduced in the following redox reaction?
MnO4⁻(aq)+ H2C2O4(aq)→ Mn2+(aq)+ CO2(g)

Accepted Answer

A) C 
B) O 
C) Mn 
D) H 
A) C 
B) O 
C) Mn 
D) H

Question 3

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V:
Zn(s)+ 2H+(aq)→ Zn2+(aq)+ H2(g)
With PH2 = 1.0 atm and [Zn2+] = 1.0 M,the cell potential is 0.66 V.The concentration of H+ in the cathode compartment is ________ M.

Accepted Answer

A) 2.0 × 10-2 
B) 4.2 × 10-4 
C) 1.4 × 10-1 
D) 4.9 × 101  
E) 1.0 × 10-12 
A) 2.0 × 10-2 
B) 4.2 × 10-4 
C) 1.4 × 10-1 
D) 4.9 × 101  
E) 1.0 × 10-12

Question 4

For the reaction below,determine the standard free energy change,ΔG°.
Cu(s)+ Sn2+(aq)→ Cu2+(aq)+ Sn(s)E°cell = -0.48 V

Accepted Answer

A) -46.3 kJ 
B) +46.3 kJ 
C) -92.6 kJ 
D) +92.6 kJ 
A) -46.3 kJ 
B) +46.3 kJ 
C) -92.6 kJ 
D) +92.6 kJ

Question 5

Explain the use of a salt bridge.

Accepted Answer

The salt bridge allo

Question 6

What is the reduction half-reaction for the following overall galvanic cell reaction?
Zn2+(aq)+ 2 Ag(s)→ Zn(s)+ 2 Ag+(aq)

Accepted Answer

A) Ag(s)+ e- → Ag+(aq) 
B) Ag+(aq)+ e- → Ag(s) 
C) Zn2+(aq)+ 2 e- → Zn(s) 
D) Zn2+(aq)+ e- → Zn(s) 
A) Ag(s)+ e- → Ag+(aq) 
B) Ag+(aq)+ e- → Ag(s) 
C) Zn2+(aq)+ 2 e- → Zn(s) 
D) Zn2+(aq)+ e- → Zn(s)

Question 7

How many electrons are transferred in the following reaction? (The reaction is unbalanced. )
Ca(s)+ Cr3+(aq)→ Cr(s)+ Ca2+(aq)

Accepted Answer

A) 6 
B) 2 
C) 3 
D) 1 
E) 4 
A) 6 
B) 2 
C) 3 
D) 1 
E) 4

Question 8

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. )
3 Cl2(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe3+(aq)

Accepted Answer

A) 4.16 V 
B) -1.40 V 
C) -1.32 V 
D) 1.32 V 
E) 1.40 V 
A) 4.16 V 
B) -1.40 V 
C) -1.32 V 
D) 1.32 V 
E) 1.40 V

Question 9

A galvanic cell consists of a Mg2+/Mg half-cell and a standard hydrogen electrode.If the Mg2+/Mg half-cell standard cell functions as the anode,and the standard cell potential is 2.37 V,what is the standard reduction potential for the Mg2+/Mg half-cell?

Accepted Answer

A) -2.37 V 
B) -1.18 V 
C) +1.18 V 
D) +2.37 V 
A) -2.37 V 
B) -1.18 V 
C) +1.18 V 
D) +2.37 V

Question 10

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr3+ ions for 320.minutes?

Accepted Answer

A) 27.6 g 
B) 49.2 g 
C) 82.4 g 
D) 248 g 
A) 27.6 g 
B) 49.2 g 
C) 82.4 g 
D) 248 g

Question 11

Give the criteria for a spontaneous reaction.

Accepted Answer

A) ΔG° cell > 0,K > 1 B) ΔG° > 0,E°cell > 0,K > 1 C) ΔG° > 0,E°cell 1 D) ΔG° cell > 0,K 0,E°cell < 0,K < 1 A) ΔG° cell > 0,K > 1 B) ΔG° > 0,E°cell > 0,K > 1 C) ΔG° > 0,E°cell 1 D) ΔG° cell > 0,K 0,E°cell < 0,K < 1

Question 12

Explain the significance of the standard hydrogen electrode (SHE)in the tabulation of standard reduction potentials of other species.

Accepted Answer

The SHE is used to construct an electroc

Question 13

The standard emf for the cell using the overall cell reaction below is +0.48 V:
Zn(s)+ Ni2+(aq)→ Zn2+(aq)+ Ni(s)
The emf generated by the cell when [Ni2+] = 2.50 M and [Zn2+] = 0.100 M is ________ V.

Accepted Answer

A) 0.40 
B) 0.50 
C) 0.52 
D) 0.56 
E) 0.44 
A) 0.40 
B) 0.50 
C) 0.52 
D) 0.56 
E) 0.44

Question 14

What element is being reduced in the following redox reaction?
H2O2(l)+ ClO2(aq)→ ClO2⁻(aq)+ O2(g)

Accepted Answer

A) H 
B) O 
C) Cl 
D) N 
E) C 
A) H 
B) O 
C) Cl 
D) N 
E) C

Question 15

Which of the following is the strongest reducing agent?

Accepted Answer

A) Sn2+(aq) 
B) Cr3+(aq) 
C) Sn4+(aq) 
D) Cr(s) 
E) Sn(s) 
A) Sn2+(aq) 
B) Cr3+(aq) 
C) Sn4+(aq) 
D) Cr(s) 
E) Sn(s)

Question 16

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. )
Sn(s)+ 2 Ag⁺(aq)→ Sn2+(aq)+ 2 Ag(s)

Accepted Answer

A) 1.74 V 
B) 0.94 V 
C) 1.08 V 
D) -1.08 V 
E) -1.74 V 
A) 1.74 V 
B) 0.94 V 
C) 1.08 V 
D) -1.08 V 
E) -1.74 V

Question 17

Determine the cell notation for the redox reaction given below.
3 Cl2(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe3+(aq)

Accepted Answer

A) Cl2(g)∣ Cl⁻(aq)∣ Pt ∣∣ Fe(s)∣ Fe3+(aq) 
B) Cl⁻(aq)∣ Cl2(g)∣ Pt ∣∣ Fe3+(aq) ∣ Fe(s) 
C) Fe3+(aq)∣ Fe(s)∣∣ Cl⁻(aq)∣ Cl2(g)∣ Pt 
D) Fe(s)∣ Cl2(g)∣∣ Fe3+(aq)∣ Cl⁻(aq)∣ Pt 
E) Fe(s)∣ Fe3+(aq)∣∣ Cl2(g)∣ Cl⁻(aq)∣ Pt 
A) Cl2(g)∣ Cl⁻(aq)∣ Pt ∣∣ Fe(s)∣ Fe3+(aq) 
B) Cl⁻(aq)∣ Cl2(g)∣ Pt ∣∣ Fe3+(aq) ∣ Fe(s) 
C) Fe3+(aq)∣ Fe(s)∣∣ Cl⁻(aq)∣ Cl2(g)∣ Pt 
D) Fe(s)∣ Cl2(g)∣∣ Fe3+(aq)∣ Cl⁻(aq)∣ Pt 
E) Fe(s)∣ Fe3+(aq)∣∣ Cl2(g)∣ Cl⁻(aq)∣ Pt

Question 18

Match the following.
-Q = K

Accepted Answer

A) Ecell = E°cell 
B) Ecell = 0 
C) E°cell cell cell > 0
F)Ecell > 0 
A) Ecell = E°cell 
B) Ecell = 0 
C) E°cell cell cell > 0
F)Ecell > 0

Question 19

What mass of silver can be plated onto an object in 33.5 minutes at 8.70 A of current?
Ag⁺(aq)+ e⁻ → Ag(s)

Accepted Answer

A) 19.6 g 
B) 0.326 g 
C) 9.78 g 
D) 3.07 g 
E) 0.102 g 
A) 19.6 g 
B) 0.326 g 
C) 9.78 g 
D) 3.07 g 
E) 0.102 g

Question 20

How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu2+ ions to produce 5.00 moles of copper metal?

Accepted Answer

A) 0.187 hours 
B) 0.373 hours 
C) 2.68 hours 
D) 5.36 hours 
A) 0.187 hours 
B) 0.373 hours 
C) 2.68 hours 
D) 5.36 hours

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.

What element is being reduced in the following redox reaction? MnO₄⁻(aq)+ H₂C₂O₄(aq)→ Mn²⁺(aq)+ CO₂(g)

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s)+ 2H⁺(aq)→ Zn²⁺(aq)+ H₂(g) With P_H₂ = 1.0 atm and [Zn²⁺] = 1.0 M,the cell potential is 0.66 V.The concentration of H⁺ in the cathode compartment is ________ M.

For the reaction below,determine the standard free energy change,ΔG°. Cu(s)+ Sn²⁺(aq)→ Cu²⁺(aq)+ Sn(s)E°_cell= -0.48 V

Explain the use of a salt bridge.

What is the reduction half-reaction for the following overall galvanic cell reaction? Zn²⁺(aq)+ 2 Ag(s)→ Zn(s)+ 2 Ag⁺(aq)

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) Ca(s)+ Cr³⁺(aq)→ Cr(s)+ Ca²⁺(aq)

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. ) 3 Cl₂(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe³⁺(aq)

A galvanic cell consists of a Mg²⁺/Mg half-cell and a standard hydrogen electrode.If the Mg²⁺/Mg half-cell standard cell functions as the anode,and the standard cell potential is 2.37 V,what is the standard reduction potential for the Mg²⁺/Mg half-cell?

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr³⁺ ions for 320.minutes?

Give the criteria for a spontaneous reaction.

Explain the significance of the standard hydrogen electrode (SHE)in the tabulation of standard reduction potentials of other species.

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s)+ Ni²⁺(aq)→ Zn²⁺(aq)+ Ni(s) The emf generated by the cell when [Ni²⁺] = 2.50 M and [Zn²⁺] = 0.100 M is ________ V.

What element is being reduced in the following redox reaction? H₂O₂(l)+ ClO₂(aq)→ ClO₂⁻(aq)+ O₂(g)

Which of the following is the strongest reducing agent?

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. ) Sn(s)+ 2 Ag⁺(aq)→ Sn²⁺(aq)+ 2 Ag(s)

Determine the cell notation for the redox reaction given below. 3 Cl₂(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe³⁺(aq)

Match the following. -Q = K

What mass of silver can be plated onto an object in 33.5 minutes at 8.70 A of current? Ag⁺(aq)+ e⁻ → Ag(s)

How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu²⁺ ions to produce 5.00 moles of copper metal?

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

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Filters

Exam 18: Electrochemistry

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.

What element is being reduced in the following redox reaction? MnO4⁻(aq)+ H2C2O4(aq)→ Mn2+(aq)+ CO2(g)

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s)+ 2H+(aq)→ Zn2+(aq)+ H2(g) With PH2 = 1.0 atm and [Zn2+] = 1.0 M,the cell potential is 0.66 V.The concentration of H+ in the cathode compartment is ________ M.

For the reaction below,determine the standard free energy change,ΔG°. Cu(s)+ Sn2+(aq)→ Cu2+(aq)+ Sn(s)E°cell = -0.48 V

Explain the use of a salt bridge.

What is the reduction half-reaction for the following overall galvanic cell reaction? Zn2+(aq)+ 2 Ag(s)→ Zn(s)+ 2 Ag+(aq)

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) Ca(s)+ Cr3+(aq)→ Cr(s)+ Ca2+(aq)

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. ) 3 Cl2(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe3+(aq)

A galvanic cell consists of a Mg2+/Mg half-cell and a standard hydrogen electrode.If the Mg2+/Mg half-cell standard cell functions as the anode,and the standard cell potential is 2.37 V,what is the standard reduction potential for the Mg2+/Mg half-cell?

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr3+ ions for 320.minutes?

Give the criteria for a spontaneous reaction.

Explain the significance of the standard hydrogen electrode (SHE)in the tabulation of standard reduction potentials of other species.

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s)+ Ni2+(aq)→ Zn2+(aq)+ Ni(s) The emf generated by the cell when [Ni2+] = 2.50 M and [Zn2+] = 0.100 M is ________ V.

What element is being reduced in the following redox reaction? H2O2(l)+ ClO2(aq)→ ClO2⁻(aq)+ O2(g)

Which of the following is the strongest reducing agent?

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. ) Sn(s)+ 2 Ag⁺(aq)→ Sn2+(aq)+ 2 Ag(s)

Determine the cell notation for the redox reaction given below. 3 Cl2(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe3+(aq)

Match the following. -Q = K

What mass of silver can be plated onto an object in 33.5 minutes at 8.70 A of current? Ag⁺(aq)+ e⁻ → Ag(s)

How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu2+ ions to produce 5.00 moles of copper metal?

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Radioactivity and Nuclear Chemistry

Filters

What element is being reduced in the following redox reaction? MnO₄⁻(aq)+ H₂C₂O₄(aq)→ Mn²⁺(aq)+ CO₂(g)

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s)+ 2H⁺(aq)→ Zn²⁺(aq)+ H₂(g) With P_H₂ = 1.0 atm and [Zn²⁺] = 1.0 M,the cell potential is 0.66 V.The concentration of H⁺ in the cathode compartment is ________ M.

For the reaction below,determine the standard free energy change,ΔG°. Cu(s)+ Sn²⁺(aq)→ Cu²⁺(aq)+ Sn(s)E°_cell= -0.48 V

What is the reduction half-reaction for the following overall galvanic cell reaction? Zn²⁺(aq)+ 2 Ag(s)→ Zn(s)+ 2 Ag⁺(aq)

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) Ca(s)+ Cr³⁺(aq)→ Cr(s)+ Ca²⁺(aq)

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. ) 3 Cl₂(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe³⁺(aq)

A galvanic cell consists of a Mg²⁺/Mg half-cell and a standard hydrogen electrode.If the Mg²⁺/Mg half-cell standard cell functions as the anode,and the standard cell potential is 2.37 V,what is the standard reduction potential for the Mg²⁺/Mg half-cell?

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr³⁺ ions for 320.minutes?

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s)+ Ni²⁺(aq)→ Zn²⁺(aq)+ Ni(s) The emf generated by the cell when [Ni²⁺] = 2.50 M and [Zn²⁺] = 0.100 M is ________ V.

What element is being reduced in the following redox reaction? H₂O₂(l)+ ClO₂(aq)→ ClO₂⁻(aq)+ O₂(g)

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. ) Sn(s)+ 2 Ag⁺(aq)→ Sn²⁺(aq)+ 2 Ag(s)

Determine the cell notation for the redox reaction given below. 3 Cl₂(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe³⁺(aq)

How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Cu²⁺ ions to produce 5.00 moles of copper metal?