Question 1

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 2

What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current?

Accepted Answer

A) 73.5 g 
B) 24.5 g 
C) 220.g 
D) 147 g 
E) 8.17 g 
A) 73.5 g 
B) 24.5 g 
C) 220.g 
D) 147 g 
E) 8.17 g

Question 3

Describe how water can be made to be a good conductor of electrical current.

Accepted Answer

A) use pure water 
B) heat the water 
C) add salt 
D) chill the water 
E) vaporize the water 
A) use pure water 
B) heat the water 
C) add salt 
D) chill the water 
E) vaporize the water

Question 4

What is the oxidizing agent in the redox reaction represented by the following cell notation? 
$\quad$$\quad$$\quad$Sn(s)| Sn2+(aq) $\|$ Ag+(aq)| Ag(s)

Accepted Answer

A) Sn(s) 
B) Ag+(aq) 
C) Sn2+(aq) 
D) Ag(s) 
E) Pt(s) 
A) Sn(s) 
B) Ag+(aq) 
C) Sn2+(aq) 
D) Ag(s) 
E) Pt(s)

Question 5

What is the reaction at the cathode in a breathalyzer?

Accepted Answer

A) Ethanol is oxidized to acetic acid. 
B) Acetic acid is reduced to ethanol. 
C) Oxygen is reduced. 
D) Hydrogen is oxidized. 
E) Ethanol is oxidized to acetaldehyde. 
A) Ethanol is oxidized to acetic acid. 
B) Acetic acid is reduced to ethanol. 
C) Oxygen is reduced. 
D) Hydrogen is oxidized. 
E) Ethanol is oxidized to acetaldehyde.

Question 6

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? 
$\quad$$\quad$$\quad$Ni(s)| Ni2+(aq)|| Cl2(g)| Cl-(aq)| C(s)

Accepted Answer

A) Ni(s)+ 2Cl-(aq)→ Ni2+(aq)+ Cl2(g) 
B) Ni(s)+ Cl2(g)→ Ni2+(aq)+ 2Cl-(aq) 
C) Ni2+(aq)+ 2Cl-(aq)→ Ni(s)+ Cl2(g) 
D) Ni2+(aq)+ 2Cl-(aq)→ NiCl2(s) 
A) Ni(s)+ 2Cl-(aq)→ Ni2+(aq)+ Cl2(g) 
B) Ni(s)+ Cl2(g)→ Ni2+(aq)+ 2Cl-(aq) 
C) Ni2+(aq)+ 2Cl-(aq)→ Ni(s)+ Cl2(g) 
D) Ni2+(aq)+ 2Cl-(aq)→ NiCl2(s)

Question 7

The standard emf for the cell using the overall cell reaction below is +2.20 V: 
$\quad$$\quad$2Al(s)+ $3 \mathrm { I } _ { 2 }$ (s)? $2 \mathrm { AL }  ^ { 3 + }$ (aq)+ $6 \mathrm { I } ^ { - }$ (aq)
The emf generated by the cell when [ $\mathrm { Al } ^ { 3 + }$ ] = 4.5 × $10 ^ { - 3 }$ mol L-1 and [ $\mathrm { I } ^ { - }$ ] = 0.15 mol L-1 is $\text { V. }$

Accepted Answer

A) 2.55 
B) 2.44 
C) 2.08 
D) 2.36 
E) 2.32 
A) 2.55 
B) 2.44 
C) 2.08 
D) 2.36 
E) 2.32

Question 8

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ $\mathrm { Mg } ^ { 2 + }$ ] = 0.500 M and [ $\mathrm { Fe } ^ { 3 + }$ ] = 2.00 M 
$\quad$$\quad$Mg(s)+ $\mathrm { Fe } ^ { 3 + }$ (aq)? $\mathrm { Mg } ^ { 2 + }$ (aq)+ Fe(s)
E°(Mg2+/Mg)= -2.37 V and E°(Fe3+/Fe)= -0.036 V

Accepted Answer

A) +2.09 V 
B) -3.18 V 
C) +2.35 V 
D) +0.36 V 
E) -1.51 V 
A) +2.09 V 
B) -3.18 V 
C) +2.35 V 
D) +0.36 V 
E) -1.51 V

Question 9

A galvanic cell consists of a Zn2+/Zn half-cell and a standard hydrogen electrode.If the Zn2+/Zn half-cell standard cell functions as the anode,and the standard cell potential is 0.76 V,what is the standard reduction potential for the Zn2+/Zn half-cell?

Accepted Answer

A) -0.76 V 
B) -0.38 V 
C) +0.38 V 
D) +0.76 V 
A) -0.76 V 
B) -0.38 V 
C) +0.38 V 
D) +0.76 V

Question 10

What mass of silver can be plated onto an object in 33.5 minutes at 8.70 A of current? 
$\quad$$\quad$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 11

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 12

Determine the redox reaction represented by the following cell notation: 
$\quad$$\quad$Mg(s)| Mg2+(aq) $\|$ Cu2+(aq)| Cu(s)

Accepted Answer

A) Cu(s)+ Mg2+(aq)? Mg(s)+ Cu2+(aq) 
B) Mg(s)+ Cu2+(aq)? Cu(s)+ Mg2+(aq) 
C) 2Mg(s)+ Cu2+(aq)? Cu(s)+ 2Mg2+(aq) 
D) 2Cu(s)+ Mg2+(aq)? Mg(s)+ 2Cu2+(aq) 
E) 3Mg(s)+ 2Cu2+(aq)? 2Cu(s)+ 3Mg2+(aq) 
A) Cu(s)+ Mg2+(aq)? Mg(s)+ Cu2+(aq) 
B) Mg(s)+ Cu2+(aq)? Cu(s)+ Mg2+(aq) 
C) 2Mg(s)+ Cu2+(aq)? Cu(s)+ 2Mg2+(aq) 
D) 2Cu(s)+ Mg2+(aq)? Mg(s)+ 2Cu2+(aq) 
E) 3Mg(s)+ 2Cu2+(aq)? 2Cu(s)+ 3Mg2+(aq)

Question 13

What is electrolysis?

Accepted Answer

An electrical curren

Question 14

Which of the following metals will dissolve in HCl?

Accepted Answer

A) Au; E°(Au3+/Au)= +1.50V 
B) Ag; E°(Ag+/Ag)= +0.80V 
C) Cu; E°(Cu2+/Cu)= +0.34V 
D) Al; E°(Al3+/Al)= -1.66V 
E) Pt; E°(Pt2+/Pt)= +1.19V 
A) Au; E°(Au3+/Au)= +1.50V 
B) Ag; E°(Ag+/Ag)= +0.80V 
C) Cu; E°(Cu2+/Cu)= +0.34V 
D) Al; E°(Al3+/Al)= -1.66V 
E) Pt; E°(Pt2+/Pt)= +1.19V

Question 15

Why,if we multiply a reaction by 2,don't we multiply its E°red by 2?

Accepted Answer

Half-cell potentials (E°)are a

Question 16

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

Accepted Answer

A) I-(aq)+ Zn2+(aq); if E°(I2/I-)= + 0.54V and E°(Zn2+/Zn)= -0.76V 
B) Ca(s)+ Mg2+(aq); if E°(Ca2+/Ca)= -2.76V and E°(Mg2+/Mg)= -2.37V 
C) H2(g)+ Cd2+(aq); if E°(Cd2+/Cd)= -0.40V 
D) Ag(s)+ Sn2+(aq); if E°(Ag+/Ag)= + 0.80V and E°(Sn2+/Sn)= -0.14V 
E) Ag+(aq)+ Mn2+(aq); if E°(Ag+/Ag)= + 0.80V and E°(MnO4-/Mn2+)= +1.51V 
A) I-(aq)+ Zn2+(aq); if E°(I2/I-)= + 0.54V and E°(Zn2+/Zn)= -0.76V 
B) Ca(s)+ Mg2+(aq); if E°(Ca2+/Ca)= -2.76V and E°(Mg2+/Mg)= -2.37V 
C) H2(g)+ Cd2+(aq); if E°(Cd2+/Cd)= -0.40V 
D) Ag(s)+ Sn2+(aq); if E°(Ag+/Ag)= + 0.80V and E°(Sn2+/Sn)= -0.14V 
E) Ag+(aq)+ Mn2+(aq); if E°(Ag+/Ag)= + 0.80V and E°(MnO4-/Mn2+)= +1.51V

Question 17

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: 
$\quad$$\quad$$\quad$Al(s)| Al3+(aq,0.115 mol L-1) $\|$ Al3+(aq,3.89 mol L-1)| Al(s)
E°(Al3+/Al)= -1.66 V

Accepted Answer

A) +1.66 V 
B) +0.060 V 
C) 0.00 V 
D) +0.090 V 
E) +0.030 V 
A) +1.66 V 
B) +0.060 V 
C) 0.00 V 
D) +0.090 V 
E) +0.030 V

Question 18

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C.(The equation is balanced.) 
$\quad$$\quad$Pb(s)+ Br2(l)→ Pb2+(aq)+ 2 Br⁻(aq)
Pb2+(aq)+ 2 e- → Pb(s)$\quad$$\quad$ E° = -0.13 V
Br2(l)+ 2 e- → 2 Br- (aq)$\quad$$\quad$E° = +1.07 V

Accepted Answer

A) +1.20 V 
B) +0.94 V 
C) -0.94 V 
D) -1.20 V 
E) -0.60 V 
A) +1.20 V 
B) +0.94 V 
C) -0.94 V 
D) -1.20 V 
E) -0.60 V

Question 19

What is undergoing oxidation in the redox reaction represented by the following cell notation? 
$\quad$$\quad$$\quad$Fe(s)| Fe3+(aq) $\|$ Cl2(g)| Cl- (aq)| Pt(s)

Accepted Answer

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

Question 20

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: 
$\quad$$\quad$$\quad$Sn(s)| Sn2+(aq,0.010 mol L-1) $\|$ Ag+(aq,1.00 mol L-1)| Ag(s)
E°(Sn2+/Sn)= -0.14 V and E°(Ag+/Ag)= +0.80 V

Accepted Answer

A) +1.18 V 
B) -1.18 V 
C) +1.00 V 
D) +0.94 V 
E) -0.94 V 
A) +1.18 V 
B) -1.18 V 
C) +1.00 V 
D) +0.94 V 
E) -0.94 V

Exam 18: Electrochemistry

Which of the following is the strongest reducing agent?

What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current?

Describe how water can be made to be a good conductor of electrical current.

What is the oxidizing agent in the redox reaction represented by the following cell notation? \quad\quad\quad Sn(s)| Sn2+(aq) ∥\|∥ Ag+(aq)| Ag(s)

What is the reaction at the cathode in a breathalyzer?

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? \quad\quad\quad Ni(s)| Ni2+(aq)|| Cl2(g)| Cl-(aq)| C(s)

A galvanic cell consists of a Zn2+/Zn half-cell and a standard hydrogen electrode.If the Zn2+/Zn half-cell standard cell functions as the anode,and the standard cell potential is 0.76 V,what is the standard reduction potential for the Zn2+/Zn half-cell?

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

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?

Determine the redox reaction represented by the following cell notation: \quad\quad Mg(s)| Mg2+(aq) ∥\|∥ Cu2+(aq)| Cu(s)

What is electrolysis?

Which of the following metals will dissolve in HCl?

Why,if we multiply a reaction by 2,don't we multiply its E°red by 2?

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

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: \quad\quad\quad Al(s)| Al3+(aq,0.115 mol L-1) ∥\|∥ Al3+(aq,3.89 mol L-1)| Al(s) E°(Al3+/Al)= -1.66 V

What is undergoing oxidation in the redox reaction represented by the following cell notation? \quad\quad\quad Fe(s)| Fe3+(aq) ∥\|∥ Cl2(g)| Cl- (aq)| Pt(s)

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: \quad\quad\quad Sn(s)| Sn2+(aq,0.010 mol L-1) ∥\|∥ Ag+(aq,1.00 mol L-1)| Ag(s) E°(Sn2+/Sn)= -0.14 V and E°(Ag+/Ag)= +0.80 V

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

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 Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

What is the oxidizing agent in the redox reaction represented by the following cell notation? $\quad$ $\quad$ $\quad$ Sn(s)| Sn²⁺(aq) $\|$ Ag⁺(aq)| Ag(s)

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? $\quad$ $\quad$ $\quad$ Ni(s)| Ni²⁺(aq)|| Cl₂(g)| Cl^-(aq)| C(s)

A galvanic cell consists of a Zn²⁺/Zn half-cell and a standard hydrogen electrode.If the Zn²⁺/Zn half-cell standard cell functions as the anode,and the standard cell potential is 0.76 V,what is the standard reduction potential for the Zn²⁺/Zn half-cell?

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

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?

Determine the redox reaction represented by the following cell notation: $\quad$ $\quad$ Mg(s)| Mg²⁺(aq) $\|$ Cu²⁺(aq)| Cu(s)

Why,if we multiply a reaction by 2,don't we multiply its E°_red by 2?

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: $\quad$ $\quad$ $\quad$ Al(s)| Al³⁺(aq,0.115 mol L^-1) $\|$ Al³⁺(aq,3.89 mol L^-1)| Al(s) E°(Al³⁺/Al)= -1.66 V

What is undergoing oxidation in the redox reaction represented by the following cell notation? $\quad$ $\quad$ $\quad$ Fe(s)| Fe³⁺(aq) $\|$ Cl₂(g)| Cl^- (aq)| Pt(s)

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: $\quad$ $\quad$ $\quad$ Sn(s)| Sn²⁺(aq,0.010 mol L^-1) $\|$ Ag⁺(aq,1.00 mol L^-1)| Ag(s) E°(Sn²⁺/Sn)= -0.14 V and E°(Ag⁺/Ag)= +0.80 V