Question 1

Which relationship is NOT correctly defined?

Accepted Answer

A) Work = E F1F1F1S1F1F1F10 q 
B) (F1F1F1S1F1F1F10G = -n · F · 
E)  
C)   
D) P = E F1F1F1S1F1F1F10 I 
E) q = n F1F1F1S1F1F1F10N F1F1F1S1F1F1F10F 
A) Work = E F1F1F1S1F1F1F10 q 
B) (F1F1F1S1F1F1F10G = -n · F · 
E)  
C)   
D) P = E F1F1F1S1F1F1F10 I 
E) q = n F1F1F1S1F1F1F10N F1F1F1S1F1F1F10F B

Question 2

For the cell diagram below write out and balance the reaction that occurs in the cell.
Pt|HOCl (aq,1 M),HClO2 (aq,1 M),H+ (aq,1 M)||   (aq,1 M),H+ (aq,1 M)| MnO2 (s)|Pt

Accepted Answer

2 + 2 H⁺ + 3 HOCl ⇋ 2 MnO₂ + 3 HClO₂ + H₂O

Question 3

Which is true when electrochemical cells are used as chemical probes?
I.All concentrations in the half-cells must be known except for the analyte of interest.
II. The analyte concentration is calculated from the equilibrium cell potential.
III. Equilibrium between the half-cells is established.
IV. Equilibrium within each half-cell is established and is assumed to remain at equilibrium.
V. Half-cells other than the S.H.E.can be used to determine pH.

Accepted Answer

A) II,III,and IV 
B) I,IV,and V 
C) I and II 
D) III,IV,and V 
E) I,II,and V 
A) II,III,and IV 
B) I,IV,and V 
C) I and II 
D) III,IV,and V 
E) I,II,and V B

Question 4

EoF1F1F1S1F1F1F10 is defined as:

Accepted Answer

A) the formal half-cell potential for compounds that are neither acids nor bases. 
B) the formal half-cell potential at 20 F1F1F1S1F1F1F10C. 
C) the formal half-cell potential at pH 7. 
D) the inverse of E°. 
E) None of these answers is the definition of E°F1F1F1S1F1F1F10. 
A) the formal half-cell potential for compounds that are neither acids nor bases. 
B) the formal half-cell potential at 20 F1F1F1S1F1F1F10C. 
C) the formal half-cell potential at pH 7. 
D) the inverse of E°. 
E) None of these answers is the definition of E°F1F1F1S1F1F1F10.

Question 5

A galvanic cell is at equilibrium when:

Accepted Answer

A) Ecell is a constant value. 
B) cell resistance is very low. 
C) Ecell = 0 V. 
D) Ecell fluctuates between F1F1F1S1F1F1F10 E°cell. 
E) cell resistance is infinitely large. 
A) Ecell is a constant value. 
B) cell resistance is very low. 
C) Ecell = 0 V. 
D) Ecell fluctuates between F1F1F1S1F1F1F10 E°cell. 
E) cell resistance is infinitely large.

Question 6

All of the following are true for the measurement of standard reduction potentials,except:
I standard conditions for reduction potentials is 25 oC and A = 1 for all aqueous and gaseous species.
II reduction potentials are measured relative to the standard hydrogen electrode (S.H.E. ).
III standard reduction potentials are measured while connected to the negative electrode of the potentiometer.
IV the E° for the S.H.E.is defined as 0 volts.

Accepted Answer

A) I and IV 
B) I and III 
C) I only 
D) III only 
E) II and IV 
A) I and IV 
B) I and III 
C) I only 
D) III only 
E) II and IV

Question 7

For the line notation below,which is NOT true? Fe(s)| Fe2+ (aq,A = 1)|| Cu2+ (aq,A = 1)| Cu (s)

Accepted Answer

A) Fe is the anode. 
B) || represents the salt bridge. 
C) Cu is the anode. 
D) 1 M Cu2+ is the electrolyte concentration and species for the copper electrode. 
E) 1 M Fe2+ is the electrolyte concentration and species for the iron electrode. 
A) Fe is the anode. 
B) || represents the salt bridge. 
C) Cu is the anode. 
D) 1 M Cu2+ is the electrolyte concentration and species for the copper electrode. 
E) 1 M Fe2+ is the electrolyte concentration and species for the iron electrode.

Question 8

For the reaction below,the oxidizing agent is____________________ and it____________________ electrons,and the reducing agent is____________________ and it____________________ electrons. 8 H+ +   + 5 Cu+ ⇋ Mn2+ + 5 Cu2+ + 4 H2O

Accepted Answer

A)   
;gains 5;Cu+;loses 1 
B) H+;loses 1;Cu+;gains 1 
C) H+;gains 1;
 
;loses 5 
D) Cu+;loses 1;
 
;gains 1 
E) Cu+;loses 1;H+;gains 1 
A)   
;gains 5;Cu+;loses 1 
B) H+;loses 1;Cu+;gains 1 
C) H+;gains 1;
 
;loses 5 
D) Cu+;loses 1;
 
;gains 1 
E) Cu+;loses 1;H+;gains 1

Question 9

Calculate E°F1F1F1S1F1F1F10 for the half-cell below. O2 + 4 H+ + 4 e− ⇋ 2 H2O E° = 1.229 V

Accepted Answer

A) 1)643 V 
B) 0)815 V 
C) 0)307 V 
D) 1)229 V 
E) 0)711 V 
A) 1)643 V 
B) 0)815 V 
C) 0)307 V 
D) 1)229 V 
E) 0)711 V

Question 10

Calculate the standard potential when the two half-cells below are connected via a salt bridge and potentiometer.Which species are the reducing agent and oxidizing agent?   + 2 H+ + 2 e- ⇋   + H2O E° = 1.589 V
Mg(OH)2 (s)+ 2 e- ⇋ Mg (s)+ 2 OH- E° = -2.690 V

Accepted Answer

4.279 V, @#IMG-DLM& is the oxi

Question 11

A galvanic cell with a large equilibrium constant has a____________________ cell potential.

Accepted Answer

A) negative 
B) constant 
C) zero voltage 
D) positive 
E) variable 
A) negative 
B) constant 
C) zero voltage 
D) positive 
E) variable

Question 12

A cell is constructed according to the cell diagram below.If the measured potential is 1.00 V,what is the pH of the dichromate cell? Fe|Fe2+ (aq,1M)||   (aq 1 M),Cr2+ (aq,1 M),H+ (aq,x M)|Pt   + 14 H+ + 6 e− ⇋ 2 Cr3+ + 7 H2O E° = 1.36 V
Fe2+ + 2 e− ⇋ Fe (s)____________________ E° = −0.44 V

Accepted Answer

A) 1)931 
B) 5)797 
C) 12.162 
D) 6)081 
E) 4)054 
A) 1)931 
B) 5)797 
C) 12.162 
D) 6)081 
E) 4)054

Question 13

Which is NOT correct for when the silver and vanadium half-cells are connected via a salt bridge and a potentiometer?
Ag+ + 1 e- → Ag (s)E° = 0.7993 V
V2+ + 2 e- → V (s)E° = −1.125 V
I Ag+ is reduced.
II V is oxidized.
III Eocell = 1.924 V
IV V2+ is reduced.
V Ag is oxidized.

Accepted Answer

A) I and II 
B) III,IV,and V 
C) I,II,and III 
D) III only 
E) IV and V 
A) I and II 
B) III,IV,and V 
C) I,II,and III 
D) III only 
E) IV and V

Question 14

Calculate the equilibrium constant for the reaction between Sn metal and Zn2+ solution. Sn + Zn2+ ⇋ Sn2+ + Zn
Sn2+ + 2 e− → Sn (s)E° = −0.141 V
Zn2+ + 2 e− → Zn (s)E° = −0.762 V

Accepted Answer

A) 9)86 × 1020 
B) 1)21 × 10−21 
C) 3)37 × 1030 
D) 3)18 × 10−11 
E) 1)84 × 1015 
A) 9)86 × 1020 
B) 1)21 × 10−21 
C) 3)37 × 1030 
D) 3)18 × 10−11 
E) 1)84 × 1015

Question 15

Which of the following is NOT true for galvanic cells?

Accepted Answer

A) Galvanic cells are spontaneous. 
B) Oxidation occurs at the anode and reduction occurs at the cathode. 
C) Electrons move toward more negative electrical potential. 
D) Galvanic cells are composed of two half-cells connected by salt bridge. 
E) The salt bridge maintains electroneutrality throughout the cell. 
A) Galvanic cells are spontaneous. 
B) Oxidation occurs at the anode and reduction occurs at the cathode. 
C) Electrons move toward more negative electrical potential. 
D) Galvanic cells are composed of two half-cells connected by salt bridge. 
E) The salt bridge maintains electroneutrality throughout the cell.

Question 16

A bromide probe is constructed from a saturated silver bromide half-cell and a Ni2+/Ni half-cell.If the measured potential is 0.952 V and [Ni2+] = 1 M,what is the bromide concentration?
AgBr (s)+ e− ⇋ Ag(s)+ Br− E° = 0.071 V
Ni2+ + 2 e− ⇋ Ni (s)E° = −0.714 V

Accepted Answer

Question 17

Calculate the potential for the half-cell below for [   ] = 0.100 M,[   ] = 0.500 M and the pH = 10.50.
2   + 3 H2O + 4 e− ⇋   + 6 OH- E° = −0.566 V

Accepted Answer

Question 18

Calculate Eo and K for the cell composed of a bromate/bromide half-cell and a chlorate/chlorine dioxide half-cell.   + 2 H+ + e− ⇋ ClO2 + H2O E° = 1.130 V   + 3 H2O + 6 e− ⇋ Br− + 6 OH− E° = 0.613 V

Accepted Answer

E^° = 0.517

Question 19

The half-cells below are connected via a salt-bridge and potentiometer.What is the voltage read by the potentiometer when AAg+ = 2.00 and AV2+ = 1.50? Ag+ + 1 e− → Ag (s)Eo = 0.7993 V
V2+ + 2 e− → V (s)Eo = −1.125 V

Accepted Answer

A) 1)912 V 
B) −0.326 V 
C) −0.313 V 
D) 1)937 V 
E) 1)924 V 
A) 1)912 V 
B) −0.326 V 
C) −0.313 V 
D) 1)937 V 
E) 1)924 V

Question 20

For the silver half-reaction,Ag+ + 1 e- → Ag (s),when the concentration of silver cation is increased,the reduction potential:

Accepted Answer

A) becomes more positive. 
B) becomes more negative. 
C) remains constant. 
D) increases or decreases depending on the voltage of the other half-reaction. 
E) increases or decreases depending on the temperature. 
A) becomes more positive. 
B) becomes more negative. 
C) remains constant. 
D) increases or decreases depending on the voltage of the other half-reaction. 
E) increases or decreases depending on the temperature.

Exam 15: Fundamentals of Electrochemistry

Which relationship is NOT correctly defined?

For the cell diagram below write out and balance the reaction that occurs in the cell. Pt|HOCl (aq,1 M),HClO2 (aq,1 M),H+ (aq,1 M)|| (aq,1 M),H+ (aq,1 M)| MnO2 (s)|Pt

Eo is defined as:

A galvanic cell is at equilibrium when:

For the line notation below,which is NOT true? Fe(s)| Fe2+ (aq,A = 1)|| Cu2+ (aq,A = 1)| Cu (s)

For the reaction below,the oxidizing agent is____________________ and it____________________ electrons,and the reducing agent is____________________ and it____________________ electrons. 8 H+ + + 5 Cu+ ⇋ Mn2+ + 5 Cu2+ + 4 H2O

Calculate E° for the half-cell below. O2 + 4 H+ + 4 e− ⇋ 2 H2O E° = 1.229 V

Calculate the standard potential when the two half-cells below are connected via a salt bridge and potentiometer.Which species are the reducing agent and oxidizing agent? + 2 H+ + 2 e- ⇋ + H2O E° = 1.589 V Mg(OH)2 (s)+ 2 e- ⇋ Mg (s)+ 2 OH- E° = -2.690 V

A galvanic cell with a large equilibrium constant has a____________________ cell potential.

A cell is constructed according to the cell diagram below.If the measured potential is 1.00 V,what is the pH of the dichromate cell? Fe|Fe2+ (aq,1M)|| (aq 1 M),Cr2+ (aq,1 M),H+ (aq,x M)|Pt + 14 H+ + 6 e− ⇋ 2 Cr3+ + 7 H2O E° = 1.36 V Fe2+ + 2 e− ⇋ Fe (s)____________________ E° = −0.44 V

Which is NOT correct for when the silver and vanadium half-cells are connected via a salt bridge and a potentiometer? Ag+ + 1 e- → Ag (s)E° = 0.7993 V V2+ + 2 e- → V (s)E° = −1.125 V I Ag+ is reduced. II V is oxidized. III Eocell = 1.924 V IV V2+ is reduced. V Ag is oxidized.

Calculate the equilibrium constant for the reaction between Sn metal and Zn2+ solution. Sn + Zn2+ ⇋ Sn2+ + Zn Sn2+ + 2 e− → Sn (s)E° = −0.141 V Zn2+ + 2 e− → Zn (s)E° = −0.762 V

Which of the following is NOT true for galvanic cells?

A bromide probe is constructed from a saturated silver bromide half-cell and a Ni2+/Ni half-cell.If the measured potential is 0.952 V and [Ni2+] = 1 M,what is the bromide concentration? AgBr (s)+ e− ⇋ Ag(s)+ Br− E° = 0.071 V Ni2+ + 2 e− ⇋ Ni (s)E° = −0.714 V

Calculate the potential for the half-cell below for [ ] = 0.100 M,[ ] = 0.500 M and the pH = 10.50. 2 + 3 H2O + 4 e− ⇋ + 6 OH- E° = −0.566 V

Calculate Eo and K for the cell composed of a bromate/bromide half-cell and a chlorate/chlorine dioxide half-cell. + 2 H+ + e− ⇋ ClO2 + H2O E° = 1.130 V + 3 H2O + 6 e− ⇋ Br− + 6 OH− E° = 0.613 V

The half-cells below are connected via a salt-bridge and potentiometer.What is the voltage read by the potentiometer when AAg+ = 2.00 and AV2+ = 1.50? Ag+ + 1 e− → Ag (s)Eo = 0.7993 V V2+ + 2 e− → V (s)Eo = −1.125 V

For the silver half-reaction,Ag+ + 1 e- → Ag (s),when the concentration of silver cation is increased,the reduction potential:

The Analytical Process

Chemical Measurements

Tools of the Trade

Experimental Error

Statistics

Quality Assurance and Calibration Methods

Chemical Equilibrium

Let the Titrations Begin

Activity and the Systematic Treatment of Equilibrium

Monoprotic Acid-Base Equilibria

Polyprotic Acid-Base Equilibria

Acid-Base Titrations

Edta Titrations

Advanced Topics in Equilibrium

Electrodes and Potentiometry

Redox Titrations

Electroanalytical Techniques

Fundamentals of Spectrophotometry

Applications of Spectrophotometry

Spectrophotometers

Atomic Spectroscopy

Mass Spectrometry

Introduction to Analytical Separations

Gas Chromatography

High-Performance Liquid Chromatography

Chromatographic Methods and Capillary Electrophoresis

Gravimetric and Combustion Analysis

Sample Preparation

Filters

For the cell diagram below write out and balance the reaction that occurs in the cell. Pt|HOCl (aq,1 M),HClO₂ (aq,1 M),H⁺ (aq,1 M)|| (aq,1 M),H⁺ (aq,1 M)| MnO₂ (s)|Pt

E^o is defined as:

For the line notation below,which is NOT true? Fe(s)| Fe²⁺ (aq,A = 1)|| Cu²⁺ (aq,A = 1)| Cu (s)

For the reaction below,the oxidizing agent is and it electrons,and the reducing agent is and it electrons. 8 H⁺ + + 5 Cu⁺ ⇋ Mn²⁺ + 5 Cu²⁺ + 4 H₂O

Calculate E^° for the half-cell below. O₂ + 4 H⁺ + 4 e⁻ ⇋ 2 H₂O E° = 1.229 V

Calculate the standard potential when the two half-cells below are connected via a salt bridge and potentiometer.Which species are the reducing agent and oxidizing agent? + 2 H⁺ + 2 e^- ⇋ + H₂O E° = 1.589 V Mg(OH)₂ (s)+ 2 e^- ⇋ Mg (s)+ 2 OH^- E° = -2.690 V

Which is NOT correct for when the silver and vanadium half-cells are connected via a salt bridge and a potentiometer? Ag⁺ + 1 e^- → Ag (s)E° = 0.7993 V V²⁺ + 2 e^- → V (s)E° = −1.125 V I Ag⁺ is reduced. II V is oxidized. III E^o_cell = 1.924 V IV V²⁺ is reduced. V Ag is oxidized.

Calculate the equilibrium constant for the reaction between Sn metal and Zn²⁺ solution. Sn + Zn²⁺ ⇋ Sn²⁺ + Zn Sn²⁺ + 2 e⁻ → Sn (s)E° = −0.141 V Zn²⁺ + 2 e⁻ → Zn (s)E° = −0.762 V

A bromide probe is constructed from a saturated silver bromide half-cell and a Ni²⁺/Ni half-cell.If the measured potential is 0.952 V and [Ni²⁺] = 1 M,what is the bromide concentration? AgBr (s)+ e⁻ ⇋ Ag(s)+ Br⁻ E^° = 0.071 V Ni²⁺ + 2 e⁻ ⇋ Ni (s)E^° = −0.714 V

Calculate the potential for the half-cell below for [ ] = 0.100 M,[ ] = 0.500 M and the pH = 10.50. 2 + 3 H₂O + 4 e⁻ ⇋ + 6 OH^- E° = −0.566 V

Calculate E^o and K for the cell composed of a bromate/bromide half-cell and a chlorate/chlorine dioxide half-cell. + 2 H⁺ + e⁻ ⇋ ClO₂ + H₂O E° = 1.130 V + 3 H₂O + 6 e⁻ ⇋ Br⁻ + 6 OH⁻ E° = 0.613 V

The half-cells below are connected via a salt-bridge and potentiometer.What is the voltage read by the potentiometer when A_Ag⁺ = 2.00 and A_V²⁺ = 1.50? Ag⁺ + 1 e⁻ → Ag (s)E^o = 0.7993 V V²⁺ + 2 e⁻ → V (s)E^o = −1.125 V

For the silver half-reaction,Ag⁺ + 1 e^- → Ag (s),when the concentration of silver cation is increased,the reduction potential: