Question 1

Based on the balanced chemical equation shown below,determine the mass percent of Fe3+ in a  sample of iron ore,if 22.40 mL of a 0.1000 M stannous chloride,SnCl2(aq),solution is required to completely react with the Fe3+ present in the ore sample.The chemical equation for the reaction is: 2 Fe3+(aq)+ Sn2+(aq)→ 2 Fe2+(aq)+ Sn4+(aq).

Accepted Answer

A) 8.982% 
B) 14.06% 
C) 28.11% 
D) 56.22%

Question 2

A galvanic cell consists of one half-cell that contains Ag(s)and Ag+(aq),and one half-cell that contains Pb(s)and Pb2+(aq).What species are produced at the electrodes under standard conditions? Ag+(aq)+ e- → Ag(s)E° = +0.80 V
Pb2+(aq)+ 2 e- → Pb(s)E° = -0.13 V

Accepted Answer

A) Ag(aq)is formed at the cathode and,Pb(s)is formed at the anode. 
B) Ag(s)is formed at the cathode,and Pb2+(aq)is formed at the anode. 
C) Pb(s)is formed at the cathode,and Ag+(aq)is formed at the anode. 
D) Pb2+(aq)is formed at the cathode,and Cu(s)is formed at the anode.

Question 3

In the shorthand notation for a galvanic cell,a double vertical line (∣∣)represents

Accepted Answer

A) a single phase boundary 
B) a cathode 
C) a gas 
D) a salt bridge

Question 4

-The cell reaction 2 Fe3+(aq)+ Zn(s)→ Zn2+(aq)+ 2 Fe2+(aq)occurs in the galvanic cell shown above.Where should the Fe3+(aq)and Fe2+(aq)be found?

Accepted Answer

A) Half-cell (
A) contains Fe3+(aq)and half-cell (
B) contains Fe2+(aq). 
B) Half-cell (
A) contains Fe2+(aq)and half-cell (
B) contains Fe3+(aq). 
C) Half-cell (
A) contains Fe3+(aq)and Fe2+(aq). 
D) Half-cell (
B) contains Fe3+(aq)and Fe2+(aq).

Question 5

What is the shorthand notation that represents the following galvanic cell reaction? Fe(s)+ Cu(NO3)2(aq)→ Fe(NO3)2(aq)+ Cu(s)

Accepted Answer

A) Fe(s)∣ Fe2+(aq)∣∣ Cu2+(aq)∣ Cu(s) 
B) Cu(s)∣ Cu2+(aq)∣∣ Fe2+(aq)∣ Fe(s) 
C) Fe(s)∣ NO3-(aq)∣∣ NO3-(aq)∣ Cu(s) 
D) Cu(s)∣ Cu(NO3)2(aq)∣∣ Fe(NO3)2(aq)∣ Fe(s)

Question 6

Given   and  calculate E at 25°C for a cell based on the reaction:

Accepted Answer

A) -0.09 V 
B) +0.12 V 
C) +0.15 V 
D) +0.30 V

Question 7

Identify the anode and cathode half-reactions and categorize each as either oxidation or reduction.

Accepted Answer

A) Anode reaction: Ag+(aq)+ e- → Ag(s)(oxidation)
Cathode reaction: Cu(s)→ Cu2+(aq)+ 2e- (reduction) 
B) Anode reaction: Ag+(aq)+ e- → Ag(s)(reduction)
Cathode reaction: Cu(s)→ Cu2+(aq)+ 2e- (oxidation) 
C) Anode reaction: Cu(s)→ Cu2+(aq)+ 2e- (oxidation)
Cathode reaction: Ag+(aq)+ e- → Ag(s)(reduction) 
D) Anode reaction: Cu(s)→ Cu2+(aq)+ 2e- (reduction)
Cathode reaction: Ag+(aq)+ e- → Ag(s)(oxidation)

Question 8

According to the balanced equation shown below,1.00 mole of oxalic acid,H2C2O4,reacts with ________ moles of permanganate ion,MnO4-. 5 H2C2O4(aq)+ 2 MnO4-(aq)+ 6 H+(aq)→ 10 CO2(g)+ 2 Mn2+(aq)+ 8 H2O(l)

Accepted Answer

A) 0.400 
B) 1.00 
C) 2.00 
D) 2.25

Question 9

The standard cell potential for the following galvanic cell is 0.71 V. Pb(s)|Pb²⁺(aq)||Al³⁺(aq)|Al This reaction has an equilibrium constant,K = ________.

Accepted Answer

The answer of The standard cell potential for the following...

Question 10

For the reaction 2 Al(s)+ 3 Co2+(aq)→ 2 Al3+(aq)+ 3 Co(s),ΔG° is -799 kJ.What is E° for a standard cell based on this reaction?

Accepted Answer

A) +1.38 V 
B) +2.76 V 
C) +4.14 V 
D) +8.28 V

Question 11

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 80.0 minutes?

Accepted Answer

A) 14.7 g 
B) 21.9 g 
C) 43.8 g 
D) 48.4 g

Question 12

Based on the balanced chemical equation shown below,what volume of 0.250 M K2S2O3(aq),is needed to completely react with 12.44 mL of 0.125 M KI3(aq)? 2 S2O32-(aq)+ I3-(aq)→ S4O62-(aq)+ 3 I-(aq)

Accepted Answer

A) 3.11 mL 
B) 6.22 mL 
C) 12.4 mL 
D) 49.8 mL

Question 13

Given that Br2(g)+ 2 e- → 2 Br-(aq)is the reduction half-reaction for the overall reaction  what is the oxidation half reaction?

Accepted Answer

A) Ag(s)→ Ag+(aq)+ e- 
B) Ag(s)+ Br-(aq)→ AgBr(s)+ e- 
C) Ag(s)+ Br2(g)+ e- → AgBr(s)+ Br-(aq) 
D) 2 Br-(aq)→ Br2(g)+ 2 e-

Question 14

Doubling all the coefficients in the equation for the cell reaction

Accepted Answer

A) doubles both E° and ΔG°. 
B) doubles E°,but does not change ΔG°. 
C) doubles ΔG°,but does not change E°. 
D) does not change E° or ΔG°.

Question 15

For a particular cell based on the reaction: 3 AgCl(s)+ Al(s)→ 3 Ag(s)+ Al3+(aq)+ 3 Cl-(aq)
E = +1.750 V and E° = +1.884 V at 25°C.
What is the value of the equilibrium constant,K,at 25°C for the reaction?

Accepted Answer

A) 3.6 × 1029 
B) 6.7 × 1031 
C) 4.8 × 1088 
D) 3.0 × 1095

Question 16

Shown below are the reactions occurring in the direct methanol fuel cell (DMFC). I.2 CH3OH(aq)+ 2 H2O(l)→ 2 CO2(g)+12 H+(aq)+12 e-
II.3 O2(g)+ 12 H+(aq)+ 12 e- → 6 H2O(l)
Overall 2 CH3OH(aq)+ 3 O2(g)→ 2 CO2(g)+ 4 H2O(l)
Which is the anode reaction,and what is being oxidized in the overall reaction?

Accepted Answer

A) I,CH3OH 
B) I,H2O 
C) II,O2 
D) II,H+

Question 17

The nickel-cadmium battery cell has a standard potential of +1.20 V.The cell reaction is 2 NiO(OH)(s)+ Cd(s)+ 2 H2O(l)→ 2 Ni(OH)2(s)+ Cd(OH)2(s).
What is the standard free energy change for this reaction?

Accepted Answer

A) -38.7 kJ 
B) -116 kJ 
C) -232 kJ 
D) -463 kJ

Question 18

Calculate the value of the reaction quotient,Q,for the galvanic cell expressed using shorthand notation below.Use the balanced chemical equation that has the smallest whole number stoichiometric coefficients. Zn(s)∣ Zn2+(aq,0.0100 M)∣∣ Ag+(aq,1.10 M)∣ Ag(s)

Accepted Answer

A) 121 
B) 110 
C) 9.09 × 10-3 
D) 8.26 × 10-3

Question 19

What are the coefficients in front of IO3-(aq)and I-(aq)when the following equation is balanced in an acidic solution? ________ IO3-(aq)+ ________ I-(aq)→ ________ I2(aq)

Accepted Answer

A) 1,3 
B) 1,5 
C) 2,3 
D) 2,5

Question 20

When the equation MnO₄^-(aq)+ C₂O₄^2-(aq)→ Mn²⁺(aq)+ CO₂(g)is balanced in acidic solution using the smallest whole numbers,the coefficient in front of the CO₂(g)is ________.

Accepted Answer

The answer of When the equation MnO₄^-(aq)+ C₂O₄^2-(aq)→ Mn²⁺(aq)+ CO₂(g)is...

Exam 18: Electrochemistry

A galvanic cell consists of one half-cell that contains Ag(s) and Ag⁺(aq) ,and one half-cell that contains Pb(s) and Pb²⁺(aq) .What species are produced at the electrodes under standard conditions? Ag⁺(aq) + e^- → Ag(s) E° = +0.80 V Pb²⁺(aq) + 2 e^- → Pb(s) E° = -0.13 V

In the shorthand notation for a galvanic cell,a double vertical line (∣∣) represents

-The cell reaction 2 Fe³⁺(aq) + Zn(s) → Zn²⁺(aq) + 2 Fe²⁺(aq) occurs in the galvanic cell shown above.Where should the Fe³⁺(aq) and Fe²⁺(aq) be found?

What is the shorthand notation that represents the following galvanic cell reaction? Fe(s) + Cu(NO₃) ₂(aq) → Fe(NO₃) ₂(aq) + Cu(s)

Given and calculate E at 25°C for a cell based on the reaction:

Identify the anode and cathode half-reactions and categorize each as either oxidation or reduction.

According to the balanced equation shown below,1.00 mole of oxalic acid,H₂C₂O₄,reacts with ________ moles of permanganate ion,MnO₄^-. 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l)

The standard cell potential for the following galvanic cell is 0.71 V. Pb(s)|Pb²⁺(aq)||Al³⁺(aq)|Al This reaction has an equilibrium constant,K = ________.

For the reaction 2 Al(s) + 3 Co²⁺(aq) → 2 Al³⁺(aq) + 3 Co(s) ,ΔG° is -799 kJ.What is E° for a standard cell based on this reaction?

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 80.0 minutes?

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃(aq) ,is needed to completely react with 12.44 mL of 0.125 M KI₃(aq) ? 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)

Given that Br₂(g) + 2 e^- → 2 Br^-(aq) is the reduction half-reaction for the overall reaction what is the oxidation half reaction?

Doubling all the coefficients in the equation for the cell reaction

For a particular cell based on the reaction: 3 AgCl(s) + Al(s) → 3 Ag(s) + Al³⁺(aq) + 3 Cl^-(aq) E = +1.750 V and E° = +1.884 V at 25°C. What is the value of the equilibrium constant,K,at 25°C for the reaction?

The nickel-cadmium battery cell has a standard potential of +1.20 V.The cell reaction is 2 NiO(OH) (s) + Cd(s) + 2 H₂O(l) → 2 Ni(OH) ₂(s) + Cd(OH) ₂(s) . What is the standard free energy change for this reaction?

Calculate the value of the reaction quotient,Q,for the galvanic cell expressed using shorthand notation below.Use the balanced chemical equation that has the smallest whole number stoichiometric coefficients. Zn(s) ∣ Zn²⁺(aq,0.0100 M) ∣∣ Ag⁺(aq,1.10 M) ∣ Ag(s)

What are the coefficients in front of IO₃^-(aq) and I^-(aq) when the following equation is balanced in an acidic solution? IO₃^-(aq) + I^-(aq) → I₂(aq)

When the equation MnO₄^-(aq)+ C₂O₄^2-(aq)→ Mn²⁺(aq)+ CO₂(g)is balanced in acidic solution using the smallest whole numbers,the coefficient in front of the CO₂(g)is ________.

Exam 18: Electrochemistry

A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq) ,and one half-cell that contains Pb(s) and Pb2+(aq) .What species are produced at the electrodes under standard conditions? Ag+(aq) + e- → Ag(s) E° = +0.80 V Pb2+(aq) + 2 e- → Pb(s) E° = -0.13 V

In the shorthand notation for a galvanic cell,a double vertical line (∣∣) represents

-The cell reaction 2 Fe3+(aq) + Zn(s) → Zn2+(aq) + 2 Fe2+(aq) occurs in the galvanic cell shown above.Where should the Fe3+(aq) and Fe2+(aq) be found?

What is the shorthand notation that represents the following galvanic cell reaction? Fe(s) + Cu(NO3) 2(aq) → Fe(NO3) 2(aq) + Cu(s)

Given and calculate E at 25°C for a cell based on the reaction:

Identify the anode and cathode half-reactions and categorize each as either oxidation or reduction.

According to the balanced equation shown below,1.00 mole of oxalic acid,H2C2O4,reacts with ________ moles of permanganate ion,MnO4-. 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l)

The standard cell potential for the following galvanic cell is 0.71 V. Pb(s)|Pb2+(aq)||Al3+(aq)|Al This reaction has an equilibrium constant,K = ________.

For the reaction 2 Al(s) + 3 Co2+(aq) → 2 Al3+(aq) + 3 Co(s) ,ΔG° is -799 kJ.What is E° for a standard cell based on this reaction?

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 80.0 minutes?

Based on the balanced chemical equation shown below,what volume of 0.250 M K2S2O3(aq) ,is needed to completely react with 12.44 mL of 0.125 M KI3(aq) ? 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq)

Given that Br2(g) + 2 e- → 2 Br-(aq) is the reduction half-reaction for the overall reaction what is the oxidation half reaction?

Doubling all the coefficients in the equation for the cell reaction

For a particular cell based on the reaction: 3 AgCl(s) + Al(s) → 3 Ag(s) + Al3+(aq) + 3 Cl-(aq) E = +1.750 V and E° = +1.884 V at 25°C. What is the value of the equilibrium constant,K,at 25°C for the reaction?

The nickel-cadmium battery cell has a standard potential of +1.20 V.The cell reaction is 2 NiO(OH) (s) + Cd(s) + 2 H2O(l) → 2 Ni(OH) 2(s) + Cd(OH) 2(s) . What is the standard free energy change for this reaction?

Calculate the value of the reaction quotient,Q,for the galvanic cell expressed using shorthand notation below.Use the balanced chemical equation that has the smallest whole number stoichiometric coefficients. Zn(s) ∣ Zn2+(aq,0.0100 M) ∣∣ Ag+(aq,1.10 M) ∣ Ag(s)

What are the coefficients in front of IO3-(aq) and I-(aq) when the following equation is balanced in an acidic solution? ________ IO3-(aq) + ________ I-(aq) → ________ I2(aq)

When the equation MnO4-(aq)+ C2O42-(aq)→ Mn2+(aq)+ CO2(g)is balanced in acidic solution using the smallest whole numbers,the coefficient in front of the CO2(g)is ________.

A galvanic cell consists of one half-cell that contains Ag(s) and Ag⁺(aq) ,and one half-cell that contains Pb(s) and Pb²⁺(aq) .What species are produced at the electrodes under standard conditions? Ag⁺(aq) + e^- → Ag(s) E° = +0.80 V Pb²⁺(aq) + 2 e^- → Pb(s) E° = -0.13 V

-The cell reaction 2 Fe³⁺(aq) + Zn(s) → Zn²⁺(aq) + 2 Fe²⁺(aq) occurs in the galvanic cell shown above.Where should the Fe³⁺(aq) and Fe²⁺(aq) be found?

What is the shorthand notation that represents the following galvanic cell reaction? Fe(s) + Cu(NO₃) ₂(aq) → Fe(NO₃) ₂(aq) + Cu(s)

According to the balanced equation shown below,1.00 mole of oxalic acid,H₂C₂O₄,reacts with ________ moles of permanganate ion,MnO₄^-. 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l)

The standard cell potential for the following galvanic cell is 0.71 V. Pb(s)|Pb²⁺(aq)||Al³⁺(aq)|Al This reaction has an equilibrium constant,K = ________.

For the reaction 2 Al(s) + 3 Co²⁺(aq) → 2 Al³⁺(aq) + 3 Co(s) ,ΔG° is -799 kJ.What is E° for a standard cell based on this reaction?

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 80.0 minutes?

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃(aq) ,is needed to completely react with 12.44 mL of 0.125 M KI₃(aq) ? 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)

Given that Br₂(g) + 2 e^- → 2 Br^-(aq) is the reduction half-reaction for the overall reaction what is the oxidation half reaction?

For a particular cell based on the reaction: 3 AgCl(s) + Al(s) → 3 Ag(s) + Al³⁺(aq) + 3 Cl^-(aq) E = +1.750 V and E° = +1.884 V at 25°C. What is the value of the equilibrium constant,K,at 25°C for the reaction?

The nickel-cadmium battery cell has a standard potential of +1.20 V.The cell reaction is 2 NiO(OH) (s) + Cd(s) + 2 H₂O(l) → 2 Ni(OH) ₂(s) + Cd(OH) ₂(s) . What is the standard free energy change for this reaction?

Calculate the value of the reaction quotient,Q,for the galvanic cell expressed using shorthand notation below.Use the balanced chemical equation that has the smallest whole number stoichiometric coefficients. Zn(s) ∣ Zn²⁺(aq,0.0100 M) ∣∣ Ag⁺(aq,1.10 M) ∣ Ag(s)

What are the coefficients in front of IO₃^-(aq) and I^-(aq) when the following equation is balanced in an acidic solution? IO₃^-(aq) + I^-(aq) → I₂(aq)

When the equation MnO₄^-(aq)+ C₂O₄^2-(aq)→ Mn²⁺(aq)+ CO₂(g)is balanced in acidic solution using the smallest whole numbers,the coefficient in front of the CO₂(g)is ________.