Consider an electrochemical cell involving the overall reaction 2AgBr(s) + Pb(s) $\rarr$ Pb2+ + 2Ag(s) + 2Br-.Each half-reaction is carried out in a separate compartment. The anion included in the lead half-cell is NO3-. The cation in the silver half-cell is K+. The two half-cells are connected by a KNO3 salt bridge. If [Pb2+] = 1.0 M, what concentration of Br- ion will produce a cell emf of 0.25 V at 298 K Given: AgBr(s) + e- $\rarr$ Ag + Br-, E$\circ$ = +0.07 V.

A) 0.02 M B) 0.14 M C) 0.38 M D) 1.0 M E) 7.0 M A) 0.02 M B) 0.14 M C) 0.38 M D) 1.0 M E) 7.0 M

For the electrochemical cell Ni(s) | Ni2+(1 M) || H+(1 M) | H2(1 atm) | Pt(s), which one of the following changes will cause a decrease in the cell voltage

A) Increase the pressure of H2 to 2.0 atm. B) Decrease the mass of the nickel electrode. C) Lower the pH of the cell electrolyte. D) Decrease the concentration of Ni2+ ion. E) None of the above. A) Increase the pressure of H2 to 2.0 atm. B) Decrease the mass of the nickel electrode. C) Lower the pH of the cell electrolyte. D) Decrease the concentration of Ni2+ ion. E) None of the above.

An electrochemical cell based on the following reaction has a standard cell voltage (E$\circ$cell) of 0.48 V: Sn(s) + Cu2+(aq) $\rarr$ Sn2+(aq) + Cu(s) What is the standard reduction potential of tin(II) (E$\circ$(Cu2+/Cu) = 0.34 V)

A) -0.14 V B) 0.14 V C) -0.82 V D) 0.82 V E) none of these A) -0.14 V B) 0.14 V C) -0.82 V D) 0.82 V E) none of these

Determine the equilibrium constant, Keq, at 25$\circ$C for the reaction 2Br- (aq) + I2(s) $\leftrightharpoons$ Br2(l) + 2I- (aq).

A) 5.7 * 10-19 B) 18.30 C) 1.7 * 1054 D) 1.9 * 1018 E) 5.7 * 10-55 A) 5.7 * 10-19 B) 18.30 C) 1.7 * 1054 D) 1.9 * 1018 E) 5.7 * 10-55

When an aqueous solution of AgNO3 is electrolyzed, a gas is observed to form at the anode. The gas is

A) H2. B) O2. C) NO. D) NO2. A) H2. B) O2. C) NO. D) NO2.

Calculate the standard cell emf for the following cell: Mg | Mg2+ || NO3- (acid soln)| NO(g) | Pt

A) 3.33 V B) 1.41 V C) -1.41 V D) 8.46 V E) -8.46 V A) 3.33 V B) 1.41 V C) -1.41 V D) 8.46 V E) -8.46 V

Calculate $\Delta$G$\circ$ for the electrochemical cell Pb(s) | Pb2+(aq) || Fe3+(aq) | Fe2+(aq) | Pt(s).

A) -1.2 x 102 kJ/mol B) -1.7 x 102 kJ/mol C) 1.7 x 102 kJ/mol D) -8.7 x 101 kJ/mol E) -3.2 x 105 kJ/mol A) -1.2 x 102 kJ/mol B) -1.7 x 102 kJ/mol C) 1.7 x 102 kJ/mol D) -8.7 x 101 kJ/mol E) -3.2 x 105 kJ/mol

How long will it take to produce 78 g of Al metal by the reduction of Al3+ in an electrolytic cell with a current of 2.0 A

A) 0.01 s B) 420 s C) 13 h D) 116 h E) 1.0 * 1012 s A) 0.01 s B) 420 s C) 13 h D) 116 h E) 1.0 * 1012 s

A galvanic cell has the overall reaction: 2Fe(NO3)2(aq) + Pb(NO3)2(aq) $\rarr$ 2Fe(NO3)3(aq) + Pb(s) Which is the half reaction occurring at the cathode

A) NO3-(aq) + 4H+(aq) + 3e- $\rarr$ NO(g) + 2H2O(l) B) NO3-(aq) + 2H+(aq) + e- $\rarr$ NO2(g) + H2O(l) C) Fe2+(aq) $\rarr$ Fe3+(aq) + e- D) Pb2+(aq) + 2e- $\rarr$ Pb(s) E) Fe2+(aq) + e- $\rarr$ Fe3+(aq) A) NO3-(aq) + 4H+(aq) + 3e- $\rarr$ NO(g) + 2H2O(l) B) NO3-(aq) + 2H+(aq) + e- $\rarr$ NO2(g) + H2O(l) C) Fe2+(aq) $\rarr$ Fe3+(aq) + e- D) Pb2+(aq) + 2e- $\rarr$ Pb(s) E) Fe2+(aq) + e- $\rarr$ Fe3+(aq)

Write the formula of the weakest reducing agent given the following standard reduction potentials in acid solution: $\begin{array}{ll} \mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightarrow 2 \mathrm{H}_{2} \mathrm{O} & \mathrm{E}^{\circ}=+1.23 \mathrm{~V} \\ \mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}^{2+} & \mathrm{E}^{\circ}=+0.13 \mathrm{~V} \\ \mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(\mathrm{~s}) & \mathrm{E}^{\circ}=-0.76 \mathrm{~V} \end{array}$

A) Zn(s) B) Sn2+ C) O2 D) H2O E) None of the above A) Zn(s) B) Sn2+ C) O2 D) H2O E) None of the above

Given the following standard reduction potentials, $\begin{array}{ll} \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(\mathrm{s}) & \mathrm{E}^{0}=0.80 \mathrm{~V} \\ \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(\mathrm{aq})+\mathrm{e}^{-} \rightarrow \mathrm{Ag}(\mathrm{s})+2 \mathrm{NH}_{3}(\mathrm{aq}) & \mathrm{E}^{\circ}=0.04 \mathrm{V} \end{array}$ calculate the formation constant of Ag(NH3)2+ at 25$\circ$C.

A) 6.1 * 10-15 B) 1.5 * 10-13 C) 6.9 * 1012 D) 1.6 * 1014 E) None of these A) 6.1 * 10-15 B) 1.5 * 10-13 C) 6.9 * 1012 D) 1.6 * 1014 E) None of these

Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s) What is the balanced overall (net) cell reaction

A) 2H+(aq) + 2Ag+(aq) $\rarr$ H2(g) + 2Ag(s) B) H2(g) + 2Ag(s) $\rarr$ H+(aq) + 2Ag+(aq) C) 2H+(aq) + 2Ag(s) $\rarr$ H2(g) + 2Ag+(aq) D) H2(g) + Ag+(aq) $\rarr$ H+(aq) + Ag(s) E) H2(g) + 2Ag+(aq) $\rarr$ 2H+(aq) + 2Ag(s) A) 2H+(aq) + 2Ag+(aq) $\rarr$ H2(g) + 2Ag(s) B) H2(g) + 2Ag(s) $\rarr$ H+(aq) + 2Ag+(aq) C) 2H+(aq) + 2Ag(s) $\rarr$ H2(g) + 2Ag+(aq) D) H2(g) + Ag+(aq) $\rarr$ H+(aq) + Ag(s) E) H2(g) + 2Ag+(aq) $\rarr$ 2H+(aq) + 2Ag(s)

Exam 18: Electrochemistry

Consider an electrochemical cell involving the overall reaction 2AgBr(s) + Pb(s) $\rarr$ Pb²⁺ + 2Ag(s) + 2Br^-.Each half-reaction is carried out in a separate compartment. The anion included in the lead half-cell is NO₃^-. The cation in the silver half-cell is K⁺. The two half-cells are connected by a KNO₃ salt bridge. If [Pb²⁺] = 1.0 M, what concentration of Br^- ion will produce a cell emf of 0.25 V at 298 K Given: AgBr(s) + e^- $\rarr$ Ag + Br^-, E^$\circ$ = +0.07 V.

(Multiple Choice)

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Question 61

For the electrochemical cell Ni(s) | Ni²⁺(1 M) || H⁺(1 M) | H₂(1 atm) | Pt(s), which one of the following changes will cause a decrease in the cell voltage

(Multiple Choice)

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Question 62

An electrochemical cell based on the following reaction has a standard cell voltage (E^$\circ$_cell) of 0.48 V: Sn(s) + Cu²⁺(aq) $\rarr$ Sn²⁺(aq) + Cu(s) What is the standard reduction potential of tin(II) (E^$\circ$(Cu²⁺/Cu) = 0.34 V)

(Multiple Choice)

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Question 63

Determine the equilibrium constant, K_eq, at 25^$\circ$C for the reaction 2Br^- (aq) + I₂(s) $\leftrightharpoons$ Br₂(l) + 2I^- (aq).

(Multiple Choice)

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Question 64

When an aqueous solution of AgNO₃ is electrolyzed, a gas is observed to form at the anode. The gas is

(Multiple Choice)

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Question 65

Which of these metals will not be oxidized in hydrochloric acid under standard conditions at 25^$\circ$C

(Multiple Choice)

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Question 66

Calculate the value of E^$\circ$_cell for the following reaction: 2Au(s) + 3Ca²⁺(aq) $\rarr$ 2Au³⁺(aq) + 3Ca(s)

(Multiple Choice)

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Question 67

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO₄(aq) and Pb(NO₃)₂ (aq) solutions, respectively. If sulfuric acid is then added to the Pb(NO₃)₂ solution, thereby forming a precipitate of PbSO₄, the cell potential will decrease.

(True/False)

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Question 68

For the electrochemical cell, Fe(s) | Fe²⁺(aq) || Cu²⁺(aq) | Cu⁺(aq) | Pt(s), determine the equilibrium constant (K_eq) at 25^$\circ$C for the reaction that occurs.

(Multiple Choice)

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Question 69

Calculate the standard cell emf for the following cell: Mg | Mg²⁺ || NO₃^- (acid soln)| NO(g) | Pt

(Multiple Choice)

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Question 70

Which one of the following reactions must be carried out in an electrolytic cell rather than in a galvanic cell

(Multiple Choice)

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Question 71

Calculate $\Delta$ G^$\circ$ for the electrochemical cell Pb(s) | Pb²⁺(aq) || Fe³⁺(aq) | Fe²⁺(aq) | Pt(s).

(Multiple Choice)

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Question 72

How long will it take to produce 78 g of Al metal by the reduction of Al³⁺ in an electrolytic cell with a current of 2.0 A

(Multiple Choice)

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Question 73

A galvanic cell has the overall reaction: 2Fe(NO₃)₂(aq) + Pb(NO₃)₂(aq) $\rarr$ 2Fe(NO₃)₃(aq) + Pb(s) Which is the half reaction occurring at the cathode

(Multiple Choice)

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Question 74

Write the formula of the weakest reducing agent given the following standard reduction potentials in acid solution: +4+4\rightarrow2 =+1.23 +2\rightarrow =+0.13 +2\rightarrow() =-0.76

(Multiple Choice)

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Question 75

Under acidic conditions the correctly balanced redox reaction for MnO₄^-(aq) + C₂O₄^2-(aq) $\rarr$ Mn²⁺(aq) + CO₂(aq) is: 2MnO₄^-(aq) + 5C₂O₄^2-(aq) + 8H⁺(aq) $\rarr$ 2Mn²⁺(aq) + 10CO₂(aq) + 8H₂O(l)

(True/False)

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Question 76

How many coulombs (C) of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca²⁺ ion to calcium metal

(Multiple Choice)

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Question 77

Given the following standard reduction potentials, ()+\rightarrow() =0.80 ()+\rightarrow()+2() =0.04 calculate the formation constant of Ag(NH₃)₂⁺ at 25^$\circ$C.

(Multiple Choice)

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Question 78

Given the following notation for an electrochemical cell Pt(s) | H₂(g) | H⁺(aq) || Ag⁺(aq) | Ag(s) What is the balanced overall (net) cell reaction

(Multiple Choice)

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Question 79

Gold can be electrochemically "plated" onto a less expensive metal by submerging the object in a solution of gold(III) and applying an electric current to drive the following half-reaction: Au³⁺ + 3e^- $\rarr$ Au(s) How many grams of gold will be formed if a current of 2.37 A is applied for 71 minutes

(Multiple Choice)

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Question 80

Showing 61 - 80 of 154

Exam 18: Electrochemistry

For the electrochemical cell Ni(s) | Ni2+(1 M) || H+(1 M) | H2(1 atm) | Pt(s), which one of the following changes will cause a decrease in the cell voltage

An electrochemical cell based on the following reaction has a standard cell voltage (E ∘\circ∘ cell) of 0.48 V: Sn(s) + Cu2+(aq) →\rarr→ Sn2+(aq) + Cu(s) What is the standard reduction potential of tin(II) (E ∘\circ∘ (Cu2+/Cu) = 0.34 V)

Determine the equilibrium constant, Keq, at 25 ∘\circ∘ C for the reaction 2Br- (aq) + I2(s) ⇋\leftrightharpoons⇋ Br2(l) + 2I- (aq).

When an aqueous solution of AgNO3 is electrolyzed, a gas is observed to form at the anode. The gas is

Which of these metals will not be oxidized in hydrochloric acid under standard conditions at 25 ∘\circ∘ C

Calculate the value of E ∘\circ∘ cell for the following reaction: 2Au(s) + 3Ca2+(aq) →\rarr→ 2Au3+(aq) + 3Ca(s)

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO4(aq) and Pb(NO3)2 (aq) solutions, respectively. If sulfuric acid is then added to the Pb(NO3)2 solution, thereby forming a precipitate of PbSO4, the cell potential will decrease.

For the electrochemical cell, Fe(s) | Fe2+(aq) || Cu2+(aq) | Cu+(aq) | Pt(s), determine the equilibrium constant (Keq) at 25 ∘\circ∘ C for the reaction that occurs.

Calculate the standard cell emf for the following cell: Mg | Mg2+ || NO3- (acid soln)| NO(g) | Pt

Which one of the following reactions must be carried out in an electrolytic cell rather than in a galvanic cell

Calculate Δ\DeltaΔ G ∘\circ∘ for the electrochemical cell Pb(s) | Pb2+(aq) || Fe3+(aq) | Fe2+(aq) | Pt(s).

How long will it take to produce 78 g of Al metal by the reduction of Al3+ in an electrolytic cell with a current of 2.0 A

A galvanic cell has the overall reaction: 2Fe(NO3)2(aq) + Pb(NO3)2(aq) →\rarr→ 2Fe(NO3)3(aq) + Pb(s) Which is the half reaction occurring at the cathode

Write the formula of the weakest reducing agent given the following standard reduction potentials in acid solution: +4+4\rightarrow2 =+1.23 +2\rightarrow =+0.13 +2\rightarrow() =-0.76

Under acidic conditions the correctly balanced redox reaction for MnO4-(aq) + C2O42-(aq) →\rarr→ Mn2+(aq) + CO2(aq) is: 2MnO4-(aq) + 5C2O42-(aq) + 8H+(aq) →\rarr→ 2Mn2+(aq) + 10CO2(aq) + 8H2O(l)

How many coulombs (C) of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca2+ ion to calcium metal

Given the following standard reduction potentials, ()+\rightarrow() =0.80 ()+\rightarrow()+2() =0.04 calculate the formation constant of Ag(NH3)2+ at 25 ∘\circ∘ C.

Given the following notation for an electrochemical cell Pt(s) | H2(g) | H+(aq) || Ag+(aq) | Ag(s) What is the balanced overall (net) cell reaction

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For the electrochemical cell Ni(s) | Ni²⁺(1 M) || H⁺(1 M) | H₂(1 atm) | Pt(s), which one of the following changes will cause a decrease in the cell voltage

An electrochemical cell based on the following reaction has a standard cell voltage (E^$\circ$_cell) of 0.48 V: Sn(s) + Cu²⁺(aq) $\rarr$ Sn²⁺(aq) + Cu(s) What is the standard reduction potential of tin(II) (E^$\circ$(Cu²⁺/Cu) = 0.34 V)

Determine the equilibrium constant, K_eq, at 25^$\circ$C for the reaction 2Br^- (aq) + I₂(s) $\leftrightharpoons$ Br₂(l) + 2I^- (aq).

When an aqueous solution of AgNO₃ is electrolyzed, a gas is observed to form at the anode. The gas is

Which of these metals will not be oxidized in hydrochloric acid under standard conditions at 25^$\circ$C

Calculate the value of E^$\circ$_cell for the following reaction: 2Au(s) + 3Ca²⁺(aq) $\rarr$ 2Au³⁺(aq) + 3Ca(s)

A battery is constructed by placing copper and lead electrodes in contact with 1.0 molar CuSO₄(aq) and Pb(NO₃)₂ (aq) solutions, respectively. If sulfuric acid is then added to the Pb(NO₃)₂ solution, thereby forming a precipitate of PbSO₄, the cell potential will decrease.

For the electrochemical cell, Fe(s) | Fe²⁺(aq) || Cu²⁺(aq) | Cu⁺(aq) | Pt(s), determine the equilibrium constant (K_eq) at 25^$\circ$C for the reaction that occurs.

Calculate the standard cell emf for the following cell: Mg | Mg²⁺ || NO₃^- (acid soln)| NO(g) | Pt

Calculate $\Delta$ G^$\circ$ for the electrochemical cell Pb(s) | Pb²⁺(aq) || Fe³⁺(aq) | Fe²⁺(aq) | Pt(s).

How long will it take to produce 78 g of Al metal by the reduction of Al³⁺ in an electrolytic cell with a current of 2.0 A

A galvanic cell has the overall reaction: 2Fe(NO₃)₂(aq) + Pb(NO₃)₂(aq) $\rarr$ 2Fe(NO₃)₃(aq) + Pb(s) Which is the half reaction occurring at the cathode

Under acidic conditions the correctly balanced redox reaction for MnO₄^-(aq) + C₂O₄^2-(aq) $\rarr$ Mn²⁺(aq) + CO₂(aq) is: 2MnO₄^-(aq) + 5C₂O₄^2-(aq) + 8H⁺(aq) $\rarr$ 2Mn²⁺(aq) + 10CO₂(aq) + 8H₂O(l)

How many coulombs (C) of electrical charge must pass through an electrolytic cell to reduce 0.44 mol Ca²⁺ ion to calcium metal

Given the following standard reduction potentials, ()+\rightarrow() =0.80 ()+\rightarrow()+2() =0.04 calculate the formation constant of Ag(NH₃)₂⁺ at 25^$\circ$C.

Given the following notation for an electrochemical cell Pt(s) | H₂(g) | H⁺(aq) || Ag⁺(aq) | Ag(s) What is the balanced overall (net) cell reaction