A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours.Calculate the mass of cadmium metal deposited.

A) 3.2 × 10-7 g B) 1.2 × 10-3 g C) 4.2 g D) 8.4 g E) 16.8 g A) 3.2 × 10-7 g B) 1.2 × 10-3 g C) 4.2 g D) 8.4 g E) 16.8 g

Calculate the cell emf for the following reaction at 25°C: 2Ag+(0.010 M)+ H2(1 atm)$\rarr$ 2Ag(s)+ 2H+(pH = 10.0)

A) 1.04 V B) 1.27 V C) 0.92 V D) 0.56 V E) 0.80 V A) 1.04 V B) 1.27 V C) 0.92 V D) 0.56 V E) 0.80 V

Calculate $\Delta$G° for the electrochemical cell Fe(s)| Fe2+(aq)|| Sn4+(aq)| Sn2+(aq)| Pt(s)

A) -5.5 x 101 kJ/mol B) -1.1 x 102 kJ/mol C) 6.0 x 101 kJ/mol D) 1.1 x 105 kJ/mol E) 1.2 x 102 kJ/mol A) -5.5 x 101 kJ/mol B) -1.1 x 102 kJ/mol C) 6.0 x 101 kJ/mol D) 1.1 x 105 kJ/mol E) 1.2 x 102 kJ/mol

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° = +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

Consider the following reaction: 2Fe2+(aq)+ Cu2+ $\rarr$ 2Fe3+(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

A) 0.43 V B) 1.11 V C) 0.78 V D) -0.43 V E) 0 V A) 0.43 V B) 1.11 V C) 0.78 V D) -0.43 V E) 0 V

The measured voltage of the cell Pt(s)| H2 (1.0 atm)| H+(aq)|| Ag+(1.0 M)| Ag(s)is 1.02 V at 25°C.Calculate the pH of the solution.

A) 1.86 B) 1.69 C) 3.72 D) 3.89 E) 7.43 A) 1.86 B) 1.69 C) 3.72 D) 3.89 E) 7.43

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl2 for 4.50 hours.How many moles of calcium metal should be deposited?

A) 5.83 × 10-5 mol B) 0.210 mol C) 0.420 mol D) 0.840 mol E) 1.95 × 109 mol A) 5.83 × 10-5 mol B) 0.210 mol C) 0.420 mol D) 0.840 mol E) 1.95 × 109 mol

For the electrochemical cell Pt(s)| H2(1 atm)| H+(1 M)|| Cu2+(1 M)| Cu(s), which one of the following changes will cause an increase in the cell voltage?

A) Lower the H2(g)pressure. B) Increase the size/mass of the copper electrode. C) Lower the H+(aq)concentration. D) Decrease the concentration of Cu2+ ion. E) None of the above. A) Lower the H2(g)pressure. B) Increase the size/mass of the copper electrode. C) Lower the H+(aq)concentration. D) Decrease the concentration of Cu2+ ion. E) None of the above.

Exam 18: Electrochemistry

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?

(Short Answer)

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Question 41

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl₂ for 2.5 hours.Calculate the mass of cadmium metal deposited.

(Multiple Choice)

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Question 42

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25°C?

(Multiple Choice)

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Question 43

Which of these metals will reduce water to hydrogen in basic solution under standard conditions?

(Multiple Choice)

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Question 44

Aluminum does not corrode as does iron, because

(Multiple Choice)

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Question 45

Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M)+ H₂(1 atm) $\rarr$ 2Ag(s)+ 2H⁺(pH = 10.0)

(Multiple Choice)

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Question 46

Complete and balance the following redox equation.What is the coefficient of OH^-when the equation is balanced using the set of smallest whole-number coefficients? MnO₄^- + I^- $\rarr$ MnO₂ + IO₃^- (basic solution)

(Multiple Choice)

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Question 47

Which of these metals will not be oxidized in hydrochloric acid under standard conditions at 25°C?

(Multiple Choice)

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Question 48

Calculate E°_cell for the following electrochemical cell: Ni(s)| Ni²⁺(aq)|| Hg₂²⁺(aq)| Hg(l)| Pt(s)

(Short Answer)

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Question 49

Given the following standard reduction potentials, calculate the formation constant of Ag(NH₃)₂⁺at 25°C.

(Multiple Choice)

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Question 50

Calculate $\Delta$ G° for the electrochemical cell Fe(s)| Fe²⁺(aq)|| Sn⁴⁺(aq)| Sn²⁺(aq)| Pt(s)

(Multiple Choice)

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Question 51

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° = +0.07 V.

(Multiple Choice)

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Question 52

Consider the following reaction: 2Fe²⁺(aq)+ Cu²⁺ $\rarr$ 2Fe³⁺(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

(Multiple Choice)

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Question 53

The measured voltage of the cell Pt(s)| H₂ (1.0 atm)| H⁺(aq)|| Ag⁺(1.0 M)| Ag(s)is 1.02 V at 25°C.Calculate the pH of the solution.

(Multiple Choice)

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Question 54

Write the formula of the strongest reducing agent.given the following standard reduction potentials in acid solution

(Short Answer)

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Question 55

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl₂ for 4.50 hours.How many moles of calcium metal should be deposited?

(Multiple Choice)

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Question 56

For the electrochemical cell Pt(s)| H₂(1 atm)| H⁺(1 M)|| Cu²⁺(1 M)| Cu(s), which one of the following changes will cause an increase in the cell voltage?

(Multiple Choice)

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Question 57

Which of the following is true concerning a galvanic cell?

(Multiple Choice)

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Question 58

Using a table of standard electrode potentials, decide which of the following statements is completely true.

(Multiple Choice)

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Question 59

Consider an electrochemical cell based on the following cell diagram: Pt | Pu³⁺(aq), Pu⁴⁺(aq)|| Cl₂(g), Cl^-(aq)| Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu⁴⁺/Pu³⁺)?

(Multiple Choice)

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Question 60

Showing 41 - 60 of 154

Exam 18: Electrochemistry

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours.Calculate the mass of cadmium metal deposited.

Which of these metals will be oxidized in hydrochloric acid under standard conditions at 25°C?

Which of these metals will reduce water to hydrogen in basic solution under standard conditions?

Aluminum does not corrode as does iron, because

Calculate the cell emf for the following reaction at 25°C: 2Ag+(0.010 M)+ H2(1 atm) →\rarr→ 2Ag(s)+ 2H+(pH = 10.0)

Complete and balance the following redox equation.What is the coefficient of OH- when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + I- →\rarr→ MnO2 + IO3- (basic solution)

Which of these metals will not be oxidized in hydrochloric acid under standard conditions at 25°C?

Calculate E°cell for the following electrochemical cell: Ni(s)| Ni2+(aq)|| Hg22+(aq)| Hg(l)| Pt(s)

Given the following standard reduction potentials, calculate the formation constant of Ag(NH3)2+ at 25°C.

Calculate Δ\DeltaΔ G° for the electrochemical cell Fe(s)| Fe2+(aq)|| Sn4+(aq)| Sn2+(aq)| Pt(s)

Consider the following reaction: 2Fe2+(aq)+ Cu2+ →\rarr→ 2Fe3+(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

The measured voltage of the cell Pt(s)| H2 (1.0 atm)| H+(aq)|| Ag+(1.0 M)| Ag(s)is 1.02 V at 25°C.Calculate the pH of the solution.

Write the formula of the strongest reducing agent.given the following standard reduction potentials in acid solution

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl2 for 4.50 hours.How many moles of calcium metal should be deposited?

For the electrochemical cell Pt(s)| H2(1 atm)| H+(1 M)|| Cu2+(1 M)| Cu(s), which one of the following changes will cause an increase in the cell voltage?

Which of the following is true concerning a galvanic cell?

Using a table of standard electrode potentials, decide which of the following statements is completely true.

Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq)|| Cl2(g), Cl- (aq)| Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu4+/Pu3+)?

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A current of 0.80 A was applied to an electrolytic cell containing molten CdCl₂ for 2.5 hours.Calculate the mass of cadmium metal deposited.

Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M)+ H₂(1 atm) $\rarr$ 2Ag(s)+ 2H⁺(pH = 10.0)

Complete and balance the following redox equation.What is the coefficient of OH^-when the equation is balanced using the set of smallest whole-number coefficients? MnO₄^- + I^- $\rarr$ MnO₂ + IO₃^- (basic solution)

Calculate E°_cell for the following electrochemical cell: Ni(s)| Ni²⁺(aq)|| Hg₂²⁺(aq)| Hg(l)| Pt(s)

Given the following standard reduction potentials, calculate the formation constant of Ag(NH₃)₂⁺at 25°C.

Calculate $\Delta$ G° for the electrochemical cell Fe(s)| Fe²⁺(aq)|| Sn⁴⁺(aq)| Sn²⁺(aq)| Pt(s)

Consider the following reaction: 2Fe²⁺(aq)+ Cu²⁺ $\rarr$ 2Fe³⁺(aq)+ Cu. When the reaction comes to equilibrium, what is the cell voltage?

The measured voltage of the cell Pt(s)| H₂ (1.0 atm)| H⁺(aq)|| Ag⁺(1.0 M)| Ag(s)is 1.02 V at 25°C.Calculate the pH of the solution.

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl₂ for 4.50 hours.How many moles of calcium metal should be deposited?

For the electrochemical cell Pt(s)| H₂(1 atm)| H⁺(1 M)|| Cu²⁺(1 M)| Cu(s), which one of the following changes will cause an increase in the cell voltage?

Consider an electrochemical cell based on the following cell diagram: Pt | Pu³⁺(aq), Pu⁴⁺(aq)|| Cl₂(g), Cl^-(aq)| Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu⁴⁺/Pu³⁺)?