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Exam 19: Electrochemistry

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Question 1

Multiple Choice

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Under standard-state conditions, which of the following half-reactions occurs at the cathode during the electrolysis of aqueous nickel sulfate at 25°C?

A) 2H₂O $\to$ O₂ + 4H⁺ + 4e^-
B) Ni²⁺ + 2e^- $\to$ Ni
C) 2H₂O + 2e^- $\to$ H₂ + 2OH^-
D) Ni $\to$ Ni²⁺ + 2e^-

E) A) and C)
F) B) and C)

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Question 2

Multiple Choice

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Complete and balance the following redox equation. The sum of the smallest whole-number coefficients is Br₂ $\to$ BrO₃^- + Br^- (basic solution)

A) 9
B) 12
C) 18
D) 21
E) None of the above.

F) A) and B)
G) A) and E)

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Question 3

Multiple Choice

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Complete and balance the following redox equation using the set of smallest whole-number coefficients. Now sum the coefficients of all species in the balanced equation. (Remember the coefficients that are equal to one.) The sum of the coefficients is BrO₃^-(aq) + Sb³⁺(aq) $\to$ Br^-(aq) + Sb⁵⁺(aq) (acidic solution)

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO₃(aq)using a current of 6.0 A?

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn²⁺ || NO₃^- (acid soln) , NO(g) | Pt

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, what will happen to the cell potential?

What concentration of Ni²⁺ ion remains in solution after electrolysis of 100.mL of 0.250 M NiSO₄ solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

In an electrolytic cell, electrical energy is used to cause a chemical reaction to occur that would otherwise be nonspontaneous.

The half-reaction occurring at the cathode during electrolysis of an aqueous copper(II) iodide solution is

Complete and balance the following redox reaction under acidic conditions: MnO₄^-(aq)+ C₂O₄^2-(aq) $\to$ Mn²⁺(aq)+ CO₂(aq)

Given the following standard reduction potentials in acid solution write the formula of the weakest reducing agent.

You wish to electroplate a metal utensil with a surface area of 736 cm² with gold to give an average thickness of 0.025 mm over the entire surface.Starting with a solution of excess Au³⁺ and applying a constant current of 14 A, how long will it take to electroplate the utensil? The density of gold is 19.3 g/cm³.

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl₂. If E_cell is found to be 0.24 V, what is the pH of the acetic acid solution?

Complete and balance the following redox reaction under acidic conditions: Cu(s)+ NO₃^-(aq) $\to$ Cu²⁺(aq)+ NO₂(g)

Complete and balance the following redox equation using the smallest whole-number coefficients. What is the coefficient of Sn in the balanced equation? Sn + HNO₃ $\to$ SnO₂ + NO₂ + H₂O (acidic solution)

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO₂(s) + Cl^- $\to$ Pb²⁺ + Cl₂(g) (acidic solution)

Given the following standard reduction potentials in acid solution write the formula of the strongest oxidizing agent.

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

Complete and balance the following redox reaction under acidic conditions: Cr₂O₇^2-(aq)+ I^-(aq) $\to$ Cr³⁺(aq)+ IO₃^-(aq)

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO₄ for 90.0 min?