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Exam 17: Electron Transfer Reactions

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Question 1

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Consider an electrochemical cell of the type shown in the figure where the redox half-reaction in both compartments has the identical standard potentials: Use the Nernst equation to calculate the potential developed by this cell.(If needed, refer to Table 17-1 in the text)

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Question 2

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For the reaction given below, which half reaction occurs at the cathode?Pb(s) + PbO₂(s) + 2HSO₄^-(aq) + 2H₃O⁺(aq) $\rarr$ 2PbSO₄(aq) +4H₂O(l)

A) Pb $\rarr$ PbSO₄
B) PbO₂ $\rarr$ PbSO₄
C) HSO₄^- $\rarr$ PbSO₄
D) H₃O⁺ $\rarr$ H₂O
E) PbSO₄ $\rarr$ PbO₂

F) A) and B)
G) A) and C)

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Question 3

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Explain electrolytic reactions and cells.

Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NO₃) ₂ electrolyte connected through a salt bridge to a Ag wire coated in AgCl(s) immersed in an aqueous KCl solution. Is the standard cell and balanced galvanic cell reaction:(If needed, refer to Table 17-1 in the text )

Which of the species listed is the strongest oxidizing agent?‪ (If needed, refer to Table 17-1 in the text)

Explain the chemistry of everyday redox reactions.

Balance the following half reaction under acidic conditions:OCl^- $\rightarrow$ Cl^-

Consider an automobile which is powered by a perfectly efficient fuel cell that consumes hydrogen and oxygen in the following redox reaction: 2H₂(g) + O₂(g) $\rightarrow$ 2 H₂O (l)If the electric system requires a current of 500 amperes, how many g of H₂ are consumed per hour?(If needed, refer to Table 17-1 in the text )

Balance redox reactions using the half-reaction method.

Which of the species listed is the strongest reducing agent? (If needed, refer to Table 17-1 in the text )

Calculate standard cell potentials.

What is the role of the electrolyte in a galvanic cell?

An electrochemical cell is constructed that contains Cr³⁺(aq) and Cr metal as the electrode in one compartment and Cu²⁺(aq) and copper metal in the other compartment. Calculate the expected standard potential upon appropriately connecting the cell and describe the direction of electron and cation flow.(If needed, refer to Table 17-1 in the text)

Balance the following half reaction under basic conditions: MnO₄^- $\rightarrow$ MnO_2(s)

Relate cell potential to the reaction conditions.

Draw a figure illustrating how a cell would be arranged for the redox reaction of copper with silver ion but using indirect electron transfer and a salt bridge with KNO₃ solution. Indicate the direction of electron flow in the wire and the movement of ions in the salt bridge.

Nitrogen has many possible oxidation numbers; put the following nitrogen compounds in order of increasing oxidation number: NO₂, HNO₃, NO₂^-, NO.

The following reaction occurs in a galvanic cell: NiO₂ + Cd + H₂O $\rarr$ Cd(OH) ₂ + Ni(OH) ₂ + 2 OH^-Which redox process in this battery occurs at a passive electrode?

For a brine electrolysis cell (see redox reaction below) operating at 60,000 amps, how many kg of NaOH and Cl₂ would be produced in 24.0 hours? 2 NaCl (aq) + 2 H₂O $\rightarrow$ 2 NaOH (aq) + Cl₂(g) + H₂ (g)

Platinum metal is quite resistant to oxidation as may be deduced by its reduction potential:Pt²⁺ + 2e $\rarr$ $\quad$ Pt E° $\thickapprox$ 1.2 VExamine a table of reduction potentials (Table 17-1 in the text) and determine two elements capable of oxidizing platinum under standard conditions.