Exam 17: Electron Transfer Reactions

Calculate the standard potential of voltaic cells that combine the following half reactions:Pb to PbSO₄ and PbO₂ to PbSO₄ (acid solution)(If needed, refer to Table 17-1.in the text )

Use the half-reaction method to balance the following redox reaction: Cl₂ $\rightarrow$ Cl^- + ClO^- (basic solution)

Consider the redox process: Cd(OH)₂ + Ni(OH)₂ + 2 OH^- $\rightarrow$ NiO₂ + Cd + H₂OWrite the equation for the spontaneous process and determine the free energy change for the spontaneous process.

An electrolytic cell driving the following redox reaction has a current of 4.02 amps passed through it for 2.32 hours. How much Ag will be dissolved and how much Cu will be deposited?2 Ag (s) + Cu⁺² (aq) $\rightarrow$ 2 Ag⁺ (aq) + Cu (s)

For the reaction given, which half reaction occurs at the cathode? NiO₂ + Cd + H₂O $\rarr$ Cd(OH)₂ + Ni(OH)₂ + 2 OH^-

Assign oxidation numbers to all the elements in LiAlH₄.

Calculate the standard potential of the redox reaction: 2 Na + S $\rightarrow$ Na₂S (E° for S + 2e^- = S^2- = -0.508 V(If needed, refer to Table 17-1. in the text)

An electrochemical cell is made by immersing a piece of Cd metal into a solution of 0.100 M CdSO₄ and a Zn electrode into a solution of 1.00 M ZnSO₄ and placing a salt bridge to allow ion flow between the two solutions.a) What voltage will be produced by the cell and b) what metal is the anode? (Cd²⁺ + 2e^- $\rightarrow$ Cd; E° = -0.402 V)(If needed, refer to Table 17-1 in the text)

Determine what causes the following electrolytic cell (which includes 50 g of metallic Ag and 1 L of 0.15 M Cu(NO₃)₂ ) to cease operation and determine how long the cell can sustain a current of 5 amps. 2 Ag (s) + Cu⁺² (aq) $\rightarrow$ 2 Ag⁺ (aq) + Cu (s)

If the coefficient of I^- is 1, determine the number of electrons transferred: OCl^- + I^- $\rightarrow$ Cl^- + IO^-

Assign oxidation numbers to all the elements in HCO₂H.

Determine the coefficient for Sn⁺² in the following balanced redox reaction.MnO₄^- + Sn²⁺ $\rarr$ Sn⁴⁺ + Mn²⁺ (acidic solution)

The lead-acid battery used in automobiles utilizes the following redox reaction: PbO₂(s) + Pb (s) + 2 HSO₄^- (aq) + 2 H₃O⁺ (aq) $\rightarrow$ 2 PbSO₄(s) + 4 H₂O (l) E°= 2.04 VWhat mass of H₂ being oxidized by O₂ under standard acid conditions would be required to give the same amount of electrons as one mole of lead oxide?(If needed, refer to Table 17-1 in the text)

Assign oxidation numbers to all the elements in sodium bicarbonate, NaHCO₃.

Consider the redox reaction of triiodide and oxygen:I₃^- + O₂ $\rarr$ I₂ + OH^- (basic solution)If the coefficient of I₃^- is 4 in the balanced equation, what is the coefficient of OH^-?

For the reaction given below, identify the anode and describe what happens to the electrode as the reaction continues. 3Fe(s) + Cr₂O₇^2-(aq) + 14 H⁺(aq) $\rarr$ 3Fe²⁺(aq) + 2 Cr⁺³(aq) + 7H₂O(l)

Assign oxidation numbers to all the elements in KCN.

Which elements are changing oxidation states in the following reaction? Zn(s) + 2 MnO₂(s) + H₂O(l) $\rarr$ Zn(OH)₂(s) + Mn₂O₃(s)

Calculate the standard free energy change for the redox reaction between silver ion and copper to give copper (II) and silver metal.(If needed, refer to Table 17-1 in the text)

Consult a table of reduction potentials (Table 17-1 in the text) and determine which two metals are capable of reducing iron (II) to iron under standard conditions.