Exam 17: Electron Transfer Reactions

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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 )

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

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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.  Consider the redox process: Cd(OH)<sub>2</sub> + Ni(OH)<sub>2</sub> + 2 OH<sup>-</sup><sup> </sup> \rightarrow NiO<sub>2</sub> + Cd + H<sub>2</sub>OWrite the equation for the spontaneous process and determine the free energy change for the spontaneous process.

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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)

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

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Assign oxidation numbers to all the elements in LiAlH4.

(Multiple Choice)
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Calculate the standard potential of the redox reaction: 2 Na + S \rightarrow Na2S (E° for S + 2e- = S2- = -0.508 V(If needed, refer to Table 17-1. in the text)

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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)

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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)

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

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Assign oxidation numbers to all the elements in HCO2H.

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

(Multiple Choice)
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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)

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

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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-?

(Multiple Choice)
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For the reaction given below, identify the anode and describe what happens to the electrode as the reaction continues. 3Fe(s) + Cr2O72-(aq) + 14 H+(aq) \rarr 3Fe2+(aq) + 2 Cr+3(aq) + 7H2O(l)

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Assign oxidation numbers to all the elements in KCN.

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

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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)

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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.

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