Exam 17: Electron Transfer Reactions

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Calculate the standard free energy changes for the following redox reaction: 2 Ag+(aq) + Sn2+(aq) \rightarrow 2 Ag(s) + Sn4+(aq) [E°(Sn4+, 2+) = 0.151 V](If needed, refer to Table 17-1 in the text)

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What are the possible oxidation states of corroded iron?(If needed, refer to Table 17-1 in the text)

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Balance the following half reaction under neutral conditions:HSO3- \rightarrow SO42-

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For the working galvanic cell shown at standard conditions, determine the balanced reaction and direction of electron flow through the wire. For the working galvanic cell shown at standard conditions, determine the balanced reaction and direction of electron flow through the wire.   (If needed, refer to Table 17-1 in the text ) (If needed, refer to Table 17-1 in the text )

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Consider the Daniell cell where the cell reaction and standard potential are:Zn(s) + Cu2+ (aq) \rarr Zn2+ (aq) + Cu (s) \quad E° = 1.10 VIf the cell is initially at standard conditions ([Cu2+] = [Zn2+] = 1.00 M), what are the concentrations of Cu2+ and Zn2+ when the cell potential has fallen to 1.06 V?If needed, use the following equation: Δ\Delta G° = -nFE°, E°  Consider the Daniell cell where the cell reaction and standard potential are:Zn(s) + Cu<sup>2+</sup><sup> </sup>(aq)  \rarr Zn<sup>2+</sup><sup> </sup>(aq) + Cu (s)  \quad E° = 1.10 VIf the cell is initially at standard conditions ([Cu<sup>2+</sup>] = [Zn<sup>2+</sup>] = 1.00 M), what are the concentrations of Cu<sup>2+</sup><sup> </sup>and Zn<sup>2+</sup> when the cell potential has fallen to 1.06 V?If needed, use the following equation: \Delta G° = -nFE°, E°   , E = E° -   , moles e<sup>-</sup> =   (If needed, refer to Table 17-1in the text) , E = E° -  Consider the Daniell cell where the cell reaction and standard potential are:Zn(s) + Cu<sup>2+</sup><sup> </sup>(aq)  \rarr Zn<sup>2+</sup><sup> </sup>(aq) + Cu (s)  \quad E° = 1.10 VIf the cell is initially at standard conditions ([Cu<sup>2+</sup>] = [Zn<sup>2+</sup>] = 1.00 M), what are the concentrations of Cu<sup>2+</sup><sup> </sup>and Zn<sup>2+</sup> when the cell potential has fallen to 1.06 V?If needed, use the following equation: \Delta G° = -nFE°, E°   , E = E° -   , moles e<sup>-</sup> =   (If needed, refer to Table 17-1in the text) , moles e- =  Consider the Daniell cell where the cell reaction and standard potential are:Zn(s) + Cu<sup>2+</sup><sup> </sup>(aq)  \rarr Zn<sup>2+</sup><sup> </sup>(aq) + Cu (s)  \quad E° = 1.10 VIf the cell is initially at standard conditions ([Cu<sup>2+</sup>] = [Zn<sup>2+</sup>] = 1.00 M), what are the concentrations of Cu<sup>2+</sup><sup> </sup>and Zn<sup>2+</sup> when the cell potential has fallen to 1.06 V?If needed, use the following equation: \Delta G° = -nFE°, E°   , E = E° -   , moles e<sup>-</sup> =   (If needed, refer to Table 17-1in the text) (If needed, refer to Table 17-1in the text)

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Assign oxidation numbers to all the elements in NO2-.

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For the reaction given below, which half reaction occurs at the anode? 2 H2(g) + O2(g) \rarr 2 H2O(l)

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Use oxidation numbers to show what is being oxidized and what is being reduced in a redox reaction.

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Calculate the standard potential of the aluminium air battery in which the active materials Al(s) andO2, and the electrolyte is aqueous KOH.(If needed, refer to Table 17-1 in the text)

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Which of the following are redox reactions? I. 2 N2 + 3 H2 \rarr 2 NH3 II. 4 Al + 3 O2 \rarr 2 Al2O3 III. 2 NO2 \rarr N2O4 IV. FeCl3 (aq) + 6 NH3(aq) (\rarr\)Fe(NH3)63+ (aq) + 3 Cl- (aq) V. Cu2+ + Zn \rarr Cu + Zn2+

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Balance the following half reaction under basic conditions:NO3- \rightarrow NO2-

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Consider the redox reaction of nitric acid and copper: Cu + HNO3 \rarr Cu(NO3)2 + NO (acidic solution)If the coefficient of Cu is 3 in the balanced equation, what is the coefficient of HNO3?

(Multiple Choice)
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The same charge of 1.07 x 104 C is passed through three solutions: one each of Au3+, Cu+ and Pb2+ with strips of the metals as cathodes. In which cell will the greatest mass of metal be reduced and what is the mass of that metal?

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Describe galvanic cells.

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Balance the following half reaction under acidic conditions:I2O5 \rightarrow I2

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Consider the Daniell cell for which the cell reaction and standard potential are:Zn(s) + Cu2+ (aq) \rightarrow Zn2+ (aq) + Cu (s) E° = 1.10 VIf the cell is initially at standard conditions ([Cu2+] = [Zn2+] = 1.00 M) and assuming it contains 1 L of electrolyte, determine the mass of Zn(s) lost when the cell potential falls to 1.06 V?(If needed, refer to Table 17-1in the text)

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Balance the reaction and calculate the standard potential for: Zr + H2O \rightarrow ZrO2 + H2Given: ZrO2 + 4e- + 4 H3O+ \rightarrow Zr + 6 H2O (E°=-1.43 V)(If needed, refer to Table 17-1 in the text)

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Assign oxidation numbers to all the elements in titanium nitride, Ti3N4.

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Calculate the equilibrium constants for the following redox reaction: 2 Cu2+ (aq) + Sn2+ (aq) \rightarrow 2 Cu+ (aq) + Sn4+ (aq)[E°(Sn4+, 2+) = 0.151 V] [E°(Cu2+, 1+) = 0.153 V](If needed, refer to Table 17-1 in the text)

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Ships, storage tanks, and other large metal items may be protected from corrosion by(If needed, refer to Table 17-1in the text )

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