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A voltaic cell consists of a Pb/ Pb2+ half-cell and a Cu/Cu2+ half-cell at 25°C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively.

b. What is the cell potential when the concentration of Cu 2+ has fallen to 0.200 M?

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A voltaic cell consists of a Pb/ Pb2+ half-cell and a Cu/Cu2+ half-cell at 25°C. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively.

a. What is the initial cell potential?

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An electrochemical cell is based on these two half-reactions:

Ox: Sn(s) → Sn2+(aq, 2.00 M) + 2e
Red: ClO2(g, 0.100 atm) + e → ClO2(aq, 2.00 M)

Calculate the cell potential at 25 °C.

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A voltaic cell employs the redox reaction:
2Fe3+(aq) + 3Mg(s) → 2Fe(s) + 3Mg2+(aq).

Calculate the cell potential at 25°C under each set of conditions

c. [Fe3+] = 2.00 M; [Mg2+] = 1.5 x 103 M

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A voltaic cell employs the redox reaction:
2Fe3+(aq) + 3Mg(s) → 2Fe(s) + 3Mg2+(aq).

Calculate the cell potential at 25°C under each set of conditions

b. [Fe3+] = 1.0 X 103 M; [Mg2+] = 2.50 M

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A voltaic cell employs the redox reaction:
2Fe3+(aq) + 3Mg(s) → 2Fe(s) + 3Mg2+(aq)

Calculate the cell potential at 25°C under each set of conditions.

a. standard cond itions

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Calculate Δrxn and cell for a redox reaction with n = 3 that has an equilibrium constant of K = 0.050 (at 25 °C).

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Calculate the equilibrium constant for the reaction between Fe 2+(aq) and Zn(s) (at 25°C).

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Calculate the equilibrium constant for each of the reactions in Problem 66.

a. 2 Fe3+(aq) + 3 Sn(s) → 2 Fe(s) + 3 Sn 2+(aq)

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Use tabulated electrode potentials to calculate Δ G°rxn for each reaction at 25°C.

c. Br2(l) + 2 I (aq) → 2 Br (aq) + I2(s)

 

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Use tabulated electrode potentials to calculate Δ G°rxn for each reaction at 25°C.

b. O2(g) + 2 H2O(l) + 2 Cu(s) → 4 OH(aq) + 2 Cu 2+(aq)

 

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Use tabulated electrode potentials to calculate Δ G°rxn for each reaction at 25°C.

a. 2 Fe3+(aq) + 3 Sn(s) → 2 Fe(s) + 3 Sn 2+(aq)

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Which metal is the best reducing agent?

a. Mn

b. Al

c. Ni

d. Cr

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Which metal cation is the best oxidizing agent?

a. Pb2+

b. Cr3+

c. Fe2+

d. Sn2+

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Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written.

c. PbO2(s) + 4 H+(aq) + Sn(s) → Pb 2+(aq) + 2 H2O (l) + Sn2+(aq)

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Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written.

b. Br2(l) + 2 I (aq) → 2 Br (aq) + I 2(s)

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Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written.

a. O2(g) + 2 H2O (l) + 4 Ag(s) → 4 OH  (aq) + 4 Ag +(aq)

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Determine whether or not each metal dissolves in 1 M HIO 3. For those metals that do dissolve, write a balanced redox equation for the reaction that occurs.

a. Au

b. Cr

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Determine whether or not each metal dissolves in 1 M HCl. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves.

a. Cu

b. Fe

c. Au

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Which metal can be oxidized with an Sn 2+ solution but not with an Fe 2+ solution?

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Determine whether or not each redox reaction occurs spontaneously in the forward direction.

d. 2 Al(s) + 3 Pb 2+(aq) → 2 Al 3+(aq) + 3 Pb(s)

 

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Determine whether or not each redox reaction occurs spontaneously in the forward direction.

c. Fe(s) + Mn2+(aq) → Fe2+(aq) + Mn(s)

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Determine whether or not each redox reaction occurs spontaneously in the forward direction.

b. 2 Ag+(aq) + Ni(s) → 2 Ag(s) + Ni 2+(aq)

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Determine whether or not each redox reaction occurs spontaneously in the forward direction.
a. Ca2+(aq) + Zn(s) → Ca(s) + Zn2+(aq)

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Make a sketch of the voltaic cell represented by the line notation. Write the overall balanced equation for the reaction and calculate E°cell.

Mn(s) | Mn2+(aq) || ClO2(aq) | ClO2(g) | Pt(s)

 

 

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